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Article

Photoelectrocatalytic Processes of TiO2 Film: The Dominating Factors for the Degradation of Methyl Orange and the Understanding of Mechanism

by
Yuhui Xiong
1,†,
Sijie Ma
2,†,
Xiaodong Hong
2,
Jiapeng Long
1,* and
Guangjin Wang
2,*
1
School of Materials Science and Engineering, Shenyang University of Chemical Technology, Shenyang 110142, China
2
School of Materials Science and Hydrogen Energy, Foshan University, Foshan 528051, China
*
Authors to whom correspondence should be addressed.
†
These authors contributed equally to this work.
Molecules 2023, 28(24), 7967; https://doi.org/10.3390/molecules28247967
Submission received: 3 November 2023 / Revised: 22 November 2023 / Accepted: 1 December 2023 / Published: 6 December 2023
(This article belongs to the Special Issue Electroanalysis of Biochemistry and Material Chemistry)
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Abstract

:
Various thicknesses of TiO2 films were prepared by the sol–gel method and spin-coating process. These prepared TiO2 films exhibit thickness-dependent photoelectrochemical performance. The 1.09-μm-thickTiO2 film with 20 spin-coating layers (TiO2-20) exhibits the highest short circuit current of 0.21 mAcm−2 and open circuit voltage of 0.58 V among all samples and exhibits a low PEC reaction energy barrier and fast kinetic process. Photoelectrocatalytic (PEC) degradation of methyl orange (MO) by TiO2 films was carried out under UV light. The roles of bias, film thickness, pH value, and ion properties were systematically studied because they are the four most important factors dominating the PEC performance of TiO2 films. The optimized values of bias, film thickness, and pH are 1.0 V, 1.09 μm, and 12, respectively, which were obtained according to the data of the PEC degradation of MO. The effect of ion properties on the PEC efficiency of TiO2-20 was also analyzed by using halide as targeted ions. The “activated” halide ions significantly promoted the PEC efficiency and the order was determined as Br > Cl > F. The PEC efficiency increased with increasing Cl content, up until the optimized value of 30 × 10−3 M. Finally, a complete degradation of MO by TiO2-20 was achieved in 1.5 h, with total optimization of the four factors: 1.0 V bias, 1.09-μm-thick, pH 12, and 30 × 10−3 M Cl ion content. The roles of reactive oxygen species and electric charge of photoelectrodes were also explored based on photoelectrochemical characterizations and membrane-separated reactors. Hydrogen peroxide, superoxide radical, and hydroxyl radical were found responsible for the decolorization of MO.

1. Introduction

Energy and environmental crises have become serious threats to human society in the world today. Industrialization and population growth are major factors that result in environmental pollution and energy shortages [1]. Organic materials including dyes dumped into the water by organic industries are hazardous to aquatic life. The production of synthetic dyes has increased rapidly to meet the demands of the textile, food, printing, ink, tannery, paper, pharmaceutical, and cosmetic industries. However, the chemicals used in the production of these dyes are toxic and carcinogenic [2]. Therefore, it is obligatory for the scientific community to explore ways for overcoming the issues related to industrial effluents loaded with dye contaminants [3].
Photoelectrocatalysis (PECs) has attracted considerable interest since the discovery of the Honda–Fujishima effect [4] in 1972, especially following the serial stories reported by Carey et al. [5,6] that degradation-resistant organics such as polychlorinated biphenyl can be decomposed by TiO2 photoelectrode. In 1989, Tanaka, K. et al. [7] proved that reactive oxygen species (ROSs) such as hydroxyl radicals (•OH) play a key role in photocatalysis, achieving great progress in photocatalytic (PC) mechanism. Furthermore, ROSs can be more effectively produced in photoelectrocatalytic (PEC) processes in a voltage bias photoelectrode, contributing significantly to the PEC synergy effect and enhanced PEC efficiency [8,9]. PECs combines the advantages of both PC and electrocatalytic technologies. Palanisamy’s group [10] demonstrated that the PEC process effectively eliminated 76.2% of amoxicillin within 120 min at 0.8 V, outperforming the removal rates attained by the PC (52.6%) and electrocatalytic (32.3%) processes. PECs can both make use of the solar energy and regulate the photocatalytic process by using photoelectrodes with an appropriate external bias. Moreover, the PEC process is convenient for recycling photoelectrodes, avoiding the dilemma encountered in the photocatalytic process. PECs have been regarded as a technique revolution owing to the combination of photocatalysis, electrocatalysis, and solar energy utilization [11].
Various factors affecting PEC performance have been widely reported for TiO2 photoelectrodes. Zhao’s group [12] observed that anatase TiO2 with a {001} crystal plane exposed shows prominent PEC activity. Wang and co-authors [13] demonstrated that the PEC efficiency increases when the UV light intensity ranges from 700 μWcm−2 to 2.5 mWcm−2. Iltaf Shah et al. [2] revealed that a basic alkaline medium is more suitable for a higher degradation rate of ethyl violet dye than acidic and neutral media. Lu Li and his teammates [14] announced that the PEC kinetics constant (K’) was a 6.0-fold increase compared to the PC system. They observed that the PEC degradation efficiency of o-chlorophenol was 96.6% in 180 min under optimum conditions (bias: 0.5 V, solution pH: 6.3). Yan et al. [15] claimed that the PEC efficiency is approximately proportional to the thickness of the TiO2 film; however, excessive thickness causes deterioration of the PEC efficiency. Anderson’s team [16] reported the effect of bias, pH, inorganic ions on the PEC efficiency. Particularly, halide ions can be “activated” by a photoelectrode with sufficient bias and transformed into an “active halide” with highly catalytic oxidation activity, greatly improving the PEC efficiency of decomposing seawater to produce hydrogen [17]. To conclude, extensive investigations have been carried out on one or several of the factors affecting the PEC efficiency of TiO2, including the crystal phase, light source and light intensity, film thickness, bias, ion properties, and pH value [11]. However, a systematic study on the factors dominating the PEC efficiency and related mechanisms is still absent so far.
Numerous metal oxides such as TiO2, SnO2, ZnO, WO3, and Cu2O have been used as photoelectrodes in PECs [18]. TiO2 is considered one of the most important photoelectrodes due to its high activity, stability, and low cost [19]. Various forms of nanostructured TiO2 film have been used in various applications such as detectors, memories, high-efficiency hydrolysis, diodes, transistors, sensors, etc. [20,21]. With regard to the feasibility of the application of TiO2 photoelectrodes, film thickness, bias, ion properties, and pH value are the four most important factors. Therefore, in this study, we initiate a systematic study on the four factors dominating the PEC efficiency. The roles of ROSs and the electric charge of electrodes were also investigated to explore the related PEC mechanisms based on photoelectrochemical characterizations combined with membrane-separated reactors. This study might be beneficial to PEC research fields involved in the appropriate choice and optimization of experimental conditions and parameters.

