Next Article in Journal
Effects of Soil Amendments on Heavy Metal Immobilization and Accumulation by Maize Grown in a Multiple-Metal-Contaminated Soil and Their Potential for Safe Crop Production
Previous Article in Journal
A Relevant Screening of Organic Contaminants Present on Freshwater and Pre-Production Microplastics
Font Type:
Arial Georgia Verdana
Font Size:
Aa Aa Aa
Line Spacing:
Column Width:

Removal of Heavy Metals from Wastewaters: A Challenge from Current Treatment Methods to Nanotechnology Applications

Ruxandra Vidu
Ecaterina Matei
Andra Mihaela Predescu
Badriyah Alhalaili
Cristian Pantilimon
Claudia Tarcea
1 and
Cristian Predescu
Faculty of Materials Science and Engineering, University Politehnica of Bucharest,060042 Bucharest, Romania
Department of Electrical & Computer Engineering, University of California, Davis, CA 95616, USA
Nanotechnology and Advanced Materials Program, Kuwait Institute for Scientific Research, Kuwait City 13109, Kuwait
Authors to whom correspondence should be addressed.
Toxics 2020, 8(4), 101;
Submission received: 29 September 2020 / Revised: 5 November 2020 / Accepted: 6 November 2020 / Published: 10 November 2020
(This article belongs to the Section Environmental Chemistry)


Removing heavy metals from wastewaters is a challenging process that requires constant attention and monitoring, as heavy metals are major wastewater pollutants that are not biodegradable and thus accumulate in the ecosystem. In addition, the persistent nature, toxicity and accumulation of heavy metal ions in the human body have become the driving force for searching new and more efficient water treatment technologies to reduce the concentration of heavy metal in waters. Because the conventional techniques will not be able to keep up with the growing demand for lower heavy metals levels in drinking water and wastewaters, it is becoming increasingly challenging to implement technologically advanced alternative water treatments. Nanotechnology offers a number of advantages compared to other methods. Nanomaterials are more efficient in terms of cost and volume, and many process mechanisms are better and faster at nanoscale. Although nanomaterials have already proved themselves in water technology, there are specific challenges related to their stability, toxicity and recovery, which led to innovations to counteract them. Taking into account the multidisciplinary research of water treatment for the removal of heavy metals, the present review provides an updated report on the main technologies and materials used for the removal of heavy metals with an emphasis on nanoscale materials and processes involved in the heavy metals removal and detection.

1. Introduction

In the rapid global industrialization, there is a constant effort to improve the use-reuse cycle of water and to protect water resources through legislation, which is the driving force for research and innovation. In addition to numbers and statistics, there is the health factor that cannot be quantified when it comes to people. Water pollution with heavy metals is one of the most harmful pollution throughout the globe due to their non-degradable properties. Despite the national and international standards stipulated by the World Health Organization (WHO) and the United States Environmental Protection Agency (USEPA) that the drinking water should not exceed a maximum concentration of a few to a few tens of µg/L [1,2], heavy metals can accumulate in the ecosystem and enter the human body through food. Table 1 summarizes the acceptable limitations of various heavy metals according to the World Health Organization [2] and the United States Environmental Protection Agency (USEPA) [1]. That is why the need for efficient, fast, reliable and accurate methods to completely remove heavy metals from wastewaters including sewage irrigation, exhaust emissions, and mining became increasingly important for our safe drinking water.
Because heavy metals do not degrade in nature, they contaminate natural resources. In waters, heavy metals such as cadmium, chromium, arsenic, lead and mercury are highly toxic for human health even at trace levels (Figure 1). In concentrations higher than a few µg/L, heavy metals affect the normal development and function of organs, poisoning the human body and damaging internal organs and tissues by various mechanisms such as enzymes denaturation, ions replacement and proteins inactivation.
Because wastewater effluents show different severities in terms of contamination with pollutants, they are treated differently depending on their specific use. Pathogens and heavy metals represent factors that are unwanted in the water discharge from treatment plants, but certain elements such as nitrates and phosphorus can be beneficial if the effluent is used for agriculture, or they can be detrimental if the water is dumped into rivers [4,5].
Therefore, the development of tools and technologies to quantify, analyze and monitor heavy metals has become as important as the development of new technologies for the removal of heavy metal ions (HMIs) from waters. Nanotechnology can bridge the instrument-based analysis and technologies for HMIs removal. Santhosh et al. [6] have extensively reviewed the performance of nanomaterials in water treatment methods that make use of the adsorption, photocatalytic and antibacterial activity of nanomaterials. Advanced oxidation processes are technologies for the treatment of wastewaters and effluents with refractory organic pollutants that show future promise [7] and that use semiconductor photocatalysts to remove a large number of toxic pollutants.
Electrochemistry is an interdisciplinary study of the charge transfer at interfaces, which has a contradictory duality in the case of water treatment, and more specifically of the removal of HMIs from wastewater, i.e., it is both a source of heavy metals and a remedy. Electrochemistry is a source of water pollution because there are industries that are based entirely on electrochemical processes such as electroplating industries that dispose their solutions containing Zn, Pb, Cu, Cd, Cr and cyanides into the waters and the battery industry that poisons the waters with Pb, Hg and Cd. Besides water pollution from industries, there is corrosion, which is also an electrochemical process that contaminates the water with heavy metals coming from the metal plumbing, usually Pb. Miniaturization of electronics and devices is the driving force in the development of integrated nanostructures [8,9].
Whether it is nanomaterials, nanoparticles or nanomembranes, they do share the same properties and characteristics. Figure 2 shows how the main surface properties of nanomaterials and their unique characteristics combine and work together to confer them higher efficiency than the same bulk material. In Figure 2, nano-based materials used in adsorption studies, nanoscale metal oxides used in photocatalysis and nanoporous membranes for filtration and desalination are shown in the middle row, while their tunable properties, process variable and intrinsic properties are represented as satellite hexagons around them. This figure illustrates the complex and sometimes unique combination of variables, which is critically important in understanding the relationship between nanomaterial, composition and properties for high performance in a given application.
Several reviews have been published on water remediation for HMIs removal. Babel et al. [10] presented a critical analysis of the application of chemical extraction, bioleaching, electroreclamation, and supercritical fluid extraction, in removing heavy metals from contaminated sludge. Hua et al. [11] have extensively reviewed nanostructured metal oxides and porous host supported nanoparticles including their synthesis, physicochemical properties, adsorption characteristics and mechanism, as well as their application in HMIs removal. In a more recent review, comprehensive information on different adsorbents that are used for heavy metal removal, as well as on the commercially available and natural bioadsorbents used for removal of Cr, Cd and Cu, are provided [12].
Because of the multidisciplinary aspect of the research on the removal of heavy metals, the present review provides an updated report on the nanoscale materials and processes involved in the heavy metals’ removal and detection. New developments in the field of water treatment as well as existing technologies and future potential of those technologies that could greatly benefit from implementation of recent nanotechnology developments are presented. There are great opportunities for nanotechnology to clearly impact this area of water treatment and bridge various techniques to improve large scale applicability nanoscience-based technologies for HMIs removal.

2. Chemical and Physical Methods

2.1. Chemical Precipitation

Chemical methods are extensively used in water treatment for retaining metals, inorganic compounds, oils, fats and different organic materials from wastewaters. Precipitation is a process of leading pollutants, which are dissolved or suspended in solution, to form a solid precipitate which can be later separated from the liquid. The ions and particles can be easily removed with a large precipitate. Coagulants such as polymers are used in order to gather the small suspended particles into larger precipitates. The polymer molecules can be charged or neutral (i.e., cationic, anionic or nonionic). Because of the interaction between ions and charged particles in liquid, the polymers behave either as bonds between particles or particles neutralizer in solution. Depending on the contaminants that have to be removed, specific precipitation methods can be used [13].

2.1.1. Hydroxide Precipitation

In hydroxide precipitation, soluble heavy metal ions are converted into insoluble metal compounds by adding hydroxide. The aim of metals treatment by hydroxide precipitation is to form precipitates by adjusting the water pH. Theoretical and experimental studies were performed by Tunay et al. [14] to understand the mechanism of ligand-sharing effect of metals, which are added to wastewater to ensure effective removal of complexed heavy metals. This work indicated that high pH precipitation occurred when organic ligand can be effectively bound by a coagulant or pH adjustment agent, thus freeing the heavy metal to form hydroxide or carbonate solids [14]. After metal precipitation and solids forming, they can be very easily removed from waters. The main factors influencing the metal precipitation are the metal concentrations and water pH. Hydroxide precipitation is efficiently used in the case of small quantities of heavy metals in water (1–100 mg/L) and in acidic or neutral pH media.

2.1.2. Sulfide Precipitation

A more complete heavy metals removal from wastewaters is provided by sulfides rather than hydroxides for the precipitation process. Usually, metal sulfides possess solubility several orders smaller in comparison with the corresponding hydroxides, making this technique superior to the hydroxide precipitation. Unlike hydroxide precipitation, sulfide precipitation is not sensitive to the presence of many chelating agents or complexes. Chromates and dichromates removal take place without the initial step of chromium reduction to Cr(III) [15]. Sulfide precipitation with Na2S was found to be highly effective in the removal of Cd, Zn and Cu from wastewaters by more than 99%, and As and Se removals by more than 98 and 92%, respectively [16]. The resulting sulfide metal sludges are better compressed and more stable than the hydroxide precipitation, demonstrating better dewatering and density characteristics.

2.1.3. Other Techniques Using Chemical Precipitation

Other reagents used in wastewater treatment by chemical precipitation are as follows:
  • Ferrous sulfate is usually used together with lime for water softening. The aggregates consist of calcium sulfate and ferric hydroxide. The condition for a successful removal process is that the wastewater must contain dissolved oxygen that is required by the chemical reaction to form the precipitate [17].
  • Aluminum for the removal of phosphate and water softening. The reaction takes place with phosphate or various alkaline compounds (i.e., bicarbonate, hydroxide or carbonate) that form insoluble aluminum slats [17].
  • Ferric chloride forming insoluble iron salts together with phosphates or alkaline compounds [17,18].
  • Polymers, which can be anionic, cationic or nonionic. They can be used for neutralization or as links coagulants after they are added to wastewaters [19].
Chemical precipitation has been used in order to remove heavy metals from municipal and industrial waters. Even though the chemical precipitation is a well-established technique, today’s research concentrates on merging this method with different other treatment techniques such as reverse osmosis and photochemical oxidation in order to boost the efficiency of heavy metal removal from wastewaters [20]. Table 2 presents the advantages and disadvantages of the chemical precipitation function of the coagulant used in the process.

2.2. Ion Exchange

Ion exchange process represents an efficient tool in the environmental protection with waste waters application. Over the last years, new or improved classical materials were tested as ion exchangers [21]. A large class of pollutants as metal ions could be identified in liquid effluents from industrial to nuclear [22,23,24,25,26,27] such as Cd2+, Pb2+ and Hg2+, as well as radionuclides as 137Cs, 89Sr, 235U, 59Fe, 57Co, 65Zn and anionic species: CrO4−2 and AsO4−3 [23,25]. For all these metal ions, a variety of removal methods were tested from precipitation [26], as an inexpensive and simple technique, to biological techniques with high costs and the same disadvantage regarding high quantity of sludge generation, such as precipitation [24]. Moreover, Hoch and co-workers reported good results with photocatalysis technique, but they identified the risk of appearance of undesirable compounds such as Cr(III) from Cr(VI) that is necessary to be removed [22].
In this context, ion-exchange technique is recognized as adequate and cost-effective technique, with high possibility for regeneration of used exchangers. Usually, conventional materials such as organic polymers or inorganic zeolites, clay are used as exchanger materials [28,29,30]. The removal capacity through ion exchange depends on chemistry selectivity of species, for example, organic materials with sulfonate, amino, thiol or amide functional groups are applied for water treatment with cadmium and nickel removal [31,32].
With the same efficiency, polymeric with carboxylate groups are able to removed Cd, Ni, Cu and Pb as traces from waste waters [33,34,35,36,37]. Even if there are some good results within these conventional materials, a few disadvantages are important enough to be mentioned: low capacity of reuse, kinetics and chemical and thermal stability for organic resin reuse [38,39,40,41,42].
This is the reason for which appears as a necessity to identify and testing new materials with ion exchange capacity. Thus, in the last years, the tendency was to obtain and test excellent materials, which expose multiple functional groups, high surface area and chemical and thermal stability [43,44,45,46,47]. In this context, metal-organic ion exchange materials are found as a combination between conventional materials with great porosity and binding groups [21,48,49]. An example of this type of materials could be zeolite nanoparticles impregnated with polysulfone used to remove Pb and Cd from waste waters [21].

2.3. Adsorption

2.3.1. Carbon-Based Adsorbents

Absorbents are generally characterized by heterogeneous and irregular surfaces, which promote the adsorption of HMIs. After the sorption of pollutants, the surface becomes smoother. When the impregnation with nanoparticles is used to modify the surface of adsorbents, macro-clusters are formed while the surface becomes more regular. Further surface treatment processes such as carbonization and calcination return the adsorbent surface to porous. Although other surface modifications such as chemical modification reduce the total surface area, they offer control on adjusting the functional groups in order to increase the adsorption capacity. Yang et al. [50] have recently reviewed the effects of various functional groups on HMIs adsorption onto different carbon materials, emphasizing the importance surface modification of carbon adsorbents in optimizing their physicochemical and sorptive properties in the development of new technologies for environmental remediation.

2.3.2. Carbon Nanotube (CNT) Absorbents

Table 3 presents a summary of the maximum adsorption capacities for some heavy metal ions on multiwalled carbon nanotubes (MWCNTs), single-walled carbon nanotubes (SWCNTs), oxidized CNTs and activated charcoal (granular activated charcoal (GAC) and powder activated charcoal (PAC).
Table 3 shows that the removal of Ni2+ by oxidized SWCNTs, (MWCNTs) and granular activated carbon (GAC) [58]. These adsorbents were investigated under the same conditions, and the results showed that SWCNTs and MWCNTs increased performance of Ni2+ sorption compared to GAC, which can be explained by the fact that the CNTs possess increased surface when compared to the GAC. According to Yang et al. [57], adsorption of Ni2+ on MWCNTs increases with the pH. Sorption affinity between Zn2+ and CNT surface is stronger than sorption affinity between Ni2+ and CNT surface [53].
The results reported by Wang et al. [52] have shown a high adsorption of Pb2+ by MWCNTs. The Pb2+ adsorption on MWCNTs proved to be faster than AC and more, Pb2+ can be recycled under acidified MWCNTs.
Regarding the removal of Zn2+, purified SWCNT and MWCNT are better adsorbents than powder activated carbon (PAC) under the same initial concentration even if the PAC has a high surface than carbon nanotubes [59]. Sorption affinity between carbon nanotubes and zinc ions is higher than the affinity between Pb2+ and carbon nanotubes. According to Naghizadeh et al. [56], Cd2+ has a lower affinity for activated carbon to MWCNTs, and the capacities of Cd2+ adsorption on AC and MWCNTs are 2.9 mg/g and 4.1 mg/g, respectively. Comparing the removal of Pb2+, Cu2+ and Cd2+ by oxidized MWCNTs, the results indicate that Pb2+ has an increased adsorption capacity compared to Cd2+ and Cu2+. The adsorption of various HMIs on oxidized MWCNTs is ordered as follows: Cd2+ < Cu2+ < Ni2+ < Pb2+. The maximum adsorption capacities of Zn2+ on SWCNTs, MWCNTs and PAC, which were calculated using the Langmuir model, are 43.66, 32.68 and 13.41 mg/g [60], respectively.

2.3.3. Low-Cost Bioadsorbents

The studies on low cost adsorbents have been focused on the separation of HMIs such as Pb2+, Zn2+, Ni2+ and Cd2+ from wastewaters. The results have shown that the percentages of HMIs removal depended on the amount of adsorbent, adsorbent concentration, pH and contact time.
Eggshells and their derivatives demonstrated a great potential for removing wastewater contaminated with nickel and silver ions. Comparing Eggshells and Eggshells with membrane, the values showed fast removal of Ni2+ and Ag for Eggshell membrane [61]. Moreover, according to Park et al. [62], the calcined eggshells showed a great potential for the adsorption of Cd2+ and Cr while the natural eggshells enhanced the adsorption of Pb2+. The removal efficiency for cadmium, zinc, chrome and lead was studied using chicken eggshells in aqueous solution [63] and wastewater [64]. These studies focused on the optimum pH, contact time, agitation speed and adsorbent dosages obtained from the experiment showed the ability of chicken eggshells for removing 99.7% of Cu2+ [63], 99% of Zn2+ [63], 85% of Cr, 82% of Pb2+, 86% Cd2+ [64] and 96.43% Fe [65]. These results can be explained by the increased number of active binding sites [63,66]. Eggshells are used also for wastewater treatment from battery productions due to their high removal efficiency and their natural characteristic as a pH adjuster [67]. These results also demonstrated that eggshells can be used pre-treatment of wastewaters due to the fact that they may remove a large quantity of heavy metals [62].
Agricultural Waste. Based on the previous study, agricultural water has the ability to remove heavy metals [68]. A good adsorbent with removal efficiency higher than 90% at pH 5 for heavy metals such as iron, copper and lead is Coconut husk [69,70]. More, a removal efficiency of 93% in 3 h of contact time, initial concentration of 25 mg/L of Zn2+ and pH 6.3 was obtained by the coconut shell after it was treated with acid and coated with chitosan. Another good adsorbent is coconut coir activated carbon, which was studied for copper and cadmium in water [71]. Rice husk is a low-cost adsorbent and contribute to economic yield [72]. Comparing polyaniline/rice husk with polyaniline and polyaniline/saw dust, polyaniline/rice husk showed a better efficiency removal of Cd2+ (93.08%) [73]. Comparing with values of the other adsorbents, the rice husk treated showed a higher adsorption capacity due to his surface area and pore size [74]. Nutshell has found to have ability to reduce heavy metals when modified cashew nuts. The maximum adsorption capacity of Cu2+ (406.6 mg/g), Cd2+ (436.7 mg/g), Zn2+ (455.7 mg/g) and Ni2+ (456.3 mg/g) [75]. Comparing chestnut shell pretreated with NaOH and pretreated with acid formaldehyde, the results showed that chestnut shell retreated with NaOH was more efficient in removing heavy metals [76,77,78]. Inyang et al. [79] reviewed the biochar as a low-cost adsorbent for the removal of heavy metal removal; they found that the sorption mechanisms depends on different biochars and HMI contaminants.

