Skip to main content


  • Research article
  • Open Access

Investigation of photocatalytic degradation of phenol by Fe(III)-doped TiO2 and TiO2 nanoparticles

  • 1,
  • 1Email author,
  • 1,
  • 2 and
  • 3
Journal of Environmental Health Science and Engineering201412:101

  • Received: 26 October 2013
  • Accepted: 28 May 2014
  • Published:


In this study Fe (III)-doped TiO2 nanoparticles were synthesized by sol–gel method at two atomic ratio of Fe/Ti, 0.006 and 0.034 percent. Then the photoactivity of them was investigated on degradation of phenol under UV (<380 nm) irradiation and visible light (>380 nm). Results showed that at appropriate atomic ratio of Fe to Ti (% 0.034) photoactivity of Fe(III)–doped TiO2 nanoparticles increased. In addition, the effects of various operational parameters on photocatalytic degradation, such as pH, initial concentration of phenol and amount of photocatalyst were examined and optimized. At all different initial concentration, highest degradation efficiency occurred at pH = 3 and 0.5 g/L Fe(III)–doped TiO2 dosage. With increase in initial concentration of phenol, photocatalytic degradation efficiency decreased. Photoactivity of Fe (III)-doped TiO2 under UV irradiation and visible light at optimal condition (pH = 3 and catalyst dosage = and 0.5 g/L) was compared with P25 TiO2 nanoparticles. Results showed that photoactivity of Fe(III)-doped TiO2 under visible light was more than P25 TiO2 photoactivity, but it was less than P25 TiO2 photoactivity under UV irradiation. Also efficiency of UV irradiation alone and amount of phenol adsorption on Fe(III)-doped TiO2 at dark condition was investigated.


  • Aqueous solution
  • Phenol
  • Fe (III)-doped TiO2
  • P25 TiO2
  • Sol–gel method


Phenolic compounds constitute an important group of wastewater pollutants produced by chemical, petrochemical, paint, textile, pesticide plants, food–processing and biotechnological industries [1]. As the phenolic compounds toxicity is an important problem, their concentration unfortunately prevents of micro-organisms activity in biological wastewater treatment plant. Therefore, the presence of phenols strongly reduces the biological biodegradation of the other components [2]. However some of the most conventional technologies for phenolic compounds degradation such as granular activated carbon (GAC) adsorption and biological treatment are effective in water treatment but they are slow processes and at higher concentrations of the organic contaminants, they present some difficulties during the operation [2]. So now applying of various advanced techniques in the fields of environmental protection has become prevalent.

Photoassisted catalytic decomposition of aqueous and gaseous contaminants by application of semiconductors as photocatalysts is one of the promising technologies [3, 4]. Among various oxide semiconductor photocatalysts, titanium dioxide has been proved to be the most suitable catalyst for widespread environmental applications, considering its biological and chemical inertness, strong oxidizing power, non–toxicity, insolubility, comparatively low cost and long term stability against photo corrosion and chemical corrosion [46]. The photocatalytic activity of semiconductor is the result of the production of excited electrons in its conduction band, along with corresponding positive holes in the valence band under UV illumination [5], that react with contaminants adsorbed on the photocatalyst surface [4]. However, the relatively large band gap of TiO2 (3.2 eV) limits the efficiency of photocatalytic reactions due to high recombination rate of photogenerated electrons and holes formed in photocatalytic process and low absorption capability of visible light [7]. In this respect, strategies may be suggested to electron–hole recombination rate reduction and photocatalyst efficiency increase [1]. Also shifting the absorption edge to larger wavelengths by adding dopants (metal ions or non-metal) to TiO2, while keeping a good control of the main particle size to produce nanoscale configurations of the catalysts can be considered [1, 5, 8].

Doping TiO2 with transition metal cations is an efficient strategy to reduce electron–hole recombination rate and increase photocatalytical efficiency [8]. Noble metals such as Pt are most studied, and other metals such as Au, Pd, Ru, and Fe have been reported to be useful for photocatalytic reactions [4]. Among these various metal ions, Fe(III) has been proved to be a successful doping element [5, 7, 8] where its radii (0.64 Å) is similar to that of Ti(IV) (0.68 Å), hence Fe(III) will easily substitute Ti(IV) into the lattices of TiO2. As Fe(II)/Fe(III) energy level lies close to that of Ti(III)/Ti(IV), Fe(III) can provide a shallow trap for photo-generated hole and electron in anatase. Illuminating Fe(III) can enhance the photogenerated electron–hole pair separation and quantum yield [4, 9]. Consequenly the doping technique seems to be one of the most important factors for controlling the reactivity of Fe(III)-doped titania [10].