2. Results

2.1. Structure, Morphology, and Optimal Properties of TiO2 Films

Figure 1a shows the X ray diffraction (XRD) pattern of TiO2-20. All the diffraction peaks in the pattern are well-indexed to TiO2 and F-doped tin oxide (FTO). The peaks located at 2θ = 25.3°, 37.8°, 39.2°, 48.1°, 55.1°, 56.2°, and 69.1° are attributed to anatase types of TiO2. No other diffraction peak arises from possible impurities, indicating that a pure-phase TiO2 film is produced. The variation curves of thickness and absorbance of the films are given as the number of layers in Figure 1b. It is obvious that both the thickness and absorbance of the films increase with increasing layers of coatings.
Figure 2a–c shows the scanning electron microscopy (SEM) images of TiO2-1, TiO2-4, and TiO2-20. TiO2-1 has a uniform, smooth, and dense surface (Figure 2c). We observed that the surface morphologies of TiO2-2 and -3 are similar to that of TiO2-1. Cracks began to appear in TiO2-4 and then gradually widened as the layers increased. SEM images of TiO2-4 and -20 in Figure 2b,c are given, respectively, as representative examples. The inset in Figure 2a is the high-magnification SEM image of TiO2-1. The surface morphology in the red box in Figure 2b,c is similar to that of the inset. The results indicate that all TiO2 films are composed of nanoparticles with a size of 20–30 nm. The microstructure of the TiO2 films was further investigated with transmission electron microscopy (TEM). Figure 2d shows the representative TEM images of TiO2-20. Grain crystal particles of TiO2-20 shown in the TEM image can be clearly observed, which also indicate that TiO2-20 is composed of 20−30 nm size nanoparticles.

2.2. Photoelectrochemical Properties of TiO2 Photoelectrodes

Before the measurement of PEC regulation of MO by TiO2 photoelectrodes, the cyclic voltammetry (CV) technique was used to examine the charge transfer between the FTO and the electrolyte. Figure 3a shows that the onset potentials for the anodic and cathodic dark current are essentially independent of the film thickness and scan rate. Representative samples of TiO2-1, -8, -20, and -32 displayed nearly perfect blocking characteristics, indicating that all the films are pinhole free [22]. The result is also supported by the SEM data showing that the surface of the FTO substrate is completely covered by a very thin and compact TiO2 coating. Moreover, even if there are cracks in some of the TiO2 samples such as TiO2-20, the inner coatings contacting the FTO substrates are still uniform and dense enough to separate FTO substrates from electrolytes, blocking charge transfer between them. In this case, charge transfer can only proceed between the TiO2 photoelectrode and the electrolyte in the PEC reaction. The position of the flat-band potential was obtained by taking the x intercept of the Mott–Schottky plots of the TiO2 films (Figure 3b), which gave all the samples a considerably negative flat-band potential, for example, −0.51 V for TiO2-20. The positive slope of the plots again proved the n-type nature of the TiO2 films. The application of a potential over the flat-band potential can suppress the charge carrier recombination. Thus, a zero or positive bias over the flat-band potential on the TiO2 film electrodes may improve the PEC efficiency.
Figure 4a,b shows the variation in the short circuit current (ISC) and open circuit voltage (VOC) as the layers of TiO2 coatings. The data of ISC, VOC, and film thickness were abstracted from Figure S3. The behavior of the anode photocurrent and shift to negative potential under irradiation in Figure S3 indicate an n-type semiconductor behavior. The ISC and VOC increased at first and then decreased as the film thickness increased. TiO2-20 achieved the highest ISC of 0.21 mAcm−2 and VOC of 0.58 V. The thickness-dependent photoelectrochemical properties of the TiO2 films were also observed by M. L. Hitchman [23] and M. Rodríguez-Pérez [24] in polycrystalline anatase. EIS is particularly useful for explaining the interface charge transport and recombination [25]. Figure 4c shows Nyquist plots of the TiO2-1, -8, -16, -20, -24, -32. The zoom of the high-frequency range in Figure 4d indicates that the semicircle part of TiO2-20 has a minimum diameter among all the TiO2 films. In the same frequency, a small impedance semicircle indicates a large capacitance value at the corresponding time constant and a low Faraday current impedance, signifying a fast kinetic process [26]. Thus, TiO2-20 was chosen and used for the follow-up PEC experiment owing to its fast kinetic process and low PEC reaction energy barrier.

