Next Article in Journal / Special Issue
Preparation and Photocatalytic Properties of Sr2−xBaxTa3O10−yNz Nanosheets
Previous Article in Journal / Special Issue
Conversion of CO2 via Visible Light Promoted Homogeneous Redox Catalysis
Font Type:
Arial Georgia Verdana
Font Size:
Aa Aa Aa
Line Spacing:
Column Width:

Photocatalytic Water Treatment by Titanium Dioxide: Recent Updates

School of Applied Sciences and Engineering, Monash University, Churchill VIC, 3842, Australia
School of Chemistry, Monash University, Clayton VIC, 3800, Australia
Dipartimento di Scienze Chimiche e Geologiche, Università di Cagliari, Complesso Universitario Monserrato, CA 09042, Italy
Author to whom correspondence should be addressed.
Catalysts 2012, 2(4), 572-601;
Submission received: 7 October 2012 / Revised: 7 December 2012 / Accepted: 10 December 2012 / Published: 19 December 2012
(This article belongs to the Special Issue Photocatalysts)


Photocatalytic water treatment using nanocrystalline titanium dioxide (NTO) is a well-known advanced oxidation process (AOP) for environmental remediation. With the in situ generation of electron-hole pairs upon irradiation with light, NTO can mineralize a wide range of organic compounds into harmless end products such as carbon dioxide, water, and inorganic ions. Photocatalytic degradation kinetics of pollutants by NTO is a topic of debate and the mostly reporting Langmuir-Hinshelwood kinetics must accompanied with proper experimental evidences. Different NTO morphologies or surface treatments on NTO can increase the photocatalytic efficiency in degradation reactions. Wisely designed photocatalytic reactors can decrease energy consumption or can avoid post-separation stages in photocatalytic water treatment processes. Doping NTO with metals or non-metals can reduce the band gap of the doped catalyst, enabling light absorption in the visible region. Coupling NTO photocatalysis with other water-treatment technologies can be more beneficial, especially in large-scale treatments. This review describes recent developments in the field of photocatalytic water treatment using NTO.

Graphical Abstract

1. Introduction

Realizing the importance of keeping our planet clean, researchers are actively working for eco-friendly alternative technologies for all areas of daily life. Sustainable energy production and pollutant destruction are two of the areas in which intense research is being carried out. Semiconductor-mediated photocatalysis is a well-established technique for pollutant degradation and hydrogen (clean fuel) production by water splitting. Photocatalysis can be defined as a “catalytic reaction involving the production of a catalyst by absorption of light” [1]. The appropriate positioning of valence (VB) and conduction (CB) bands in semiconductors (Figure 1a) makes them suitable materials for the absorption of light and photocatalytic action. Nanocrystalline titanium dioxide (NTO) is a multifunctional semiconductor photocatalyst that can be an energy catalyst (in water splitting to produce hydrogen fuel), an environmental catalyst (in water and air purification), or an electron transport medium in dye-sensitized solar cells (Figure 1b) [2,3,4,5]. Compared to other available semiconductor photocatalysts, NTO is unique in its chemical and biological inertness, photostability (i.e., not prone to photoanodic corrosion), and low cost of production [6]. Photocatalytic water and air purification using NTO is a predominant advanced oxidation process (AOP) because of its efficiency and eco-friendliness. Homogeneous photo-Fenton technique is another efficient AOP for the oxidation of water contaminants [7,8]. However, the photo-Fenton process requires the use of ferrous sulfate (FeSO4) and hydrogen peroxide (H2O2). For example, in the photo-Fenton oxidation of catechol, H2O2 (2000 mg L−1) and FeSO4 (500 mg L−1) were used in the experiment that reported the highest activity [7]. In contrast, NTO photocatalysis may not require any additional reagents beyond the NTO catalyst.
Figure 1. (a) VB and CB positions in metals, semiconductors, and insulators; (b) Tree diagram showing applications of TiO2.
Figure 1. (a) VB and CB positions in metals, semiconductors, and insulators; (b) Tree diagram showing applications of TiO2.
Catalysts 02 00572 g001
The spectrum of compounds that are susceptible to the destructive power of NTO photocatalysis is remarkable, comprising families of dyes, pesticides, herbicides, pharmaceuticals, cosmetics, phenolic compounds, toxins, and more. Recent examples of compounds photocatalytically degraded by NTO are given in Table 1. It is obvious from the table that researchers are focused on the photocatalytic degradation of real pollutant systems, such as cosmetics and pharmaceutical wastewaters [9,10], paper mill wastewater [11], grey water [12], and municipal wastewater [13]. Cheaper sources of TiO2, such as bulk-synthesized TiO2 pigment [14] and iron-containing industrial TiO2 by-products [15], have been explored for the photocatalytic degradation of phenol and humic acids. Interestingly, their activities were found to be comparable with those of the commercially available Degussa P25 TiO2 photocatalyst, the benchmark TiO2 photocatalyst for all applications. A report by Kim et al. describes the successful, elegant, and simultaneous use of NTO as both an energy and an environmental photocatalyst [16]. Their surface-fluorinated and -platinized NTO catalyst generated hydrogen gas when degrading 4-chlorophenol and bisphenol compounds. The selective degradation of contaminants is another promising area in photocatalytic water treatment. Selective degradation could be useful for mixtures of highly toxic pollutants in low concentrations and less harmful compounds in higher concentrations [17,18]. The former can be degraded by means of NTO photocatalysis, whereas the latter can be removed by less-expensive biological wastewater treatments [18]. In addition, valuable compounds must be recovered from wastewater; selective photocatalysis can be a useful tool. Recently, one of the authors reported the complete selective degradation of methyl orange and methylene blue dyes by base-modified nanocrystalline anatase (the most active form of TiO2) photocatalysts [19]. Among the two sol-gel-derived anatase photocatalysts, TSC60, with positive surface charge, selectively adsorbed and degraded the anionic dye methyl orange. In contrast, the second catalyst, TAH60, with negative surface charge, showed selective adsorption of the cationic dye methylene blue, followed by its degradation, from an aqueous mixture containing methyl orange and methylene blue dyes.