Among many existing preparation methods, sol–gel is widely used to prepare metal ion doped TiO2 due to its flexibility to control pore structures and dopant concentration, and high level of chemical purity [5]. The role of iron ions in TiO2 lattice have been discussed extensively in the literature [4, 7, 8, 1113]. Fe(III) ions can act as electron and hole trappers to reduce the photo-generated hole–electron recombination rate and enhance the photocatalytic activity [4, 8, 11, 12].

The main purpose of this work was to investigate of photoactivity of Fe(III)-doped TiO2 nanoparticles in degradation of phenol under UV and visible light irradiation and then compared of results at the optimal condition (pH and catalyst dosage) with P25 TiO2 photoactivity under UV and visible light irradiation. The effects of various experimental parameters on photocatalytic degradation, such as pH, initial concentration of phenol and amount of photocatalyst were examined and optimized. Sol–gel method was selected to synthesis of Fe(III)-doped TiO2 nanoparticles due to its flexibility to control pore structures and dopant concentration, and high level of chemical purity [5]. Also efficiency of UV irradiation alone and amount of phenol adsorption on Fe(III)-doped TiO2 at dark condition was investigated.

Materials and methods

Preparation of the Fe(III)-doped TiO2 photocatalysts

121.775 mL absolute propanol and 62.77 mL TTIP were mixed and stirred for about 10 minutes. For adjusting pH of solution to 3, 2 mL nitric acid was added dropwise to the solution during 30 minutes, stirring was continued at long of this time (30 minutes). Then 8.33 mL double distilled water and 121.775 mL absolute propanol was vigorously stirred and added dropwise to the parent solution. For doped TiO2, Fe(NO3)3.9H2O were added to this solution and stirring continued for 90 minutes. For gel formation and exit of alcohol, the formed sol was stirred by use of a simple magnetic stirrer at room temperature for 24 h; after that the wet gel was dried under vacuum at 85°C for about 12 h and then calcined at 500 ± 50°C for 2–3 h [14].


The X–ray diffraction (XRD) patterns were obtained by a diffractometer (D8 Advanced Bruker AXS) with Cu Kα radiation. Carbon monochromator was used to determine the identity of each phase. A transmission electron microscope (TEM), (FEG Philips CM 200) was applied to observe the morphology of catalysts and estimate the particle size. The surface morphology was observed using a scanning electron microscope (SEM), (Model CamScan MV2300) equipped with an energy dispersive spectroscopy system (EDX, Oxford). In order to prevent the charge build–up during SEM observations, samples were coated with gold.


Photoactivity studies were conducted at the atmospheric pressure and room temperature (25°C). Photocatalytic degradation experiments were carried out in a 2 L Pyrex batch reactor of cylindrical shape (contained 1.5 L phenol solution). The reactor was placed in a box without any pore to prevent of entrance or exist of light from outside and inside. A 27 W low pressure lamp (Trojan) was used as the UV light source that was placed in a quartz jacket (50 mm inside diameter and 300 mm height) and submerged at the center of the cylindrical vessel to provide better irradiation. Visible light source was a 27 W lamp, that to making of similar condition, it also was placed in quartz jacket and submerged at the center of the cylindrical vessel. The distance between the light source and the bottom of the vessel was 1.5 cm. In order to assist the solution homogeneity, a simple magnetic stirrer was used. Phenol and all other chemicals were purchased from Merck Co. (Germany) and were of reagent grade quality.