2.3. PEC Degradation of MO by TiO2 Photoelectrodes

We carried out the PEC degradation of MO using the PEC reactor as shown in Scheme 1a. Figure 5a shows the variation in the degradation rate of pristine MO using the TiO2-20 photoelectrode, with the potential bias ranging from 0 V to 1.2 V. Generally, in the PEC process, the degradation rate increased with an increasing bias, up until the optimized value of 1.0 V. Song et al. [27] and Zanoni et al. [28] reported similar results, in which at the optimal potential bias (for a given light intensity and film thickness), the electrons and holes were so well separated that enhancing the potential bias led to no significant improvement in the PEC activity. The PEC degradation of MO was further carried out using different thicknesses of TiO2 photoelectrodes. As expected, TiO2-20 achieved the highest degradation rate of 88.6% in 6 h among the representative samples at a bias of 1.0 V (Figure S4). This result is in accordance with the data of photoelectrochemical characterizations. Therefore, PEC regulation of MO by TiO2-20 with a 1.0 V bias was chosen and used for the tests of different pH, halide ion, and concentrations of Cl, respectively.
Figure 5b shows the degradation rates of MO by TiO2-20 with 1.0 V bias at different pH levels of 1, 4, 7, 9, and 12. The pH value of the solution was adjusted by dropwise adding H2SO4 and NaOH. The pH value of original MO solution in the control experiment was 5.8. One can see that the increasing pH value contributes to an enhanced degradation rate. Moreover, the degradation rates of all pH-adjusted MO solutions are higher than that of the pristine one. The reason is that the high conductivity of the MO solution increases the mass transfer and improves the PEC efficiency due to the addition of electrolytes H2SO4 and/or NaOH [29].
The influence of different electrolytes on the PEC degradation of organics has extensively been investigated in NaCl, NaNO3 and Na2SO4, NaBr, and NaClO4 [15,29,30]. The effects depend on the types and concentrations of negatively charged ions [11]. Halide ions can be transformed into “active halide” with highly catalytic oxidation activity, substantially improving the PEC efficiency and producing organic halides of industrial and medicinal importance [17]. Thus, in this study, we focused on the effect of halide ions on the PEC efficiency of TiO2-20. Iodine ion (I−) was not included here because of its highly chemical reduction [31]. Figure 5c shows the degradation of MO by halide ions F, Cl, and Br. The order of the PEC efficiency was determined as Br > Cl > F. The halide ions can be activated to form highly oxidizing free radicals, significantly improving the PEC efficiency [30]. Considering that the Cl ion is very important and spreads over the water on earth, we carried out PEC experiments on the degradation of MO with different concentrations of Cl ion. Figure 5d shows that the addition of Cl greatly increased the photocurrent and PEC efficiency. The degradation rate rapidly increased as the Cl content increased from 0 to 10 × 10−3 M. However, the increase in the degradation rate slowed down as the concentration of Cl ranged from 10 × 10−3 M to 30 × 10−3 M. Moreover, excessive Cl content caused a decrease in degradation rate. The results indicate that the content of “active” Cl reached nearly its maximum, meaning that increasing the content of Cl cannot produce more “active” Cl but suppresses the PEC efficiency. In all, the PEC efficiency can be substantially improved by optimizing factors dominating the PEC performance of TiO2 films. A complete degradation of MO by TiO2-20 was achieved in 1.5 h in the PEC process with total optimization of the four factors: a thickness of 1.09 μm, a bias of 1.0 V, a content of 30 × 10−3 M Cl ion, and pH 12. The PEC degradation efficiency of MO by TiO2-20 is pretty high and typical examples of comparative literature values are included in Table 1.

2.4. The Contrast of PEC and PC Degradation of MO

The contrast of the PEC and PC efficiency of TiO2-20 was carried out using PCMS and PECMS reactors, as shown in Scheme 1c,d. Figure 6a shows that the degradation rate of MO by TiO2-20 in the PCMS reactor is 41.5% in 6 h in the PC process, while that with a 1.0 bias in the PCEMS reactor is 100% in 5 h in the PEC process. Figure 6b shows that the TiO2-20 in the PC reactor earned 26.3% degradation of MO, while the same TiO2-20 with 0 V bias using the PEC reactor gained an enhanced degradation rate of 32.3%. It is expected that the application of a potential (0 V) over the flat-band potential (−0.51 V for TiO2-20) can suppress the charge carrier recombination and improve the PEC efficiency according to data of photoelectrochemical characterizations. These results indicate that the PEC process under electrochemical control achieves a much higher degradation rate than the PC one.
A comparison of the PEC efficiency of TiO2-20 in a PEC reactor with the PC efficiency of TiO2 powder in a PC reactor was also carried out. The film mass of TiO2-20 was determined as 3.81 mg by measuring the difference of mass between FTO and TiO2-20-coated FTO. Figure 6b shows that the single TiO2-20 film can decolor 26.3% of MO, while TiO2 powder (3.81 mg) can decompose 44.3% of MO in 6 h. The reason is that the TiO2 powder is highly dispersed and has much larger contact area with MO solution than that of the single TiO2-20 film. However, the TiO2 film photoelectrode is very easy to be recycled and reused compared to the TiO2 powder catalyst. Moreover, the TiO2 film photoelectrode is convenient for the PEC process. Particularly, the PEC efficiency can be improved by electrochemical regulation; for example, TiO2-20 with a bias of 0.5 V can achieve an equivalent degradation rate of MO as a 3.81 mg TiO2 powder (Figure 6b).

2.5. The Roles of ROSs and Electric Charge of Electrodes

The general principle of PECs is well-documented in the pioneering work and follow-up studies [4,37,38,39,40,41,42]. Scheme 2 shows the energy level diagram of the TiO2 film and the events possibly occurring during the PEC process. Under UV irradiation, the electrons (e−) in TiO2 are excited to the conduction band, which creates holes (h+) in the valence band. The excited holes can oxidize water into oxygen and interact with O2 and H2O to form an assortment of ROSs, (i.e., •OH, H2O2). The excited electrons are collected and removed by an external circuit to the counter electrode, where they are frequently captured by oxygen to form ROSs (i.e., •O2−, H2O2). Here, we carried out PC and PEC tests to explore the origin of ROSs with a partition system (see Scheme 1c,d) under different conditions.
Figure 7a shows that the •OH and•O2− yield increased with increased irradiation time in both TiO2 and Pt cells of the PCEMS reactor (Scheme 1d). The species of •OH in the TiO2 of the PCEMS reactor were probably produced by a hole-induced oxidation process [43]:
H2O + h+→•OH + H+
The •OH yield in the Pt cell of the PCEMS reactor should originate from the Pt electrode because •OH in TiO2 cell has a very short lifetime and cannot pass through the membrane to the Pt cell. It well known that electrons can react with O2 to produce •O2−, and then H2O2 and •OH through a reductive process (Formulas (2)–(6)) [44,45]. The very low •OH yield suggests that a low level of kinetics evolution of •OH proceeds in the Pt cell of a PCEMS reactor.
O 2 + e − → • O 2 − → 2 H + H 2 O 2
O2 + 2H2O + 2 e−→H2O2 + 2OH−
H2O2 +•O2−→•OH + OH−+ O2
2•OH→H2O2
H 2 O 2 → h v 2 • O H
Figure 7b shows that all of the H2O2 yields increased at first and became stable with prolonged irradiation time due to the decomposition of H2O2 in parallel with its production. The equilibrium concentration of H2O2 in the TiO2 and blank cells of the PEMS reactor was estimated to be 1.48 and 4.8 μM, respectively. It is no doubt that no PC process happened in the blank cell of the PEMS reactor so the supply of H2O2 in the blank cell attributed to the diffusion of H2O2, which was produced in the PC process of the TiO2 cell in the PEMS reactor and had a long life span and could pass through the membrane [46].
The equilibrium concentration for H2O2 in the TiO2 and Pt cells of the PECMS reactor significantly increased up to 4.58 and 3.5 μM, respectively. Although H2O2 can be derived from •OH according to Formulas (3) and (5), the formation kinetics reaction of H2O2 is very slow due to its second-order reaction. In this case, the much higher H2O2 yield in the TiO2 cell compared to the Pt cell of the PECMS reactor suggests that H2O2 can be probably produced from other sources. We believe that the supply of H2O2 in the TiO2 cell of the PECMS reactor originates from the back electrons (see the red arrow in Scheme 2) of TiO2 [47], which were transferred to the solution and underwent a reductive process as Formulas (2)–(5). The related mechanism and detailed descriptions on back electrons will be published elsewhere.
Note that an 8.5% degradation of MO was observed in 6 h in the blank cell of the PCMS and little degradation of MO under light control indicates that UV light cannot decompose MO in our experimental conditions (Figure 6a). In addition, ROSs including •OH and•O2− were produced in the TiO2 cell of the PCMS, but they cannot pass through the semi-membrane because of their short lifetime. In this case, only H2O2 is responsible for the 8.5% degradation of MO in the blank cell of the PCEMS. It is reported that •O2− with highly catalytic oxidation activity can also decompose MO [48]. So, H2O2, •O2−, and •OH were responsible for the decolorization of MO. The much higher yields of H2O2, •O2−, and •OH in the TiO2 cell than those in the Pt cell of the PCEMS reactor suggest that the TiO2 photoelectrode plays a major role in the PEC process.