2. Mechanism and Kinetics

Photocatalytic destruction of pollutants in aqueous solutions using NTO is facilitated mainly by a series of hydroxylation reactions initiated by hydroxyl radicals (·OH) [20,21,22,23,24,25,26]. Possible modes of ·OH generation during NTO photocatalysis are shown in Figure 2. Upon UV light illumination, electron-hole pairs are formed in the NTO semiconductor photocatalyst. Holes are positive charges, which when in contact with water molecules, produce ·OH and H+ ions. Electrons react with dissolved oxygen to form superoxide ions (O2·), which react with water molecules to produce hydroxide ions (OH) and peroxide radicals (·OOH). Peroxide radicals combine with H+ ions to form ·OH and OH, and holes oxidize OH to ·OH. Thus, all species eventually facilitate the formation of ·OH, and these radicals attack the pollutants present in the aqueous solution.
Medanna et al. reported [20] the formation of 51 stable intermediates in the photocatalytic degradation of the mosquito repellent N,N-diethyl-m-toluamide (DEET) using titanium dioxide under simulated solar light. Using a technique that coupled high-performance liquid chromatography with high-resolution mass spectrometry, they also identified several isomeric species. The degradation of DEET began with ·OH-mediated mono- and polyhydroxylation reactions, followed by the oxidation and ring-opening reactions of intermediates. All the identified intermediates underwent complete mineralization after 4 h irradiation. The ·OH-initiated photocatalytic oxidation of quinolones [21], i.e., flumequine and nalidixic acid, using NTO under solar light passed through fourteen stable intermediates that were identified using liquid chromatography-time of flight-mass spectrometry. In another example, five hydroxylated intermediates (Scheme 1a) were identified in the degradation of a pesticide, carbofuran [22]. The role of ·OH in the initiation of this photocatalytic degradation was confirmed by the knowledge of carbofuran adsorption on P25 catalyst and by conduction of the experiments using a non-aqueous solvent, acetonitrile. Carbofuran showed a negligible adsorption (~1%) on Degussa P25 TiO2 catalyst. The absence of adsorption eliminates the possibility of the direct oxidation of carbofuran by surface-generated holes [22], which is considered to be a minor secondary reaction in NTO photocatalytic degradation [25,26] on TiO2 catalysts under UV illumination. When this experiment was conducted in the non-aqueous solvent, acetonitrile, total inhibition of carbofuran degradation was observed [22], due to the low production of ·OH in acetonitrile. These findings show that the photocatalytic degradation of aqueous pollutants is initiated mainly by ·OH attack. However, An et al. reported [25] secondary mechanistic pathways for the photocatalytic degradation of the antivirus drug lamivudine by UV-irradiated NTO. These secondary pathways originated from photogenerated holes on NTO, which caused the initial oxidation of the lamivudine adsorbed on the NTO surface (Scheme 1b). It is important to note that these secondary degradation pathways initiated by photogenerated holes were minor side reactions; the major degradation pathway of lamivudine was through ·OH attack.
Table 1. Recent examples of pollutants photocatalytically degraded by NTO.
Table 1. Recent examples of pollutants photocatalytically degraded by NTO.
ContaminantPhotocatalytic systemRef.
Reactive violet 5UV/Anatase powder (Sigma Aldrich) [27]
Blue 9, Red 51& Yellow 23 Solar/TiO2 (Degussa P25)[28]
Methyl orangeUV/TiO2 on glass[29]
Methylene blueUV/TiO2 (Merck) on volcanic ash[30]
Rhodamine BUV/TiO2 bilayer[31]
Pesticides & herbicides
Organophosphate & PhosphonoglycineUV/TiO2 immobilized on silica gel[32]
AzimsulfuronUV/TiO2 coated on glass rings[33]
Swep residuesSimulated sunlight/TiO2 (Degussa P25)[34]
Pharmaceuticals & cosmeticsElectrocoagulation & UV/TiO2/H2O2[35]
UV/TiO2 (Aeroxide P25)[9,10,36]
TiO2/Fe3O4 & TiO2/SiO2/Fe3O4[37]
BenzylparabenUV/TiO2 (Degussa P25)[38]
Oxolinic acidUV/TiO2 (Degussa P25)[39]
Atenolol & propranololUV/Commercial TiO2s[40]
Solar/TiO2 (six commercial samples)/H2O2[41]
Ciprofloxacin, ofloxacin, norfloxacin & enrofloxacinUV/TiO2 (Degussa P25)[42]
Simulated solar/TiO2 P25[43]
LamivudineUV/TiO2 (Degussa P25)[25]
OxytetracyclineUV/TiO2 (Degussa P25)[44]
N,N-diethyl-m-toluamide (Insect repellent)UV/TiO2 (Degussa P25)[20,45]
15 emerging contaminantsSolar UV/TiO2 coated on glass spheres[47]
Grey waterUV/TiO2 (Aeroxide P25)[12]
Microcystins (Cyanotoxin)UV/TiO2 film[48,49]
UV/Doped TiO2[50]
UV/ Nitrogen doped TiO2[51]
Lipid vesicles & E. coli cells UV/TiO2 (Degussa P25)[52]
Bacterial colony UV/TiO2 on titanium beads[53]
UV/TiO2-coated bio-film [54]
Paper mill wastewaterSolar/TiO2[11]
Endocrine disrupting compoundsUV/TiO2 (Degussa P25)[55]
Municipal waste waterSolar/sol-gel TiO2 & Degussa P25[13]
Contaminated soilPlasma/TiO2 ((Degussa P25)[56]
Figure 2. Photocatalytic generation of hydroxyl radicals.
Figure 2. Photocatalytic generation of hydroxyl radicals.
Catalysts 02 00572 g002
Scheme 1. Photocatalytic degradation pathways of (a) carbofuran and (b) lamivudine (Reproduced from [22] and [25] respectively, copyright (2011), with permission from Elsevier).
Scheme 1. Photocatalytic degradation pathways of (a) carbofuran and (b) lamivudine (Reproduced from [22] and [25] respectively, copyright (2011), with permission from Elsevier).
Catalysts 02 00572 g008
The kinetics of the photocatalytic degradation of aqueous pollutants by NTO is still a subject of debate [57,58,59]. Several recent reports claim that it follows the Langmuir-Hinshelwood model (L-H model) of kinetics [21,22,25,26]. However, the validity of L-H model in photocatalytic degradation reactions could be a misconception or rather an easier way of interpretation [60]. Therefore reporting L-H model of kinetics in photocatalytic degradation without proper experimental evidences is dubious. The kinetic profile for the degradation of methylparaben, a bactericide and antimicrobial agent in personal care products, by NTO photocatalysis has been reported to follow the L-H model, where the rate expression can be shown as follows [26].
Catalysts 02 00572 i001
where r is the reaction rate, kLH is the apparent L-H rate constant, θ is the surface coverage of methylparaben, KL is the Langmuir adsorption constant, and Ceq is the equilibrium concentration. At low concentrations of methylparaben, KL Ceq (KLCeq << 1) is negligible and Equation (1) becomes a pseudo-first-order rate expression [26], as denoted below.
Catalysts 02 00572 i002
Integrating Equation (2)
Catalysts 02 00572 i003
Equations (1)–(3) account for the adsorption of the reactant (methylparaben) only but do not consider the adsorption on NTO of any intermediates or products formed during the course of the degradation reaction. When the adsorption of intermediates or products must be considered [21], a modified rate equation results, as shown below.
Catalysts 02 00572 i004
where Ki and Ci are the adsorption constant and concentration of intermediates at any given time, respectively. When the initial concentration of pollutants is very low, 1 + KL Ceq + Catalysts 02 00572 i005 is negligible and the reaction follows pseudo-first-order kinetics, as shown in Equations (2) and (3).
Sirtori et al. have reported that the photocatalytic degradation by NTO follows L-H kinetics at low pollutant concentrations and below the catalyst saturation level [21]. It deviates from the pseudo-first-order kinetics under several conditions. The NTO catalyst concentration and the light flux have been found to influence the degradation kinetics of methylparaben [26]. According to the L-H model, the photocatalytic degradation rate of methylparaben should increase with an increase in the NTO catalyst loading because of the additional available active sites (θ) for adsorption. This was observed up to a certain catalyst loading (catalyst saturation), but above that limit, the experimental kinetics results did not fit the L-H model [26]. This was mainly ascribed to three reasons: at higher NTO loading, (i) deactivation of activated NTO could occur upon collision with ground state NTO catalysts, (ii) there is a higher possibility of agglomeration and sedimentation of NTO, and (iii) there is decreased light penetration through the reaction medium. UV light flux has been found to be an important influence on the degradation kinetics of methylparaben in aqueous medium [26]. At low UV light flux (1.2 × 1015 photons s−1 cm−2 < Ф < 4.0 × 1015 photons s−1 cm−2), methylparaben degradation followed L-H kinetics, where electron-hole pairs mainly resulted in chemical reactions rather than recombination. However, at intermediate UV light intensities (4.0 × 1015 photons s−1 cm−2 < Ф < 5.8 × 1015 photons s−1 cm−2), the methylparaben degradation rate varied as a functional order between zero and one. In this medium UV light region, the recombination of electron-hole pairs was predominant over degradation. The random selection of a particular concentration of the pollutant is not enough to study the dependence of rate on photon flow [60]. Concentration of the pollutant is also important as demonstrated by Serpone et al. [60] where the order of the photocatalytic reaction varied between zero (at low pollutant concentration) and one (at high pollutant concentration) in the same range of light irradiance. Therefore a complete study should focus on different concentrations of pollutant to know the dependence of light irradiance on the photocatalytic reaction rate.
Wang et al. posited a rate expression that was different from the conventional pseudo-first-order rate equation, to explain the kinetics of sulfosalicylic acid degradation in aqueous solution using NTO [57]. Their proposed rate equation considers factors such as the lifetime and concentration of ·OH, pH, and adsorption of intermediates on NTO. The rate equation can be represented as follows.
Catalysts 02 00572 i006
Catalysts 02 00572 i007
where, τ is the lifetime of ·OH and k4 is the rate constant for the reaction of ·OH with the adsorbed pollutant on NTO. KQ and Ki are the adsorption equilibrium constants of sulfosalicylic acid and the intermediates, respectively, and Ceq and Ci are their equilibrium concentrations. Adsorption of the identified intermediates of sulfosalicylic acid degradation on NTO was found to be insignificant [57]; hence, Equation (5) can be simplified as
Catalysts 02 00572 i008
Integrating Equation (7), we get
Catalysts 02 00572 i009
Catalysts 02 00572 i010
The order of the degradation reaction will then be determined by three different adsorption situations: (i) weak adsorption (KQ Ceq<< 1); (ii) medium adsorption (0.1< KQ Ceq < 10), and (iii) strong adsorption (KQ Ceq > 10) [57]. In the case of weak adsorption of the pollutant on NTO, Equation (8) reduces to the pseudo-first-order expression, as shown in Equation (3). Medium adsorption leads to Equation (8), which was observed in the case of sulfosalicylic acid degradation kinetics. In the case of strong adsorption, the rate is independent of KQ and adsorption does not affect the rate of the reaction; here, the reaction will follow a zero-order kinetic model and the rate expression becomes
Catalysts 02 00572 i011
Pace of photocatalytic degradation of a particular pollutant also depends on other factors such as alkalinity, and the presence of natural organic matter, [61] especially in real systems. Carbonate and bicarbonate ions, which are responsible for the alkalinity of water, have been found to decrease the rate of the photocatalytic degradation of microcystine-LR [61]. Also, the presence of humic acid and fulvic acid (natural organic matter) reduced the rate of microcystine-LR degradation [61].

3. Activity Enhancement

Recent efforts to enhance the photocatalytic activity of NTO include the synthesis of mesoporous TiO2 [62,63,64,65,66,67,68,69,70,71,72], the use of different TiO2 morphologies (nanowires, nanotubes, and nanospheres) [73,74,75,76], reducing the agglomeration in NTO powders [77,78,79], and surface treatments of NTO [80,81,82,83]. Synthesis of mesoporous NTO is a means to achieve TiO2 photocatalysts with improved photocatalytic activities. Some of the recently reported mesoporous TiO2 photocatalysts exhibited superior photocatalytic activity than the bench mark Degussa P25 TiO2 photocatalyst. TiO2 photocatalysts with active {001} facets were derived hydrothermally by using ammonium fluoride [62] or mild sulfuric acid [63] capping agents and showed superior dye degradation activity in comparison with the Degussa P25. Mesoporous TiO2 catalysts synthesized by using F127 triblock copolymer [64], polystyrene [65], and silica [66] (through etching and recalcination method) have been reported for the efficient degradation of methanol, methyl orange and rhodamine B pollutants, respectively. These synthesized mesoporous catalysts outperformed the commercially available Degussa P25 and Hombicat UV-100 [64] photocatalyts in their photocatalytic activity.
NTO nanowires obtained by the post-calcination of hydrothermally derived titanates were found to be more efficient than Degussa P25 in the degradation of humic acid [73] and Reactive Brilliant Blue X-BR [75]. These nanowires also caused less serious fouling than P25 in microfiltration membranes. In another study [74], NTO nanotubes obtained by the anodic oxidation of titanium metal plate were 25–40% more efficient than the nanoparticle-based experimental system for the degradation of rhodamine B. Anatase submicrospheres consisting of NTO nanorods (20–30 nm in diameter) with thorn-like shells have been reported [76]. This morphology resulted in multiple reflections of the incident light, and the catalyst was found to be equally comparable with P25 in the degradation of methylene blue dye solution under UV irradiation.
The agglomeration of NTO during its formation can reduce the dispersion of TiO2 in aqueous suspensions, contributing to decreased photocatalytic activity. The agglomeration of TiO2 can be minimized by changing the pH of the reaction mixture [78], adsorbing polyallylamine hydrochloride on the TiO2 surface [78], adopting a flame hydrolysis synthesis route [79], or ball milling of the TiO2 powder [77]. All attempts were successful in reducing the agglomeration of NTO in aqueous suspensions, but the photocatalytic activities were found to depend not only on agglomeration but also on several other factors. Recently reported surface treatments include surface fluorination [81], high-energy electron beam treatment [82], modification with S-1-dodecyl-S'-(α,α'-dimethyl-α''-acetic acid) trithiocarbonate (DDAT) [83], and incorporation of a TiO2 microsphere layer [80]. During the photooxidation of catechol and phenol, an electrochemical surface-fluorinated NTO electrode could reduce electron-hole recombination and also displace the oxidizable organic compounds and poisoning species from the surface [81]. This resulted in the superior performance of the fluorinated TiO2 versus the bare TiO2 electrode. In the high-energy electron beam treatment of NTO, the carbon content on the TiO2 surface was increased by the burning of impurities already present on the catalyst [82]. This increased the hydrophilicity and the photocatalytic activity of the electron beam-treated TiO2 in the degradation of methylene blue dye. Modifying NTO with DDAT caused a red shift in the absorbance of the modified catalyst through a ligand-to-metal charge transfer transition, which enhanced its visible light activity towards the degradation of 2,4-dichlorophenol, when compared to the as-prepared TiO2 catalyst [83]. The formation of a TiO2 microsphere layer over a nanostructured TiO2 layer (deposited on Pyrex glass by spin coating) increased the contact area for methylene blue dye in aqueous solution, resulting in faster degradation kinetics [80].