2.4. Membrane Filtration

The development of membranes and their filtration technologies has shown several advantages in the field of heavy metal removal due to their high efficiency, low space occupancy and simple design. The processes related to membrane filtration have been separated into reverse osmosis, ultrafiltration, electrodialysis and nanofiltration [70].

2.4.1. Ultrafiltration (UF)

This method is used when faced with low transmembrane pressures in order to remove dissolved and colloidal materials. The pores used in this type of membrane are larger than the metal ions (as hydrated ions) and only low molecular weight complexes can pass unhindered through the membrane. In order to increase the removal efficiency, two technologies were developed such as micellar enhanced ultrafiltration (MEUF) and polymer enhanced ultrafiltration (PEUF) [80]. Table 4 presents the removal efficiency of heavy metals depending on the membrane used in each technology.

2.4.2. Reverse Osmosis (RO)

In this method, a semi-permeable membrane is used, which separates the pollutant by allowing only the passage of the purified fluid. The method has the possibility to remove a large range of species, and it is used extensively in the desalination process [79]. In recent years, it has also been used in wastewater treatment and environmental engineering.

2.4.3. Nanofiltration (NF)

This filtration method is a combination of UF and RO and incorporates advantages of both techniques when it is used in the removal of HMIs such as nickel, chromium, copper and arsenic from wastewater. Table 5 presents a comparison between the efficiencies of heavy metals removal by RO, NF and combined RO+NF. The most notable advantages of this method are simplicity, reliability and low energy consumption combined with a high rate of removal [39].

2.5. Coagulation and Flocculation

Coagulation and flocculation are processes used to remove the heavy metals from wastewaters, which also require sedimentation and filtration to collect the foam. Some of the most known coagulants used for wastewaters treatment are aluminum, ferrous sulfate and ferric chloride, which produce particulates and pollutants from wastewaters through particles charge neutralization. El Samrani et al. [94] obtained excellent results with respect to the removal of HMIs from waters by coagulation combining sewer overflow with ferric chloride and polyaluminum chloride (PAC). Suspended particles and hydrophobic colloids are the essential pollutants removed with this method. A new type of coagulant such as amphoteric polyelectrolyte (sodium xanthogenate with polyethyleneimine) was introduced in the method for removal of both soluble heavy metals and insoluble substance [95].
Flocculation refers to the use of polymers in order to form links between the flocs and formation of large aggregates. The suspended particles flocculate, and they can be detached by filtration, flotation or straining. Although many types of flocculants like PAC, polyacrylamide (PAM) or polyferric sulfate (PFS) are used for wastewaters treatment, it is impossible to use them for removal of heavy metals. Chang et al. investigated the use of a new kind of flocculant, i.e., macromolecule heavy metal flocculant (by reacting chitosan with mercaptoacetic acid) with good results regarding the turbidity removal as well as heavy metals removal from waters [96].
Even if coagulation and flocculation are efficiently and widely used techniques for heavy metals removal from waters, the use of nanostructures materials as coagulants/flocculants is not reported in the literature. A very important aspect in using nanomaterials in wastewater treatment is the small sludge quantity that results in comparison with classical coagulation/flocculation techniques.

2.6. Flotation

Flotation is used for isolating HMIs from the liquid phase using bubble attachment. The most used processes for water decontamination are dissolved air flotation (DAF), ion flotation and precipitation flotation. DAF allows bubbles to stick to particles, forming aggregates that ascent to the water due to their low density and are easily collected and removed as sludge [97]. Ion flotation surfactants are used for passing on the ionic metal species in hydrophobic wastewaters. The removal of cadmium, lead and copper from aqueous solutions was studied by Yuan et al. The results indicated removal efficiencies of more than 70% [98]. Precipitate flotation is also a flotation method based on precipitate formation which can be afterwards removed by attachment to air bubbles. The precipitation can occur by metal hydroxide formation or as salt [99].

3. Electrochemical Depolluting Treatments

Electrochemistry applied to remove HMIs from wastewaters has the advantage to recover the metals while treating the water from electroplating, food, oil, textile processing, etc. Among the most commonly used water purification technologies are electrodeposition, electrocoagulation (EC), electroflotation (EF) and electrooxidation (EO).
Besides corrosion, electrochemical industries produce effluents that are the main cause for water heavy metal pollution such as battery industry (Hg, Pb, Cd, etc.) or electroplating waste. The electrochemical recovery of metals from wastewaters has been adapted from the long-practiced electrometallurgy, in which metals were recovered from mine waters. Although the basic electrochemical mechanism based on cathodic deposition is very simple, i.e.,
Mn + + ne M ,
the search for improvement in current efficiency and use of less expensive materials continues.

3.1. Electrodialysis (ED)

This method involves the use of a separation membrane and electric potential in order to remove pollutants from a solution as it passes through the system. Figure 3 illustrates the principles of electrodialysis. Separation membranes exhibit anionic or cationic characteristics. As the solution passes through the membranes, the ions are attracted towards the anode or cathode [100].
Tzanetakis et. al. [101] have performed experiments with electrodialysis in order to remove Ni(II) and Co(II) ions from synthetic solutions and compared the capabilities of two cation-exchange membranes made from perfluorosulfonic Nafion 117 and sulfonated polyvinyldifluoride membrane (SPVDF). The sulfonated PVDF membrane is a low-cost membrane that showed chemical, thermal and mechanical behavior was similar to the Nafion 117. Moreover, separation of elements was possible when a mixture of nickel and cobalt was used. The separation took place in the presence of ethylenediaminetetra-acetic acid (EDTA) when the [Ni-EDTA]-2 complex was preferentially formed and retained, while the cobalt ions passed through the SPVDF membrane [101].
At concentrations of more than 500 ppm, the separation performance is reduced considerably. In order to increase the efficiency, high ion exchange capacity is required for the exchange membranes. Jakobsen et al. [102] examined the removal of cadmium from wastewater by exposing the solution to an electrical DC field. The proportion of liquid solution to solid sludge was 1.4 and 2. The sludge was mixed with citric acid, HNO3 or distilled water, with a removal efficiency for each of the experiments of 70%, 67% and 69%, respectively.

3.2. Electroflotation (EF)

This technique is commonly used in the wastewaters treatment and has applications in the removal of heavy metal ions from industrial wastewaters. In the electroflotation process, pollutants, iron or solid particles adhere to tiny bubbles of H2 or O2 that were formed on the electrodes of the floatation cell and float to the surface. Some additives, aluminum or ferric salts are commonly brought into the waters for diminishing the suspended particles and complete a natural separation. Belkacem et al. [103] investigated the removal of iron, nickel, copper, zinc, lead and cadmium using aluminum electrodes. The removal efficiencies reached 99%. When electroflotation is used in aqueous media, water electrolysis forms very fine bubbles of hydrogen and oxygen toward the reactions:
Cathode :   2 H 2 O   +   2 e     2 OH   +   H 2 ( g )
Anode :   H 2 O     2 H +   +   1 / 2 O 2 g   +   2 e
The gas evolution process can be split in three physical processes: nucleation, growth and detachment. The bubbles nucleation takes place at electrode surfaces from highly supersaturated solutions [104]. They are removed from the electrode by forces of buoyancy or liquid shearing forces that pull the bubbles away. In electroflotation, the bubbles size depends mainly on the nature of the electrode material and its location in the electromotive series. The solution pH influences the bubble size, i.e., smaller hydrogen bubbles are formed in neutral or alkaline media in comparison with the acidic media. Unlike hydrogen, oxygen bubbles achieve a minimum size in acidic media, increasing in diameter as the pH increases. The detachment size of the bubbles is also influenced by the shape of the electrode surface. There have been conflicting investigations regarding the effect of current density on bubble size. An increased current density was reported by Mansour et al. [105] by increasing the diameter of hydrogen bubbles, which was explained by the coalescence of the bubbles at high current densities. On the other hand, Kektar and Burns et al. [106,107] have concluded the opposite.

3.3. Electrocoagulation (EC)

In electrocoagulation, electrical current is used in an electrochemical setting to remove metals from water. It is usually combined with other wastewater treatments to remove pollutants, especially heavy metals, from various industrial wastewaters such as electroplating and food industry. Unlike the traditional coagulation techniques, electrocoagulation uses an electrical current to remove pollutants, which proved to be beneficial especially in the case of heavy metal. Moreover, the electricity required to operate the electrocoagulation process may be provided by renewable energy sources such as solar, wind, geothermal, biogas and small hydro. Electrocoagulation is very similar to chemical coagulation. In electrocoagulation, the coagulants are required to be immersed electrochemically in the polluted waters using aluminum or iron sacrificial anodes. Pollutants are then kept into the solution through electrical charges. When these ions interact with ions charged with reversed electrical charges by applying certain electrocoagulation conditions, they lose stability and precipitate in a constant configuration.
The electrocoagulation process offers many advantages in comparison with the traditional coagulation technique [108]. The main advantages include no additional chemicals introduced in the wastewaters before treatment, the electrocoagulation process is straightforward, pollutants can be easily neutralized, and there is no secondary pollution. The equipment required for operating the electrocoagulation technology is simple and easy to use. The costs of operation are low, and the process automatization is possible. Moreover, the smallest colloidal particles can be efficiently removed by electrocoagulation due to the fact that they move faster under the applied electric field, which facilitates the agglomeration.
For the electrocoagulation process to take place, there are three successive steps necessary, as follows:
  • Formation of coagulants by electrolytic oxidation of the sacrificial anode electrodes.
  • Destabilization of the contaminants, particulate suspension and breaking of emulsions.
  • Aggregation of the destabilized phases to form flocs.
The flocs formed during the process are large and stable and can be separated by simple filtration techniques. The flocs are carried to the top of the solution by the gas bubbles formed during water electrolysis where they are concentrated, collected and then removed. Compared to other treatments, the flocks from the electrocoagulation process can be reused with lower costs as result of lower solids content. From the electrocoagulation process results low quantity sludge that can be easily processed and dewatered because of its composition, i.e., metallic oxides and hydroxides. Electrocoagulation process can be also used in rural areas where electricity is not available or with limited access to electricity, remote areas or isolated areas, by attaching a solar panel or other renewables to the water treatment system [109]. Table 6 shows the removal efficiency of several heavy metal ions, along with the electrode material and initial concentration of HMIs in solution.
A comprehensive review on electrocoagulation was published by Al-Qodah et al. [118]. The removal efficiency depends on several factors such as the initial concentration in the water, the electrode material and the pH of the water. Figure 4 presents the removal efficiency of Cr(III), Cr(VI), As(III) and Hg as a function of the initial concentration of HMIs in water (adapted from [109,119]).
The arrangement of electrodes in the electrocoagulation process and the electrode material are very important with respect to the cost analysis. The treatment of textile water was investigated by Kobya et al. [115] using three different ways of electron arrangement:
Monopolar electrodes in parallel connection, where current is divided between all electrodes;
Monopolar electrodes in a serial connections system, where every couple of sacrificial electrodes are connected with each other;
Bipolar electrode in serial connections where there is not any electrical connection between the inner electrodes because the outer electrodes are linked to power.
The spacing between electrodes is very important for the removal of pollutants. In order to diminish the energy consumption, it is indicated to use larger spaces between electrodes for effluent with high conductivity treatment. Otherwise, in case of effluents with low conductivity, the energy consumption can be diminished by smaller spacing between electrodes.
The process of electro-coagulation is extensively used for removing solids in suspension, dissolved metals, tannins and dyes. These contaminants that are present in wastewater are maintained in the solution through electrical charges. Table 7 shows several water treatment methods to remove heavy metal ions. Saturating the water with ions of opposite electrical charge to that of the heavy metal ions leads to the destabilization of the latter, and they start to precipitate into a stable form, facilitating the removal from the water. A variety of pollutants can be eliminated through electrocoagulation such as arsenic [120], strontium and cesium [121], phosphate [122], sulfide, sulfate and sulfite [119], boron [123], fluoride [124], nitrate [113], chromium [125], cadmium [114], zinc [115], nickel [126], mercury [127], and cobalt [128] as well as oil [129], chemical oxygen demand [130], color [131] and organic substances [132]. The removal efficiency of HMIs by different methods is presented in Figure 5, where electrocoagulation has a better efficiency for Cu and Cr ions removal than reverse osmosis and better removal efficiency for Cr than chemical precipitation.
The following considerations are the main factors affecting the efficiency of the electrocoagulation process:
Current density. In terms of current density in the electrocoagulation system, it is the main factor that “decides” the quantity of Al3+ or Fe2+ ions discharged from the electrodes. Each element has a specific electrochemical equivalent mass: 335.6 mg/(Ah) for Al and 1041 mg/(Ah) for Fe. Using a higher current leads to the possibility of using a smaller electrocoagulation unit, but this current also heats up the water and can result in a waste of electrical energy. Moreover, a current that exceeds the necessary parameters results in a decrease of process efficiency. The current density suggested for a long operation of the electrocoagulation system without maintenance is 20–25 A/m2. If the electrodes are periodically cleaned, this value can change depending on the operating factors.
Addition of NaCl. Generally, table salt is used so that the water conductivity can be increased to facilitate treatment. Usually, in wastewater, there are certain anions present, such as HCO3 and SO42−, which have the added disadvantage of precipitating Ca2+ or Mg2+ ions. These ions adhere to the surface of the electrodes and insulate them, resulting in an increase in potential and a decrease of current efficiency. Chloride ions are used to inhibit these adverse effects, and it is usually recommended that there should be approximately 20% Cl- ions present in the water in order for the electrocoagulation process to proceed normally.
pH Effect. pH can affect the electrocoagulation of water or wastewater though and increase or decrease of current efficiency as well as its influence on the solubility of metal hydroxides. In the case of aluminum, the efficiency of removal of ions through current density is higher in acidic or alkaline conditions, while most pollutants react more positively to a pH of approximately 7.
Temperature. Increasing the temperature usually results in a modification in pore size of Al(OH)3 gel. These pores reduce in size, and the generated flocs tend to deposit themselves on the surface of the electrode. Similar to the current efficiency, the power consumption also gives a maximum at slightly lower value of temperature, 35 °C, for treating oil-containing wastewater [47]. This process can be explained due to the opposite effect that temperature has on water, resulting in a higher conductivity at higher temperature, meaning lower energy consumption.
Power supply. The passing of a current inside an electrochemical reactor can only be done by overcoming different types of potentials: anode overpotential, ohmic potential drop, cathode overpotential and equilibrium potential difference [20]. The anode overpotential is comprised of concentration overpotential as well as activation overpotential, and it can also be influenced by a passive overpotential of the passive film on the surface of the anode. The cathode overpotential is determined by concentration overpotential and activation overpotential.
The main advantages for using electrocoagulation processes in the treatment of water as compared to coagulation process are the following: (I) organic matter is separated faster and effective, (II) there is no need for pH control, (III) the small amount of chemicals used in the process, (IV) a small amount of sludge is produced and (V) low operation costs.
Among disadvantages, the most important are (I) high concentrations of iron and aluminum ions in the effluent that have to be removed and (II) that the hydroxide does not present an appropriate grain size to ensure its precipitation. This results in difficulty to ensure separation, which also results in an increase in voltage in order to overcome the lack of hydraulic properties of the material.

3.4. Electrochemical Technologies in Wastewater Treatment

In electrochemical processes, the most important factors are potential, current, current density, ia (current per electrode area), current efficiency, CE (i.e., how much current is consumed to produce a certain product vs total consumption). For metal recovery, the electrochemical reactors are also defined by their performance given by the space–time yield of the reactor, YST, i.e., the amount of product produced by the reactor volume in unit time:
Y ST   =   i a M / 1000 z F   ×   C E .
Electrochemical deposition is effective in recovery heavy metals from wastewater streams [100]. The main advantage of using electrochemical treatment of clean water is that it does not introduce additional chemicals. Moreover, heavy metal ions can be removed selectively by electrochemical treatment.
Figure 6 presents a comparative analysis of the removal efficiency for heavy metals as a function of the method of their removal. Among the electrochemical methods, electroflotation shows consistent good removal efficiencies for all the heavy metals tested, followed by electrochemical removal, while electrocoagulation shows poor efficiencies (lower than 50% for Cr, Ni and Pb).