3. Materials and Methods

3.1. Materials

Tetrabutyl titanate (99% purity), sodium sulfate (99.0% purity), absolute ethanol (99.9% purity), sodium fluoride, sodium chloride, sodium bromide, MO, sulfuric acid, sodium hydroxyl, and nitric acid were purchased from Sinopharm Group (Shanghai, China). 2,3-bis(2-methoxy-4-nitro-5-sulfophehyl)-2H-tetrazolium-5-carboxanilide (XTT) (>98% purity), Terephthalic acid (TA) (98% purity), and horseradish peroxidase (POD) (activity: 250–330 units/mg solid) were received from Sigma-Aldrich (Shanghai, China). FTO glass was obtained from Youxuan Technology Corp. (Liaoning, China). All were used as obtained. The solutions used in this work were prepared with deionized water further purified with a Millipore Milli-Q (Millipore, Bedford, MA, USA) purification system (resistivity 18.6 MΩ).

3.2. The Preparation of TiO2 Film Photoelectrodes and TiO2 Powder

In this step, 15 mL ethanol containing 0.3 mL water was added dropwise into the mixture of 5 mL tetrabutyl titanate, 30 mL ethanol, and 0.3 mL nitric acid, stirring vigorously. Then, the whole mixture was continuously stirred for 2 h. A colorless and transparent TiO2gel was obtained by keeping the whole mixture sealed for one day. On an FTO glass substrate (1.5 × 2.5 cm2), a thin film of sol was spin-coated at 2000 rpm for 30 s, followed by annealing in air with different ramping rates to the final 500 °C. FTO substrates with 1, 2, 4, 8, 16, 20, 24, 32 layers of coatings were achieved by repeating the spin-coating process and were denoted as TiO2-1, -2, -4, -8, -16, -20, -24, and -32, respectively. TiO2 electrodes with 1 × 1 cm2 of surface exposed were prepared by sealing them with epoxy resin. TiO2-20 was chosen for XRD measurement. TiO2 powder was collected by scraping the films off several TiO2-20 samples.

3.3. Characterization of TiO2 Films

XRD measurements were carried out on a PW 1840 powder X-ray diffractometer, using Cu Ka (1.54Å) as the incident radiation. SEM images were obtained on a field-emission scanning electron microscopy (JSM-6700F, JEOL, Tokyo, Japan) at 30 kV. TEM were carried out with JEOL JEM100CXII. The absorption spectra were measured by a UV–vis spectrophotometer (CARY5000, Varian, Australia). The thickness of films was determined by a step profiler (Dektak XT, Bruker, Germany). Photoelectrochemical measurements and characterizations were conducted by a three-electrode system with a TiO2 film electrode as working electrode, Pt plate electrode as counter electrode, and Ag/AgCl electrode as reference electrode, respectively, on a CHI660D station (Chenhua, Shanghai, China). The electrolytes were either 0.5 × 10−3 M K4Fe(CN)6 + 0.5 × 10−3 M K3Fe(CN)6 or air-saturated 1.0 × 10−3 M Na2SO4 solution. The light source was a UV-LED whose spectrum was given in Figure S1. The light intensity was measured by a light meter (LI-COR, Lincoln, NE, USA), and the light intensity for the experiments was fixed at 100 mW/cm2.

3.4. Detection of •OH,•O2− and H2O2

The production of •OH was detected by a photoluminescence (PL) method by using terephthalic acid (TA) as a probe molecule [49]. The experimental procedure was similar to the measurement of PEC and PC activity except that the MO aqueous solution was replaced by the 5 × 10–4 M TA aqueous solution with a concentration of 2 × 10–3 M NaOH. The superoxide radical (•O2− was measured by XTT [50,51], which can be reduced by •O2− to form XTT-formazan. The formazan has an absorption spectrum (measured by UV/Vis spectrophotometer (Blue Star A, Fort Lauderdale, FL, USA) with a peak at 470 nm can be used to quantify the relative amount of superoxide. H2O2 was analyzed photometrically by the Peroxidase (POD)-catalyzed oxidation product of DPD [52,53], which was measured by UV/Vis spectrophotometer (CARY5000, Varian, Australia) at 551 nm.

3.5. PC and PEC Experiments of TiO2 Photoelectrodes

Scheme 1 shows four kinds of reactors: (a) PEC reactor, in which TiO2 film, Pt were used as working electrode, counter electrode, respectively; (b) PC reactor, in which TiO2 film was dipped in solution; (c) membrane-separated (MS) reactor, and (d) PEC membrane-separated (PECMS) reactors which are the same as (a), (b), respectively, except that the reactors are separated into two compartments by a semipermeable membrane. The photographs of experimental set-up of PEC, PC reactors and MS, PECMS reactors are given in Figure S2. The pore size of the semipermeable membrane was 5 nm, whereas that of MO was about 6–8 nm in size so that MO cannot pass through the membrane. PEC degradation of MO was conducted with the TiO2film as working electrode, Pt wire electrode as counter electrode, respectively, on a DXW-12V100A DC Voltage Regulator (Suzhou, China). At different time intervals, aliquots of the sample were collected. The MO concentration was analyzed by recording variations in the absorption band maximum at 465 nm (defined as At) in the UV-vis spectra of MO by using a UV-vis spectrophotometer. MO concentration of the reaction solution was defined as A0′. The degradation efficiency of MO was calculated according to the equation: degradation rate (%) = (A0′ – At)/A0′ × 100%. The liquid phase degradation of MO was used for the evaluation of the PC activity of the TiO2 powder.