4. Immobilization of TiO2

Immobilization of TiO2 on various substrates is an important research area with its photocatalytic water treatment applications [84]. The primary aim of doing so is to avoid the post separation difficulties associated with the powder form of the TiO2 catalyst. However, there are several other advantages including higher surface area, superior adsorption properties [30,85,86], and increased surface hydroxyl groups or reduced charge recombination [87] are achievable in immobilized systems. Immobilization of TiO2 can be done on powder/pellet substrates [30,85,86], soft/thin materials [54,88,89,90,91,92,93] or on rigid/thick substrates. Some of the recent examples of powder/pellet substrates include activated carbon [85], vermiculite (magnesium-aluminium silicates) [86], and volcanic ash [30]. Sedimentation of these TiO2 immobilized systems could be easier than the TiO2 catalyst alone systems, since they are heavier particles. TiO2 immobilized on soft/thin substrates, normally referred as TiO2 membrane or films, are applicable in ultra filtration and bacterial inactivation. Since they are immobilized with TiO2, they can act as self cleaning surfaces. Recent examples of this category include TiO2 immobilized on alumina (1.5 micron thick) [88,89,90], polyvinylidene difluoride [91], glass filter [92], cellulose fibres [93], and sponge [54]. Various immobilization techniques such as chemical vapour deposition [89,90], slip coating [88], dip coating [88], film casting [91], electrospinning [92,93] and dip-evaporation [54] has been employed to achieve the immobilization of TiO2 on soft/thin substrates.
Immobilization of TiO2 on rigid substrates is mostly done on glass [31,33,87,94,95,96,97,98]. Main advantage with glass substrate is the transparency of the system even after the immobilization. This can allow the penetration of light which can result in improved photocatalysis. Dionysiou et al. [94] have reported a non-ionic surfactant (Tween20) templated self assembly pathway to immobilize TiO2 on borosilicate glass by the dip coating technique. The use of surfactant resulted in a uniform and crack free TiO2 surface with partially ordered mesoporosity to the calcined borosilicate glass TiO2 films. Addition of Degussa P25 to the surfactant containing TiO2 sol imparted a bimodal mesoporous structure to the catalyst immobilized system which improved the structural integrity of the films [95]. The use of a non-ionic fluoro surfactant (Zonyl FS-300) instead of Tween 20, and the addition of ethylene diamine into the TiO2 sol for dip coating; nitrogen and fluorine co-doped visible light active TiO2 coating on borosilicate glass was achieved (after calcination) [96]. Interestingly, the surface was found to be hydrophilic under both UV and visible (400-510 nm) light exposure while the undoped TiO2 surface was hydrophilic only under UV light [97]. They could also achieve sulfur doped visible light active (after calcination) TiO2 coating by adding sulfuric acid (sulfur precursor) and polyoxyethylene (80) sorbitan monooleate surfactant (as pore directing agent) into the TiO2 sol [98]. All these TiO2 immobilized borosilicate glass systems were successfully tested for the photocatalytic degradation of creatinine [94,95], microcystines [96,98,99,100], and cylindrospermopsin [100] under UV/visible light irradiation.
The role of surface defects in the TiO2 surface on the photocatalytic degradation mechanism is demonstrated by Zhuang et al [31]. They produced three TiO2 immobilized systems (with normal surface, surface defects and with interface defects) on quartz by either using dip coating techniques alone or using both dip coating and cold plasma treatment techniques. The normal TiO2 surface mainly promoted N-deethylation of rhodamine B (Rh B) dye while the TiO2 surface with defects was very efficient for cycloreversion of RhB. The TiO2 surface with interface defects showed both mechanisms and was found to be the best system for the Rh B dye degradation.

5. Photocatalytic Reactors

Reactor design is an intense focus for photocatalytic water treatment. Here, reviewed photocatalytic reactors can be divided in to two categories, i.e., (i) lab-scale reactors [74,101,102,103,104,105,106,107,108,109,110,111], where the volume of reactant solution is <1 L, and (ii) pilot plant-scale reactors [44,112,113,114,115,116], where the reactor volume is >5 L. Recent innovations in lab-scale reactors include the use of energy-efficient UV/visible light emitting diodes (LEDs) as light sources [101,102,103,104,105], the design of rotating disc-type reactor models [74,106], the fabrication of NTO-immobilized catalytic beds [107,108], and post-separation/reuse of NTO powder catalysts [109,110,111]. LEDs are light sources that need less energy and, therefore, LED-based photocatalytic reactors are more energy-efficient systems. The combination of UV-LEDs and NTO powder [101], NTO nanotubes [102], or immobilized NTO [103,104] has been reported for the degradation of various dyes such as methyl orange, methylene blue, rhodamine B, and malachite green. The UV-LED photoreactor developed by Nickels et al. [104] was equipped with a microcirculating fluid pump (to keep the reactant solution constantly mixed) and an in-stream sensor unit (Figure 3). The sensor unit, an assembly of a liquid flow cell with transparent windows, an LED lamp, and a photodiode monitor, enabled the real-time evaluation of the decrease in the concentration of methyl orange dye. Other attributes of the reactor, such as its light weight, low production cost, and flexibility, make this design ideal for both laboratory and field work applications, as claimed by the authors. Visible LEDs with carbon-nitrogen co-doped NTO achieved the visible light degradation of bisphenol [105]. The reactor consisted of four strips of visible LEDs, i.e., white, green, blue, and yellow, which covered the wavelength range of 450 to 600 nm.
Rotating disc reactor design in NTO photocatalysis has several merits as first demonstrated by Dionysiou et al. [117,118]. A NTO-coated borosilicate rotating disc (diameter = 6 cm) was reported for the degradation of methyl orange dye [106]. The aqueous methyl orange solution film thickness on the disc was optimized by adjusting the flow rate of the reactant feed and the rotating speed of the disc. Zhang et al. designed a rotating disc reactor of TiO2 nanotubes by the anodization of a Ti metal plate [74]. Half of the disc was always immersed in the bulk solution of the reactant rhodamine B dye, whereas the other half was exposed to air. They observed a faster degradation rate for rhodamine B dye on the air-exposed disc surface than in the bulk of the solution. This TiO2 nanotube disc reactor was 20–25% more efficient than the TiO2 nanoparticle-coated disc system.
Figure 3. Schematic of the UV-LED-based photocatalytic reactor equipped with a real time in-stream sensor unit (Adapted with permission from [104]. Copyright (2012) American Chemical Society).
Figure 3. Schematic of the UV-LED-based photocatalytic reactor equipped with a real time in-stream sensor unit (Adapted with permission from [104]. Copyright (2012) American Chemical Society).
Catalysts 02 00572 g003
Recently reported immobilized catalytic bed designs include a NTO-coated pebble bed photocatalytic reactor [107] and an ETS-10 (Engelhard titanosilicate structure 10)-coated optic fiber reactor [108]. The former consisted of a Perplex TM sheet onto which NTO-coated pebbles were affixed [107]. The arrangement of the pebbles was such that the pebbles in one row formed an equilateral triangle with the pebbles in the next row. Keeping the reactor in a horizontal position, textile dye solution (0.66 L) was degraded under sunlight irradiation. In the other example, the ETS-10-coated optic fiber reactor showed 4–5 times greater quantum efficiency than an ETS-10 slurry reactor in degrading methylene blue dye solution under UV light illumination [108]. The reactor consisted of optical fibers, uniformly coated with ETS-10, inserted in an acrylic cylinder.
Post separation of NTO powder catalysts in slurry reactors is one of the major challenges in photocatalytic water treatment. Toward this end, Kim et al. [109] reported a reactor design in which the P25 powder catalyst could be separated from the treated water by a submerged microfiltration membrane. They used this reactor system in conjunction with reverse osmosis for the photocatalytic treatment of seawater samples. In another reactor design, Suryaman et al. [110] achieved the natural sedimentation of the P25 powder catalyst after phenol degradation in pipe water. Treated water overflowed from the separation tank, whereas the P25 catalyst settled at the bottom of the separation tank. The use of NTO pellets is another option to avoid post separation requirements in photocatalytic reactors. With a patented “drum reactor” design [111], McCullagh et al. reported the degradation of methylene blue dye solution by Hombikat TiO2 pellets. The reactor had three cylinders with paddles, which contained TiO2 pellets. Each cylinder was supplied with 36 W UV lamps and was connected to a 12 V motor to effect cylinder rotation.
Recently reported pilot plant photocatalytic reactors have mainly utilized natural sunlight as a light source [44,112,113,115,116]. However, an UV light-based pilot plant reactor has also been reported [114]. The use of NTO in powder [44,112,114,116] or immobilized forms [113,115] has also been examined. Table 2 depicts some recent examples of pilot plant photocatalytic reactors used for the degradation of various contaminants.
Table 2. Examples of large-scale photocatalytic reactors.
Table 2. Examples of large-scale photocatalytic reactors.
Reactor typeExperimental conditionVolume (L)pollutantRef.
Compound parabolic collector pilot-plant0.2 g L−1/solar22 & 110Cork boiling and bleaching waste water[112]
Concentric parabolic concentrator pilot-plantTiO2 coated paper (20 g m−2)/solar16.2Humic substances[113]
Membrane pilot system0.05 g L−1/UV-32 pharmaceuticals[114]
Thin film fixed-bed reactorTiO on the reactor walls/solar-Yellow Cibacron FN-2R [115]
Tubular continuous flow pilot-plant0.1 g L−1/solar7p-nitrophenol, naphthalene, dibenzothiophene[116]
Compound parabolic collector pilot-plant0.5 g L−1/solar6Oxytetracyclin[44]

6. Doping

The band gaps (3–3.2 eV) of NTO semiconductors, which absorb from the UV region of the solar spectrum, are drawbacks in photocatalysis; only about 5% of sunlight comprises UV radiation. Modification of the band gap in NTO is, therefore, a well-studied research area. Modifications can be effected either in bulk or on the surface of TiO2 (Scheme 2). Surface modifications are usually achieved by anchoring colored inorganic semiconductors (for example, CdS and CdSe) [119] or organic dyes on the TiO2 surface [120], where they act as sensitizers. However, most of these sensitizers are susceptible to photocorrosion or degradation in aqueous solutions and are not suitable for photocatalytic water-treatment applications. Instead, they are good candidates for solar cell devices. On the other hand, bulk modification is mainly effected by doping metals or non-metals into bulk NTO. The modified catalysts appear to be photo-stable in aqueous solution and can be used in photocatalytic water purification.
Scheme 2. Different methods of modificationon NTO.
Scheme 2. Different methods of modificationon NTO.
Catalysts 02 00572 g009
Figure 4. Creation of additional bands inNTO by doping.
Figure 4. Creation of additional bands inNTO by doping.
Catalysts 02 00572 g004
Doping NTO with metals and non-metals creates new energy levels between the VB and CB of TiO2 [121], which in turn reduces its band gap and helps the doped catalyst to absorb in the visible region (Figure 4). Recently, researchers have reported the successful doping of vanadium [122], iron [123], rhodium [50], palladium [124], and silver [125] metals, and carbon [105,126], nitrogen [51,96,105,121,124,127,128], sulfur [98,129], fluorine [96], and iodine [130] non-metals in NTO to achieve the visible light photocatalytic degradation of various chemicals and Escherichia coli in aqueous solution (Table 3). In all reports, except in silver doping, the visible light photocatalytic activity was mainly attributed to the associated red shift that originated from the creation of local bands between the VB and CB of NTO (Figure 4). Silver doping in P25 by a photoreduction method did not reduce the band gap of the doped catalyst, but superior photocatalytic degradation of oxalic acid was still observed, when compared to un-doped P25, under artificial sunlight [125]. This was explained by the formation of silver oxalate, which absorbed from the visible region and was subsequently degraded.
Not all doping in NTO will exhibit positive effects, as reported in the cases of rhodium, carbon, and platinum doping. Rhodium doping afforded the highest activity for microcystin-LR degradation under visible light, followed by the carbon-doped catalyst [50]. In contrast, the platinum-doped NTO catalyst did not exhibit efficient visible light degradation because of the interference from chloride radicals generated by the homolytic cleavage of the platinum–chlorine bond in the platinum precursor. The synthetic route for the doped NTO catalyst also influences its activity. For example, hydrothermally derived vanadium-doped TiO2 showed higher activity than its sol-gel-derived counterpart in the degradation of an aqueous solution of isobutanol [122]. The addition of ammonium fluoride during hydrothermal treatment caused further enhancement in the activity of doped catalyst. The higher crystallinity resulting from the hydrothermal treatment and the hydrophobic surface formation by ammonium fluoride were responsible for these observations [122]. Heat treatment has a great influence in the characteristics and activity of doped NTO catalysts, especially in the case of nitrogen doping. Gohin et al. [128] observed a color change of anatase nanoparticles from slight yellow (at 500 °C) to darkish green (above 650 °C) at different nitridation temperatures using urea as a nitrogen source. The yellow color at 500 °C resulted from the formation of localized N 2p states above the VB of TiO2. However, the darkish green color change, observed above 650 °C, was due to the reduction of Ti4+ in anatase to Ti3+ by ammonia (from the decomposition of the urea precursor). These Ti3+ species were found to have detrimental effects on photocatalytic activity because they can act as recombination centers. The sample nitridated at 500 °C exhibited superior photocatalytic activity under visible light irradiation. However, whether Ti3+ in doped NTO can reduce [130] or increase [98,128] the electron-hole pair recombination is still open to debate. The selection of pollutants is very important in visible light-induced photocatalytic degradation using doped NTO catalysts [125,129]. For example, when 4-methoxyresorcinol, quinoline, and 1-(p-anisyl)neopentanol were subjected to visible light photocatalytic degradation with sulfur-doped TiO2 (sol-gel method), only 4-methoxyresorcinol (at pH = 8.5) was destroyed [129]. The reason was the formation of a charge transfer complex (which absorbed the visible light) between 4-methoxyresorcinol and the catalyst, whereas quinoline and 1-(p-anisyl)neopentanol cannot form such charge transfer complexes. This limits the use of the abovementioned sulfur-doped TiO2 catalyst in the degradation of compounds that cannot form charge transfer complexes. Other factors that influence the activity of the doped NTO catalyst include dopant concentration [124,126], the crystal phase of the NTO [127], and the intensity of light irradiance [105]. Doped NTO photocatalysts have also been reported for their photocatalytic activity with UV light irradiation in pollutant degradation [131,132], nitrate reduction, and in bacterial disinfection [133,134].
Even though doped NTO catalysts can operate in the visible region, several issues must be considered before their wide use in photocatalytic water treatment. The visible light photocatalytic activity in most of the bulk modified NTO is far lower than the activity of unmodified catalyst under UV irradiation [50,122,129]. In addition, NTO catalysts modified by metal/non-metal doping sometimes have poor activity under UV irradiation [50,122,129]. Here, the doped species could act as recombination centers. Leaching of the doped species is another problem [129], which is a serious concern, especially when the dopants are toxic metals. Furthermore, doping is never a guarantee of high photoreactivity in the doped NTO catalyst, since reactivity is a complex function of dopant concentration, distribution, energy levels in the TiO2 lattice, d-electron configuration, and light intensity [135]. The choice of doped TiO2 as a photocatalyst versus un-doped TiO2 only depends on whether the requirement of low efficiency visible light activity outweighs the higher performance of photocatalysis under UV light [129]. Sometimes, even the smaller fraction of UV radiation in solar light can degrade selected pollutants effectively with unmodified NTO (Figure 5) [45].