4. Electrochemical Detection and Removal of Heavy Metals

Because of ineffective elimination of HMIs to accepted values by conventional treatments [26,27], new electrode materials have been developed. For instance, titanium dioxide (TiO2) on metallic titanium has been used for many photoelectrochemical oxidations processes. However, changing the TiO2 morphology from film to hierarchical TiO2 nanotubes (TiO2-NTs) improves electron percolation at the TiO2 interface due to the enlarged surface area associated with the high structural organization, which increases the reactions at surface/electrolyte interface and reduces the recombination levels of electron/hole [138,139]. Because TiO2 nanotubes have low toxicity, good stability and high efficiency, TiO2-NTs have been an ideal material for organic pollutants removal applications. Figure 7 shows a self-explanatory illustration of the formation process of TiO2-NTs/SnO2-Sb electrodes.
The use of mixed metal oxide (MMO) anodes has been extended to anode material for electrochemical oxidation of certain pollutants that are very difficult, if not impossible, to remove from aqueous environment. These electrodes with high oxygen evolution potentials are used to remove difficult organic pollutants in water through electrochemical oxidation, depending of the mechanisms involved (i.e., by direct oxidation or mediated oxidation with the MMO anodes) including dyes, pesticides and herbicides, phenolic compounds, pharmaceuticals, antibiotics and hormones, plasticizers, perfluorinated chemicals, surfactants and derivatives, chelating agents and microcystin toxins [140]. Since major reactions take place in the MMO anode surface, increasing the anode surface can be achieved by template synthesis. Examples include vertically aligned TiO2-NTs used as template for deposition of PbO2 [141], SnO2 [142] and WO3 [138].
Carbon nanotubes (CNTs) based electrodes are another example of electrode developed to address the challenges encountered in certain pharmaceutical waters. Modified multiwall carbon nanotubes (MWCNTs) electrode doped with Ce was used to remove ceftazidime by electro-oxidation, which is an aqueous antibiotic. Cerium doping of the MWCNTs electrode films alters the morphology of the electrode surface and improves the oxidation ability of the electrode [143]. Cyclic voltammetry showed that the modified MWCNTs electrodes present a wider oxidation peak and generally display stronger capacities of generating reactive groups. In addition, the oxidation peak potential of the modified MWCNTs electrodes was smaller than that of the unmodified MWCNTs electrodes. The electrochemical removal of ceftazidime in an aqueous solution on the modified MWCNTs electrodes showed that the removal efficiency of ceftazidime with an initial concentration of 1mg/L was approximately 100% after 60 min electrolysis in a 1 g/L Na2SO4 electrolyte with a current density of 3mA/cm2 and an electrode spacing of 1 cm [143].
There are a number of methods for growing nanostructures but for detection, the surface area of the nanostructures should be very large and uniform. The most useful method to obtain ordered nanostructures with high aspect ratio is template synthesis (TSy), which provides quantifiable results.

4.1. Methods to Obtain Nanostructured Electrodes

Nanostructured electrodes can be obtained with or without templates. However, nanostructure array with high aspect ratios (L/d > 20) are typically obtained in porous templates with transversal pores. For this particular nanotube and nanowire arrays, several methods have been developed depending on the system to be obtained and the properties of the template. Electroless and electrochemical deposition are the main methods developed for obtaining nanotube or nanowire arrays, which also allows the seamless integration of these nanostructure arrays into devices such as sensors.

4.1.1. Electroless Deposition

Electroless process was developed based on the reduction process of metallic ions from solution and oxidation of a compound from solution, as reducing agent, followed by film deposition as a result of the internal current produced in the process. According to Sudagar et al. [144], electroless process is an autocatalytic method which appears due the presence of a cation of the metal reduced by the electrons presented onto the metal surface of a substrate or a catalyst responsible for beginning deposition process.
Although nanowires can be obtained without a template, it is necessary to use a template when nanowires with high aspect ratios are needed. There are a few materials used as templates that have transversal pores, as follows: (i) insulating materials such as alumina and (ii) track-etched polymers like polycarbonate (PCTE) and polyethylenterephtalate (PET). In the electroless deposition process, gold or other metal deposition takes place on the entire surface of the membrane used as template including the inside walls of the pores.
Polymeric membranes: Au electroless deposition is typically obtained using PCTE filtration membranes with various diameters, from 30 to 200 nm. In this method, commercial gold electroless plating solution (Oromerse Part B, Technic Inc.) is diluted 40 times with water prior to use to obtain a typical composition of 7.9 × 10−3 M Na3Au(SO3)2 and 0.127M Na2SO3. Electroless deposition procedure starts with immersing the PCTE template membrane for 2 h in methanol, followed by sensitization with SnCl2 solution and trifluoroacetic acid in 50:50 methanol–water for 45 min. After membrane sensitization, a solution of Ag[(NH3)2]NO3 is added. Then, the membrane is immersed in an Au plating bath containing formaldehyde. Another option is to add formaldehyde after soaking of membrane into gold electroless bath at about −4 °C. Electroless deposition is extended for different times, and finally, the membrane is washed with water, immersed in HNO3 for 12 h, washed again with water and dried at room temperature [145].
Martin et al. [146], who first introduced the electroless metal deposition process for nanoporous PCTE templates, have shown that this process requires a chemical reducing agent in order to deposit, as slow as possible, a metal from solution onto a surface that is not electronically conductive. The presence a catalyst can accelerate the metal reduction rate.
Figure 8 presents an illustration of the Au electroless deposition process. The PCTE membrane is first sensitized by immersing it into tin chloride solution SnCl2 and trifluoroacetic acid, using a mixture of 50/50 methanol/water as solvent. After washing with methanol, Sn2+ attach to the surface of the membrane, which was covered by a thin layer of poly(viny1pyrrolidone) (PVP) to improve hydrophilicity. Then, the membrane is activated in an aqueous solution of ammoniac and AgNO3. A redox reaction takes place with the oxidation of Sn (II) to Sn (IV) and the reduction of Ag (I) to Ag (0). Good results on the activation of Sn (II) and reduction of Ag (I) were obtained using glass substrate.
After Ag coating, the membrane is immersed into Au plating solution, which consists of Na3Au(SO3)2, Na2SO3 and formaldehyde. In this step, Ag is replaced by Au and the membrane becomes coated by Au. In the case of gold deposition, it is essential that the formation of Au nuclei takes place before the growth process begins, as these Au nuclei act as “catalytic sites” for the next Au deposition, when formaldehyde is added to reduce Au and increase the Au deposition rate. All Au ions are reduced to Au atoms by formaldehyde, which acts as reducing agent, according to the following reaction:
2 Au +   +   HCHO   +   3 OH HCOO   +   2 H 2 O   +   2 Au
As the Au coating advance and the entire pore surface is coated, Au nanotubes form. A rapid growing of the nuclei can lead to pore clogging pretty fast, which will stop the deposition process inside that pore. Nanowires can also be obtained by this method at longer deposition time, in about 24 h [146,147].
Anodized Aluminum membrane (AAO). Another template used for nanowires synthesis is the porous aluminum oxide (anodic aluminum oxide, AAO) membrane, which exhibits better stability and chemical inertia compared to PCTE [148]. AAO templates are obtained using an aluminum foil (99.99%-Merck). First, the foil is chemically treated under normal conditions using NaOH and washed with distilled water and acetone. To obtain a uniform AAO array template, the second step consists of surface anodization by applying a constant voltage and a mixture of acids [149].
Because the AAO membrane is not conductive, electroless deposition technique was used to obtain ordered Cu, Ni and Co nanotubes inside AAO membrane template [150]. The nanotube dimensions were imposed by the membrane size, i.e., the outside diameter of the nanotubes was given by the pore size, while the length of the nanotubes was equal to the thickness of the template. The electroless deposition is similar for all metals deposited and usually starts with a redox reaction in SnCl2 and HCl, followed by an activation process [146,150]. Due to the advantage regarding the obtaining of nanowires without electronically conductive surface, electroless deposition could offer a good alternative for nanowires synthesis. For short time electroless deposition, nanotubes can be obtained while nanowires are obtained at longer deposition times. Besides metal nanostructures, metallic alloys can be also obtained. Yuan et al. [151] obtained Co-P nanowires with magnetic properties in AAO template using cobalt-plating bath made using cobalt chloride, sodium hypophosphite, sodium citrate and ammonium chloride [151]. Several metallic nanowires were produced by electroless deposition, which will be briefly presented below.
Au nanowires (Au NWs) with strong mechanical resistance, stability, and minimal defects were obtained using cyanide-complexed gold solution [146,152,153,154]. An important aspect of this method is the environmental impact and the high toxicity of gold cyanide, as the most commonly electrolyte used in this process [155,156,157]. Although the cyanide solution prolongs the life of the electroplating bath, new alternative methods appeared lately to prevent this disadvantage. For example, gold sulfite [158] and hydrogen tetrachloroaurate (HAuCl4) have been the subject of several reports on the synthesis of Au NWs by electrodeposition or electroless deposition [159,160,161]. Wang et al. [161] synthesized Au NWs at different temperatures in one-step process using ethanol as a reducing agent for HAuCl4.
According to Kan et al. [160], Au NWs could be obtained using mesoporous silica by immersing the silica in HAuCl4 solution, followed by drying and heating at about 300 °C, without any reduction treatment. An explanation of the mechanism of Au nanowires formation could be diffusion of Au atoms along of silica-controlled pores combined with a nucleation process that takes place at low rates.
An interesting method for Au NWs growth was developed by Kim et al. [162]. In this method, Au seeds nanoparticles were prepared using NaBH4 to reduce HAuCl4. The Au nanoparticles generated an in situ process of autocatalytic reduction of Au (I), thus expanding the seed nanoparticles. The synthesis of Au NWs was performed by adding these Au nanoparticles to a solution mixture containing gold precursor HAuCl4, ascorbic acid that was used for the reduction of Au (III) to Au (I), and a structural directing agent CTAB (hexadecyl-trimethylammonium bromide) [162].
Ag Nanowires. A facile electroless synthesis for silver nanowires (Ag NWs) using polyvinylpyrrolidone (PVP) surfactants can be developed on different substrates such as polyethylene terephthalate (PET) or glass at room temperature. The PVP molecules around Ag NWs offer good protection and stability of these NWs [163].
Promising results were obtained with ion-track etched mica templates used for growing of metal thin films. In the rhombohedral pores of the template, distinctive nanowires can be deposited having an aspect ratio of up to 70. Based on Sn(II)/Ag(I) redox system, Ag nanoparticle seeds could be accumulated on the template surface. Moreover, this method worked for Pt NWs too [164].
Ni Nanowires. Besides, Au and Ag, Ni NWs can be obtained using chemical reagents such as source of Ni (NiCl2·6H2O), reducing agent (hydrazine monohydrate: N2H4·H2O), solvent as ethylene glycol (EG), complexing agent (chloroplatinic acid hexahydrate: H2PtCl6·6H2O) and nucleating agent (trisodium citrate dehydrate: Na3C6H5O7·2H2O). Moreover, sodium hydroxide (NaOH) was used. Reaction took place under temperature in a water bath where two parallel neodymium magnets separated were placed for assuring the direction of Ni NWs formation. After the reaction, nickel nanowires were washed with ethanol. Nanowires made of iron group metals (Fe, Co, Ni) display a strong potential for certain applications from catalytic materials to magnetic materials because of their magnetic shape anisotropy [165].
Co Nanowires. Metallic Co NWs were prepared by electroless deposition at room temperature using propylene glycol under external magnetic field. The Co NWs obtained had a mean diameter of about 190 nm and lengths up to 160 µm Co. Due the strong magnetic interactions that appeared in the direction of the applied magnetic field, the Co nanoparticles were assembled [166].

4.1.2. Electrochemical Template Synthesis of Nanostructures

Electrochemical nanotechnology (nanoelectrochemistry) has become increasingly important due to certain unique properties observed at nanoscale. A decrease in the size of the electrode causes changes in the form of the diffusion layer from linear to spherical. The diffusion layer is formed as oxidized species are consumed at the electrode surface. This results in a concentration gradient between bulk concentration and depleted regions that leads to a decrease of the diffusion limited current during long operations. The behavior of nanoelectrodes during different operation times has led to the consideration of the diffusion mechanic as being planar during short usage and spherical during long operations. On the other hand, for electrodes at the nanoscale, diffusion phenomena are very fast so that normally mass transfer limitations are negligible, and surface kinetics control the deposition process. For multiscale nanostructures such as nanotubes, nanofibers, and nanocables, it is important to know which characteristic length scale, nm or µm, governs the deposition process [167,168,169]. For the µm scale, diffusion limitations can be important if the surface deposition processes are relatively fast.
Electrochemical template synthesis is mainly used to obtain arrays of nanoelectrodes. The advantages of using nanoelectrode arrays are generally due to their small size that results in maintaining a very steady current and a strong current/unit area. Moreover, this system ensures a small potential drop that makes it favorable for use in measurements in solutions with low concentrations of electrolyte. Another important advantage is that the array can function at room temperature in order to perform electrodeposition processes. This inhibits interdiffusion between adjacent layers in the deposition of multilayered nano-sized materials.
Electrochemical template synthesis of a material within the pores (Figure 9) begins by coating one face of the template with a metal film (usually via either ion sputtering or thermal evaporation) and using this metal film as a cathode for electroplating [170,171]. This method has been used to prepare a variety of metal nanowires in both track-etch and alumina templates. Additionally, the potentiostatic growth of the nanowire array through the etch tracks can be performed under convection control in an electrochemical jet cell [172]. The lengths of the nanowires can be controlled by varying the deposition time. This ability to control the length or aspect ratio (length to diameter) of the metal nanowires is especially important in optical applications because the optical properties depend on the aspect ratio.
This method can also be used to prepare hollow metal tubules [173]. To obtain tubules, the pore walls must be first chemically modified (i.e., molecular anchor must be applied) so that the electrodeposited metal preferentially deposits on the pore wall. For example, gold tubules have been prepared by attaching a cyanosilane to the walls of the alumina template membrane prior to metal depositions [174]. This method has the added benefit of being used to tailor the pore walls in alumina membranes for different applications using silanes that are commercially available.
The most important aspect in the electrochemical template synthesis is the conductive surface used as electrode, which can be formed on a given template in two ways as depicted in Figure 9 and Figure 10. When the conductive layer is deposited on one face of the membrane (Figure 9), the nanowires can grow through the pores of the membrane, which acts as a template. The main advantage of this method is the possibility of growing nanowire arrays directly into a device such as sensor, thus increasing the manufacturing process efficiency and reducing the costs.
Figure 9 illustrates the formation of an array of nanoelectrodes in a membrane, where the electrode material was applied on one of the two facets of the membrane. Another way to make the surface conductive for further electrochemical deposition is to use electroless deposition, as illustrated in Figure 10, where the conductive layer is deposited on the walls of the pores, creating nanotube structures. Ku et al. [175] obtained Au/Te nanocable-like structures using electroless deposition of Au to coat the inner wall of the pores and then an electrochemical process to grow Te inside the Au nanotube.