4. Conclusions

The effects of bias, film thickness, pH value, and ion properties on the PEC performance of TiO2 films were systematically studied under UV irradiation. At an optimized bias of 1.0 V, the TiO2-20 photoelectrode can degrade 84.5% of MO in 6 h, which outperforms the other TiO2 film samples. We observed that a high pH value contributed to enhanced degradation of MO. The “activated” halide ions can significantly promote PEC efficiency and the order of PEC efficiency was determined as Br > Cl > F. The degradation rate increased with an increasing Cl content in an MO solution, up until the optimized value of 30 × 10−3 M. However, excessive Cl content causes a decrease in degradation rate. The PEC efficiency can be significantly improved and a complete degradation of MO was achieved in 1.5 h using TiO2-20 with 1.0 V bias and 30 × 10−3 M Cl ion content at Ph 12. The roles of ROSs and electric charge of electrodes were investigated to explore the related PEC mechanisms and H2O2, •O2−, and •OH were found responsible for the decolorization of MO.

Supplementary Materials

The following supporting information can be downloaded at: https://www.mdpi.com/article/10.3390/molecules28247967/s1, Figures S1–S4. Figure S1: The light spectrum of the UV lamp used in irradiation experiments. The peak is located at 365 nm. Figure S2: The photographs of experimental set-up of (a) PC, PEC reactors and (b) MS, PECMS reactors. Figure S3: The short circuit photocurrent (a), open circuit potential (b) and (c) absorbance of TiO2-1, -2,-4, -8, -16, -20, -24 and -32. (d) variation of film thickness as the layers of coatings. Figure S4: PEC degradation of MO byTiO2-1, -8, -16,-20 and 32 photoelectrodes at 1.0 V bias under UV irradiation.

Author Contributions

Conceptualization, J.L. and G.W.; methodology and data analysis, Y.X. and S.M.; writing—original draft preparation, Y.X. and S.M.; writing—review and editing, X.H.; supervision and funding acquisition, J.L. and G.W. All authors have read and agreed to the published version of the manuscript.

Funding

This research received no external funding.

Institutional Review Board Statement

Not applicable.

Informed Consent Statement

Not applicable.

Data Availability Statement

Data are contained within the article and Supplementary Materials.

Conflicts of Interest

The authors declare no conflict of interest.