7. Coupling with Other Treatment Technologies

Combining NTO photocatalysis with other oxidation techniques was found to be very effective in pollutant destruction. These technologies include electrocatalysis [35,136,137,138], sonocatalysis/Fenton process [139], biodegradation [140,141,142,143,144], and wetland technology [145]. The combination of NTO photocatalysis with any of these techniques can not only improve the total efficiency of the degradation but also has the advantage of treating large quantities of wastewater (in real systems), especially with electrocatalysis, biodegradation, and wetland technology. Electrocoagulation (using an iron cathode/anode (12.50 cm × 2.50 cm × 0.10 cm) at a current density of 763 Am−2 for 90 min) of an effluent from pharmaceutical and cosmetic companies removed the majority of the suspended particles, followed by further purification using NTO photocatalysis [35].
Table 3. Recent examples of metal- and non-metal-doped NTO photocatalysis.
Table 3. Recent examples of metal- and non-metal-doped NTO photocatalysis.
Doped catalystSynthesis routePollutantRef.
Vanadium/TiO2 (λ > 430 nm)sol-gel and hydrothermalisobutanol[122]
Iron/TiO2 (λ > 420 nm)co-thermal hydrolysismethyl orange[123]
Rhodium/TiO2 (visible light)impregnationmicrocystin-LR[50]
artificial solar lightphotoreduction oxalic acid[125]
solar irradiationelectrospinningE. coli[92]
Sulfur/ TiO2 (495 nm filter)sol-gel4-methoxyresorcinol, quinoline &1-(p anisyl) neopentanol[129]
(λ > 420 nm)sol-gel, self-assemblymicrocystin-LR[98]
Nitrogen/P25 (λ > 420 nm)millingrhodamine B[127]
(λ = 390 & 470 nm)sol-gel rhodamine 6G [128]
Solar and visible lightsol-gelmicrocystin-LR[51]
Carbon/TiO2 (Artificial solar light)high pressure heatingmethylene blue[126]
Iodine/TiO2 (spectrum close to sunlight)hydrothermalphenol[130]
Nitrogen-Palladium co-doped TiO2 (visiblelight)sol-geleosin yellow [124]
Carbon-nitrogen co-doped TiO2 (λ = 465, 523 & 589 nm)solvothermalbisphenol A[105]
Fluorine-nitrogen co-doped TiO2 (λ > 420 nm)sol-gelmicrocystin-LR[96]
The effluent had an initial chemical oxygen demand (COD) value of 1753 mg L−1, which was reduced to 160 mg L−1 and 50 mg L−1 after electrocoagulation and electrocoagulation/photocatalysis, respectively. Here, the electrocoagulation pre-treatment removed the suspended particles, and thus, the turbidity in the effluent. Thereby, the working load of the TiO2 catalyst was reduced and the transparency of the medium was increased, such that UV radiation could pass through easily. In an another study, the synergic effect of TiO2 photocatalysis and boron-doped diamond (BDD) anodic oxidation improved the total organic carbon (TOC) reduction in the degradation of X-3B dye in an experimental set up, as shown in Figure 6a [136]. Figure 6b represents the efficiency (as a function of time) of different reaction systems employed in the decolorization of X-3B dye, in which the systems using TiO2 photocatalysis and BDD anodic oxidation showed the highest activities. The removal of bromate by reduction to bromide [137] and the degradation of chlortetracycline [138] in high efficiencies were also achieved by photoelectrocatalysis using Ti/TiO2 as the photocathode and photoanode, respectively. Another example for the synergic effect of different AOPs is the combined ultrasound-, Fenton-, and TiO2-photoassisted mineralization of bisphenol A [139]. By this combined approach, 93% dissolved organic carbon (DOC) removal was achieved, whereas DOC removals by the individual processes were 5, 6, and 22% for TiO2 photocatalysis, ultrasound, and photo-Fenton, respectively [139]. Here, ultrasound eliminated the initial substrate and provided H2O2 for the photocatalytic reactions. TiO2 photocatalysis and photo- Fenton treatments were mainly responsible for the total mineralization of the intermediates generated by the ultrasound technique.
Figure 5. Photocatalytic degradation of microcystin-LR under (a) solar light irradiation and (b) visible light (440–460 nm), in the presence of commercial (P25 and Kronos), reference (Ref-TiO2), and nitrogen-doped (N-TiO2) TiO2 materials. (Reprinted from [51]. Copyright (2012), with permission from Elsevier).
Figure 5. Photocatalytic degradation of microcystin-LR under (a) solar light irradiation and (b) visible light (440–460 nm), in the presence of commercial (P25 and Kronos), reference (Ref-TiO2), and nitrogen-doped (N-TiO2) TiO2 materials. (Reprinted from [51]. Copyright (2012), with permission from Elsevier).
Catalysts 02 00572 g005
Biological oxidation is one of the oldest techniques for water treatment. The combination of biological oxidation followed by NTO photocatalysis was employed (Figure 7a) for the mineralization of a mixture containing 2-chlorophenol, 2,4-dichlorophenol, 2,4,5-trichlorophenol, and pentachlorophenol in tap water (total concentration was 100 mg L−1, each component was 25 mg L−1) [140]. The order of the treatments was very important, as the combined biological–photocatalytic treatment removed chlorophenols at a rate of 25.8 mg h−1, whereas, for the combined photocatalytic–biological treatment, the removal rate was only 10.5 mg h−1. Similar observations were reported for the degradation of dyes [141], cyproconazole [142], and a tetracycline/tylosin mixture [143], in which the TiO2 photocatalytic pre-treatment eradicated the activity of biological oxidation. In this case, some of the intermediates generated during photocatalysis were not biodegradable. In contrast to the above observations, Chen et al. reported the feasibility of using NTO photocatalysis as a pre-treatment followed by the use of a constructed wetland [145]. In their experiment (Figure 7b), they initially treated domestic and agricultural wastewaters (COD was 36.2 ± 7.4) by TiO2 (coated on α-alumina) photocatalysis before transfer to a bench-scale wetland system. With a hydraulic retention time of 2 days, they reduced the levels of halomethanes and haloacetic acids below the maximum allowed contamination thresholds for drinking water. The intermediates generated by the photocatalytic treatment were biodegradable, which made the wetland treatment fruitful. However, they did not attempt the wetland pre-treatment followed by NTO photocatalysis. From these contrasting observations, we think that the order of treatment is crucial, and varies according to the nature of the contaminants.
Figure 6. (a) Schematic of the anodic oxidation- and photocatalysis-coupled reactor and (b) comparison of degradation performance in different experimental systems [136].
Figure 6. (a) Schematic of the anodic oxidation- and photocatalysis-coupled reactor and (b) comparison of degradation performance in different experimental systems [136].
Catalysts 02 00572 g006
Figure 7. Schematic of the coupling of (a) biological [140] and (b) wetland treatment technologies [145] with photocatalysis.
Figure 7. Schematic of the coupling of (a) biological [140] and (b) wetland treatment technologies [145] with photocatalysis.
Catalysts 02 00572 g007

8. Conclusions and Future Prospects

Photocatalytic water treatment by NTO is a hot topic of environmental research and a versatile technique for pollutant degradation. Having a long history of active investigation since the 1970s, photocatalytic water treatment by NTO still retains its importance in contemporary research. This is because of the unique properties of TiO2, its ability to completely mineralize a wide spectrum of pollutants, its cheap operating costs, and simple experimental design. By reviewing recent developments in this area, the authors have arrived at the following conclusions.
  • A large number of individual compounds have been successfully tested for photocatalytic degradation by NTO, and researchers are now more focused on real systems, which is promising for the commercialization of the technology. Selective photocatalysis by NTO is a potential research area where researchers can find several opportunities.
  • Photocatalytic degradation of pollutants by NTO is mainly triggered by ·OH radicals, along with the direct oxidation of adsorbed pollutants by surface-generated holes; however, the latter is a minor secondary degradation pathway. The kinetics of photocatalytic degradation by NTO was found to depend on catalyst loading, the extent of adsorption, and light intensity. However, several reports claim that it follows L-H reaction kinetics, especially below catalyst saturation. This is an area where more studies must be conducted in order to clarify the ambiguities in photocatalytic degradation kinetics.
  • Different NTO morphologies have been synthesized and found to be effective for the photocatalytic degradation of various compounds. Surface treatment of NTO is another option for increasing catalytic activity.
  • The design of photocatalytic reactors is a key area where intense research is in progress. An ideal photocatalytic reactor should be simple, energy efficient, less expensive to build and operate, and able to handle high wastewater volumes. Reactors operating with solar radiation or LEDs and reactor designs that do not require post separation of the catalyst hold great promise.
  • Doping NTO with metals and non-metals was investigated to achieve absorption from the visible region by reducing the band gap of the doped catalyst. However, the practicability of applying doped NTO catalysts in photocatalytic water treatment needs reconsideration because of the low catalytic activity of the doped NTO catalysts under visible light and because of the possibility of dopant leaching.
  • NTO photocatalysis in conjunction with other treatment technologies was explored by several groups. Coupling NTO photocatalysis with other technologies has great potential in large-scale water treatment, and further research is necessary.