4.1.3. Electrochemical Template Synthesis for Nanostructure Arrays

Various composite nanostructures can be fabricated using electrochemical methods such as template synthesis. It is well-known that electrodeposition in AAO results in nanowire arrays of Fe [176,177], Co [166,173,178] and Ni [148,178,179,180] and their alloys. Composite materials composed of a variety of conductors, insulators, semiconductors and photoconductors were obtained. The number of different components that each composite can accommodate depends only on the template (initial diameter of the template pore, the thickness of the membrane) and the deposition technique (e.g., rate of material deposition, temperature).
Nanowires and Nanotubes Array: Nanowire and nanotube structures with monodisperse diameters and lengths can be fabricated. Generally, 1D nanostructures show superior properties and functionality when compared to their larger forms. Small structures with large surface area and nanoscale quantum confinement effects have unique chemical, optical and electronic properties compared to bulk materials. These are the simplest structures that can be obtained inside the pores, yet they are still complex. The template method can be used for the synthesis of metals, alloys, semiconductors or composites in space confined volumes of the membrane pores.
In membranes with transverse pores, hollow or filled cylindrical structures can be created, depending on the synthesis method. An important feature of this method is the possibility to tailor the size of nanotubes and nanowires for specific applications. Moreover, template synthesis for metal nanostructure fabrication is an attractive alternative solution to overcome nanofibrils fabrication using lithographic methods. Using template strategy combined with electrodeposition technique, nanometer-sized metallic wires, super conducting nanowires and magnetic multilayers can be fabricated [175], which exhibit physical properties different from those found in the bulk.
Gold. Gold NTs and NWs are generally obtained by electrochemical plating or electroless displacement. Because electroless deposition results in a more uniform Au deposition [146], it is the preferred method for Au nanotubes while electrochemical deposition is the preferred technique for nanowire template synthesis [147,181,182,183,184].
Among the earliest applications of the TSy of Au nanostructures was preparing ensembles of nanoelectrodes. Such electrodes are simply obtained by Au deposition in PCTE membranes by either electroless or electrochemical deposition. The electrodes can be in the form of nanoelectrode ensembles or arrays of gold nanotubes. Nanoelectrode ensembles are simply Au nanodiscs (i.e., the active electrode area) ensemble into the membrane [147]. The electrochemical signal of the cyclic voltammogram at these nanoelectrode ensembles is very strong, making the electrodes useful in ultra-trace detection of electroactive species.
Electrode ensembles of nanotubular Au obtained by electroless deposition provide a novel approach as glucose biosensors. Glucose oxidase (Gox) has been studied through immobilization onto preformed monolayers (mercaptoethylamine or mercaptopropionic acid) on electroless gold by cross-linking with glutaraldehyde [185,186]. Under optimized conditions, the detection limit was 2 × 10−4 M.
Arrays of Au nanotubes can be obtained after the polycarbonate membrane is removed to obtain freestanding nanowires. With their large electroactive surface area, arrays of Au nanotubes provide additional advantages in electroanalytical applications. One of the applications is as a novel template for making glucose sensors with a large amount of enzyme electrochemical entrapped into the ultra-thin nanotube array. Glucose sensors based on the traditional electrodes (such as platinum, gold or glassy carbon) monitor glucose by detecting hydrogen peroxide. On arrays of Au nanotubes, glucose sensors show a high sensitivity and high selectivity H2O2 detection. The sensitivity is amongst the highest values reported in the literature for comparable biosensor systems [185,186,187]. Another application of the arrays of single crystalline gold nanowires is in field emission [188].
Electrochemical deposition offers the possibility to create single crystal Au nanowires with an average aspect ratio of 100 in the pores of PCTE membranes [189,190]. The potentiostatic EC-TSy of Au nanowires results in “cigar like” structures [191]. The wire diameter, which should reflect the pore diameter, varies in the cross section: The wire’s diameter is noticeably smaller at both ends than in the middle. Morphology studies performed with transmission electron microscope (TEM) indicate that the surfaces of nanowires obtained by electrochemical deposition are smooth and exhibit single crystal structure [192]. Additional high-resolution TEM and electron diffraction [154,193,194,195,196,197] have shown that the most prevalent planar defects in face-centered cubic metallic nanocrystals is twinning. In single-crystal Au nanowires, microtwins were seen to depend on the growth direction of nanowires, i.e., twinning was observed in single-crystal NWs with a [111] growth orientation, but not in NWs that had a growth direction in [100] and [110]. Metallic characteristics as shown by the I–V curves of individual nanowire were revealed by AFM measurements performed with a conductive tip operating in contact mode at room temperature in air [192].
Silver. Single crystal Ag nanowires have been fabricated by electrochemical [189,190] or electroless deposition [103,126] in the pores of PCTE membranes. However, Ag NWs with high aspect ratio of 100 have been obtained via electrochemical deposition [189,190]. The electroless deposition is an inexpensive solution to the challenges posed by Ag NWs fabrication for various applications in optics, electronics and biological fields. Besides the classic electroless deposition of metals, a modified method can be used to obtain single crystal nanowires [198]. The initiation layer for silver crystal growth is represented by a gold film grown on one side of the membrane pores and the pores act as guiding funnels for growing the silver into a cylindrical nanostructure.
Cobalt. The electrodeposition of Co as well as other ferromagnetic metals (e.g., Fe, and Ni) in membrane nanopores results in a high-density surface distribution of ferromagnetic columns isolated by membrane, and high perpendicular anisotropy in the magnetic field. These unique properties induced by the size, shape and distribution of the ferromagnetic nanostructures are beneficial for enhancing the recording density media.
Cobalt has a hexagonal closed packed (hcp) crystal structure with the c axis as the easy axis of magnetization. Co NWs have enhanced magnetic coercivity [199]. Additionally, resonance phenomena have been observed for Co nanowires array [200,201].
Co nanowire arrays are generally obtained by electrochemical deposition into polycarbonate membranes with nanosize pores [199,202,203,204]. Different electrodeposition techniques were studied to investigate the effect of deposition parameters on the crystallographic and magnetic properties. Similar to the majority of nanowires (e.g., Ni, Cu, Au and polypyrrole) synthesized by potentiostatic electrochemical deposition inside the PCTE membrane, Co NWs have a “cigar like” structure [191].
In the chronoamperometric method [199], the diffusion-limited current varies in time. For short times, the diffusion controlled limiting current, i, obey the Cottrell equation, i.e., i = k·t-1/2, where k is a specific constant for a given system. At longer time, radii of the diffusion zones from each nanoelectrode increase gradually, expand and overlap. In the end, the diffusion controlled limiting current is observed, when the current enters a constant steady-state. Although steady state condition is achieved during electrochemical deposition of Co, variations in deposit concentration between the pore opening and surrounding area of the recessed nanoelectrodes are observed.
Nickel. Polycrystalline Ni nanowires/nanotubes arrays can be designed by either electroless [205] or electrochemical deposition [189,190,191]. For electroless Ni deposition, the reducing agent in the Ni deposition was hypophosphite, which resulted in Ni-P alloy nanotubes [205] with an inner diameter and wall thickness of about 180 nm and 20 nm, respectively. These Ni NTs array have an exposed area that is over 8 times larger than a flat surface, which recommends them in sensor applications. Additionally, the nanoscale structure of these tubules leads to high redox response. For instance, the cyclic voltammetry measurements of Ni NTs electrode array have shown that the Ni(OH)2/NiOOH redox reaction had an electrochemical response that was 40 times larger compared to a flat surface electrode. Charge storage capacity has been found to be improved by combining overcharge oxidation of the electrode arrays with various heat treatments, which is important in advancing the performance of a nickel hydroxide electrode for nickel metal hydride batteries [205].
Nickel nanowires fabricated using the electrodeposition have been characterized for their magnetic properties. A single Ni nanowire has been grown in a single pore [179]. For current densities i < 108 A/cm2, the cyclic voltammograms of a single Ni NW present a linear behavior. The electrical measurements indicated that the wire was of excellent quality, had a low contact resistance and could sustain considerably high current densities (about 3 × 108 A/cm2). In single Ni wires, anisotropic magneto resistance was observed only when the magnetic field was applied perpendicular to wires. In this case, a change in the maximum resistance of about 1% was observed [179]. Nickel nanowires, with large aspect ratios (L/D = 1000), have around 2–3% of the typical anisotropic magneto resistance (AMR) [206]. When the array has a low-density Ni nanowire of various pore diameters enclosed in the PCTE membrane, the behavior of the resonance field vs. angle does not depend on the diameter or the density of nanowires. Moreover, the effective anisotropy field is broadened due to the presence of a substructure in the absorption spectra. The magnetization reversal of Ni nanowires was studied by anisotropic magneto resistance measurements at temperatures between 15 and 300 K [200,201] and an extra uniaxial anisotropy induced by the contraction of the membrane at low temperature has been observed.
Copper. Potentiostatic electrochemical template synthesis is the main method used to fabricate single crystal Cu nanowires in PCTE membranes [190,191,207,208]. The deposition process was studied in detail for different voltages [208]. The overall deposition process was found to consist of several steps that are dominated by charge transfer (at short times), transition zone (where there are compatible rates between charge transfer and diffusion), and the diffusion region. In the beginning, the length of the remaining empty pore is significantly larger than the thickness of the diffusion layers, and diffusion of ions inside the pores has a linear behavior. In time, radial diffusion of ions toward the mouth of the pore becomes significant; the diffusion layers increase, expand and overlap the neighboring pores and take over the entire surface. Overgrown NWs form caps on top of the membrane, similar to “mushrooms”. After that, linear diffusion is observed as in the case of thin films deposition.
Under controlled electrochemical conditions, single-crystalline Cu nanowires can be produced [209,210]. Additionally, single Cu nanowire has been prepared by replication of a single-ion track template [211]. A promising way of measuring nanowire properties is to use single-pore membranes. A single Cu nanowire was grown by electrochemical deposition and connected with electrodes for I–V measurements [211]. Current-voltage measurements confirmed that the Cu nanowire has an ohmic current-voltage behavior. The wire had a truncated shape and the estimated diameters were 25 and 110 nm. A low contact resistance was obtained, and the maximum current density was more than 108 A/cm2, which also indicates the high morphological quality of nanowire.

4.2. Electrochemical Detection of Heavy Metals

The electrochemical treatment of wastewaters is an efficient technology as demonstrated for wastewater with high concentrations of HMIs [183]. Electrochemistry is present and assists other processes used in water treatment such as in oxidation and micro electrolysis, flotation, flocculation, coagulation. Moreover, in the case of metal hydroxides (MeO) that can adsorb pollutants by co-precipitation, MeO can be used as sacrificial anodes.
Synthesis of nanostructures directly affects the mechanism and the kinetics of nanostructure growth. A better control of the process enables a better control of the morphology–structure–properties at nanoscale. This aspect becomes important in the development of low cost, large scale synthesis. Buledi et al. [212] have recently reviewed the nanomaterial-based sensors for the detection of HMIs. Figure 11 presents just an example of the versatility of nanomaterials to detect toxic heavy metals such Hg, Ni, Co, Cu Cd, Pb and Mn from waters using electrochemical methods. Figure 11 also shows that multiple heavy metals can be detected using a single nanostructured electrode. With the development of novel nanomaterials and advanced processes, the detection limits of the heavy metal ions increased owing to increased surface area and electronic conductivity.
Various methods can be employed to synthesize nanomaterials such as electrochemical deposition (In2O3 NWs [213]), electroless deposition, sol-gel (In2O3 NTs [214]), sputtering (In2O3 NRs [215]), physical evaporation [216], molecular beam epitaxy (In2O3 NWs [217]), laser ablation (In2O3 NWs [218]), in template metalorganic chemical vapor deposition (MOCVD): In2O3 NWs [219], thermal chemical vapor deposition: In2O3 [220], etc. Miniaturization of electronics and devices is the driving force in the development of integrated nanostructures
Tubular nanostructures have intrinsic multi-functionalities that go beyond the research efforts to obtain nanotubes of various materials while posing challenges for both top-down and bottom-up approaches to nanotubes. This can be ascribed to the strong adsorption properties, large specific surface area and rich active sites of the composite. Nanotubes hold promise as candidates for highly effective nanodevices due to their four sites for attachment of other functional materials: (1) the outer surface is used for attachment, (2) the tube opening is used for loading, (3) inner surface is used for filling and (4) the interstitial region of the tube is used for doping.
Similar to multiwall CNTs, oxide nanotubes can be obtained by two different methods developed based on the template used:
  • Structure-directed agents, i.e., tubular assembly of a surfactant that encapsulate oxides; similar to multiwall CNTs, oxide nanotubes obtained by this method have a multiwall structure composed of a mixture of oxide and organic components [221]. Unlike CNTs, oxide nanotubes can be obtained in gram quantities by chemistry synthesis at low temperature.
  • Template directed growth: nanoporous alumina (AAO) or carbon nanotubes as templates. Polycrystalline nanotubes of ZrO2 [222], V2O5 [223], etc. For certain applications, the synthesis of single-crystalline oxide nanotube is required. Li et al. obtained single-crystalline In2O3 NTs [224] and single-crystalline MgO NTs [225].
  • Fill in nanotubes Hollow cavities with high aspect ratio such as nanotubes can be filled in to create nanocable structures. Ajayan and Iijima were first to insert by capillarity low-melting-point metals in the hollow cavities of carbon nanotubes [226,227]. This method also works well with oxides due to their high-melting points. Li et al. [224] obtained single-crystalline In2O3 NTs loaded with metallic In by evaporating a mixture of indium and indium oxide in vacuum and single-crystalline MgO NTs filled with Ga [225]. The removal of the template without destroying the nanotubes remains an unresolved problem.
Among other methods of detection, the electrochemical methods are fast and versatile, in situ detection being also possible. The electrochemical methods for heavy metal ion detection include static techniques, potentiostatic, galvanostatic, impedance and electrochemi-luminescence. Among the potentiostatic techniques, where the applied potential is independently controlled, there are several methods that are specifically applied to the detection of heavy metal ions (HMIs). Among the potentiostatic techniques that proved very sensitive to the detection of trace HMIs is anodic stripping voltammetry (ASV) [228]. This process has a pre-concentration step, in which the HMIs are concentrated on the electrode surface. The next step is the dissolution process, in which the adatoms are oxidized back into the solution. The stripping peak current recorded during the anodic dissolution is proportional to metal concentration. The size and the quality of the electrode is very important in the detection of heavy metal ions. Figure 12 shows the differential pulse anodic stripping voltammetry (DPASV) curves obtained on bismuth oxycarbide in the simultaneous detection of 2, 3 and 4 ions. The bismuth modified electrode is considered a “green” electrode [229,230,231], has been extensively studied, and many studies have reported that adding a certain concentration of bismuth ions to the solution can improve the sensitivity of the sensor by co-deposition with heavy metal ions. The detection limits are usually lower that the national standards.

5. Conclusions

Water is the most important resource for living beings, and one of the greatest challenges of our time is to keep it accessible, affordable and reliable for our planet. Heavy metal ions (HMIs) are among the most dangerous pollutants. This review presents an updated overview of general chemical and physical methods with the aid of nanotechnology that are recently performed to treat and purify water based on the removal of HMIs such as As, Hg, Cd, Pb, Cr, Ni, Zn and Cu. Various electrochemical depolluting treatments are discussed such as electrodialysis, electrofiltration, electrocoagulation and recent electrochemical technologies in wasterwater treatment. Nanomaterials designed for water treatments have large specific surface area, which offers numerous and rich active sites, and strong adsorption properties. Based on the utilization of nanotechnology, there are high potential and opportunities for wastewater treatment and purification.
The interactions between toxic HMIs and nanomaterials can change the surface properties in a variety of adsorption mechanisms from electrostatic interaction to physical adsorption, to surface complexation and precipitation or ion exchange. One key area of research is the optimization of physico-chemical properties of the surface at nanoscale level so that new materials and technologies can be developed and implemented for water remediation. Wastewaters are complex systems that require several steps of treatment, for which nanomaterials can play their role and be optimized to reduce and eventually eliminate the toxic HMIs. To progress in the research on advanced materials and nanotechnologies, further studies are needed in the following directions: (I) develop inexpensive and environmentally-friendly nanomaterials and methods to functionalize their surface for unique tunable physicochemical properties, (II) develop extensive characterization methods to understand the adsorption behaviors and mechanisms of nanomaterials and to increase their effectiveness, (III) quantity and quality evaluation of the nanomaterials when used as nanoparticles-support composites, and (IV) develop customized electrochemical electrodes and techniques for complex wastewaters. Research generated by the development of technologies for HMIs removal would find direct applications in other areas of the environment field, such as air remediation and energy, due to the nature of the nanometer-scale mechanisms that these processes have in common.

Author Contributions

Conceptualization, R.V.; writing—original draft preparation, R.V., E.M., A.M.P., B.A., C.P. (Cristian Pantilimon), C.T.; writing—review and editing, R.V., E.M., A.M.P., B.A.; visualization, R.V., C.P. (Cristian Pantilimon); supervision, R.V., C.P. (Cristian Predescu); project administration, R.V., C.P. (Cristian Predescu); funding acquisition, R.V., C.P. (Cristian Predescu). All authors have read and agreed to the published version of the manuscript.


This research was funded by the POC Program, Grant no. 49/05.09.2016, Project ID P_37_649.

Conflicts of Interest

The authors declare no conflicts of interest.