References

  1. Pereira, J.C. Environmental issues and international relations, a new global (dis)orderthe role of International Relations in promoting a concerted international system. Rev. Bras. Política Int. 2015, 58, 191–209. [Google Scholar] [CrossRef]
  2. Yahya, R.; Shah, A.; Kokab, T.; Ullah, N.; Hakeem, M.K.; Hayat, M.; Haleem, A.; Shah, I. Electrochemical Sensor for Detection and Degradation Studies of Ethyl Violet Dye. ACS Omega 2022, 7, 34154–34165. [Google Scholar] [CrossRef] [PubMed]
  3. Hayat, M.; Shah, A.; Hakeem, M.K.; Irfan, M.; Haleem, A.; Khan, S.B.; Shah, I. A designed miniature sensor for the trace level detection and degradation studies of the toxic dye Rhodamine B. RSC Adv. 2022, 12, 15658–15669. [Google Scholar] [CrossRef] [PubMed]
  4. Fujishima, A.; Honda, K. Electrochemical photolysis of water at a semiconductor electrode. Nature 1972, 238, 37–38. [Google Scholar] [CrossRef] [PubMed]
  5. Carey, J.H.; Lawrence, J.; Tosine, H.M. Photodechlorination of PCB’s in the presence of titanium dioxide in aqueous suspensions. Bull. Environ. Contam. Toxicol. 1976, 16, 697–701. [Google Scholar] [CrossRef] [PubMed]
  6. Pruden, A.L.; Ollis, D.F. Photoassisted heterogeneous catalysis: The degradation of trichloroethylene in water. J. Catal. 1983, 82, 404–417. [Google Scholar] [CrossRef]
  7. Tanaka, K.; Kato, H.; Kikuchi, T.; Yagishita, A. High flux VUV beamline for photochemical processing study at Photon Factory (abstract). Rev. Sci. Instrum. 1989, 60, 2252. [Google Scholar] [CrossRef]
  8. Gerischer, H.; Heller, A. Photocatalytic Oxidation of Organic Molecules at TiO2 Particles by Sunlight in Aerated Water. J. Electrochem. Soc. 1992, 139, 113–118. [Google Scholar] [CrossRef]
  9. Nosaka, Y. Water Photo-Oxidation over TiO2-History and Reaction Mechanism. Catalysts 2022, 12, 1557. [Google Scholar] [CrossRef]
  10. Alaydaroos, A.H.; Sydorenko, J.; Palanisamy, S.; Chiesa, M.; Al Hajri, E. Efficient photoelectrocatalytic degradation of amoxicillin using nano-TiO2 photoanode thin films: A comparative study with photocatalytic and electrocatalytic methods. Chemosphere 2023, 339, 139629. [Google Scholar] [CrossRef]
  11. Zhang, Y.; Xiong, X.; Han, Y.; Zhang, X.; Shen, F.; Deng, S.; Xiao, H.; Yang, X.; Yang, G.; Peng, H. Photoelectrocatalytic degradation of recalcitrant organic pollutants using TiO2 film electrodes: An overview. Chemosphere 2012, 88, 145–154. [Google Scholar] [CrossRef] [PubMed]
  12. Zhang, H.; Wang, Y.; Liu, P.; Han, Y.; Yao, X.; Zou, J.; Cheng, H.; Zhao, H. Anatase TiO2 crystal facet growth: Mechanistic role of hydrofluoric acid and photoelectrocatalytic activity. ACS Appl. Mater. Interfaces 2011, 3, 2472–2478. [Google Scholar] [CrossRef] [PubMed]
  13. Wang, N.; Li, X.; Wang, Y.; Quan, X.; Chen, G. Evaluation of bias potential enhanced photocatalytic degradation of 4-chlorophenol with TiO2 nanotube fabricated by anodic oxidation method. Chem. Eng. J. 2009, 146, 30–35. [Google Scholar] [CrossRef]
  14. Li, L.; Jiang, L.; Yang, L.; Li, J.; Lu, N.; Qu, J. Optimization of Degradation Kinetics towards O-CP in H3PW12O40/TiO2 Photoelectrocatalytic System. Sustainability 2019, 11, 3551. [Google Scholar] [CrossRef]
  15. Xiaoli, Y.; Huixiang, S.; Dahui, W. Photoelectrocatalytic degradation of phenol using a TiO2/Ni thin-film electrode. Korean J. Chem. Eng. 2003, 20, 679–684. [Google Scholar] [CrossRef]
  16. Selcuk, H.; Sene, J.J.; Anderson, M.A. Photoelectrocatalytichumic acid degradation kinetics and effect of pH, applied potential and inorganic ions. J. Chem. Technol. Biotechnol. 2003, 78, 979–984. [Google Scholar] [CrossRef]
  17. Li, Z.; Luo, L.; Li, M.; Chen, W.; Liu, Y.; Yang, J.; Xu, S.M.; Zhou, H.; Ma, L.; Xu, M.; et al. Photoelectrocatalytic C-H halogenation over an oxygen vacancy-rich TiO2 photoanode. Nat. Commun. 2021, 12, 6698. [Google Scholar] [CrossRef] [PubMed]
  18. Farooq, U.; Ahmad, T.; Naaz, F.; Islam, S.U. Review on Metals and Metal Oxides in Sustainable Energy Production: Progress and Perspectives. Energy Fuels 2023, 37, 1577–1632. [Google Scholar] [CrossRef]
  19. Pattnaik, A.; Sahu, J.N.; Poonia, A.K.; Ghosh, P. Current perspective of nano-engineered metal oxide based photocatalysts in advanced oxidation processes for degradation of organic pollutants in wastewater. Chem. Eng. Res. Des. 2023, 190, 667–686. [Google Scholar] [CrossRef]
  20. Ge, S.; Sang, D.; Zou, L.; Yao, Y.; Zhou, C.; Fu, H.; Xi, H.; Fan, J.; Meng, L.; Wang, C. A Review on the Progress of Optoelectronic Devices Based on TiO2 Thin Films and Nanomaterials. Nanomaterials 2023, 13, 1141. [Google Scholar] [CrossRef]
  21. Jiao, M.; Zhao, X.; He, X.; Wang, G.; Zhang, W.; Rong, Q.; Nguyen, D. High-Performance MEMS Oxygen Sensors Based on Au/TiO2 Films. Chemosensors 2023, 11, 476. [Google Scholar] [CrossRef]
  22. Kavan, L.; Tétreault, N.; Moehl, T.; Grätzel, M. Electrochemical Characterization of TiO2 Blocking Layers for Dye-Sensitized Solar Cells. J. Phys. Chem. C 2014, 118, 16408–16418. [Google Scholar] [CrossRef]
  23. Hitchman, M.L.; Tian, F. Studies of TiO2 thin films prepared by chemical vapour deposition for photocatalytic and photoelectrocatalytic degradation of 4-chlorophenol. J. Electroanal. Chem. 2002, 538–539, 165–172. [Google Scholar] [CrossRef]
  24. Rodríguez-Pérez, M.; Rodríguez-Gutiérrez, I.; Vega-Poot, A.; García-Rodríguez, R.; Rodríguez-Gattorno, G.; Oskam, G. Charge transfer and recombination kinetics at WO3 for photoelectrochemical water oxidation. Electrochim. Acta 2017, 258, 900–908. [Google Scholar] [CrossRef]
  25. Todinova, A.; Idigoras, J.; Salado, M.; Kazim, S.; Anta, J.A. Universal Features of Electron Dynamics in Solar Cells with TiO2 Contact: From Dye Solar Cells to Perovskite Solar Cells. J. Phys. Chem. Lett. 2015, 6, 3923–3930. [Google Scholar] [CrossRef] [PubMed]
  26. Gomes, W.P.; Vanmaekelbergh, D. Impedance spectroscopy at semiconductor electrodes: Review and recent developments. Electrochim. Acta 1996, 41, 967–973. [Google Scholar] [CrossRef]
  27. Song, X.M.; Wu, J.M.; Yan, M. Photocatalytic and photoelectrocatalytic degradation of aqueous Rhodamine B by low-temperature deposited anatase thin films. Mater. Chem. Phys. 2008, 112, 510–515. [Google Scholar] [CrossRef]