This work was financially supported by Monash Research Graduate School (MRGS) and the Gippsland Campus, Monash. Manoj A. Lazar is grateful to Lane McDonald for the proof reading of the revisions.


  1. Verhoeven, J.W. Glossary of terms used in photochemistry. Pure Appl. Chem. 1996, 68, 2223–2286. [Google Scholar] [CrossRef]
  2. Pelaez, M.; Nolan, N.T.; Pillai, S.C.; Seery, M.K.; Falaras, P.; Kontos, A.G.; Dunlop, P.S.M.; Hamilton, J.W.J.; Byrne, J.A.; O’Shea, K.; et al. A review on the visible light active titanium dioxide photocatalysts for environmental applications. Appl. Catal. B 2012, 125, 331–349. [Google Scholar] [CrossRef]
  3. Khin, M.M.; Nair, A.S.; Babu, V.J.; Murugan, R.; Ramakrishna, S. A review on nanomaterials for environmental remediation. Energy Environ. Sci. 2012, 5, 8075–8109. [Google Scholar]
  4. Malato, S.; Fernandez-Ibanez, P.; Maldonado, M.I.; Blanco, J.; Gernjak, W. Decontamination and disinfection of water by solar photocatalysis: Recent overview and trends. Catal. Today 2009, 147, 1–59. [Google Scholar] [CrossRef]
  5. Chong, M.N.; Jin, B.; Chow, C.W.K.; Saint, C. Recent developments in photocatalytic water treatment technology: A review. Water Res. 2010, 44, 2997–3027. [Google Scholar] [CrossRef]
  6. Mills, A.; LeHunte, S. An overview of semiconductor photocatalysis. J. Photochem. Photobiol. A 1997, 108, 1–35. [Google Scholar]
  7. Lofrano, G.; Rizzo, L.; Grassi, M.; Belgiorno, V. Advanced oxidation of catechol: A comparison among photocatalysis, fenton and photo-fenton processes. Desalination 2009, 249, 878–883. [Google Scholar] [CrossRef]
  8. Vilar, V.J.P.; Pinho, L.X.; Pintor, A.M.A.; Boaventura, R.A.R. Treatment of textile wastewaters by solar-driven advanced oxidation processes. Sol. Energy 2011, 85, 1927–1934. [Google Scholar] [CrossRef]
  9. Rizzo, L.; Meric, S.; Guida, M.; Kassinos, D.; Belgiorno, V. Heterogenous photocatalytic degradation kinetics and detoxification of an urban wastewater treatment plant effluent contaminated with pharmaceuticals. Water Res. 2009, 43, 4070–4078. [Google Scholar]
  10. Radjenovic, J.; Sirtori, C.; Petrovic, M.; Barcelo, D.; Malato, S. Solar photocatalytic degradation of persistent pharmaceuticals at pilot-scale: Kinetics and characterization of major intermediate products. Appl. Catal. B 2009, 89, 255–264. [Google Scholar] [CrossRef]
  11. Ghaly, M.Y.; Jamil, T.S.; El-Seesy, I.E.; Souaya, E.R.; Nasr, R.A. Treatment of highly polluted paper mill wastewater by solar photocatalytic oxidation with synthesized nano TiO2. Chem. Eng. J. 2011, 168, 446–454. [Google Scholar] [CrossRef]
  12. Sanchez, M.; Rivero, M.J.; Ortiz, I. Photocatalytic oxidation of grey water over titanium dioxide suspensions. Desalination 2010, 262, 141–146. [Google Scholar] [CrossRef]
  13. Miranda-Garcia, N.; Suarez, S.; Sanchez, B.; Coronado, J.M.; Malato, S.; Maldonado, M.I. Photocatalytic degradation of emerging contaminants in municipal wastewater treatment plant effluents using immobilized TiO2 in a solar pilot plant. Appl. Catal. B 2011, 103, 294–301. [Google Scholar]
  14. Saravanan, P.; Pakshirajan, K.; Saha, P. Degradation of phenol by TiO2-based heterogeneous photocatalysts in presence of sunlight. J. Hydro-Environ. Res. 2009, 3, 45–50. [Google Scholar] [CrossRef]
  15. Poblete, R.; Otal, E.; Vilches, L.F.; Vale, J.; Fernandez-Pereira, C. Photocatalytic degradation of humic acids and landfill leachate using a solid industrial by-product containing TiO2 and Fe. Appl. Catal. B 2011, 102, 172–179. [Google Scholar] [CrossRef]
  16. Kim, J.; Choi, W. Hydrogen producing water treatment through solar photocatalysis. Energy Environ. Sci. 2010, 3, 1042–1045. [Google Scholar]
  17. Sharabi, D.; Paz, Y. Preferential photodegradation of contaminants by molecular imprinting on titanium dioxide. Appl. Catal. B 2010, 95, 169–178. [Google Scholar] [CrossRef]
  18. Zhang, G.; Choi, W.; Kim, S.H.; Hong, S.B. Selective photocatalytic degradation of aquatic pollutants by titania encapsulated into FAU-type zeolites. J. Hazard. Mater. 2011, 188, 198–205. [Google Scholar] [CrossRef]
  19. Lazar, M.A.; Daoud, W.A. Selective adsorption and photocatalysis of low-temperature base-modified anatase nanocrystals. RSC Adv. 2012, 2, 447–452. [Google Scholar]
  20. Medana, C.; Calza, P.; Dal Bello, F.; Raso, E.; Minero, C.; Baiocchi, C. Multiple unknown degradants generated from the insect repellent deet by photoinduced processes on TiO2. J. Mass Spectrom. 2011, 46, 24–40. [Google Scholar] [CrossRef]
  21. Sirtori, C.; Zapata, A.; Malato, S.; Gernjak, W.; Fernandez-Alba, A.R.; Aguera, A. Solar photocatalytic treatment of quinolones: Intermediates and toxicity evaluation. Photochem. Photobiol. Sci. 2009, 8, 644–651. [Google Scholar] [CrossRef]
  22. Lopez-Alvarez, B.; Torres-Palma, R.A.; Penuela, G. Solar photocatalitycal treatment of carbofuran at lab and pilot scale: Effect of classical parameters, evaluation of the toxicity and analysis of organic by-products. J. Hazard. Mater. 2011, 191, 196–203. [Google Scholar]
  23. Lu, C.-S.; Chen, C.-C.; Mai, F.-D.; Li, H.-K. Identification of the degradation pathways of alkanolamines with TiO2 photocatalysis. J. Hazard. Mater. 2009, 165, 306–316. [Google Scholar] [CrossRef]
  24. Stapleton, D.R.; Konstantinou, I.K.; Mantzavinos, D.; Hela, D.; Papadaki, M. On the kinetics and mechanisms of photolytic/TiO2-photocatalytic degradation of substituted pyridines in aqueous solutions. Appl. Catal. B 2010, 95, 100–109. [Google Scholar] [CrossRef]
  25. An, T.C.; An, J.B.; Yang, H.; Li, G.Y.; Feng, H.X.; Nie, X.P. Photocatalytic degradation kinetics and mechanism of antivirus drug-lamivudine in TiO2 dispersion. J. Hazard. Mater. 2011, 197, 229–236. [Google Scholar]
  26. Lin, Y.; Ferronato, C.; Deng, N.; Wu, F.; Chovelon, J.-M. Photocatalytic degradation of methylparaben by TiO2: Multivariable experimental design and mechanism. Appl. Catal. B 2009, 88, 32–41. [Google Scholar] [CrossRef]
  27. Chung, Y.-C.; Chen, C.-Y. Degradation of azo dye reactive violet 5 by TiO2 photocatalysis. Environ. Chem. Lett. 2009, 7, 347–352. [Google Scholar] [CrossRef]
  28. Dias, M.G.; Azevedo, E.B. Photocatalytic decolorization of commercial acid dyes using solar irradiation. Water Air Soil Pollut. 2009, 204, 79–87. [Google Scholar] [CrossRef]
  29. Lopez, L.; Daoud, W.A.; Dutta, D. Preparation of large scale photocatalytic TiO2 films by the sol-gel process. Surf. Coat. Technol. 2010, 205, 251–257. [Google Scholar]
  30. Esparza, P.; Borges, M.E.; Diaz, L.; Alvarez-Galvan, M.C.; Fierro, J.L.G. Photodegradation of dye pollutants using new nanostructured titania supported on volcanic ashes. Appl. Catal. A 2010, 388, 7–14. [Google Scholar] [CrossRef]
  31. Zhuang, J.D.; Dai, W.X.; Tian, Q.F.; Li, Z.H.; Xie, L.Y.; Wang, J.X.; Liu, P.; Shi, X.C.; Wang, D.H. Photocatalytic degradation of rhb over TiO2 bilayer films: Effect of defects and their location. Langmuir 2010, 26, 9686–9694. [Google Scholar]
  32. Echavia, G.R.M.; Matzusawa, F.; Negishi, N. Photocatalytic degradation of organophosphate and phosphonoglycine pesticides using TiO2 immobilized on silica gel. Chemosphere 2009, 76, 595–600. [Google Scholar]
  33. Pelentridou, K.; Stathatos, E.; Karasali, H.; Lianos, P. Photodegradation of the herbicide azimsulfuron using nanocrystalline titania films as photocatalyst and low intensity black light radiation or simulated solar radiation as excitation source. J. Hazard. Mater. 2009, 163, 756–760. [Google Scholar] [CrossRef]
  34. Fabbri, D.; Crime, A.; Davezza, M.; Medana, C.; Baiocchi, C.; Prevot, A.B.; Pramauro, E. Surfactant-assisted removal of swep residues from soil and photocatalytic treatment of the washing wastes. Appl. Catal. B 2009, 92, 318–325. [Google Scholar] [CrossRef]
  35. Boroski, M.; Rodrigues, A.C.; Garcia, J.C.; Sampaio, L.C.; Nozaki, J.; Hioka, N. Combined electrocoagulation and TiO2 photoassisted treatment applied to wastewater effluents from pharmaceutical and cosmetic industries. J. Hazard. Mater. 2009, 162, 448–454. [Google Scholar] [CrossRef]
  36. Choina, J.; Duwensee, H.; Flechsig, G.U.; Kosslick, H.; Morawski, A.W.; Tuan, V.A.; Schulz, A. Removal of hazardous pharmaceutical from water by photocatalytic treatment. Cent. Eur. J. Chem. 2010, 8, 1288–1297. [Google Scholar]
  37. Alvarez, P.M.; Jaramillo, J.; Lopez-Pinero, F.; Plucinski, P.K. Preparation and characterization of magnetic TiO2 nanoparticles and their utilization for the degradation of emerging pollutants in water. Appl. Catal. B 2010, 100, 338–345. [Google Scholar] [CrossRef]
  38. Lin, Y.X.; Ferronato, C.; Deng, N.S.; Chovelon, J.M. Study of benzylparaben photocatalytic degradation by TiO2. Appl. Catal. B 2011, 104, 353–360. [Google Scholar]