  1. USEPA. 2018 Edition of the Drinking Water Standards and Health Advisories Tables; Epa 822-f-18-001; Office of Water, U.S. Environmental Protection Agency (usepa): Washington, DC, USA, 2018. [Google Scholar]
  2. Organisation, W.H. Guidelines for Drinking Water Quality, 4th ed.; World Health Organization: Geneva, Switzerland, 2017. [Google Scholar]
  3. UN. United Nations Guide to the Globally Harmonized System of Classification and Labeling of Chemicals (ghs); United Nations: Geneva, Switzerland, 2015; p. 90. [Google Scholar]
  4. Hanjra, M.A.; Blackwell, J.; Carr, G.; Zhang, F.H.; Jackson, T.M. Wastewater irrigation and environmental health: Implications for water governance and public policy. Int. J. Hyg. Environ. Health 2012, 215, 255–269. [Google Scholar] [CrossRef] [PubMed]
  5. Scheierling, S.M.; Bartone, C.R.; Mara, D.D.; Drechsel, P. Toward an agenda for improving wastewater use in agriculture. Water Int. 2011, 36, 20. [Google Scholar] [CrossRef]
  6. Santhosh, C.; Velmurugan, V.; Jacob, G.; Jeong, S.K.; Grace, A.N.; Bhatnagar, A. Role of nanomaterials in water treatment applications: A review. Chem. Eng. J. 2016, 306, 1116–1137. [Google Scholar] [CrossRef]
  7. Favier, L.; Harja, M.; Simion, A.I.; Rusu, L.; Kadmi, Y.; Pacala, M.L.; Bouzaza, A. Advanced oxidation process for the removal of chlorinated phenols in aqueous suspensions. J. Environ. Prot. Ecol. 2016, 17, 10. [Google Scholar]
  8. Ardeleanu, M.N.; Popescu, I.N.; Udroiu, I.N.; Diaconu, E.M.; Mihai, S.; Lungu, E.; Alhalaili, B.; Vidu, R. Novel pdms-based sensor system for mpwm measurements of picoliter volumes in microfluidic devices. Sensors 2019, 19, 4886. [Google Scholar] [CrossRef] [Green Version]
  9. Predescu, A.M.; Matei, E.; Berbecaru, A.C.; Pantilimon, C.; Dragan, C.; Vidu, R.; Predescu, C.; Kuncser, V. Synthesis and characterization of dextran-coated iron oxide nanoparticles. R. Soc. Open Sci. 2018, 5. [Google Scholar] [CrossRef] [Green Version]
  10. Babel, S.; del Mundo Dacera, D. Heavy metal removal from contaminated sludge for land application: A review. Waste Manag. 2006, 26, 988–1004. [Google Scholar] [CrossRef]
  11. Hua, M.; Zhang, S.; Pan, B.; Zhang, W.; Lv, L.; Zhang, Q. Heavy metal removal from water/wastewater by nanosized metal oxides: A review. J. Hazard. Mater. 2012, 211-212, 317–331. [Google Scholar] [CrossRef]
  12. Renu; Agarwal, M.; Singh, K. Heavy metal removal from wastewater using various adsorbents: A review. J. Water Reuse Desalin. 2016, 7, 387–419. [Google Scholar] [CrossRef]
  13. Chen, Q.Y.; Luo, Z.; Hills, C.; Xue, G.; Tyrer, M. Precipitation of heavy metals from wastewater using simulated flue gas: Sequent additions of fly ash, lime and carbon dioxide. Water Res. 2009, 43, 2605–2614. [Google Scholar] [CrossRef]
  14. Tünay, O.; Kabdaşli, N.I. Hydroxide precipitation of complexed metals. Water Res. 1994, 28, 2117–2124. [Google Scholar] [CrossRef]
  15. Gorny, J.; Billon, G.; Noiriel, C.; Dumoulin, D.; Lesven, L.; Made, B. Chromium behavior in aquatic environments: A review. Environ. Rev. 2016, 24, 503–516. [Google Scholar] [CrossRef]
  16. Bhattacharyya, D.; Jumawan, A.B.; Grieves, R.B. Separation of toxic heavy metals by sulfide precipitation. Sep. Sci. Technol. 1979, 14, 441–452. [Google Scholar] [CrossRef]
  17. Monea, M.C.; Löhr, D.K.; Meyer, C.; Preyl, V.; Xiao, J.; Steinmetz, H.; Schönberger, H.; Drenkova-Tuhtan, A. Comparing the leaching behavior of phosphorus, aluminum and iron from post-precipitated tertiary sludge and anaerobically digested sewage sludge aiming at phosphorus recovery. J. Clean. Prod. 2020, 247, 119129. [Google Scholar] [CrossRef]
  18. Monea, M.C.; Meyer, C.; Steinmetz, H.; Schönberger, H.; Drenkova-Tuhtan, A. Phosphorus recovery from sewage sludge – phosphorus leaching behavior from aluminum-containing tertiary and anaerobically digested sludge. Water Sci. Technol. 2020. [Google Scholar] [CrossRef]
  19. EPA. Innovative and Alternative Technology Assessment Manual; EPA 430/9-78-009; Agency, E.P.: Washington, DC, USA, 1980. [Google Scholar]
  20. Gonzalez-Munoz, M.J.; Rodriguez, M.A.; Luque, S.; Alvarez, J.R. Recovery of heavy metals from metal industry waste waters by chemical precipitation and nanofiltration. Desalination 2006, 200, 742–744. [Google Scholar] [CrossRef]
  21. Kumar, P.; Pournara, A.; Kim, K.-H.; Bansal, V.; Rapti, S.; Manos, M.J. Metal-organic frameworks: Challenges and opportunities for ion-exchange/sorption applications. Prog. Mater. Sci. 2017. [Google Scholar] [CrossRef]
  22. Hoch, L.B.; Mack, E.J.; Hydutsky, B.W.; Hershman, J.M.; Skluzacek, I.M.; Mallouk, T.E. Carbothermal synthesis of carbon-supported nanoscale zero-valent iron particles for the remediation of hexavalent chromium. Environ. Sci. Technol. 2008, 42, 2600–2605. [Google Scholar] [CrossRef]
  23. Naja, G.; Volesky, B. Toxicity and sources of Pb, Cd, Hg, Cr, As, and radionuclides in the environment. In Heavy Metals in the Environment; Springer Nature: Cham, Switzerland, 2009; pp. 13–61. [Google Scholar]
  24. Narayani, M.; Shetty, K.V. Chromium-resistant bacteria and their environmental condition for hexavalent chromium removal: A review. Crit. Rev. Environ. Sci. Technol. 2013, 43, 955–1009. [Google Scholar] [CrossRef]
  25. Sarkar, B. Heavy Metals in the Environment; CRC Press: Boca Raton, FL, USA, 2002. [Google Scholar]
  26. Tonini, D.R.; Gauvin, D.A.; Soffel, R.W.; Freeman, W.P. Achieving low mercury concentrations in chlor-alkah wastewaters. Environ. Prog. 2003, 22, 167–173. [Google Scholar] [CrossRef]
  27. Zagorodni, A. Ion exchange Materials: Properties and Applications: Properties and Applications; Elsevier: Amsterdam, The Netherlands, 2006. [Google Scholar]
  28. Fan, Q.H.; Li, Z.; Zhao, H.G.; Jia, Z.H.; Xu, J.Z.; Wu, W.S. Adsorption of pb(ii) on palygorskite from aqueous solution: Effects of ph, ionic strength and temperature. Appl. Clay Sci. 2009, 45, 111–116. [Google Scholar] [CrossRef]
  29. A.B. Application of the Ion Exchange Process for the Treatment of Radioactive Waste and Management of Spent Ion Exchangers; International Atomic Energy Agency: Vienna, Austria, 2002. [Google Scholar]
  30. Bortun, A.I.; Bortun, L.N.; Clearfield, A. Evaluation of synthetic inorganic ion exchangers for cesium and strontium removal from contaminated groundwater and wastewater. Solvent Extr. Ion Exch. 1997, 15, 909–929. [Google Scholar] [CrossRef]
  31. Chitpong, N.; Husson, S.M. High-capacity, nanofiber-based ion-exchange membranes for the selective recovery of heavy metals from impaired waters. Sep. Purif. Technol. 2017, 179, 94–103. [Google Scholar] [CrossRef] [Green Version]
  32. Ma, H.Y.; Hsiao, B.S.; Chu, B. Electrospun nanofibrous membrane for heavy metal ion adsorption. Curr. Org. Chem. 2013, 17, 1361–1370. [Google Scholar] [CrossRef]
  33. Geay, M.; Marchetti, V.; Clement, A.; Lonbinoux, B.; Gerardin, P. Decontamination of synthetic solutions containing heavy metals using chemically modified sawdusts bearing polyacrylic acid chains. J. Wood Sci. 2000, 46, 331–333. [Google Scholar] [CrossRef]
  34. Guclu, G.; Gurdag, G.; Ozgumus, S. Competitive removal of heavy metal ions by cellulose graft copolymers. J. Appl. Polym. Sci. 2003, 90, 2034–2039. [Google Scholar] [CrossRef]
  35. Kyzas, G.Z.; Siafaka, P.I.; Lambropoulou, D.A.; Lazaridis, N.K.; Bikiaris, D.N. Poly(itaconic acid)-grafted chitosan adsorbents with different cross-linking for pb(ii) and cd(ii) uptake. Langmuir 2014, 30, 120–131. [Google Scholar] [CrossRef]
  36. Okieimen, F.E.; Sogbaike, C.E.; Ebhoaye, J.E. Removal of cadmium and copper ions from aqueous solution with cellulose graft copolymers. Sep. Purif. Technol. 2005, 44, 85–89. [Google Scholar] [CrossRef]
  37. Stephen, M.; Catherine, N.; Brenda, M.; Andrew, K.; Leslie, P.; Corrine, G. Oxolane-2,5-dione modified electrospun cellulose nanofibers for heavy metals adsorption. J. Hazard. Mater. 2011, 192, 922–927. [Google Scholar] [CrossRef]
  38. Barakat, M.A. New trends in removing heavy metals from industrial wastewater. Arab. J. Chem. 2011, 4, 361–377. [Google Scholar] [CrossRef] [Green Version]
  39. Fu, F.L.; Wang, Q. Removal of heavy metal ions from wastewaters: A review. J. Environ. Manag. 2011, 92, 407–418. [Google Scholar] [CrossRef] [PubMed]
  40. Xu, T.W. Ion exchange membranes: State of their development and perspective. J. Membr. Sci. 2005, 263, 1–29. [Google Scholar] [CrossRef]
  41. Zhang, L.N.; Zhou, J.P.; Zhou, D.C.; Tang, Y.R. Adsorption of cadmium and strontium on cellulose/alginic acid ion-exchange membrane. J. Membr. Sci. 1999, 162, 103–109. [Google Scholar] [CrossRef]
  42. Zhang, L.Z.; Zhao, Y.H.; Bai, R.B. Development of a multifunctional membrane for chromatic warning and enhanced adsorptive removal of heavy metal ions: Application to cadmium. J. Membr. Sci. 2011, 379, 69–79. [Google Scholar] [CrossRef]
  43. Arthanareeswaran, G.; Devi, T.K.S.; Raajenthiren, M. Effect of silica particles on cellulose acetate blend ultrafiltration membranes: Part i. Sep. Purif. Technol. 2008, 64, 38–47. [Google Scholar] [CrossRef]
  44. Han, R.L.; Zhang, S.H.; Liu, C.; Wang, Y.T.; Jian, X.G. Effect of naa zeolite particle addition on poly(phthalazinone ether sulfone ketone) composite ultrafiltration (uf) membrane performance. J. Membr. Sci. 2009, 345, 5–12. [Google Scholar] [CrossRef]
  45. Liu, F.; Ma, B.R.; Zhou, D.; Xiang, Y.H.; Xue, L.X. Breaking through tradeoff of polysulfone ultrafiltration membranes by zeolite 4a. Microporous Mesoporous Mater. 2014, 186, 113–120. [Google Scholar] [CrossRef]
  46. Oh, S.J.; Kim, N.; Lee, Y.T. Preparation and characterization of PVDF/TiO2 organic-inorganic composite membranes for fouling resistance improvement. J. Membr. Sci. 2009, 345, 13–20. [Google Scholar] [CrossRef]
  47. Zornoza, B.; Tellez, C.; Coronas, J. Mixed matrix membranes comprising glassy polymers and dispersed mesoporous silica spheres for gas separation. J. Membr. Sci. 2011, 368, 100–109. [Google Scholar] [CrossRef]
  48. Howarth, A.J.; Liu, Y.Y.; Hupp, J.T.; Farha, O.K. Metal-organic frameworks for applications in remediation of oxyanion/cation-contaminated water. Crystengcomm 2015, 17, 7245–7253. [Google Scholar] [CrossRef]
  49. Rapti, S.; Pournara, A.; Sarma, D.; Papadas, I.T.; Armatas, G.S.; Tsipis, A.C.; Lazarides, T.; Kanatzidis, M.G.; Manos, M.J. Selective capture of hexavalent chromium from an anion-exchange column of metal organic resin-alginic acid composite. Chem. Sci. 2016, 7, 2438. [Google Scholar] [CrossRef] [PubMed]
  50. Yang, X.; Wan, Y.; Zheng, Y.; He, F.; Yu, Z.; Huang, J.; Wang, H.; Ok, Y.S.; Jiang, Y.; Gao, B. Surface functional groups of carbon-based adsorbents and their roles in the removal of heavy metals from aqueous solutions: A critical review. Chem. Eng. J. 2019, 366, 608–621. [Google Scholar] [CrossRef]
  51. Li, Y.H.; Wang, S.G.; Wei, J.Q.; Zhang, X.F.; Xu, C.L.; Luan, Z.K.; Wu, D.H.; Wei, B.Q. Lead adsorption on carbon nanotubes. Chem. Phys. Lett. 2002, 357, 263–266. [Google Scholar] [CrossRef]
  52. Wang, H.J.; Zhou, A.L.; Peng, F.; Yu, H.; Chen, L.F. Adsorption characteristic of acidified carbon nanotubes for heavy metal pb(ii) in aqueous solution. Mater. Sci. Eng. A-Structural Mater. Prop. Microstruct. Process. 2007, 466, 201–206. [Google Scholar] [CrossRef]
  53. Lu, C.Y.; Liu, C.T.; Su, F.S. Sorption kinetics, thermodynamics and competition of ni2+ from aqueous solutions onto surface oxidized carbon nanotubes. Desalination 2009, 249, 18–23. [Google Scholar] [CrossRef]
  54. Mobasherpour, I.; Salahi, E.; Ebrahimi, M. Thermodynamics and kinetics of adsorption of cu(ii) from aqueous solutions onto multi-walled carbon nanotubes. J. Saudi Chem. Soc. 2014, 18, 792–801. [Google Scholar] [CrossRef] [Green Version]
  55. Li, Y.H.; Ding, J.; Luan, Z.K.; Di, Z.C.; Zhu, Y.F.; Xu, C.L.; Wu, D.H.; Wei, B.Q. Competitive adsorption of pb2+, cu2+ and cd2+ ions from aqueous solutions by multiwalled carbon nanotubes. Carbon 2003, 41, 2787–2792. [Google Scholar] [CrossRef]
  56. Naghizadeh, A. Comparison between activated carbon and multiwall carbon nanotubes in the removal of cadmium(ii) and chromium(vi) from water solutions. J. Water Supply Res. Technol. -Aqua 2015, 64, 64–73. [Google Scholar] [CrossRef]
  57. Yang, S.T.; Li, J.X.; Shao, D.D.; Hu, J.; Wang, X.K. Adsorption of ni(ii) on oxidized multi-walled carbon nanotubes: Effect of contact time, ph, foreign ions and paa. J. Hazard. Mater. 2009, 166, 109–116. [Google Scholar] [CrossRef]
  58. Lu, C.Y.; Liu, C.; Rao, G.P. Comparisons of sorbent cost for the removal of ni2+ from aqueous solution by carbon nanotubes and granular activated carbon. J. Hazard. Mater. 2008, 151, 239–246. [Google Scholar] [CrossRef]
  59. Long, R.Q.; Yang, R.T. Carbon nanotubes as superior sorbent for dioxin removal. J. Am. Chem. Soc. 2001, 123, 2058–2059. [Google Scholar] [CrossRef] [PubMed]
  60. Lu, C.Y.; Chiu, H.S. Adsorption of zinc(ii) from water with purified carbon nanotubes. Chem. Eng. Sci. 2006, 61, 1138–1145. [Google Scholar] [CrossRef]
  61. Ho, J.H.; Yeh, Y.N.; Wang, H.W.; Khoo, S.K.; Chen, Y.H.; Chow, C.F. Removal of nickel and silver ions using eggshells with membrane, eggshell membrane, and eggshells. Food Sci. Technol. Res. 2014, 20, 337–343. [Google Scholar] [CrossRef] [Green Version]
  62. Park, H.J.; Jeong, S.W.; Yang, J.K.; Kim, B.G.; Lee, S.M. Removal of heavy metals using waste eggshell. J. Environ. Sci. 2007, 19, 1436–1441. [Google Scholar] [CrossRef]
  63. Chavan, M.; Mane, S. Removal of copper and zinc from aqueous solutions by using low cost adsorbents. Int. J. Sci. Res. (IJSR) 2015, 4, 3076–3080. [Google Scholar]
  64. Renge, V.C.; Khedkar, S.V.; Pande, S.V. Removal of heavy metals from wastewater using low cost adsorbents: A review. Sci. Rev. Chem. Commun. 2012, 2, 5. [Google Scholar]
  65. Yeddou, N.; Bensmaili, A. Equilibrium and kinetic modelling of iron adsorption by eggshells in a batch system: Effect of temperature. Desalination 2007, 206, 127–134. [Google Scholar] [CrossRef]
  66. Rohaizar, N.A.; Hadi, N.; Sien, W.C. Removal of cu (ii) from water by adsorption on chicken eggshell. Int. J. Eng. Technol. IJET-IJENS 2013, 13, 6. [Google Scholar]
  67. Arunlertaree, C.; Kaewsomboon, W.; Kumsopa, A.; Pokethitiyook, P.; Panyawathanakit, P. Removal of lead from battery manufacturing wastewater by egg shell. Songklanakarin J. Sci. Technol. 2007, 29, 12. [Google Scholar]
  68. Hegazi, H.A. Removal of heavy metals from wastewater using agricultural and industrial wastes as adsorbents. HBRC J. 2013, 9, 276–282. [Google Scholar] [CrossRef] [Green Version]
  69. Abdulrasaq, O.O.; Osinfade, G.B. Removal of copper (ii), iron (iii) and lead (ii) ions from mono-component simulated waste effluent by adsorption on coconut husk. Afr. J. Environ. Sci. Technol. 2010, 4, 6. [Google Scholar]
  70. Amuda, O.S.; Giwa, A.A.; Bello, I.A. Removal of heavy metal from industrial wastewater using modified activated coconut shell carbon. Biochem. Eng. J. 2007, 36, 174–181. [Google Scholar] [CrossRef]
  71. Chaudhuri, M.; Kutty, S.R.M.; Yusop, S.H. Copper and cadmium adsorption by activated carbon prepared from coconut coir. Nat. Environ. Pollut. Technol. 2010, 9, 4. [Google Scholar]
  72. Chakraborty, S.; Chowdhury, S.; Das Saha, P. Adsorption of crystal violet from aqueous solution onto naoh-modified rice husk. Carbohydr. Polym. 2011, 86, 1533–1541. [Google Scholar] [CrossRef]