  28. Zanoni, M.V.B.; Sene, J.J.; Anderson, M.A. Photoelectrocatalytic degradation of Remazol Brilliant Orange 3R on titanium dioxide thin-film electrodes. J. Photochem. Photobiol. A Chem. 2003, 157, 55–63. [Google Scholar] [CrossRef]
  29. Brugnera, M.F.; Rajeshwar, K.; Cardoso, J.C.; Zanoni, M.V. Bisphenol A removal from wastewater using self-organized TiO2 nanotubular array electrodes. Chemosphere 2010, 78, 569–575. [Google Scholar] [CrossRef]
  30. Selcuk, H.; Sene, J.J.; Zanoni, M.V.; Sarikaya, H.Z.; Anderson, M.A. Behavior of bromide in the photoelectrocatalytic process and bromine generation using nanoporous titanium dioxide thin-film electrodes. Chemosphere 2004, 54, 969–974. [Google Scholar] [CrossRef]
  31. De Santana, H.; Temperini, M.L.A. Spectroelectrochemical study of iodide, iodate and periodate on a silver electrode in alkaline aqueous solution. J. Chem. Interfacial Electrochem. 1991, 316, 93–105. [Google Scholar] [CrossRef]
  32. Liu, H.; Cao, X.; Liu, G.; Wang, Y.; Zhang, N.; Li, T.; Tough, R. Photoelectrocatalytic degradation of triclosan on TiO2 nanotube arrays and toxicity change. Chemosphere 2013, 93, 160–165. [Google Scholar] [CrossRef] [PubMed]
  33. 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, 199–200, 15–24. [Google Scholar] [CrossRef] [PubMed]
  34. Zhang, Q.; Fu, Y.; Wu, Y.; Zhang, Y.-N.; Zuo, T. Low-Cost Y-Doped TiO2 Nanosheets Film with Highly Reactive {001} Facets from CRT Waste and Enhanced Photocatalytic Removal of Cr(VI) and Methyl Orange. ACS Sustain. Chem. Eng. 2016, 4, 1794–1803. [Google Scholar] [CrossRef]
  35. Bai, J.; Liu, Y.; Li, J.; Zhou, B.; Zheng, Q.; Cai, W. A novel thin-layer photoelectrocatalytic (PEC) reactor with double-faced titania nanotube arrays electrode for effective degradation of tetracycline. Appl. Catal. B Environ. 2010, 98, 154–160. [Google Scholar] [CrossRef]
  36. Wu, L.; Li, F.; Xu, Y.; Zhang, J.W.; Zhang, D.; Li, G.; Li, H. Plasmon-induced photoelectrocatalytic activity of Au nanoparticles enhanced TiO2 nanotube arrays electrodes for environmental remediation. Appl. Catal. B Environ. 2015, 164, 217–224. [Google Scholar] [CrossRef]
  37. Conway, B.E. Advancer in Electrochemistry and Electrochemical Engineering. In Electrochemistry; Delahay, P., Ed.; Interscience Publishers, Inc.: Hoboken, NJ, USA, 1961. [Google Scholar]
  38. El Guibaly, F.; Colbow, K. Theory of photocurrent in semiconductor-electrolyte junction solar cells. J. Appl. Phys. 1982, 53, 1737–1740. [Google Scholar] [CrossRef]
  39. Khan, S.U.; Bockris, J.O.M. A Model for Electron Transfer at the Illuminated p-Type Semiconductor-Solution Interface. J. Phys. Chem. 1984, 88, 2504–2515. [Google Scholar] [CrossRef]
  40. Chandra, S.; Singh, S.L.; Khare, N. A theoretical model of a photoelectrochemical solar cell. J. Appl. Phys. 1986, 59, 1570–1577. [Google Scholar] [CrossRef]
  41. Hodes, G.; Howell, I.D.J.; Peter, L.M. Nanocrystalline Photoelectrochemical Cells A New Concept In Photovoltaic Cells. J. Electrochem. Soc. 1992, 139, 3136–3140. [Google Scholar] [CrossRef]
  42. Kambili, A.; Walker, A.B.; Qiu, F.L.; Fisher, A.C.; Savin, A.D.; Peter, L.M. Electron transport in the dye sensitized nanocrystalline cell. Phys. E Low-Dimens. Syst. Nanostruct. 2002, 14, 203–209. [Google Scholar] [CrossRef]
  43. Guo, Q.; Zhou, C.; Ma, Z.; Yang, X. Fundamentals of TiO2 Photocatalysis: Concepts, Mechanisms, and Challenges. Adv. Mater. 2019, 31, e1901997. [Google Scholar] [CrossRef] [PubMed]
  44. Liu, F.; Cao, H.; Xu, L.; Fu, H.; Sun, S.; Xiao, Z.; Sun, C.; Long, X.; Xia, Y.; Wang, S. Design and preparation of highly active TiO2 photocatalysts by modulating their band structure. J. Colloid Interface Sci. 2023, 629, 336–344. [Google Scholar] [CrossRef] [PubMed]
  45. Schneider, J.; Matsuoka, M.; Takeuchi, M.; Zhang, J.; Horiuchi, Y.; Anpo, M.; Bahnemann, D.W. Understanding TiO2 photocatalysis: Mechanisms and materials. Chem. Rev. 2014, 114, 9919–9986. [Google Scholar] [CrossRef] [PubMed]
  46. Rincon, A. Effect of pH, inorganic ions, organic matter and H2O2 on E. coli K12 photocatalytic inactivation by TiO2 Implications in solar water disinfection. Appl. Catal. B Environ. 2004, 51, 283–302. [Google Scholar] [CrossRef]
  47. Fox, M.A. Photoinduced Electron Transfer in Organic Systems: Control of Back Electron Transfer. In Advances in Photochemistry; Volman, D.H., Hammond, G.S., Gollnick, K., Eds.; John Wiley & Sons, Inc.: Hoboken, NJ, USA, 1986; Volume 13, pp. 238–305. [Google Scholar]
  48. Hu, Z.; Lyu, J.; Ge, M. Role of reactive oxygen species in the photocatalytic degradation of methyl orange and tetracycline by Ag3PO4 polyhedron modified with g-C3N4. Mater. Sci. Semicond. Process. 2020, 105, 104731. [Google Scholar] [CrossRef]
  49. Ishibashi, K.I.; Fujishima, A.; Watanabe, T.; Hashimoto, K. Quantum yields of active oxidative species formed on TiO2 photocatalyst. J. Photochem. Photobiol. A Chem. 2000, 134, 139–142. [Google Scholar] [CrossRef]
  50. Sutherland, M.W.; Learmonth, B.A. The Tetrazolium Dyes MTS and XTT Provide New Quantitative Assays for Superoxide and Superoxide Disrnutase. Free. Radic. Res. 1997, 27, 283–289. [Google Scholar] [CrossRef]
  51. Li, Y.; Zhang, W.; Niu, J.; Chen, Y. Mechanism of Photogenerated Reactive Oxygen Species and Correlation with the Antibacterial Properties of Engineered Metal-Oxide Nanoparticles. ACS Nano 2012, 6, 5164–5173. [Google Scholar] [CrossRef]
  52. Bader, H.; Sturzenegger, V.; Hoigné, J. Photometric method for the determination of low concentrations of hydrogen peroxide by the peroxidase catalyzed oxidation of N,N-diethyl-p-phenylenediamine (DPD). Water Res. 1988, 22, 1109–1115. [Google Scholar] [CrossRef]
  53. Wang, W.; Yu, Y.; An, T.; Li, G.; Yip, H.Y.; Yu, J.C.; Wong, P.K. Visible-light-driven photocatalytic inactivation of E. coli K-12 by bismuth vanadate nanotubes: Bactericidal performance and mechanism. Environ. Sci. Technol. 2012, 46, 4599–4606. [Google Scholar] [CrossRef]
Molecules 28 07967 g001