  39. Giraldo, A.L.; Penuela, G.A.; Torres-Palma, R.A.; Pino, N.J.; Palominos, R.A.; Mansilla, H.D. Degradation of the antibiotic oxolinic acid by photocatalysis with TiO2 in suspension. Water Res. 2010, 44, 5158–5167. [Google Scholar] [CrossRef]
  40. Hapeshi, E.; Achilleos, A.; Vasquez, M.I.; Michael, C.; Xekoukoulotakis, N.P.; Mantzavinos, D.; Kassinos, D. Drugs degrading photocatalytically: Kinetics and mechanisms of ofloxacin and atenolol removal on titania suspensions. Water Res. 2010, 44, 1737–1746. [Google Scholar] [CrossRef]
  41. Ioannou, L.A.; Hapeshi, E.; Vasquez, M.I.; Mantzavinos, D.; Fatta-Kassinos, D. Solar/TiO2 photocatalytic decomposition of beta-blockers atenolol and propranolol in water and wastewater. Sol. Energy 2011, 85, 1915–1926. [Google Scholar] [CrossRef]
  42. An, T.C.; Yang, H.; Li, G.Y.; Song, W.H.; Cooper, W.J.; Nie, X.P. Kinetics and mechanism of advanced oxidation processes (AOPs) in degradation of ciprofloxacin in water. Appl. Catal. B 2010, 94, 288–294. [Google Scholar] [CrossRef]
  43. Li, W.; Guo, C.; Su, B.; Xu, J. Photodegradation of four fluoroquinolone compounds by titanium dioxide under simulated solar light irradiation. J. Chem. Technol. Biotechnol. 2012, 87, 643–650. [Google Scholar] [CrossRef]
  44. Pereira, J.; Vilar, V.J.P.; Borges, M.T.; Gonzalez, O.; Esplugas, S.; Boaventura, R.A.R. Photocatalytic degradation of oxytetracycline using TiO2 under natural and simulated solar radiation. Sol. Energy 2011, 85, 2732–2740. [Google Scholar] [CrossRef]
  45. Adams, W.A.; Impellitteri, C.A. The photocatalysis of n,n-diethyl-m-toluamide (DEET) using dispersions of degussa p-25 TiO2 particles. J. Photochem. Photobiol. A 2009, 202, 28–32. [Google Scholar]
  46. Qourzal, S.; Barka, N.; Tamimi, M.; Assabbane, A.; Nounah, A.; Ihlal, A.; Ait-Ichou, Y. Sol-gel synthesis of TiO2-SiO2 photocatalyst for beta-naphthol photodegradation. Mater. Sci. Eng. C 2009, 29, 1616–1620. [Google Scholar] [CrossRef]
  47. Miranda-Garcia, N.; Maldonado, M.I.; Coronado, J.M.; Malato, S. Degradation study of 15 emerging contaminants at low concentration by immobilized TiO2 in a pilot plant. Catal. Today 2010, 151, 107–113. [Google Scholar]
  48. Antoniou, M.G.; Shoemaker, J.A.; de la Cruz, A.A.; Dionysiou, D.D. LC/MS/MS structure elucidation of reaction intermediates formed during the TiO2 photocatalysis of microcystin-LR. Toxicon 2008, 51, 1103–1118. [Google Scholar] [CrossRef]
  49. Sharma, V.K.; Triantis, T.M.; Antoniou, M.G.; He, X.X.; Pelaez, M.; Han, C.S.; Song, W.H.; O’Shea, K.E.; de la Cruz, A.A.; Kaloudis, T.; et al. Destruction of microcystins by conventional and advanced oxidation processes: A review. Sep. Purif. Technol. 2012, 91, 3–17. [Google Scholar] [CrossRef]
  50. Graham, D.; Kisch, H.; Lawton, L.A.; Robertson, P.K.J. The degradation of microcystin-LR using doped visible light absorbing photocatalysts. Chemosphere 2010, 78, 1182–1185. [Google Scholar] [CrossRef]
  51. Triantis, T.M.; Fotiou, T.; Kaloudis, T.; Kontos, A.G.; Falaras, P.; Dionysiou, D.D.; Pelaez, M.; Hiskia, A. Photocatalytic degradation and mineralization of microcystin-LR under UV-A, solar and visible light using nanostructured nitrogen doped TiO2. J. Hazard. Mater. 2012, 211, 196–202. [Google Scholar]
  52. Dalrymple, O.K.; Isaacs, W.; Stefanakos, E.; Trotz, M.A.; Goswami, D.Y. Lipid vesicles as model membranes in photocatalytic disinfection studies. J. Photochem. Photobiol. A 2011, 221, 64–70. [Google Scholar] [CrossRef]
  53. Amarjargal, A.; Tijing, L.D.; Yu, M.-H.; Kim, C.-H.; Park, C.-H.; Kim, D.-W.; Kim, C.-S. Characterization and photocatalytic efficiency of TiO2/Ti beads fabricated by simple heat-treatment. J. Mater. Sci. Technol. 2012, 28, 184–192. [Google Scholar]
  54. Li, G.Z.; Park, S.; Kang, D.W.; Krajmalnik-Brown, R.; Rittmann, B.E. 2,4,5-trichlorophenol degradation using a novel TiO2-coated biofilm carrier: Roles of adsorption, photocatalysis, and biodegradation. Environ. Sci. Technol. 2011, 45, 8359–8367. [Google Scholar] [CrossRef]
  55. Zhang, W.; Li, Y.; Su, Y.; Mao, K.; Wang, Q. Effect of water composition on TiO2 photocatalytic removal of endocrine disrupting compounds (EDCs) and estrogenic activity from secondary effluent. J. Hazard. Mater. 2012, 215, 252–258. [Google Scholar]
  56. Wang, T.C.; Lu, N.; Li, J.; Wu, Y. Plasma-TiO2 catalytic method for high-efficiency remediation of p-nitrophenol contaminated soil in pulsed discharge. Environ. Sci. Technol. 2011, 45, 9301–9307. [Google Scholar] [CrossRef]
  57. Wang, C.; Zhang, X.; Liu, H.; Li, X.; Li, W.; Xu, H. Reaction kinetics of photocatalytic degradation of sulfosalicylic acid using TiO2 microspheres. J. Hazard. Mater. 2009, 163, 1101–1106. [Google Scholar] [CrossRef]
  58. Montoya, J.F.; Velasquez, J.A.; Salvador, P. The direct-indirect kinetic model in photocatalysis: A reanalysis of phenol and formic acid degradation rate dependence on photon flow and concentration in TiO2 aqueous dispersions. Appl. Catal. B 2009, 88, 50–58. [Google Scholar] [CrossRef]
  59. Tasseroul, L.; Pirard, S.L.; Lambert, S.D.; Paez, C.A.; Poelman, D.; Pirard, J.-P.; Heinrichs, B. Kinetic study of p-nitrophenol photodegradation with modified TiO2 xerogels. Chem. Eng. J. 2012, 191, 441–450. [Google Scholar] [CrossRef]
  60. Emeline, A.V.; Ryabchuk, V.K.; Serpone, N. Dogmas and misconceptions in heterogeneous photocatalysis. Some enlightened reflections. J. Phys. Chem. B 2005, 109, 18515–18521. [Google Scholar] [CrossRef]
  61. Pelaez, M.; de la Cruz, A.A.; O’Shea, K.; Falaras, P.; Dionysiou, D.D. Effects of water parameters on the degradation of microcystin-LR under visible light-activated TiO2 photocatalyst. Water Res. 2011, 45, 3787–3796. [Google Scholar] [CrossRef]
  62. Wang, W.; Lu, C.; Ni, Y.; Peng, F.; Xu, Z. Enhanced performance of {001} facets dominated mesoporous TiO2 photocatalyst composed of high-reactive nanocrystals and mesoporous spheres. Appl. Surf. Sci. [CrossRef]
  63. Zhao, Z.; Sun, Z.C.; Zhao, H.F.; Zheng, M.; Du, P.; Zhao, J.L.; Fan, H.Y. Phase control of hierarchically structured mesoporous anatase TiO2 microspheres covered with {001} facets. J. Mater. Chem. 2012, 22, 21965–21971. [Google Scholar]
  64. Ismail, A.A.; Bahnemann, D.W.; Robben, L.; Yarovyi, V.; Wark, M. Palladium doped porous titania photocatalysts: Impact of mesoporous order and crystallinity. Chem. Mat. 2010, 22, 108–116. [Google Scholar] [CrossRef]
  65. Liu, J.N.; Zhang, G.W.; Ao, W.; Yang, K.; Peng, S.X.; Muller-Goymann, C. Hollow mesoporous titania microsphere with low shell thickness/diameter ratio and high photocatalysis. Appl. Surf. Sci. 2012, 258, 8083–8089. [Google Scholar]
  66. Joo, J.B.; Zhang, Q.; Dahl, M.; Lee, I.; Goebl, J.; Zaera, F.; Yin, Y.D. Control of the nanoscale crystallinity in mesoporous TiO2 shells for enhanced photocatalytic activity. Energy. Environ. Sci. 2012, 5, 6321–6327. [Google Scholar] [CrossRef]
  67. Ismail, A.A.; Bahnemann, D.W. Mesoporous titania photocatalysts: Preparation, characterization and reaction mechanisms. J. Mater. Chem. 2011, 21, 11686–11707. [Google Scholar]
  68. Nakata, K.; Fujishima, A. TiO2 photocatalysis: Design and applications. J. Photochem. Photobiol. C 2012, 13, 169–189. [Google Scholar] [CrossRef]
  69. Pan, J.H.; Dou, H.Q.; Xiong, Z.G.; Xu, C.; Ma, J.Z.; Zhao, X.S. Porous photocatalysts for advanced water purifications. J. Mater. Chem. 2010, 20, 4512–4528. [Google Scholar] [CrossRef]
  70. Robben, L.; Ismail, A.A.; Lohmeier, S.J.; Feldhoff, A.; Bahnemann, D.W.; Buhl, J.C. Facile synthesis of highly ordered mesoporous and well crystalline TiO2: Impact of different gas atmosphere and calcination temperatures on structural properties. Chem. Mat. 2012, 24, 1268–1275. [Google Scholar] [CrossRef]
  71. Han, C.; Luque, R.; Dionysiou, D.D. Facile preparation of controllable size monodisperse anatase titania nanoparticles. Chem. Commun. 2012, 48, 1860–1862. [Google Scholar] [CrossRef]
  72. Chen, D.H.; Huang, F.Z.; Cao, L.; Cheng, Y.B.; Caruso, R.A. Spiky mesoporous anatase titania beads: A metastable ammonium titanate-mediated synthesis. Chem. Eur. J. 2012, 18, 13762–13769. [Google Scholar]
  73. Zhang, X.; Pan, J.H.; Du, A.J.; Fu, W.; Sun, D.D.; Leckie, J.O. Combination of one-dimensional TiO2 nanowire photocatalytic oxidation with microfiltration for water treatment. Water Res. 2009, 43, 1179–1186. [Google Scholar] [CrossRef]
  74. Zhang, A.Y.; Zhou, M.H.; Han, L.; Zhou, Q.X. The combination of rotating disk photocatalytic reactor and TiO2 nanotube arrays for environmental pollutants removal. J. Hazard. Mater. 2011, 186, 1374–1383. [Google Scholar] [CrossRef]
  75. Sun, X.; Zhang, J.; Zhang, G.; Pan, X.; Huang, T. Preparation and characteristics of TiO2 nanotube catalysts used in hybrid photocatalysis/membrane process. Catal. Commun. 2012, 18, 76–80. [Google Scholar]