Stock solution of phenol was first prepared according to directions outlined in Standard Methods [15]. At each experimental stage, 1.5 L solution containing phenol at designed concentration (5, 10, 50, 100 and 500 mg/L) was prepared by dilution of the stock solution with double distilled water; the experiment was then carried out as follows:

Degradation of phenol by Fe(III)-doped TiO2/UV

In the first phase, photocatalytic degradation of up mentioned concentrations of phenol at three different pH (3, 7 and 11) and with three different concentrations of Fe(III)-doped TiO2 (0.25, 0.5 and 1 g/L) under UV irradiation was investigated. For all experiments pH was adjusted by NaOH (1 mol/L) and H2SO4 (0.1 mol/L). Before irradiation, the suspension was stirred continuously in dark for 30 min to ensure adsorption/desorption equilibrium. The irradiation time was 210 minutes and 10 mL of solution was withdrawn from the reactor after certain intervals (every 30 minutes). During the experiments the magnetic stirrer was employed to keep the suspensions uniform. Liquid samples were centrifuged at 6000 r/min for 10 min subsequently and filtered to separate Fe(III)-doped TiO2 particles. The concentration of phenol in the filtrates was measured using UV–vis spectrophotometer (Perkin-Elmer Lambda 25). The UV–vis spectrophotometer was set at a wavelength of 500 nm for analysis of phenol [15]. A quartz cell with a path length of 5 cm was used for spectrophotometric measurements. Based on the results of this stage, the optimum pH and photocatalyst concentration for phenol degradation were achieved. Also the effects of initial phenol concentration on degradation rate and photocatalytic degradation products of phenol under Fe(III)-doped TiO2/UV process were determined.

Degradation of phenol by Fe(III)-doped TiO2/Vis

Photocatalytic degradation of all studied phenol concentrations at optimum conditions (pH and Fe(III)-doped TiO2 concentration) based on the results of former stage, were investigated under Visible light (27 W). The irradiation time was 210 minutes and similar to before stage, after certain intervals sampling was done.

Degradation of phenol solely by UV irradiation

For this phase of the study, degradation of phenol at mentioned concentrations and the same pH (3, 7 and 11) was investigated under UV irradiation.

Phenol adsorption of Fe(III)-doped TiO2

At this stage adsorption of phenol at 10 mg/L concentration on 0.5 g/L Fe(III)-doped TiO2 nanoparticles was examined at dark (the pHs level were the same as before).

Degradation of phenol by TiO2/UV and Vis

In order to compare of photo activity of Fe(III)-doped TiO2 and TiO2 nanocatalysts under UV and Vis light, 10 mg/L of phenol at optimum conditions (pH and nanoparticles concentration) based on the results of first stage, was investigated.

Results and discussion

XRD, SEM EDX and TEM analysis

Figure 1 depicts the XRD spectrum of the Fe (III)-doped TiO2 at atomic ratio of Fe to Ti, 0.034% prepared by the sol–gel method. In Figure 2, a comparison is made between XRD patterns of Fe(III)-doped TiO2 at two atomic ratio (at.%) of Fe/Ti = 0.034 and 0.006. The diffraction picks of the sample shows the presence of both rutile and β TiO2 or nanorod TiO2 phases. No hint of iron containing phases could be resolved in these diffractograms, which suggest that the amounts of Fe were low to be detected by XRD.
Figure 1
Figure 1

XRD pattern of the Fe(III)-doped TiO 2 sample; Fe/Ti = 0.034 at.%, calcination temperature: 500 ± 50°C (R: rutile; B: β-TiO 2 ).

Figure 2
Figure 2

Comparison between XRD patterns of Fe(III)-doped TiO 2 nanopartcles at two atomic ratio (at.%) of Fe/ Ti = 0.034 and 0.006.

The SEM images of Fe (III)-doped TiO2 nanoparticles are shown in Figure 3 which confirm the presence of β TiO2. The particle size distribution determined from SEM images was less than 50 nm. The atomic ratio of Fe to Ti, 0.034% was estimated from the EDX analysis. TEM results (Figure 4 (a and b)) revealed that the sample consisted of agglomerates of particles 10–50 nm in size, which is in general agreement with the SEM findings.
Figure 3
Figure 3

SEM images of the Fe (III)-doped TiO 2 sample from two different sides.

Figure 4
Figure 4

TEM images of the Fe (III)-doped TiO 2 sample (Scale bar=100 nm in panel a; scale bar=50 nm in panel b).