Figure 1. (a) XRD pattern of TiO2-20, (b) the variation curves of film thickness and absorbance as the layers of coatings increase.
Figure 1. (a) XRD pattern of TiO2-20, (b) the variation curves of film thickness and absorbance as the layers of coatings increase.
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Figure 2. (a) SEM images of TiO2-1, (b) TiO2-4, (c) TiO2-20, and (d) TEM of TiO2-20. Inset is the close-ups of TiO2-1. Red boxes in Figure 2b,c designate two continuous small areas in surface of TiO2-4 and TiO2-20.
Figure 2. (a) SEM images of TiO2-1, (b) TiO2-4, (c) TiO2-20, and (d) TEM of TiO2-20. Inset is the close-ups of TiO2-1. Red boxes in Figure 2b,c designate two continuous small areas in surface of TiO2-4 and TiO2-20.
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Figure 3. (a) CV of FTO, TiO2-1, -8, -20, and -32. The measurement was carried out by a three-electrode system with TiO2 film as working electrode, Pt plate as counter electrode, and Ag/AgCl electrode as reference electrode, respectively, and a scan rate of 20 mV s−1. The electrolyte solution was 0.5 × 10−3 M K4Fe(CN)6 + 0.5 × 10−3 M K3Fe(CN)6 in aqueous 0.5 M KCl. (b) Mott–Schottky plots of TiO2 films; measured at 10 kHz, sweep rate 100 mVs−1. The electrolyte solution was 0.5 × 10−3 M Na2SO4.
Figure 3. (a) CV of FTO, TiO2-1, -8, -20, and -32. The measurement was carried out by a three-electrode system with TiO2 film as working electrode, Pt plate as counter electrode, and Ag/AgCl electrode as reference electrode, respectively, and a scan rate of 20 mV s−1. The electrolyte solution was 0.5 × 10−3 M K4Fe(CN)6 + 0.5 × 10−3 M K3Fe(CN)6 in aqueous 0.5 M KCl. (b) Mott–Schottky plots of TiO2 films; measured at 10 kHz, sweep rate 100 mVs−1. The electrolyte solution was 0.5 × 10−3 M Na2SO4.
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Figure 4. Patterns of variation in (a) short circuit current and (b) open circuit voltage as the layers of coatings of TiO2 films. (c) Complete range Nyquist plot and (d) zoom at high-frequency region. Measuring condition: a 20 mV of AC signal was applied for a frequency range from 100 mHz to 400 kHz under UV-LED irradiation at a direct current bias of 0 V. The electrolyte solution was 0.5 × 10−3 M Na2SO4.
Figure 4. Patterns of variation in (a) short circuit current and (b) open circuit voltage as the layers of coatings of TiO2 films. (c) Complete range Nyquist plot and (d) zoom at high-frequency region. Measuring condition: a 20 mV of AC signal was applied for a frequency range from 100 mHz to 400 kHz under UV-LED irradiation at a direct current bias of 0 V. The electrolyte solution was 0.5 × 10−3 M Na2SO4.
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Molecules 28 07967 sch001
Scheme 1. Schematic diagrams of experimental reactors with about 100 mL of volume glass container for PEC and PC regulation of MO. (a) PEC, (b) PC, (c) PEMS, and (d) PECMS reactors.
Scheme 1. Schematic diagrams of experimental reactors with about 100 mL of volume glass container for PEC and PC regulation of MO. (a) PEC, (b) PC, (c) PEMS, and (d) PECMS reactors.
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Figure 5. (a) PEC regulation of original MO by TiO2-20 at different bias. PEC regulation of MO by TiO2-20 with 1.0 V bias at different (b) pH, (c) halide ions, and (d) concentrations of Cl. The PEC reactor is depicted as Scheme 1a.
Figure 5. (a) PEC regulation of original MO by TiO2-20 at different bias. PEC regulation of MO by TiO2-20 with 1.0 V bias at different (b) pH, (c) halide ions, and (d) concentrations of Cl. The PEC reactor is depicted as Scheme 1a.
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Figure 6. (a) The PC and PEC degradation of MO by TiO2-20 using PCMS (Scheme 1c) and PECMS (Scheme 1d) reactors, respectively. (b) The PC degradation of MO by TiO2 film and powder using PC reactor shown in Scheme 1b.
Figure 6. (a) The PC and PEC degradation of MO by TiO2-20 using PCMS (Scheme 1c) and PECMS (Scheme 1d) reactors, respectively. (b) The PC degradation of MO by TiO2 film and powder using PC reactor shown in Scheme 1b.
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Scheme 2. Energy level diagram of TiO2 film and the events possibly occurring during the PEC process.
Scheme 2. Energy level diagram of TiO2 film and the events possibly occurring during the PEC process.
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Figure 7. (a) •OH, •O2−, and (b) H2O2 yield in TiO2 and Pt cell of PECMS reactor under UV irradiation.
Figure 7. (a) •OH, •O2−, and (b) H2O2 yield in TiO2 and Pt cell of PECMS reactor under UV irradiation.
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Table 1. Typical examples for pollutant degradation using PEC systems. (NPs = nanoparticles, NTs = Nanotubes).
Table 1. Typical examples for pollutant degradation using PEC systems. (NPs = nanoparticles, NTs = Nanotubes).
PhotoelectrodeTarget PollutantDegradation Rate (%)Degradation Time (min)Ref.
TiO2NPsMO10090Our work
TiO2NPsamoxicillin76.2120[10]
TiO2 NTstriclosan78.730[32]
Ti/TiO2NTsChlortetracycline74.2120[33]
Y-TiO2MO82.8360[34]
Double-faced TiO2 tetracycline96.460[35]
Au/TiO2MO54300[36]
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Xiong, Y.; Ma, S.; Hong, X.; Long, J.; Wang, G. Photoelectrocatalytic Processes of TiO2 Film: The Dominating Factors for the Degradation of Methyl Orange and the Understanding of Mechanism. Molecules 2023, 28, 7967. https://doi.org/10.3390/molecules28247967

AMA Style

Xiong Y, Ma S, Hong X, Long J, Wang G. Photoelectrocatalytic Processes of TiO2 Film: The Dominating Factors for the Degradation of Methyl Orange and the Understanding of Mechanism. Molecules. 2023; 28(24):7967. https://doi.org/10.3390/molecules28247967

Chicago/Turabian Style

Xiong, Yuhui, Sijie Ma, Xiaodong Hong, Jiapeng Long, and Guangjin Wang. 2023. "Photoelectrocatalytic Processes of TiO2 Film: The Dominating Factors for the Degradation of Methyl Orange and the Understanding of Mechanism" Molecules 28, no. 24: 7967. https://doi.org/10.3390/molecules28247967

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