  76. Zhang, X.; Pan, J.H.; Du, A.J.; Xu, S.; Sun, D.D. Room-temperature fabrication of anatase TiO2 submicrospheres with nanothornlike shell for photocatalytic degradation of methylene blue. J. Photochem. Photobiol. A 2009, 204, 154–160. [Google Scholar] [CrossRef]
  77. Farbod, M.; Khademalrasool, M. Synthesis of TiO2 nanoparticles by a combined sol-gel ball milling method and investigation of nanoparticle size effect on their photocatalytic activities. Powder Technol. 2011, 214, 344–348. [Google Scholar] [CrossRef]
  78. Li, G.; Lv, L.; Fan, H.T.; Ma, J.Y.; Li, Y.Q.; Wan, Y.; Zhao, X.S. Effect of the agglomeration of TiO2 nanoparticles on their photocatalytic performance in the aqueous phase. J. Colloid Interface Sci. 2010, 348, 342–347. [Google Scholar]
  79. Mogyorosi, K.; Balazs, N.; Sranko, D.F.; Tombacz, E.; Dekany, I.; Oszko, A.; Sipos, P.; Dombi, A. The effect of particle shape on the activity of nanocrystalline TiO2 photocatalysts in phenol decomposition. Part 3: The importance of surface quality. Appl. Catal. B 2010, 96, 577–585. [Google Scholar] [CrossRef]
  80. Bizarro, M.; Tapia-Rodriguez, M.A.; Ojeda, M.L.; Alonso, J.C.; Ortiz, A. Photocatalytic activity enhancement of TiO2 films by micro and nano-structured surface modification. Appl. Surf. Sci. 2009, 255, 6274–6278. [Google Scholar] [CrossRef]
  81. Monllor-Satoca, D.; Lana-Villarreal, T.; Gomez, R. Effect of surface fluorination on the electrochemical and photoelectrocatalytic properties of nanoporous titanium dioxide electrodes. Langmuir 2011, 27, 15312–15321. [Google Scholar]
  82. Kim, M.J.; Kim, K.D.; Tai, W.S.; Seo, H.O.; Luo, Y.; Kim, Y.D.; Lee, B.C.; Park, O.K. Enhancement of photocatalytic activity of TiO2 by high-energy electron-beam treatment under atmospheric pressure. Catal. Lett. 2010, 135, 57–61. [Google Scholar] [CrossRef]
  83. Zou, W.W.; Zhang, J.L.; Chen, F. Preparation, characterization and application of TiO2 nanoparticles surface-modified by DDAT. Mater. Lett. 2010, 64, 1710–1712. [Google Scholar] [CrossRef]
  84. Shan, A.Y.; Ghazi, T.I.M.; Rashid, S.A. Immobilisation of titanium dioxide onto supporting materials in heterogeneous photocatalysis: A review. Appl. Catal. A 2010, 389, 1–8. [Google Scholar]
  85. Zhu, B.; Zou, L. Trapping and decomposing of color compounds from recycled water by TiO2 coated activated carbon. J. Environ. Manag. 2009, 90, 3217–3225. [Google Scholar] [CrossRef]
  86. Jin, L.; Dai, B. TiO2 activation using acid-treated vermiculite as a support: Characteristics and photoreactivity. Appl. Surf. Sci. 2012, 258, 3386–3392. [Google Scholar] [CrossRef]
  87. Stathatos, E.; Papoulis, D.; Aggelopoulos, C.A.; Panagiotaras, D.; Nikolopoulou, A. TiO2/palygorskite composite nanocrystalline films prepared by surfactant templating route: Synergistic effect to the photocatalytic degradation of an azo-dye in water. J. Hazard. Mater. 2012, 211, 68–76. [Google Scholar] [CrossRef]
  88. Djafer, L.; Ayral, A.; Ouagued, A. Robust synthesis and performance of a titania-based ultrafiltration membrane with photocatalytic properties. Sep. Purif. Technol. 2010, 75, 198–203. [Google Scholar] [CrossRef]
  89. Athanasekou, C.P.; Romanos, G.E.; Katsaros, F.K.; Kordatos, K.; Likodimos, V.; Falaras, P. Very efficient composite titania membranes in hybrid ultrafiltration/photocatalysis water treatment processes. J. Membr. Sci. 2012, 392, 192–203. [Google Scholar] [CrossRef]
  90. Romanos, G.E.; Athanasekou, C.P.; Katsaros, F.K.; Kanellopoulos, N.K.; Dionysiou, D.D.; Likodimos, V.; Falaras, P. Double-side active TiO2-modified nanofiltration membranes in continuous flow photocatalytic reactors for effective water purification. J. Hazard. Mater. 2012, 211, 304–316. [Google Scholar] [CrossRef]
  91. Damodar, R.A.; You, S.-J.; Chou, H.-H. Study the self cleaning, antibacterial and photocatalytic properties of TiO2 entrapped PVDF membranes. J. Hazard. Mater. 2009, 172, 1321–1328. [Google Scholar] [CrossRef]
  92. Liu, L.; Liu, Z.; Bai, H.; Sun, D.D. Concurrent filtration and solar photocatalytic disinfection/degradation using high-performance Ag/TiO2 nanofiber membrane. Water Res. 2012, 46, 1101–1112. [Google Scholar]
  93. Bedford, N.M.; Pelaez, M.; Han, C.; Dionysiou, D.D.; Steckl, A.J. Photocatalytic cellulosic electrospun fibers for the degradation of potent cyanobacteria toxin microcystin-LR. J. Mater. Chem. 2012, 22, 12666–12674. [Google Scholar]
  94. Chen, Y.J.; Stathatos, E.; Dionysiou, D.D. Microstructure characterization and photocatalytic activity of mesoporous TiO2 films with ultrafine anatase nanocrystallites. Surf. Coat. Technol. 2008, 202, 1944–1950. [Google Scholar] [CrossRef]
  95. Chen, Y.J.; Dionysiou, D.D. Bimodal mesoporous TiO2-P25 composite thick films with high photocatalytic activity and improved structural integrity. Appl. Catal. B 2008, 80, 147–155. [Google Scholar]
  96. Pelaez, M.; Falaras, P.; Likodimos, V.; Kontos, A.G.; de la Cruz, A.A.; O’Shea, K.; Dionysiou, D.D. Synthesis, structural characterization and evaluation of sol-gel-based NF-TiO2 films with visible light-photoactivation for the removal of microcystin-LR. Appl. Catal. B 2010, 99, 378–387. [Google Scholar] [CrossRef]
  97. Kontos, A.G.; Pelaez, M.; Likodimos, V.; Vaenas, N.; Dionysiou, D.D.; Falaras, P. Visible light induced wetting of nanostructured NF co-doped titania films. Photochem. Photobiol. Sci. 2011, 10, 350–354. [Google Scholar] [CrossRef]
  98. Han, C.; Pelaez, M.; Likodimos, V.; Kontos, A.G.; Falaras, P.; O’Shea, K.; Dionysiou, D.D. Innovative visible light-activated sulfur doped TiO2 films for water treatment. Appl. Catal. B 2011, 107, 77–87. [Google Scholar] [CrossRef]
  99. Antoniou, M.G.; Nicolaou, P.A.; Shoemaker, J.A.; de la Cruz, A.A.; Dionysiou, D.D. Impact of the morphological properties of thin TiO2 photocatalytic films on the detoxification of water contaminated with the cyanotoxin, microcystin-LR. Appl. Catal. B 2009, 91, 165–173. [Google Scholar] [CrossRef]
  100. Pelaez, M.; Falaras, P.; Kontos, A.G.; de la Cruz, A.A.; O’Shea, K.; Dunlop, P.S.M.; Byrne, J.A.; Dionysiou, D.D. A comparative study on the removal of cylindrospermopsin and microcystins from water with NF-TiO2-P25 composite films with visible and UV-Vis light photocatalytic activity. Appl. Catal. B 2012, 121, 30–39. [Google Scholar] [CrossRef]
  101. Natarajan, T.S.; Thomas, M.; Natarajan, K.; Bajaj, H.C.; Tayade, R.J. Study on UV-LED/TiO2 process for degradation of rhodamine B dye. Chem. Eng. J. 2011, 169, 126–134. [Google Scholar]
  102. Natarajan, T.S.; Natarajan, K.; Bajaj, H.C.; Tayade, R.J. Energy efficient uv-led source and TiO2 nanotube array-based reactor for photocatalytic application. Ind. Eng. Chem. Res. 2011, 50, 7753–7762. [Google Scholar] [CrossRef]
  103. Natarajan, K.; Natarajan, T.S.; Bajaj, H.C.; Tayade, R.J. Photocatalytic reactor based on UV-LED/TiO2 coated quartz tube for degradation of dyes. Chem. Eng. J. 2011, 178, 40–49. [Google Scholar] [CrossRef]
  104. Nickels, P.; Zhou, H.; Basahel, S.N.; Obaid, A.Y.; Ali, T.T.; Al-Ghamdi, A.A.; El-Mossalamy, E.-S.H.; Ayoubi, A.O.; Lynch, S.A. Laboratory scale water circuit including a photocatalytic reactor and a portable in-stream sensor to monitor pollutant degradation. Ind. Eng. Chem. Res. 2012, 51, 3301–3308. [Google Scholar]
  105. Wang, X.P.; Lim, T.T. Solvothermal synthesis of C-N codoped TiO2 and photocatalytic evaluation for bisphenol a degradation using a visible-light irradiated led photoreactor. Appl. Catal. B 2010, 100, 355–364. [Google Scholar] [CrossRef]
  106. Chang, C.Y.; Wu, N.L. Process analysis on photocatalyzed dye decomposition for water treatment with TiO2-coated rotating disk reactor. Ind. Eng. Chem. Res. 2010, 49, 12173–12179. [Google Scholar]
  107. Rao, N.N.; Chaturvedi, V.; Puma, G.L. Novel pebble bed photocatalytic reactor for solar treatment of textile wastewater. Chem. Eng. J. 2012, 184, 90–97. [Google Scholar] [CrossRef]
  108. Ji, Z.X.; Callahan, D.M.; Ismail, M.N.; Warzywoda, J.; Sacco, A. Development and characterization of a titanosilicate ETS-10-coated optical fiber reactor towards the photodegradation of methylene blue. J. Photochem. Photobiol. A 2011, 217, 22–28. [Google Scholar] [CrossRef]
  109. Kim, M.J.; Choo, K.H.; Park, H.S. Photocatalytic degradation of seawater organic matter using a submerged membrane reactor. J. Photochem. Photobiol. A 2010, 216, 215–220. [Google Scholar] [CrossRef]
  110. Suryaman, D.; Hasegawa, K.; Kagaya, S.; Yoshimura, T. Continuous flow photocatalytic treatment integrated with separation of titanium dioxide on the removal of phenol in tap water. J. Hazard. Mater. 2009, 171, 318–322. [Google Scholar] [CrossRef]
  111. McCullagh, C.; Robertson, P.K.J.; Adams, M.; Pollard, P.M.; Mohammed, A. Development of a slurry continuous flow reactor for photocatalytic treatment of industrial waste water. J. Photochem. Photobiol. A 2010, 211, 42–46. [Google Scholar] [CrossRef]