Effect of initial phenol concentration

It is well known that the initial concentration of reactant plays an important role on photodegradation of organic compounds [16]. The influence of initial phenol concentration on photocatalytic degradation at five levels (5, 10, 50, 100 and 500 mg/L) was investigated (Figure 5). As shown in figure, photocatalytic degradation decreases with increasing initial concentration. Decrease in degradation rate at higher concentration is attributed the fact that light absorbed by the phenol is more than that of Fe(III)-doped TiO2. Thus light absorbed is not effective to carry out the degradation [6, 17]. Further, the equilibrium adsorption of phenol on the catalyst surface active site increases and more and more molecules of phenol are adsorbed by the catalyst [6, 17, 18]. As a result, competitive adsorption of OH on the same site decreases and consequently the amount of OH and O2•− on the surface of catalyst decreases. For all initial phenol concentrations, the catalyst dosage, irradiation time and intensity of light were constant. Since the generation of OH does not increase, the probability of phenol molecules to react with OH decreases and hence, a decrease in the degradation efficiency is observed [17]. In fact, with progress in degradation reaction especially at high initial concentration, some intermediates are formed and competitively adsorbed on the catalyst surface and also competitively react with oxidant species [1820]. Moreover, the oxidized intermediate can react with reducing species (e.g. electrons) yielding back phenol which finally results in a decrease of the degradation rate of the substrate [21].
Figure 5
Figure 5

Effect of initial concentration of phenol on the photocatalytic degradation of phenol. Fe(III)-doped TiO2 = 0.5 g/L, pH = 3.

Effect of pH

Figure 6. illustrates the effect of pH on phenol degradation (C/C0, where C0 is the initial phenol concentration and C is the phenol concentration at time t). The highest degradation efficiency occurred at pH = 3 and the lowest degradation occurred at pH = 7. This is attributed to the fact that, condition in addition to OH radicals produced by Fe(III)-doped TiO2/UV process, there are more hydrogen ions at acidic condition and these ions can cause the production of more OH radicals (as a major agent of degradation at photocatalytic reactions) to degrade phenol. This conclusion is similar to the report of Guo et al. [21], which indicated that the H+ ions have important role on OH radicals formation. But higher phenol degradation at pH = 11 in comparison with neutral pH is due to the presence of phenol molecules as negatively charged phenolate species. These anions are more reactive than phenol molecules. Also in alkaline conditions there is an increase in the concentration of OH radicals [22]. Although this increase can be cause of more degradation of phenol at alkaline pH in comparison with neutral pH, but when the concentration of OH is higher in the solution, it prevents the penetration of UV light to reach the catalyst surface. Moreover, high pH favors the formation of carbonate ions which are effective scavengers of OH ions and can reduce the degradation rate [17, 23]. These can be cause of the less degradation of phenol at alkaline pH in comparison with acidic pH.
Figure 6
Figure 6

Effect of pH on photocatalytic degradation of phenol; C 0 = 100 mg/L and Fe(III)-doped TiO 2 = 0.5 g/L.

Effect of catalyst dosage

In slurry photocatalytic processes, catalyst dosage is an important parameter that has been extensively studied. Figure 7. shows the influence of the catalyst concentration on photocatalytic degradation of phenol. As expected with the increase in concentration of catalyst from 0.25 to 0.5 g/L, degradation of phenol increases. According to some of investigations [6, 17], this is due to the fact that the increase in the number of Fe(III)-doped TiO2 particles will increase the number of photons absorbed, the available active sites and consequently the number of the phenol molecule adsorbed. But there was not a considerable increase in phenol degradation when catalyst concentration was increased to 1 g/L. This is attributed to the fact that, agglomeration and sedimentation of it under large catalyst loadings would also take place and available catalyst surface for photon absorption would actually decrease. In fact, the opacity and screening effect of excess Fe(III)-doped TiO2 act as a shield, and consequently hinder the light penetration, causing available surface area loss for light-harvesting and reduction of the catalytic activity, as reported earlier [6, 17, 21, 24, 25]. Therefore, the optimal dosage of Fe(III)-doped TiO2 was determined as 0.5 g/L.
Figure 7
Figure 7

Effect of catalyst dosage on photocatalytic degradation of phenol; C 0 = 50 mg/L and pH = 3.

Photoactivity comparison

Figure 8 shows comparison of photoactivty of Fe(III)-doped TiO2 nanoparticles with two different content of Fe and P25 TiO2 nanoparticles under UV irradiation and visible light on photocatalytic degradation of phenol at optimum condition (pH = 3, catalyst dosage = 0.5 g/L). As shown in the figure, the degradation rate of phenol under Fe(III)-doped TiO2/Vis was higher than degradation rate under TiO2/Vis. This observation confirms that Fe(III) ions play an improvement role in TiO2 structure and increases activity of TiO2 to visible light.
Figure 8
Figure 8

Comparison of photoactivty of Fe(III)-doped TiO 2 and P25 TiO 2 nanoparticles under UV and visible light.