  73. Kanwal, F.; Rehman, R.; Anwar, J.; Mahmud, T. Adsorption studies of cadmium (ii) using novel composites of polyaniline with rice husk and saw dust of eucalyptus camaldulensis. Electron. J. Environ. Agric. Food Chem. 2011, 10, 14. [Google Scholar]
  74. Foo, K.Y.; Hameed, B.H. Utilization of rice husks as a feedstock for preparation of activated carbon by microwave induced koh and k2co3 activation. Bioresour. Technol. 2011, 102, 9814–9817. [Google Scholar] [CrossRef]
  75. Kumar, P.S.; Ramalingam, S.; Abhinaya, R.V.; Kirupha, S.D.; Murugesan, A.; Sivanesan, S. Adsorption of metal ions onto the chemically modified agricultural waste. Clean-Soil Air Water 2012, 40, 188–197. [Google Scholar] [CrossRef]
  76. Ounnar, A.; Favier, L.; Bouzaza, A.; Bentahar, F.; Trari, M. Kinetic study of spiramycin removal from aqueous solution using heterogeneous photocatalysis. Kinet. Catal. 2016, 57, 200–206. [Google Scholar] [CrossRef]
  77. Vázquez, G.; Mosquera, O.; Freire, M.S.; Antorrena, G.; González-Álvarez, J. Alkaline pre-treatment of waste chestnut shell from a food industry to enhance cadmium, copper, lead and zinc ions removal. Chem. Eng. J. 2012, 184, 147–155. [Google Scholar] [CrossRef]
  78. Vázquez, G.; Sonia Freire, M.; González-Alvarez, J.; Antorrena, G. Equilibrium and kinetic modelling of the adsorption of cd2+ ions onto chestnut shell. Desalination 2009, 249, 855–860. [Google Scholar] [CrossRef]
  79. Inyang, M.I.; Gao, B.; Yao, Y.; Xue, Y.; Zimmerman, A.; Mosa, A.; Pullammanappallil, P.; Ok, Y.S.; Cao, X. A review of biochar as a low-cost adsorbent for aqueous heavy metal removal. Crit. Rev. Environ. Sci. Technol. 2016, 46, 406–433. [Google Scholar] [CrossRef]
  80. Huang, J.-H.; Zeng, G.-M.; Zhou, C.-F.; Li, X.; Shi, L.-J.; He, S.-B. Adsorption of surfactant micelles and cd 2+/zn 2+ in micellar-enhanced ultrafiltration. J. Hazard. Mater. 2010, 183, 287–293. [Google Scholar] [CrossRef] [PubMed]
  81. Danis, U.; Aydiner, C. Investigation of process performance and fouling mechanisms in micellar-enhanced ultrafiltration of nickel-contaminated waters. J. Hazard. Mater. 2009, 162, 577–587. [Google Scholar] [CrossRef] [PubMed]
  82. Landaburu-Aguirre, J.; Pongrácz, E.; Perämäki, P.; Keiski, R.L. Micellar-enhanced ultrafiltration for the removal of cadmium and zinc: Use of response surface methodology to improve understanding of process performance and optimisation. J. Hazard. Mater. 2010, 180, 524–534. [Google Scholar] [CrossRef] [PubMed]
  83. Ferella, F.; Prisciandaro, M.; De Michelis, I. Removal of heavy metals by surfactant-enhanced ultrafiltration from wastewaters. Desalination 2007, 207, 125–133. [Google Scholar] [CrossRef]
  84. Ennigrou, D.J.; Gzara, L.; Romdhane, M.R.B.; Dhahbi, M. Cadmium removal from aqueous solutions by polyelectrolyte enhanced ultrafiltration. Desalination 2009, 246, 363–369. [Google Scholar] [CrossRef]
  85. Camarillo, R.; Llanos, J.; García-Fernández, L.; Pérez, Á.; Canizares, P. Treatment of copper (ii)-loaded aqueous nitrate solutions by polymer enhanced ultrafiltration and electrodeposition. Sep. Purif. Technol. 2010, 70, 320–328. [Google Scholar] [CrossRef]
  86. Barakat, M.A.; Schmidt, E. Polymer-enhanced ultrafiltration process for heavy metals removal from industrial wastewater. Desalination 2010, 256, 90–93. [Google Scholar] [CrossRef]
  87. Molinari, R.; Poerio, T.; Argurio, P. Selective separation of copper (ii) and nickel (ii) from aqueous media using the complexation–ultrafiltration process. Chemosphere 2008, 70, 341–348. [Google Scholar] [CrossRef]
  88. Mohsen-Nia, M.; Montazeri, P.; Modarress, H. Removal of cu2+ and ni2+ from wastewater with a chelating agent and reverse osmosis processes. Desalination 2007, 217, 276–281. [Google Scholar] [CrossRef]
  89. Ipek, U. Removal of ni (ii) and zn (ii) from an aqueous solutionby reverse osmosis. Desalination 2005, 174, 161–169. [Google Scholar] [CrossRef]
  90. Chan, B.; Dudeney, A. Reverse osmosis removal of arsenic residues from bioleaching of refractory gold concentrates. Miner. Eng. 2008, 21, 272–278. [Google Scholar] [CrossRef]
  91. Tanninen, J.; Mänttäri, M.; Nyström, M. Nanofiltration of concentrated acidic copper sulphate solutions. Desalination 2006, 189, 92–96. [Google Scholar] [CrossRef]
  92. Muthukrishnan, M.; Guha, B. Effect of ph on rejection of hexavalent chromium by nanofiltration. Desalination 2008, 219, 171–178. [Google Scholar] [CrossRef]
  93. Cséfalvay, E.; Pauer, V.; Mizsey, P. Recovery of copper from process waters by nanofiltration and reverse osmosis. Desalination 2009, 240, 132–142. [Google Scholar] [CrossRef]
  94. El Samrani, A.G.; Lartiges, B.S.; Villieras, F. Chemical coagulation of combined sewer overflow: Heavy metal removal and treatment optimization. Water Res. 2008, 42, 951–960. [Google Scholar] [CrossRef]
  95. Chang, Q.; Wang, G. Study on the macromolecular coagulant pex which traps heavy metals. Chem. Eng. Sci. 2007, 62, 4636–4643. [Google Scholar] [CrossRef]
  96. Chang, Q.; Zhang, M.; Wang, J.X. Removal of cu2+ and turbidity from wastewater by mercaptoacetyl chitosan. J. Hazard. Mater. 2009, 169, 621–625. [Google Scholar] [CrossRef]
  97. Lundh, M.; Jonsson, L.; Dahlquist, J. Experimental studies of the fluid dynamics in the separation zone in dissolved air flotation. Water Res. 2000, 34, 21–30. [Google Scholar] [CrossRef]
  98. Yuan, X.Z.; Meng, Y.T.; Zeng, G.M.; Fang, Y.Y.; Shi, J.G. Evaluation of tea-derived biosurfactant on removing heavy metal ions from dilute wastewater by ion flotation. Colloids Surf. a-Physicochem. Eng. Asp. 2008, 317, 256–261. [Google Scholar] [CrossRef]
  99. Capponi, F.; Sartori, M.; Souza, M.L.; Rubio, J. Modified column flotation of adsorbing iron hydroxide colloidal precipitates. Int. J. Miner. Process. 2006, 79, 167–173. [Google Scholar] [CrossRef]
  100. Chen, G. Electrochemical technologies in wastewater treatment. Sep. Purif. Technol. 2004, 38, 11–41. [Google Scholar] [CrossRef]
  101. Tzanetakis, N.; Taama, W.; Scott, K.; Jachuck, R.; Slade, R.; Varcoe, J. Comparative performance of ion exchange membranes for electrodialysis of nickel and cobalt. Sep. Purif. Technol. 2003, 30, 113–127. [Google Scholar] [CrossRef]
  102. Jakobsen, M.R.; Fritt-Rasmussen, J.; Nielsen, S.; Ottosen, L.M. Electrodialytic removal of cadmium from wastewater sludge. J. Hazard. Mater. 2004, 106, 127–132. [Google Scholar] [CrossRef]
  103. Belkacem, M.; Khodir, M.; Abdelkrim, S. Treatment characteristics of textile wastewater and removal of heavy metals using the electroflotation technique. Desalination 2008, 228, 245–254. [Google Scholar] [CrossRef]
  104. Khosla, N.K.; Venkatachalam, S.; Somasundaran, P. Pulsed electrogeneration of bubbles for electroflotation. J. Appl. Electrochem. 1991, 21, 986–990. [Google Scholar] [CrossRef]
  105. Mansour, L.B.; Chalbi, S.; Kesentini, I. Experimental study of hydrodynamic and bubble size distributions in electroflotation process. Indian J. Chem. Technol. 2007, 14, 253–257. [Google Scholar]
  106. Burns, S.E.; Yiacoumi, S.; Tsouris, C. Microbubble generation for environmental and industrial separations. Sep. Purif. Technol. 1997, 11, 221–232. [Google Scholar] [CrossRef]
  107. Ketkar, D.R.; Mallikarjunan, R.; Venkatachalam, S. Electroflotation of quartz fines. Int. J. Miner. Process. 1991, 31, 127–138. [Google Scholar] [CrossRef]
  108. Mollah, M.Y.A.; Schennach, R.; Parga, J.R.; Cocke, D.L. Electrocoagulation (ec)—science and applications. J. Hazard. Mater. 2001, 84, 29–41. [Google Scholar] [CrossRef]
  109. Bazrafshan, E.; Mohammadi, L.; Ansari-Moghaddam, A.; Mahvi, A.H. Heavy metals removal from aqueous environments by electrocoagulation process- a systematic review. J. Environ. Health Sci. Eng. 2015, 13. [Google Scholar] [CrossRef] [PubMed] [Green Version]
  110. Verma, S.K.; Khandegar, V.; Saroha, A.K. Removal of chromium from electroplating industry effluent using electrocoagulation. J. Hazard. Toxic Radioact. Waste 2013, 17. [Google Scholar] [CrossRef]
  111. Akbal, F.; Camci, S. Copper, chromium and nickel removal from metal plating wastewater by electrocoagulation. Desalination 2011, 269, 214–222. [Google Scholar] [CrossRef]
  112. Vasudevan, S.; Lakshmi, J.; Sozhan, G. Effects of alternating and direct current in electrocoagulation process on the removal of cadmium from water. J. Hazard. Mater. 2011, 192, 26–34. [Google Scholar] [CrossRef]
  113. Malakootian, M.; Yousefi, N.; Fatehizadeh, A. Survey efficiency of electrocoagulation on nitrate removal from aqueous solution. Int. J. Environ. Sci. Technol. 2011, 8, 107–114. [Google Scholar] [CrossRef]
  114. Pociecha, M.; Lestan, D. Using electrocoagulation for metal and chelant separation from washing solution after edta leaching of pb, zn and cd contaminated soil. J. Hazard. Mater. 2010, 174, 670–678. [Google Scholar] [CrossRef]
  115. Kobya, M.; Ulu, F.; Gebologlu, U.; Demirbas, E.; Oncel, M.S. Treatment of potable water containing low concentration of arsenic with electrocoagulation: Different connection modes and fe-al electrodes. Sep. Purif. Technol. 2011, 77, 283–293. [Google Scholar] [CrossRef]
  116. Kabdasli, I.; Vardar, B.; Arslan-Alaton, I.; Tunay, O. Effect of dye auxiliaries on color and cod removal from simulated reactive dyebath effluent by electrocoagulation. Chem. Eng. J. 2009, 148, 89–96. [Google Scholar] [CrossRef]
  117. Bazrafshan, E.; Moein, H.; Mostafapour, F.K.; Nakhaie, S. Application of electrocoagulation process for dairy wastewater treatment. J. Chem. 2013, 2013. [Google Scholar] [CrossRef] [Green Version]
  118. Al-Qodah, Z.; Al-Shannag, M. Heavy metal ions removal from wastewater using electrocoagulation processes: A comprehensive review. Sep. Sci. Technol. 2017, 1–28. [Google Scholar] [CrossRef]
  119. Apaydin, K.U.; Gonullu, M.T. An investigation on the treatment of tannery wastewater by electrocoagulation. Global Nest J. 2009, 11. [Google Scholar]
  120. Akansha, J.; Nidheesh, P.V.; Gopinath, A.; Anupama, K.V.; Kumar, M.S. Treatment of dairy industry wastewater by combined aerated electrocoagulation and phytoremediation process. Chemosphere 2020, 253. [Google Scholar] [CrossRef] [PubMed]
  121. Kamaraj, R.; Vasudevan, S. Evaluation of electrocoagulation process for the removal of strontium and cesium from aqueous solution. Chem. Eng. Res. Des. 2015, 93, 522–530. [Google Scholar] [CrossRef]
  122. Mahvi, A.H.; Ebrahimi, S.J.A.-D.; Mesdaghinia, A.; Gharibi, H.; Sowlat, M.H. Performance evaluation of a continuous bipolar electrocoagulation/electrooxidation–electroflotation (eceo–ef) reactor designed for simultaneous removal of ammonia and phosphate from wastewater effluent. J. Hazard. Mater. 2011, 192, 1267–1274. [Google Scholar] [CrossRef]
  123. Isa, M.H.; Ezechi, E.H.; Ahmed, Z.; Magram, S.F.; Kutty, S.R.M. Boron removal by electrocoagulation and recovery. Water Res. 2014, 51, 113–123. [Google Scholar] [CrossRef]
  124. Bazrafshan, E.; Ownagh, K.A.; Mahvi, A.H. Application of electrocoagulation process using iron and aluminum electrodes for fluoride removal from aqueous environment. E-J. Chem. 2012, 9, 102629. [Google Scholar] [CrossRef] [Green Version]
  125. Edris Bazrafshan, E.; Mahvi, A.H.; Naseri, S.; Mesdaghinia, A.R. Performance evaluation of electrocoagulation process for removal of chromium6+ from synthetic chromium solutions using iron and aluminum electrodes. Turkish J. Eng. Env. Sci. 2008, 32, 8. [Google Scholar]
  126. Mansoorian, H.J.; Rajabizadeh, A.; Bazrafshan, E.; Mahvi, A.H. Practical assessment of electrocoagulation process in removing nickel metal from aqueous solutions using iron-rod electrodes. Desalin. Water Treat. 2012, 44, 29–35. [Google Scholar] [CrossRef]
  127. Chaturvedi, S.I. Mercury removal using al-al electrodes by electrocoagulation. Int. J. Mod. Eng. Res. (IJMER) 2013, 3, 7. [Google Scholar]
  128. Shafaei, A.; Pajootan, E.; Nikazar, M.; Arami, M. Removal of co (ii) from aqueous solution by electrocoagulation process using aluminum electrodes. Desalination 2011, 279, 121–126. [Google Scholar] [CrossRef]
  129. Pouet, M.F.; Grasmick, A. Urban wastewater treatment by electrocoagulation and flotation. Water Sci. Technol. 1995, 31, 275–283. [Google Scholar] [CrossRef]
  130. Jung, K.-W.; Hwang, M.-J.; Park, D.-S.; Ahn, K.-H. Combining fluidized metal-impregnated granular activated carbon in three-dimensional electrocoagulation system: Feasibility and optimization test of color and cod removal from real cotton textile wastewater. Sep. Purif. Technol. 2015, 146, 154–167. [Google Scholar] [CrossRef]
  131. Adjeroud, N.; Dahmoune, F.; Merzouk, B.; Leclerc, J.-P.; Madani, K. Improvement of electrocoagulation–electroflotation treatment of effluent by addition of opuntia ficus indica pad juice. Sep. Purif. Technol. 2015, 144, 168–176. [Google Scholar] [CrossRef]
  132. Bazrafshan, E.; Azizabadi, H.; Mahvi, A. Performance evaluation of electrocoagulation process for phenol removal from aqueous solutions. Fresenius Environ. Bull. 2012, 21, 364–371. [Google Scholar]
  133. Ozaki, H.; Sharma, K.; Saktaywin, W. Performance of an ultra-low-pressure reverse osmosis membrane (ulprom) for separating heavy metal: Effects of interference parameters. Desalination 2002, 144, 287–294. [Google Scholar] [CrossRef]
  134. Kryvoruchko, A.; Yurlova, L.; Kornilovich, B. Purification of water containing heavy metals by chelating-enhanced ultrafiltration. Desalination 2002, 144, 243–248. [Google Scholar] [CrossRef]
  135. Qdais, H.A.; Moussa, H. Removal of heavy metals from wastewater by membrane processes: A comparative study. Desalination 2004, 164, 105–110. [Google Scholar] [CrossRef]
  136. Kabdasli, I.; Arslan, T.; Olmez-Hanci, T.; Arslan-Alaton, I.; Tunay, O. Complexing agent and heavy metal removals from metal plating effluent by electrocoagulation with stainless steel electrodes. J. Hazard. Mater. 2009, 165, 838–845. [Google Scholar] [CrossRef]
  137. Alvarez, M.T.; Crespo, C.; Mattiasson, B. Precipitation of zn2+, cu2+ and pb2+ at bench scale using biogenic hydrogen sulphide produced from the utilization of volatile fatty acids by sulphate reducing bacteria. J. Biotechnol. 2005, 118, S181. [Google Scholar]
  138. Martins, A.S.; Nunez, L.; Lanza, M.R.D. Enhanced photoelectrocatalytic performance of tio2 nanotube array modified with wo3 applied to the degradation of the endocrine disruptor propyl paraben. J. Electroanal. Chem. 2017, 802, 33–39. [Google Scholar] [CrossRef] [Green Version]
  139. Shankar, K.; Basham, J.I.; Allam, N.K.; Varghese, O.K.; Mor, G.K.; Feng, X.; Paulose, M.; Seabold, J.A.; Choi, K.-S.; Grimes, C.A. Recent advances in the use of tio2 nanotube and nanowire arrays for oxidative photoelectrochemistry. J. Phys. Chem. C 2009, 113, 6327–6359. [Google Scholar] [CrossRef]
  140. Wu, W.Y.; Huang, Z.H.; Lim, T.T. Recent development of mixed metal oxide anodes for electrochemical oxidation of organic pollutants in water. Appl. Catal. a-Gen. 2014, 480, 58–78. [Google Scholar] [CrossRef]
  141. Tan, C.; Xiang, B.; Li, Y.; Fang, J.; Huang, M. Preparation and characteristics of a nano-pbo2 anode for organic wastewater treatment. Chem. Eng. J. 2011, 166, 15–21. [Google Scholar] [CrossRef]
  142. Chen, Y.; Hong, L.; Xue, H.; Han, W.; Wang, L.; Sun, X.; Li, J. Preparation and characterization of tio2-nts/sno2-sb electrodes by electrodeposition. J. Electroanal. Chem. 2010, 648, 119–127. [Google Scholar] [CrossRef]
  143. Hu, X.; Yu, Y.; Sun, Z.R. Preparation and characterization of cerium-doped multiwalled carbon nanotubes electrode for the electrochemical degradation of low-concentration ceftazidime in aqueous solutions. Electrochim. Acta 2016, 199, 80–91. [Google Scholar] [CrossRef]