  112. Vilar, V.J.P.; Maldonado, M.I.; Oller, I.; Malato, S.; Boaventura, R.A.R. Solar treatment of cork boiling and bleaching wastewaters in a pilot plant. Water Res. 2009, 43, 4050–4062. [Google Scholar] [CrossRef]
  113. Remoundaki, E.; Vidali, R.; Kousi, P.; Hatzikioseyian, A.; Tsezos, M. Photolytic and photocatalytic alterations of humic substances in UV (254 nm) and solar cocentric parabolic concentrator (CPC) reactors. Desalination 2009, 248, 843–851. [Google Scholar] [CrossRef]
  114. Benotti, M.J.; Stanford, B.D.; Wert, E.C.; Snyder, S.A. Evaluation of a photocatalytic reactor membrane pilot system for the removal of pharmaceuticals and endocrine disrupting compounds from water. Water Res. 2009, 43, 1513–1522. [Google Scholar] [CrossRef]
  115. Zayani, G.; Bousselmi, L.; Mhenni, F.; Ghrabi, A. Solar photocatalytic degradation of commercial textile azo dyes: Performance of pilot plant scale thin film fixed-bed reactor. Desalination 2009, 246, 344–352. [Google Scholar]
  116. Vargas, R.; Nunez, O. Photocatalytic degradation of oil industry hydrocarbons models at laboratory and at pilot-plant scale. Sol. Energy 2010, 84, 345–351. [Google Scholar] [CrossRef]
  117. Dionysiou, D.D.; Balasubramanian, G.; Suidan, M.T.; Khodadoust, A.P.; Baudin, I.; Laine, M. Rotating disk photocatalytic reactor: Development, characterization, and evaluation for the destruction of organic pollutants in water. Water Res. 2000, 34, 2927–2940. [Google Scholar] [CrossRef]
  118. Dionysiou, D.; Khodadoust, A.P.; Kern, A.M.; Suidan, M.T.; Baudin, I.; Laine, J.M. Continuous-mode photocatalytic degradation of chlorinated phenols and pesticides in water using a bench-scale TiO2 rotating disk reactor. Appl. Catal. B 2000, 24, 139–155. [Google Scholar] [CrossRef]
  119. Wang, C.; Sun, L.; Yun, H.; Li, J.; Lai, Y.; Lin, C. Sonoelectrochemical synthesis of highly photoelectrochemically active TiO2 nanotubes by incorporating cds nanoparticles. Nanotechnology 2009, 20, 295601. [Google Scholar] [CrossRef]
  120. Bach, U.; Lupo, D.; Comte, P.; Moser, J.E.; Rtel, F.W.; Salbeck, J.; Spreitzer, H.; Grätzel, M. Solid-state dye-sensitized mesoporous TiO2 solar cells with high photon-to-electron conversion efficiencies. Nature 1998, 395, 583–585. [Google Scholar]
  121. Barolo, G.; Livraghi, S.; Chiesa, M.; Paganini, M.C.; Giamello, E. Mechanism of the photoactivity under visible light of N-doped titanium dioxide. Charge carriers migration in irradiated N-TiO2 investigated by electron paramagnetic resonance. J. Phys. Chem. C 2012, 116, 20887–20894. [Google Scholar] [CrossRef]
  122. Kamegawa, T.; Sonoda, J.; Sugimura, K.; Mori, K.; Yamashita, H. Degradation of isobutanol diluted in water over visible light sensitive vanadium doped TiO2 photocatalyst. J. Alloy. Compd. 2009, 486, 685–688. [Google Scholar]
  123. Cui, L.; Wang, Y.; Niu, M.; Chen, G.; Cheng, Y. Synthesis and visible light photocatalysis of Fe-doped TiO2 mesoporous layers deposited on hollow glass microbeads. J. Solid State Chem. 2009, 182, 2785–2790. [Google Scholar] [CrossRef]
  124. Kuvarega, A.T.; Krause, R.W.M.; Mamba, B.B. Nitrogen/palladium-codoped TiO2 for efficient visible light photocatalytic dye degradation. J. Phys. Chem. C 2011, 115, 22110–22120. [Google Scholar]
  125. Wodka, D.; Bielanska, E.; Socha, R.P.; Elzbieciak-Wodka, M.; Gurgul, J.; Nowak, P.; Warszynski, P.; Kumakiri, I. Photocatalytic activity of titanium dioxide modified by silver nanoparticles. Appl. Mater. Inter. 2010, 2, 1945–1953. [Google Scholar]
  126. Kusiak-Nejman, E.; Janus, M.; Grzmil, B.; Morawski, A.W. Methylene blue decomposition under visible light irradiation in the presence of carbon-modified TiO2 photocatalysts. J. Photochem. Photobiol. A 2011, 226, 68–72. [Google Scholar] [CrossRef]
  127. Liu, G.; Wang, X.; Chen, Z.; Cheng, H.-M.; Lu, G.Q. The role of crystal phase in determining photocatalytic activity of nitrogen doped TiO2. J. Colloid Interface Sci. 2009, 329, 331–338. [Google Scholar]
  128. Gohin, M.; Maurin, I.; Gacoin, T.; Boilot, J.P. Photocatalytic activity of mesoporous films based on n-doped TiO2 nanoparticles. J. Mater. Chem. 2010, 20, 8070–8077. [Google Scholar] [CrossRef]
  129. Rockafellow, E.M.; Stewart, L.K.; Jenks, W.S. Is sulfur-doped TiO2 an effective visible light photocatalyst for remediation? Appl. Catal. B 2009, 91, 554–562. [Google Scholar] [CrossRef]
  130. Song, S.; Tu, J.J.; He, Z.Q.; Hong, F.Y.; Liu, W.P.; Chen, J.M. Visible light-driven iodine-doped titanium dioxide nanotubes prepared by hydrothermal process and post-calcination. Appl. Catal. A 2010, 378, 169–174. [Google Scholar] [CrossRef]
  131. Ma, N.; Quan, X.; Zhang, Y.; Chen, S.; Zhao, H. Integration of separation and photocatalysis using an inorganic membrane modified with Si-doped TiO2 for water purification. J. Membr. Sci. 2009, 335, 58–67. [Google Scholar]
  132. Hewer, T.L.R.; Souza, E.C.C.; Martins, T.S.; Muccillo, E.N.S.; Freire, R.S. Influence of neodymium ions on photocatalytic activity of TiO2 synthesized by sol-gel and precipitation methods. J. Mol. Catal. A 2011, 336, 58–63. [Google Scholar] [CrossRef]
  133. Van Grieken, R.; Marugan, J.; Sordo, C.; Martinez, P.; Pablos, C. Photocatalytic inactivation of bacteria in water using suspended and immobilized silver-TiO2. Appl. Catal. B 2009, 93, 112–118. [Google Scholar] [CrossRef]
  134. Liga, M.V.; Bryant, E.L.; Colvin, V.L.; Li, Q.L. Virus inactivation by silver doped titanium dioxide nanoparticles for drinking water treatment. Water Res. 2011, 45, 535–544. [Google Scholar]
  135. Choi, W.; Termin, A.; Hoffmann, M.R. The role of metal ion dopants in quantum-sized TiO2: Correlation between photoreactivity and charge carrier recombination dynamics. J. Phys. Chem. 1994, 98, 13669–13679. [Google Scholar] [CrossRef]
  136. Zhang, C.; Gu, L.; Lin, Y.; Wang, Y.; Fu, D.; Gu, Z. Degradation of x-3b dye by immobilized TiO2 photocatalysis coupling anodic oxidation on BDD electrode. J. Photochem. Photobiol. A 2009, 207, 66–72. [Google Scholar] [CrossRef]
  137. Paschoal, F.M.M.; Pepping, G.; Boldrin Zanoni, M.V.; Anderson, M.A. Photoelectrocatalytic removal of bromate using Ti/TiO2 coated as a photocathode. Environ. Sci. Technol. 2009, 43, 7496–7502. [Google Scholar] [CrossRef]
  138. Daghrir, R.; Drogui, P.; Ka, I.; El Khakani, M.A. Photoelectrocatalytic degradation of chlortetracycline using Ti/TiO2 nanostructured electrodes deposited by means of a pulsed laser deposition process. J. Hazard. Mater. 2012, 199, 15–24. [Google Scholar]
  139. Torres-Palma, R.A.; Nieto, J.I.; Combet, E.; Petrier, C.; Pulgarin, C. An innovative ultrasound, Fe2+ and TiO2 photoassisted process for bisphenol Amineralization. Water Res. 2010, 44, 2245–2252. [Google Scholar] [CrossRef]
  140. Suryaman, D.; Hasegawa, K. Biological and photocatalytic treatment integrated with separation and reuse of titanium dioxide on the removal of chlorophenols in tap water. J. Hazard. Mater. 2010, 183, 490–496. [Google Scholar] [CrossRef]
  141. Chebli, D.; Fourcade, F.; Brosillon, S.; Nacef, S.; Amrane, A. upported photocatalysis as a pre-treatment prior to biological degradation for the removal of some dyes from aqueous solutions; acid red 183, biebrich scarlet, methyl red sodium salt, orange II. J. Chem. Technol. Biotechnol. 2010, 85, 555–563. [Google Scholar]
  142. Yahiat, S.; Fourcade, F.; Brosillon, S.; Amrane, A. Photocatalysis as a pre-treatment prior to a biological degradation of cyproconazole. Desalination 2011, 281, 61–67. [Google Scholar] [CrossRef]
  143. Yahiat, S.; Fourcade, F.; Brosillon, S.; Amrane, A. Removal of antibiotics by an integrated process coupling photocatalysis and biological treatment—case of tetracycline and tylosin. Int. Biodeterior. Biodegrad. 2011, 65, 997–1003. [Google Scholar] [CrossRef]
  144. Laera, G.; Chong, M.N.; Jin, B.; Lopez, A. An integrated mbr-TiO2 photocatalysis process for the removal of carbamazepine from simulated pharmaceutical industrial effluent. Bioresour. Technol. 2011, 102, 7012–7015. [Google Scholar]
  145. Chen, K.C.; Wang, Y.H.; Lu, Y.C. Treatment of polluted water for reclamation using photocatalysis and constructed wetlands. Catal. Today 2011, 175, 276–282. [Google Scholar] [CrossRef]

Share and Cite

MDPI and ACS Style

Lazar, M.A.; Varghese, S.; Nair, S.S. Photocatalytic Water Treatment by Titanium Dioxide: Recent Updates. Catalysts 2012, 2, 572-601.

AMA Style

Lazar MA, Varghese S, Nair SS. Photocatalytic Water Treatment by Titanium Dioxide: Recent Updates. Catalysts. 2012; 2(4):572-601.

Chicago/Turabian Style

Lazar, Manoj A., Shaji Varghese, and Santhosh S. Nair. 2012. "Photocatalytic Water Treatment by Titanium Dioxide: Recent Updates" Catalysts 2, no. 4: 572-601.

Article Metrics

Back to TopTop