Also figure shows that degradation decreased at atomic ratio of Fe/Ti, 0.006% in compared with Fe/Ti atomic ratio, 0.034%. Whereas the Iron ions at TiO2 lattice can act as both electron and hole traps to reduce the recombination rate and this can increase photocatalytic activity. Therefore the decrease of photoactivity of Fe(III)-doped TiO2 with the decrease of Fe content can be due to the increase of recombination rate of photogenerated electron–hole pairs and also the decreasing of available trapping sites. The study of Hu et al. [9] also indicated that the amount of Fe is very important at photoactivity of Fe(III)-doped TiO2 and high or low level of doping decreases the photocatalytic activity of Fe(III)-doped TiO2.

This figure indicated that the efficiency of phenol degradation at optimum conditions under TiO2/UV process was higher in comparison with Fe(III)-doped TiO2/UV. It can be due to this fact that TiO2 particles are smaller and more uniform than Fe(III)-doped TiO2 particles. Also high efficiency of Fe(III)-doped TiO2 under UV irradiation in degradation of phenol compared with Fe(III)-doped TiO2 under visible light suggests that the excitation energy of the UV is higher than visible light to transit electrons of the valence band to the conduction band. This result is consistent with the results of Shamsun Nahar et al. [26] who reported that UV activity was several times higher than that under visible light irradiation.

Besides results indicated that all calculated values of -ln (C/Co) (Co is the initial phenol concentration and C is phenol concentration at time t) in degradation of phenol under both Fe(III)-doped TiO2/UV and P25 TiO2/UV processes follows a linear model with the elapse of irradiation time. This means that the pseudo first order kinetics relative to phenol is operative (Figure 9).
Figure 9
Figure 9

Pseudo first-order degradation rate of phenol (Fe(III) doped TiO 2 /UV and TiO 2 /UV processes).

However according to the results the degradation behavior of phenol by Fe(III)-doped TiO2 and P25 TiO2 under visible light obeys pseudo second order kinetics (Figure 10).
Figure 10
Figure 10

Pseudo second-order degradation rate of phenol (Fe(III)- doped TiO 2 /Vis and TiO 2 /Vis processes).

kapp values (the apparent kinetic or apparent rate constant (min−1 in pseudo first order and Lmg−1 min−1 in pseudo second order) and correlation coefficients for phenol oxidation are given in the figures. As observed in the Figure 9, kapp increases with increasing of degradation rate (TiO2 > Fe(III)-doped TiO2 (0.034) > Fe(III)-doped TiO2 (0.006)).

Effect of UV irradiation

Investigation of phenol degradation under solely UV irradiation showed that the degradation rate of phenol was low in comparison with using catalyst during 210 minutes. Also phenol adsorption on Fe(III)-doped TiO2 specimen displayed that at these conditions the changes of concentration was negligible (Table 1).
Table 1

Removal efficiency of phenol by Fe-doped TiO 2 /UV, solely UV irradiation and Fe-doped TiO 2 adsorption (percent)

Fe-doped TiO2adsorption

Solely UV irradiation

Fe-doped TiO2/UV

Time (min)






























Photocatalytic degradation of phenol has been carried out over Fe(III)-doped TiO2 (prepared by sol–gel method) and P25 TiO2 under UV irradiation and visible light. Also Effect of pH, catalyst dosage, initial phenol concentration, UV irradiation on degradation efficiency was investigated. Results showed that at appropriate atomic ratio of Fe to Ti (% 0.034) photoactivity of Fe(III)-doped TiO2 nanoparticles increased. At all different initial concentration, highest degradation efficiency occurred at pH = 3 and 0.5 g/L Fe(III)-doped TiO2 dosage. Experimental results showed that the degradation rate decreased with an increase in the initial concentration of phenol. Also photoactivity comparison showed that the photoactivity of Fe(III)-doped TiO2 nanoparticles under visible light was higher than P25 TiO2 particles. However experimental results showed that the P25 TiO2 nanoparticles under UV irradiation had higher efficiency for phenol degradation in comparison with Fe(III)-doped TiO2/UV process. According to the results concentration of Fe(III) ions in doping process has important role in photoactivity of Fe(III)-doped TiO2 nanoparticles. Photocatalytic degradation of phenol by Fe(III)-doped TiO2 and P25 TiO2 nanoparticles under UV irradiation and visible light obey pseudo first order and pseudo second order kinetics subsequently. Also degradation rate under solely UV irradiation was lower in comparison with situations that catalyst was used, and adsorption of phenol on the Fe(III)-doped TiO2 was negligible at dark.