  144. Sudhagar, P.; Juarez-Perez, E.J.; Kang, Y.S.; Mora-Sero, I. Quantum dot-sensitized solar cells. In Low-Cost Nanomaterials: Toward Greener and More Efficient Energy Applications; Lin, Z., Wang, J., Eds.; Springer Nature: Cham, Switzerland, 2014; pp. 89–136. [Google Scholar]
  145. De Leo, M.; Pereira, F.C.; Moretto, L.M.; Scopece, P.; Polizzi, S.; Ugo, P. Towards a better understanding of gold electroless deposition in track-etched templates. Chem. Mater. 2007, 19, 5955–5964. [Google Scholar] [CrossRef]
  146. Menon, V.P.; Martin, C.R. Fabrication and evaluation of nanoelectrode ensembles. Anal. Chem. 1995, 67, 1920–1928. [Google Scholar] [CrossRef]
  147. Wirtz, M.; Martin, C.R. Template-fabricated gold nanowires and nanotubes. Adv. Mater. 2003, 15, 455–458. [Google Scholar] [CrossRef]
  148. Vidu, R.; Perez-Page, M.; Quach, D.V.; Chen, X.Y.; Stroeve, P. Electrodeposition of ni and te-doped cobalt triantimonide in citrate solutions. Electroanalysis 2015, 27, 2845–2856. [Google Scholar] [CrossRef] [Green Version]
  149. Azizi, A.; Mohammadi, M.; Sadrnezhaad, S.K. End-closed nicofe-b nanotube arrays by electroless method. Mater. Lett. 2011, 65, 289–292. [Google Scholar] [CrossRef]
  150. Wang, W.; Li, N.; Li, X.T.; Geng, W.C.; Qiu, S.L. Synthesis of metallic nanotube arrays in porous anodic aluminum oxide template through electroless deposition. Mater. Res. Bull. 2006, 41, 1417–1423. [Google Scholar] [CrossRef]
  151. Yuan, X.Y.; Wu, G.S.; Xie, T.; Lin, Y.; Zhang, L.D. Self-assembly synthesis and magnetic studies of co-p alloy nanowire arrays. Nanotechnology 2004, 15, 59–61. [Google Scholar] [CrossRef]
  152. Mbindyo, J.K.N.; Reiss, B.D.; Martin, B.R.; Keating, C.D.; Natan, M.J.; Mallouk, T.E. DNA-directed assembly of gold nanowires on complementary surfaces. Adv. Mater. 2001, 13, 249. [Google Scholar] [CrossRef]
  153. Moon, J.M.; Wei, A. Uniform gold nanorod arrays from polyethylenimine-coated alumina templates. J. Phys. Chem. B 2005, 109, 23336–23341. [Google Scholar] [CrossRef] [PubMed] [Green Version]
  154. Wang, J.G.; Tian, M.L.; Mallouk, T.E.; Chan, M.H.W. Microstructure and interdiffusion of template-synthesized au/sn/au junction nanowires. Nano Lett. 2004, 4, 1313–1318. [Google Scholar] [CrossRef] [Green Version]
  155. Budden, M.G.; Wilkinson, D.S. Skin and nail lesions from gold potassium cyanide. Contact Dermat. 1978, 4, 172–173. [Google Scholar] [CrossRef]
  156. Wright, I.H.; Vesey, C.J. Acute poisoning with gold cyanide. Anaesthesia 1986, 41, 936–939. [Google Scholar] [CrossRef]
  157. Wu, M.L.; Tsai, W.J.; Ger, A.; Deng, J.F.; Tsay, S.H.; Yang, M.H. Cholestatic hepatitis caused by acute gold potassium cyanide poisoning. J. Toxicol. -Clin. Toxicol. 2001, 39, 739–743. [Google Scholar] [CrossRef]
  158. Baltrunas, G.; Valiuniene, A.; Vienozinskis, J.; Gaidamauskas, E.; Jankauskas, T.; Margarian, Z. Electrochemical gold deposition from sulfite solution: Application for subsequent polyaniline layer formation. J. Appl. Electrochem. 2008, 38, 1519–1526. [Google Scholar] [CrossRef]
  159. Hou, X.M.; Zhang, X.L.; Chen, S.T.; Fang, Y.; Li, N.; Zhai, X.M.; Liu, Y. Size-controlled synthesis of au nanoparticles and nanowires and their application as sers substrates. Colloids Surfaces a-Physicochem. Eng. Asp. 2011, 384, 345–351. [Google Scholar] [CrossRef]
  160. Kan, C.X.; Cai, W.P.; Li, Z.S.; Fu, G.H.; Zhang, L.D. Reduction effect of pore wall and formation of au nanowires inside monolithic mesoporous silica. Chem. Phys. Lett. 2003, 382, 318–324. [Google Scholar] [CrossRef]
  161. Wang, L.; Song, Y.H.; Sun, L.L.; Guo, C.L.; Sun, Y.J.; Li, Z. Controllable synthesis of gold nanowires. Mater. Lett. 2008, 62, 4124–4126. [Google Scholar] [CrossRef]
  162. Kim, F.; Sohn, K.; Wu, J.S.; Huang, J.X. Chemical synthesis of gold nanowires in acidic solutions. J. Am. Chem. Soc. 2008, 130, 14442. [Google Scholar] [CrossRef] [PubMed]
  163. Ni, C.J.; Hong, F.C.N. Electroless nanowelding of silver nanowires at room temperature. Rsc. Adv. 2014, 4, 40330–40338. [Google Scholar] [CrossRef]
  164. Muench, F.; Kunz, U.; Wardenga, H.F.; Kleebe, H.J.; Ensinger, W. Metal nanotubes and nanowires with rhombohedral cross-section electrolessly deposited in mica templates. Langmuir 2014, 30, 10878–10885. [Google Scholar] [CrossRef]
  165. Kawamori, M.; Yagi, S.; Matsubara, E. Formation of nickel nanowires by electroless deposition. In Nanotechnology; Leonte, O.M., Chen, F., Mustain, W., Eds.; ECS Transactions, The Electrochemical Society: Pennington, NJ, USA, 2012; Volume 30, pp. 1–7. [Google Scholar]
  166. Balela, M.D.L.; Yagi, S.; Matsubara, E. Fabrication of cobalt nanowires by electroless deposition under external magnetic field. J. Electrochem. Soc. 2011, 158, D210–D216. [Google Scholar] [CrossRef] [Green Version]
  167. Kim, Y.; Kim, J.G.; Noh, Y.; Kim, W.B. An overview of one-dimensional metal nanostructures for electrocatalysis. Catal. Surv. Asia 2015, 19, 88–121. [Google Scholar] [CrossRef]
  168. Perez-Page, M.; Yu, E.; Li, J.; Rahman, M.; Dryden, D.M.; Vidu, R.; Stroeve, P. Template-based syntheses for shape controlled nanostructures. Adv. Colloid Interface Sci. 2016, 234, 51–79. [Google Scholar] [CrossRef] [Green Version]
  169. Xie, Z.Q.; Xu, W.W.; Cui, X.D.; Wang, Y. Recent progress in metal-organic frameworks and their derived nanostructures for energy and environmental applications. Chemsuschem 2017, 10, 1645–1663. [Google Scholar] [CrossRef]
  170. Martin, C.R. Membrane-based synthesis of nanomaterials. Chem. Mater. 1996, 8, 1739–1746. [Google Scholar] [CrossRef]
  171. Hulteen, J.C.; Martin, C.R. A general template-based method for the preparation of nanomaterials. J. Mater. Chem. 1997, 7, 1075–1087. [Google Scholar] [CrossRef]
  172. Kautek, W.; Reetz, S.; Pentzien, S. Template electrodeposition of nanowire arrays on gold foils fabricated by pulsed-laser deposition. Electrochim. Acta 1995, 40, 1461–1468. [Google Scholar] [CrossRef]
  173. Dryden, D.M.; Vidu, R.; Stroeve, P. Nanowire formation is preceded by nanotube growth in templated electrodeposition of cobalt hybrid nanostructures. Nanotechnology 2016, 27. [Google Scholar] [CrossRef] [PubMed] [Green Version]
  174. Bao, J.C.; Xu, Z. Template synthesis of ordered nano-system and their applications. Chin. J. Inorg. Chem. 2002, 18, 965–975. [Google Scholar]
  175. Ku, J.R.; Vidu, R.; Talroze, R.; Stroeve, P. Fabrication of nanocables by electrochemical deposition inside metal nanotubes. J. Am. Chem. Soc. 2004, 126, 15022–15023. [Google Scholar] [CrossRef]
  176. Benfield, R.E.; Grandjean, D.; Dore, J.C.; Esfahanian, H.; Wu, Z.H.; Kroll, M.; Geerkens, M.; Schmid, G. Structure of assemblies of metal nanowires in mesoporous alumina membranes studied by exafs, xanes, X-ray diffraction and saxs. Faraday Discuss. 2004, 125, 327–342. [Google Scholar] [CrossRef] [Green Version]
  177. Cao, H.Q.; Xu, Z.; Sheng, D.; Hong, J.M.; Sang, H.; Du, Y.W. An array of iron nanowires encapsulated in polyaniline nanotubules and its magnetic behavior. J. Mater. Chem. 2001, 11, 958–960. [Google Scholar] [CrossRef]
  178. Dryden, D.M.; Sun, T.; McCormick, R.; Hickey, R.; Vidu, R.; Stroeve, P. Anomalous deposition of co-ni alloys in film and nanowire morphologies from citrate baths. Electrochim. Acta 2016, 220, 595–600. [Google Scholar] [CrossRef]
  179. Daub, M.; Enculescu, I.; Neumann, R.; Spohr, R. Ni nanowires electrodeposited in single ion track templates. J. Optoelectron. Adv. Mater. 2005, 7, 865–870. [Google Scholar]
  180. Vidu, R.; Predescu, A.M.; Matei, E.; Berbecaru, A.; Pantilimon, C.; Dragan, C.; Predescu, C. Template-assisted co-ni nanowire arrays. Nanomaterials 2019, 9, 1446. [Google Scholar] [CrossRef] [Green Version]
  181. Demoustier-Champagne, S.; Delvaux, M. Preparation of polymeric and metallic nanostructures using a template-based deposition method. Mater. Sci. Eng. C-Biomim. Supramol. Syst. 2001, 15, 269–271. [Google Scholar] [CrossRef]
  182. Wirtz, M.; Parker, M.; Kobayashi, Y.; Martin, C.R. Molecular sieving and sensing with gold nanotube membranes. Chem. Rec. 2002, 2, 259–267. [Google Scholar] [CrossRef] [PubMed]
  183. Wirtz, M.; Parker, M.; Kobayashi, Y.; Martin, C.R. Template-synthesized nanotubes for chemical separations and analysis. Chem. -A Eur. J. 2002, 8, 3573–3578. [Google Scholar] [CrossRef]
  184. Wirtz, M.; Yu, S.F.; Martin, C.R. Template synthesized gold nanotube membranes for chemical separations and sensing. Analyst 2002, 127, 871–879. [Google Scholar] [CrossRef]
  185. Delvaux, M.; Demoustier-Champagne, S.; Walcarius, A. Flow injection amperometric detection at enzyme-modified gold nanoelectrodes. Electroanalysis 2004, 16, 190–198. [Google Scholar] [CrossRef]
  186. Delvaux, M.; Walcarius, A.; Demoustier-Champagne, S. Electrocatalytic h2o2 amperometric detection using gold nanotube electrode ensembles. Anal. Chim. Acta 2004, 525, 221–230. [Google Scholar] [CrossRef]
  187. Delvaux, M.; Demoustier-Champagne, S. Immobilisation of glucose oxidase within metallic nanotubes arrays for application to enzyme biosensors. Biosens. Bioelectron. 2003, 18, 943–951. [Google Scholar] [CrossRef]
  188. Zhang, G.M.; Emmanuel, R.; Liu, H.W.; Liu, W.M.; Hou, S.M.; Kui, Y.Z.; Xue, Z.Q. Field emission from an array of free-standing metallic nanowires. Chin. Phys. Lett. 2002, 19, 1016–1018. [Google Scholar]
  189. Tian, M.L.; Wang, J.G.; Snyder, J.; Kurtz, J.; Liu, Y.; Schiffer, P.; Mallouk, T.E.; Chan, M.H.W. Synthesis and characterization of superconducting single-crystal sn nanowires. Appl. Phys. Lett. 2003, 83, 1620–1622. [Google Scholar] [CrossRef] [Green Version]
  190. Tian, M.L.; Wang, J.U.; Kurtz, J.; Mallouk, T.E.; Chan, M.H.W. Electrochemical growth of single-crystal metal nanowires via a two-dimensional nucleation and growth mechanism. Nano Lett. 2003, 3, 919–923. [Google Scholar] [CrossRef]
  191. Schonenberger, C.; van der Zande, B.M.I.; Fokkink, L.G.J.; Henny, M.; Schmid, C.; Kruger, M.; Bachtold, A.; Huber, R.; Birk, H.; Staufer, U. Template synthesis of nanowires in porous polycarbonate membranes: Electrochemistry and morphology. J. Phys. Chem. B 1997, 101, 5497–5505. [Google Scholar] [CrossRef]
  192. Liu, H.W.; Hou, S.M.; Zhang, G.M.; Shen, Z.Y.; Liu, W.M.; Wu, J.L.; Xue, Z.Q.; Roy, E.; Zhang, K.Y. Structure and electrical properties of gold nanowires grown with electrochemical deposition. Acta Phys. -Chim. Sin. 2002, 18, 359–363. [Google Scholar]
  193. Wang, H.; Wang, J.; Tian, M.; Bell, L.; Hutchinson, E.; Rosario, M.M.; Liu, Y.; Amma, A.; Mallouk, T. Metallic contacts with individual ru nanowires prepared by electrochemical deposition and the suppression of superconductivity in ultrasmall ru grains. Appl. Phys. Lett. 2004, 84, 5171–5173. [Google Scholar] [CrossRef]
  194. Wang, J.G.; Tian, M.L.; Mallouk, T.E.; Chan, M.H.W. Microtwinning in template-synthesized single-crystal metal nanowires. J. Phys. Chem. B 2004, 108, 841–845. [Google Scholar] [CrossRef]
  195. Wang, X.J.; Bohn, P.W. Anisotropic in-plane gradients of poly(acrylic acid) formed by electropolymerization with spatiotemporal control of the electrochemical potential. J. Am. Chem. Soc. 2004, 126, 6825–6832. [Google Scholar] [CrossRef] [PubMed]
  196. Wang, Y.C.; Fan, S.C.; Lee, K.R.; Li, C.L.; Huang, S.H.; Tsai, H.A.; Lai, J.Y. Polyamide/sds-clay hybrid nanocomposite membrane application to water-ethanol mixture pervaporation separation. J. Membr. Sci. 2004, 239, 219–226. [Google Scholar] [CrossRef]
  197. Wang, Y.H.; Yang, J.J.; Ye, C.H.; Fang, X.S.; Zhang, L.D. Thermal expansion of cu nanowire arrays. Nanotechnology 2004, 15, 1437–1440. [Google Scholar] [CrossRef]
  198. Barbic, M.; Mock, J.J.; Smith, D.R.; Schultz, S. Single crystal silver nanowires prepared by the metal amplification method. Journal Of Applied Physics 2002, 91, 9341–9345. [Google Scholar] [CrossRef]
  199. Valizadeh, S.; George, J.M.; Leisner, P.; Hultman, L. Electrochemical deposition of co nanowire arrays; quantitative consideration of concentration profiles. Electrochim. Acta 2001, 47, 865–874. [Google Scholar] [CrossRef]
  200. Pignard, S.; Goglio, G.; Huynen, I.; Radulescu, A.; Piraux, L. Ferromagnetic resonance in submicron metallic wires. IEEE Trans. Magn. 2000, 36, 3482–3484. [Google Scholar] [CrossRef]
  201. Pignard, S.; Goglio, G.; Radulescu, A.; Piraux, L.; Dubois, S.; Declemy, A.; Duvail, J.L. Study of the magnetization reversal in individual nickel nanowires. J. Appl. Phys. 2000, 87, 824–829. [Google Scholar] [CrossRef]
  202. Ge, S.H.; Li, C.; Ma, X.; Li, W.; Li, C.X. The influence of magnetic field on the crystal growth of electrodeposited co nanowires. Acta Phys. Sin. 2001, 50, 149–152. [Google Scholar]
  203. Ge, S.H.; Li, C.; Ma, X.; Li, W.; Xi, L.; Li, C.X. Approach to fabricating co nanowire arrays with perpendicular anisotropy: Application of a magnetic field during deposition. J. Appl. Phys. 2001, 90, 509–511. [Google Scholar] [CrossRef]
  204. Ge, S.H.; Ma, X.; Li, C.; Li, W. Fabrication of electro deposited co nanowire arrays with perpendicular anisotropy. J. Magn. Magn. Mater. 2001, 226, 1867–1869. [Google Scholar] [CrossRef]
  205. Tai, Y.L.; Teng, H.S. Template synthesis and electrochemical characterization of nickel-based tubule electrode arrays. Chem. Mater. 2004, 16, 338–342. [Google Scholar] [CrossRef]
  206. Ohgai, T.; Gravier, L.; Hoffer, X.; Lindeberg, M.; Hjort, K.; Spohr, R.; Ansermet, J.P. Template synthesis and magnetoresistance property of ni and co single nanowires electrodeposited into nanopores with a wide range of aspect ratios. J. Phys. D-Appl. Phys. 2003, 36, 3109–3114. [Google Scholar] [CrossRef]
  207. Pra, L.D.D.; Ferain, E.; Legras, R.; Demoustier-Champagne, S. Fabrication of a new generation of track-etched templates and their use for the synthesis of metallic and organic nanostructures. Nucl. Instrum. Methods Phys. Res. Sect. B-Beam Interact. Mater. Atoms 2002, 196, 81–88. [Google Scholar]
  208. Schuchert, I.U.; Molares, M.E.T.; Dobrev, D.; Vetter, J.; Neumann, R.; Martin, M. Electrochemical copper deposition in etched ion track membranes—Experimental results and a qualitative kinetic model. J. Electrochem. Soc. 2003, 150, C189–C194. [Google Scholar] [CrossRef]
  209. Molares, M.E.T.; Brotz, J.; Buschmann, V.; Dobrev, D.; Neumann, R.; Scholz, R.; Schuchert, I.U.; Trautmann, C.; Vetter, J. Etched heavy ion tracks in polycarbonate as template for copper nanowires. Nucl. Instrum. Methods Phys. Res. Sect. B-Beam Interact. Mater. Atoms 2001, 185, 192–197. [Google Scholar] [CrossRef]
  210. Molares, M.E.T.; Buschmann, V.; Dobrev, D.; Neumann, R.; Scholz, R.; Schuchert, I.U.; Vetter, J. Single-crystalline copper nanowires produced by electrochemical deposition in polymeric ion track membranes. Adv. Mater. 2001, 13, 62. [Google Scholar] [CrossRef]
  211. Enculescu, I.; Siwy, Z.; Dobrev, D.; Trautmann, C.; Toimil Molares, M.E.; Neumann, R.; Hjort, K.; Westerberg, I.; Spohr, R. Copper nanowires electrodeposited in etched single-ion track templates. Appl. Phys. A 2003, 77, 751–755. [Google Scholar] [CrossRef]
  212. Buledi, J.A.; Amin, S.; Haider, S.I.; Bhanger, M.I.; Solangi, A.R. A review on detection of heavy metals from aqueous media using nanomaterial-based sensors. Environ. Sci. Pollut. Res. 2020, 1–9. [Google Scholar] [CrossRef] [PubMed]
  213. Zheng, M.J.; Zhang, L.D.; Zhang, X.Y.; Zhang, J.; Li, G.H. Fabrication and optical absorption of ordered indium oxide nanowire arrays embedded in anodic alumina membranes. Chem. Phys. Lett. 2001, 334, 298–302. [Google Scholar] [CrossRef]