The authors gratefully acknowledge the Nanotechnology Department, Engineering Research Institute, for their support in doing this research.

Authors’ Affiliations

Department of Environmental Health Engineering, School of Public Health and Center for Water Quality Research (CWQR), Institute for Environmental Research (IER), Tehran University of Medical Sciences, Tehran, Iran
Department of Environmental Health Engineering, Tehran University of Medical Sciences, Tehran, Iran
Nanotechnology department, Engineering Research Institute, Tehran, Iran


  1. Adan C, Bahamonde A, Fernandez-Garcıa M, Martınez-Arias A: Structure and activity of nanosized iron-doped anatase TiO 2 catalysts for phenol photocatalytic degradation. Appl Catal B 2007, 72: 11–17. 10.1016/j.apcatb.2006.09.018View ArticleGoogle Scholar
  2. Laoufi NA, Tassalit D, Bentahar F: The degradation of phenol in water solution by TiO 2 photocatalysis in a helical reactor. Glob Nest J 2008, 10: 404–418.Google Scholar
  3. Sakthivel S, Shankar MV, Palanichamy M, Arabindoo B, Bahnemann DW, Murugesan V: Enhancement of photocatalytic activity by metal deposition: characterisation and photonic efficiency of Pt, Au and Pd deposited on TiO 2 catalyst. Water Res 2004, 38: 3001–3008. 10.1016/j.watres.2004.04.046View ArticleGoogle Scholar
  4. Hung WC, Fu SH, Tseng JJ, Chu H, Ko TH: Study on photocatalytic degradation of gaseous dichloromethane using pure and iron Ion-doped TiO 2 prepared by the sol–gel method. Chemosphere 2007, 66: 2142–2151. 10.1016/j.chemosphere.2006.09.037View ArticleGoogle Scholar
  5. Zhou M, Yu J, Cheng B, Yu H: Preparation and photocatalytic activity of Fe-doped mesoporous titanium dioxide nanocrystalline photocatalysts. Mater Chem Phys 2005, 93: 159–163.View ArticleGoogle Scholar
  6. Yang L, Yu LE, Ray MB: Degradation of paracetamol in aqueous solutions by TiO 2 photocatalysis. Water Res 2008, 42: 3480–3488. 10.1016/j.watres.2008.04.023View ArticleGoogle Scholar
  7. Sun L, Li J, Wang CL, Li SF, Chen HB, Lin CJ: An electrochemical strategy of doping Fe(III) into TiO 2 nanotube array films for enhancement in photocatalytic activity. Sol Energy Mater Sol Cells 2009, 93: 1875–1880. 10.1016/j.solmat.2009.07.001View ArticleGoogle Scholar
  8. Zhou M, Yu J, Cheng B: Effects of Fe-doping on the photocatalytic activity of mesoporous TiO 2 powders prepared by an ultrasonic method. J Hazard Mater 2006, 137: 1838–1847. 10.1016/j.jhazmat.2006.05.028View ArticleGoogle Scholar
  9. Hu X, An T, Zhang M, Sheng G, Fu J: Preparation and photocatalytic activities of Fe +3 doped nanometer TiO 2 composites. Res J Chem Environ 2007, 11: 13–21.Google Scholar
  10. Piera E, Tejedor MIT, Zorn ME, Anderson MA: Relationship concerning the nature and concentration of Fe (III) species on the surface of TiO 2 particles and photocatalytic activity of the catalyst. Appl Catal B 2003, 46: 671–685. 10.1016/S0926-3373(03)00288-1View ArticleGoogle Scholar
  11. Zhu J, Zheng W, He B, Zhang J, Anpo M: Characterization of Fe-TiO 2 photocatalysts synthesized by hydrothermal method and their photocatalytic reactivity for photodegradation of XRG dye diluted in water. J Mol Catal A Chem 2004, 216: 35–43. 10.1016/j.molcata.2004.01.008View ArticleGoogle Scholar
  12. Li Z, Shen W, He W, Zu X: Effect of Fe-doped TiO 2 nanoparticle derived from modified hydrothermal process on the photocatalytic degradation performance on methylene blue. J Hazard Mater 2008, 155: 590–594. 10.1016/j.jhazmat.2007.11.095View ArticleGoogle Scholar
  13. Liu S, Chen Y: Enhanced photocatalytic activity of TiO 2 powders doped by Fe unevenly. Catal Commun 2009, 10: 894–899. 10.1016/j.catcom.2008.12.028View ArticleGoogle Scholar
  14. Wade J: An investigation of TiO 2 -ZnFe 2 O 4 nanocomposites for visible light photocatalysis. In MSc Thesis. South Florida University: Electrical Engineering Department; 2005.Google Scholar
  15. Eaton AD, Clesceri LS, Franson MAH: Standard methods for the examination of water & wastewater. Washington DC: American Public Health Association; 2005.Google Scholar
  16. Hong SS, Ju CS, Lim CG, Ahn BH, Lim KT, Lee GD: A photocatalytic degradation of phenol over TiO 2 prepared by sol–gel method. J Ind Eng Chem 2001, 7: 99–104.Google Scholar
  17. Kashif N, Ouyang F: Parameters effect on heterogeneous photocatalysed degradation of phenol in aqueous dispersion of TiO 2 . J Environ Sci 2009, 21: 527–533. 10.1016/S1001-0742(08)62303-7View ArticleGoogle Scholar
  18. Chen D, Ray AK: Photocatalytic kinetics of phenol and its derivatives over UV irradiated TiO 2 . Appl Catal B 1999, 23: 143–157. 10.1016/S0926-3373(99)00068-5View ArticleGoogle Scholar
  19. Sobczynski A, Duczmal L, Zmudzinski W: Phenol destruction by photocatalysis on TiO 2 : an attempt to solve the reaction mechanism. J Mol Catal A Chem 2004, 213: 225–230. 10.1016/j.molcata.2003.12.006View ArticleGoogle Scholar
  20. Mahvi AH, Maleki A, Alimohamadi M, Ghasri A: Photo-oxidation of phenol in aqueous solution: toxicity of intermediates. Korean J Chem Eng 2007, 24: 79–82. 10.1007/s11814-007-5013-4View ArticleGoogle Scholar
  21. Guo Z, Ma R, Li G: Degradation of phenol by nanomaterial TiO 2 in wastewater. Chem Eng J 2006, 119: 55–59. 10.1016/j.cej.2006.01.017View ArticleGoogle Scholar
  22. Bhatkhande DS, Pangarkar VG, ACM Beenackers A: Photocatalytic degradation for environmental applications-a review. J Chem Technol Biotechnol 2002, 77: 102–116. 10.1002/jctb.532View ArticleGoogle Scholar
  23. Akbal F, Onar AN: Photocatalytic degradation of phenol. Environ Monit Assess 2003, 83: 295–302. 10.1023/A:1022666322436View ArticleGoogle Scholar
  24. Paz Y: Preferential photodegradation-why and how? C R Chim 2006, 9(5–6):774–787.View ArticleGoogle Scholar
  25. Mahvi AH, Ghanbarian M, Nasseri S, Khairi A: Mineralization and discoloration of textile wastewater by TiO 2 nanoparticles. Desalination 2009, 239: 309–316. 10.1016/j.desal.2008.04.002View ArticleGoogle Scholar
  26. Shamsun Nahar M, Hasegawa K, Kagaya S: Photocatalytic degradation of phenol by visible light-responsive iron-doped TiO 2 and spontaneous sedimentation of the TiO 2 particles. Chemosphere 2006, 65: 1976–1982. 10.1016/j.chemosphere.2006.07.002View ArticleGoogle Scholar


© Hemmati Borji et al.; licensee BioMed Central Ltd. 2014

This article is published under license to BioMed Central Ltd. This is an Open Access article distributed under the terms of the Creative Commons Attribution License (, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly credited. The Creative Commons Public Domain Dedication waiver ( applies to the data made available in this article, unless otherwise stated.