  214. Cheng, B.; Samulski, E.T. Fabrication and characterization of nanotubular semiconductor oxides in2o3 and ga2o3. Journal of Materials Chemistry 2001, 11, 2901–2902. [Google Scholar] [CrossRef]
  215. Ding, G.Q.; Shen, W.Z.; Zheng, M.J.; Zhou, Z.B. Indium oxide “rods in dots” nanostructures. Appl. Phys. Lett. 2006, 89. [Google Scholar] [CrossRef] [Green Version]
  216. Jeong, J.S.; Lee, J.Y.; Lee, C.J.; An, S.J.; Yi, G.C. Synthesis and characterization of high-quality in2o3 nanobelts via catalyst-free growth using a simple physical vapor deposition at low temperature. Chem. Phys. Lett. 2004, 384, 246–250. [Google Scholar] [CrossRef]
  217. O’Dwyer, C.; Szachowicz, M.; Visimberga, G.; Lavayen, V.; Newcomb, S.B.; Torres, C.M.S. Bottom-up growth of fully transparent contact layers of indium tin oxide nanowires for light-emitting devices. Nat. Nanotechnol. 2009, 4, 239–244. [Google Scholar] [CrossRef] [Green Version]
  218. Li, C.; Zhang, D.H.; Han, S.; Liu, X.L.; Tang, T.; Zhou, C.W. Diameter-controlled growth of single-crystalline in2o3 nanowires and their electronic properties. Adv. Mater. 2003, 15, 143. [Google Scholar] [CrossRef]
  219. Kim, H.W.; Kim, N.H.; Lee, C. An mocvd route to in2o3 one-dimensional materials with novel morphologies. Appl. Phys. a-Mater. Sci. Process. 2005, 81, 1135–1138. [Google Scholar] [CrossRef]
  220. Liu, Q.; Zou, R.J.; Bando, Y.; Golberg, D.; Hu, J.Q. Nanowires sheathed inside nanotubes: Manipulation, properties and applications. Prog. Mater. Sci. 2015, 70, 1–49. [Google Scholar] [CrossRef]
  221. Muhr, H.J.; Krumeich, F.; Schonholzer, U.P.; Bieri, F.; Niederberger, M.; Gauckler, L.J.; Nesper, R. Vanadium oxide nanotubes—A new flexible vanadate nanophase. Adv. Mater. 2000, 12, 231. [Google Scholar] [CrossRef]
  222. Bao, J.C.; Xu, D.P.; Zhou, Q.F.; Xu, Z. An array of concentric composite nanostructure of metal nanowires encapsulated in zirconia nanotubes: Preparation, characterization, and magnetic properties. Chem. Mater. 2002, 14, 4709–4713. [Google Scholar] [CrossRef]
  223. Huang, X.; Rui, X.H.; Hng, H.H.; Yan, Q.Y. Vanadium pentoxide-based cathode materials for lithium-ion batteries: Morphology control, carbon hybridization, and cation doping. Part. Part. Syst. Charact. 2015, 32, 276–294. [Google Scholar] [CrossRef]
  224. Li, Y.B.; Bando, Y.; Golberg, D. Single-crystalline in2o3 nanotubes filled with in. Adv. Mater. 2003, 15, 581–585. [Google Scholar] [CrossRef]
  225. Li, Y.B.; Bando, Y.; Golberg, D.; Liu, Z.W. Ga-filled single-crystalline mgo nanotube: Wide-temperature range nanothermometer. Appl. Phys. Lett. 2003, 83, 999–1001. [Google Scholar] [CrossRef]
  226. Ajayan, P.M.; Iijima, S. Smallest carbon nanotube. Nature 1992, 358, 23. [Google Scholar] [CrossRef]
  227. Ajayan, P.M.; Iijima, S. Capillarity-induced filling of carbon nanotubes. Nature 1993, 361, 333–334. [Google Scholar] [CrossRef]
  228. Bansod, B.; Kumar, T.; Thakur, R.; Rana, S.; Singh, I. A review on various electrochemical techniques for heavy metal ions detection with different sensing platforms. Biosens. Bioelectron. 2017, 94, 443–455. [Google Scholar] [CrossRef]
  229. Liu, Y.Y.; Liu, J.; Zhang, Q.L.; Wei, J.; Xu, G.Y. Bismuth nano-flower modified cpe for anodic stripping voltammetry detection of cd(ii). Int. J. Electrochem. Sci. 2019, 14, 4483–4495. [Google Scholar] [CrossRef]
  230. Zeng, Z.T.; Fang, S.Y.; Tang, D.; Xiao, R.; Tang, L.; Peng, B.; Gong, J.L.; Long, B.Q.; Ouyang, X.L.; Zeng, G.M. Ultrasensitive sensor based on novel bismuth carbon nanomaterial for lead and cadmium determination in natural water, contaminated soil and human plasma. Microporous Mesoporous Mater. 2019, 284, 177–185. [Google Scholar] [CrossRef]
  231. Zhang, Y.X.; Li, C.; Su, Y.C.; Mu, W.; Han, X.J. Simultaneous detection of trace cd(ii) and pb(ii) by differential pulse anodic stripping voltammetry using a bismuth oxycarbide/nafion electrode. Inorg. Chem. Commun. 2020, 111. [Google Scholar] [CrossRef]
  232. Liu, L.; Zhang, K.; Wei, Y.M. A simple strategy for the detection of cu(ii), cd(ii) and pb(ii) in water by a voltammetric sensor on a tc4a modified electrode. New J. Chem. 2019, 43, 1544–1550. [Google Scholar] [CrossRef]
  233. Gao, F.; Gao, N.N.; Nishitani, A.; Tanaka, H. Rod-like hydroxyapatite and nafion nanocomposite as an electrochemical matrix for simultaneous and sensitive detection of hg2+, cu2+, pb2+ and cd2+. J. Electroanal. Chem. 2016, 775, 212–218. [Google Scholar] [CrossRef]
Figure 1. Illustration of the main heavy metal ions (HMIs) present in wastewaters, which are listed according to their toxicity, with pictograms and main health hazards for each element, according to the United Nations Guide to the Globally Harmonized System of Classification and Labeling of Chemicals (GHS) [3].
Figure 1. Illustration of the main heavy metal ions (HMIs) present in wastewaters, which are listed according to their toxicity, with pictograms and main health hazards for each element, according to the United Nations Guide to the Globally Harmonized System of Classification and Labeling of Chemicals (GHS) [3].
Toxics 08 00101 g001
Figure 2. Nanomaterials and their surface properties that can be control in various applications.
Figure 2. Nanomaterials and their surface properties that can be control in various applications.
Toxics 08 00101 g002
Figure 3. Illustration of the electrodialysis operation principles. The membranes have anionic or cationic property. When the mixture passes through the membranes, the ions are moved to the direction of the anode or cathode.
Figure 3. Illustration of the electrodialysis operation principles. The membranes have anionic or cationic property. When the mixture passes through the membranes, the ions are moved to the direction of the anode or cathode.
Toxics 08 00101 g003
Figure 4. Removal efficiency of Cr (III), Cr (VI), As (III) and Hg function of the initial concentration of ions in the water.
Figure 4. Removal efficiency of Cr (III), Cr (VI), As (III) and Hg function of the initial concentration of ions in the water.
Toxics 08 00101 g004
Figure 5. Level of removal efficiency for Ni2+, Cu2+ and Cr as a function of the method of their removal (adapted from [109]).
Figure 5. Level of removal efficiency for Ni2+, Cu2+ and Cr as a function of the method of their removal (adapted from [109]).
Toxics 08 00101 g005
Figure 6. The efficiency of HMIs removal by different methods such as electrocoagulation (ECoag), electroflotation (EF) and electrochemical removal (EC) (adapted from [118]).
Figure 6. The efficiency of HMIs removal by different methods such as electrocoagulation (ECoag), electroflotation (EF) and electrochemical removal (EC) (adapted from [118]).
Toxics 08 00101 g006
Figure 7. Schematic illustration of the vertically aligned nanotube electrodes.
Figure 7. Schematic illustration of the vertically aligned nanotube electrodes.
Toxics 08 00101 g007
Figure 8. Illustration of the electroless deposition process.
Figure 8. Illustration of the electroless deposition process.
Toxics 08 00101 g008
Figure 9. (a) Nanoporous membrane that has one side coated with a metallic film. (b) Electrochemical deposition through the nanopores (the arrows indicate the growth direction of nanowires inside pores). (c) Nanowires obtained inside nanoporous membranes.
Figure 9. (a) Nanoporous membrane that has one side coated with a metallic film. (b) Electrochemical deposition through the nanopores (the arrows indicate the growth direction of nanowires inside pores). (c) Nanowires obtained inside nanoporous membranes.
Toxics 08 00101 g009
Figure 10. (a) Metallic nanotubes obtained inside the polycarbonate (PCTE) membrane, as electric conductive base for the electrochemical deposition of further materials. (b) Pores are filled by radial electrochemical deposition (arrows show the growth direction inside the pore). (c) Nanocable structures (i.e., filled nanotubes) formed in the PCTE membranes.
Figure 10. (a) Metallic nanotubes obtained inside the polycarbonate (PCTE) membrane, as electric conductive base for the electrochemical deposition of further materials. (b) Pores are filled by radial electrochemical deposition (arrows show the growth direction inside the pore). (c) Nanocable structures (i.e., filled nanotubes) formed in the PCTE membranes.
Toxics 08 00101 g010
Figure 11. Nanomaterials used for detection of heavy metals (adapted from [212]).
Figure 11. Nanomaterials used for detection of heavy metals (adapted from [212]).
Toxics 08 00101 g011
Figure 12. Differential pulse anodic stripping voltammetry (DPASV) curves of bismuth oxycarbide for the simultaneous detection of Cd(II) and Pb(II) (a-top left) [231]; thiacalix [4] arene-modified glassy carbon electrode for the simultaneous determination of tree HMIs (b-top middle) [232]; Hydroxyapatite-Nafion for the simultaneous detection of four HMIs (c-top right) [233]. The calibration curves are presented in (b) and (c) under the respective DPASV curves.
Figure 12. Differential pulse anodic stripping voltammetry (DPASV) curves of bismuth oxycarbide for the simultaneous detection of Cd(II) and Pb(II) (a-top left) [231]; thiacalix [4] arene-modified glassy carbon electrode for the simultaneous determination of tree HMIs (b-top middle) [232]; Hydroxyapatite-Nafion for the simultaneous detection of four HMIs (c-top right) [233]. The calibration curves are presented in (b) and (c) under the respective DPASV curves.
Toxics 08 00101 g012
Table 1. Permissible limits for various heavy metals in wastewater treatment effluents according to the World Health Organization [2] and United States Environmental Protection Agency (USEPA) [1].
Table 1. Permissible limits for various heavy metals in wastewater treatment effluents according to the World Health Organization [2] and United States Environmental Protection Agency (USEPA) [1].
Heavy MetalPermissible Limits (WHO) µg/LPermissible Limits (USEPA) µg/LHealth Hazards
Arsenic500*Carcinogenic, producing liver tumors, skin and gastrointestinal effects
Mercury10.03Corrosive to skin, eyes and muscle membrane, dermatitis, anorexia, kidney damage and severe muscle pain
Cadmium310Carcinogenic, cause lung fibrosis, dyspnea and weight loss
Lead106Suspected carcinogen, loss of appetite, anemia, muscle and joint pains, diminishing IQ, cause sterility, kidney problem and high blood pressure
Chromium5050Suspected human carcinogen, producing lung tumors, allergic dermatitis
Nickel20200Causes chronic bronchitis, reduced lung function, cancer of lungs and nasal sinus
Zinc5000*Causes short-term illness called “metal fume fever” and restlessness
Copper3000*Long term exposure causes irritation of nose, mouth, eyes, headache, stomachache, dizziness, diarrhea
* Data not available.
Table 2. Advantages and disadvantages of the chemical precipitation function of the coagulant used in the process.
Table 2. Advantages and disadvantages of the chemical precipitation function of the coagulant used in the process.
Chemical PrecipitationAdvantagesDisadvantages
Hydroxide precipitation (lime, limestone, CaCO3)Easy method, simple operation, cheap and broad applications.Accumulation of large quantity of residual sludge with water content, problematic for dewater and disposal. Not suitable for wastewaters with high heavy metals concentrations.
Sulfide precipitationLess sludge quantity, easier dehydration.Metallic sulfide precipitate is very small and difficult to settle down.
Ferrite co-precipitationEfficient for heavy metals removal with density higher than 3.8 g/cm3 (Cu, Pb, Zn, Cd, Co, Cr, Mn, Hg, Bi, Sn, As, Mo, Fe, V, Ti). Possible separation of formed precipitates by filtration or magnetic methods.High temperature, not suitable for large volume of wastewater, high energy consumption.
Table 3. The maximum adsorbents capacities for various carbon-based adsorbents.
Table 3. The maximum adsorbents capacities for various carbon-based adsorbents.
AdsorbateAdsorbentMax. Adsorption, mg/gInitial Concentration, mg/LpHRef.
Pb2+MWCNTs15.610–803, 5, 7[51]
Oxidized MWCNTs59 5[52]
SWCNTs33.55 7[53]
Cu2+MWCNTs12.34 7[54]
Oxidized MWCNTs28.495–305[55]
SWCNTs24.29 5[52]
Oxidized MWCNTs10.862–155[55]
SWCNTs24.07 7[53]
Oxidized MWCNTs38.4610–807[58]
oxidized SWCNTs47.8510–807[58]
Zn2+MWCNTs32.6810–80 [59]
SWCNTs43.6610–80 [59]
PAC13.0410–80 [59]
Table 4. Removal efficiency of heavy metals by membrane technologies.
Table 4. Removal efficiency of heavy metals by membrane technologies.
Heavy MetalCdNiZnPbAsO4CdCuCrNi
MembranePolysulfonePolycarbonateAmicon regenerated celluloseCeramicCeramicPolysulfoneCeramicPolyethersulfonePolyethersulfone
Removal efficiency92%98.6%99%99%19%99%99.5%99.5%100%
Table 5. A list of selected examples of heavy metal removal efficiencies by RO, NF and NF + RO.
Table 5. A list of selected examples of heavy metal removal efficiencies by RO, NF and NF + RO.
MembraneReverse OsmosisNanofiltrationReverse Osmosis + Nanofiltration
Heavy MetalCuNiZnAsCuCrCu
Removal Efficiency99.599.398.9As(V) 91–99%, As(III) 20–55%96–9899.595–99
Table 6. Removal efficiency of heavy metal ions for different anode/cathode electrode combination in electrocoagulation system.
Table 6. Removal efficiency of heavy metal ions for different anode/cathode electrode combination in electrocoagulation system.
Metals or Other CompoundsConcentration, mg/LElectrodes Anode/CathodeRemoval Efficiency, %References
Cr3+, Cr6+887.2, 1495.2Fe/Fe100[110]
Cu2+, Cr, Ni2+45, 44.5, 394Al/Fe100[111]
Cd2+20Al/AlAC: 97.5 DC: 96.2[112]
NO3−150Fe/Fe, Al/Al90, 89.7[113]
Pb2+, Zn2+, Cd2+170, 50, 1.5Al/SS95, 68, 66[114]
As150Al/Al, Fe/Fe93.5, 94[115]
TOC, Ni2+, Zn2+173, 248, 232SS 304-SS 30466, 90, 100[116]
Humic acid20Fe/Fe92.69[117]
Table 7. Comparison of the removal efficiency of heavy metal ions by different water treatments.
Table 7. Comparison of the removal efficiency of heavy metal ions by different water treatments.
Water Treatment MethodMetalInitial Concentration mg/LEfficiency %References
Reverse Osmosis (pH = 7–9)Ni2+2699[133]
Ultrafiltration (pH > 7)Ni2+5099[86]
Nanofiltration (pH = 4–11)Cu2+20096[135]
Electrocoagulation (pH = 8)Ni2+39499[111]
Ni2+, Zn2+248, 270, 282, 217, 232, 236100[136]
Chemical Precipitation (pH > 7)Cu2+, Zn2+, Cr3+, Pb2+10099.3–99.6[13]
Cu2+, Zn2+, Pb2+0.01, 1.34, 2.3 100, >94, >92[137]
Publisher’s Note: MDPI stays neutral with regard to jurisdictional claims in published maps and institutional affiliations.

Share and Cite

MDPI and ACS Style

Vidu, R.; Matei, E.; Predescu, A.M.; Alhalaili, B.; Pantilimon, C.; Tarcea, C.; Predescu, C. Removal of Heavy Metals from Wastewaters: A Challenge from Current Treatment Methods to Nanotechnology Applications. Toxics 2020, 8, 101.

AMA Style

Vidu R, Matei E, Predescu AM, Alhalaili B, Pantilimon C, Tarcea C, Predescu C. Removal of Heavy Metals from Wastewaters: A Challenge from Current Treatment Methods to Nanotechnology Applications. Toxics. 2020; 8(4):101.

Chicago/Turabian Style

Vidu, Ruxandra, Ecaterina Matei, Andra Mihaela Predescu, Badriyah Alhalaili, Cristian Pantilimon, Claudia Tarcea, and Cristian Predescu. 2020. "Removal of Heavy Metals from Wastewaters: A Challenge from Current Treatment Methods to Nanotechnology Applications" Toxics 8, no. 4: 101.

Note that from the first issue of 2016, this journal uses article numbers instead of page numbers. See further details here.

Article Metrics

Back to TopTop