Advanced
Preparation, Characterization and Catalytic Activity of Tin Dioxide and Zero-Valent Tin Nanoparticles
Preparation, Characterization and Catalytic Activity of Tin Dioxide and Zero-Valent Tin Nanoparticles
Journal of the Korean Chemical Society. 2012. Aug, 56(4): 484-490
Copyright © 2012, The Korean Chemical Society
  • Received : January 18, 2012
  • Accepted : June 04, 2012
  • Published : August 20, 2012
Download
PDF
e-PUB
PubReader
PPT
Export by style
Article
Author
Metrics
Cited by
TagCloud
About the Authors
H. R. Pouretedal
HR_POURETEDAL@mut-es.ac.ir
A. Shafeie
Department of Chemistry, Islamic Azad University, Shahreza Branch, Shahreza, Iran
M. H. Keshavarz

Abstract
The tin (IV) oxide nanoparticles are prepared by controlled precipitation method and calcined at temperatures of 200-600 ℃. The prepared SnO 2 nanoparticles characterized by XRD patterns, TEM image, IR and UV-Vis spectra. The XRD patterns and TEM image show the tetragonal structure and spherical morphology for SnO 2 nanoparticles, respectively. The photocatalytic activity of the prepared SnO 2 nanoparticles studied in degradation reaction of methylene blue (MB). The results show the size of nanoparticles, band-gap energy and photocatalytic activity of SnO 2 depends on the calcinations temperature. The SnO 2 nanoparticles calcined at 500 ℃ indicated the highest photoreactivity. Also, the zero-valent tin (ZVT) nanoparticles with tetragonal structure are prepared by a reducing agent and used as a catalyst in degradation of MB. In basic pH of 11, the degradation >95% of MB at time 150 min obtained at presence of ZVT nanoparticles.
Keywords
INTRODUCTION
Nanometer range semiconducting materials have been a subject of intense study for last several years due to their size dependent physical and chemical properties below a critical size characteristic of the material. 1 , 2 Photocatalytic property is a interesting property that exhibited by these nanocrystals. This property is size quantization effect which arise due to the increasing quantum confinement of the electrons and holes with diminishing size of the crystallites and the consequent changes in the electronic structures. 3 - 5
The performance and application of semiconductor photocatalyst are largely based on how much its electronic structure and photoinduced charge property at the surface or interface are realized. 5 The studies on the effects of some factors, such as material size, phase composition, structure and dopant species, on the properties of photoinduced charges, including charge transfer behavior and surface states, are of very significance to the preparation and application of semiconductor materials. 4
Semiconductor photocatalysis has attracted increasing attention as an effective technique to eliminate the pollutants in air and wastewater. While many efforts have been made to put this technique into commercial application, many problems arise, such as the fast recombination rate of the photoexcited electron-hole pairs, which is the key factor in the process of semiconductor photocatalysis. 6 , 7 Therefore, there has been much interest in lowering the recombination rate of electron-hole pairs in order to improve the photocatalytic efficiency of semiconductor photocatalysts. 8
Tin (IV) oxide has been a widely studied material over decades because of its wide range of applications as gas sensors, heat mirrors, and transparent electrodes for solar cells, opto-electronic devices and in catalysis. 9 Tin dioxide is an n -type semiconductor crystallizing in tetragonal rutile structure and having the band-gap of about 3.65 eV at bulk state. 10
Applications of Sn (0) nanoparticles are in the preparation of metal films, as Li alloy anodes for rechargeable batteries, as precursors to SnO 2 nanoparticles for use as gas sensors and in heterogeneous catalysis. 11 , 12 However, despite the unique properties of Sn (0) particles in hybrid materials or catalysis, there are only a few reports dealing with their preparation. Evaporation under ultrahigh vacuum of bulk tin followed by condensation of the vapor is by far the most common method for the synthesis of Sn (0) particles. 13 , 14
In this work, the production of SnO 2 and zero-valent tin (ZVT) nanoparticles and characterization of prepared nanoparticles is reported. The effect of calcinations temperature studied on the photocatalytic activity of SnO 2 nanoparticles. The bleaching of methylene blue is also studied in presence of SnO 2 and zero-valent tin (ZVT) nanoparticles.
EXPERIMENTAL
- Synthesis of SnO2and Sn Nanoparticles
All materials were purchased from Merck and Aldrich Company with high purity and analytical grade. The double distilled water was used to prepare the aqueous solutions.
Tin (IV) chloride (SnCl 4 ·5H 2 O) and ammonia solution (1:1) with high purity and analytical grade were used as precursor for synthesis of SnO 2 nanoparticles. A controlled precipitation procedure used to prepare the SnO 2 nanoparticles. Firstly, ammonia solution was added to 50 ml of 0.05 M SnCl 4 solution drop by drop using a decanter with control of sample pH while the mixture was stirred vigorously at 80 ℃ temperature. The pH of sample was controlled at pH of 3-4 and heating and stirring of sample was continued duration 2-3 h. The white precipitate of Sn(OH) 4 was then centrifuged at 3000-4000 rpm, washed with water and ethanol several times. The Sn(OH) 4 nanoparticles were treated by heating in temperature of 80 ℃ for about 4 h. Finally, the white SnO 2 powders were calcined in an oven at temperatures of 200-600 ℃ for about 2 h and then stored for further use.
The zero-valent tin nanoparticles were prepared by SnCl 2 as starting material, sodium borohydride (NaBH 4 ) as reducing agent and Tween80 as surfactant. Sodium borohydride solution (0.06 M) was added to a solution of 0.1 %w/w SnCl 2 and 0.2 %w/w of Tween80 so that one drop was added each of 3-4 s. The Sn nanoparticles was removed by centrifuge with 3000-4000 rpm and then dwashed with water and ethanol several times and dried at 50-60 ℃ at time 2-3 h.
- Characterization of Nanoparticles
The prepared nanoparticles characterized by using X-ray diffraction (XRD) patterns, IR spectra, UV-Vis spectra and TEM images. An X-ray Diffractometer Bruker D8ADVANCE Germany with anode of Cu (wavelength of 1.5406Å of Cu K α ) and filter of Ni apply to record the XRD patterns of nanosized powders. The nanoparticles size was estimated by a JEOL JEM-1200EXII transmission electron microscope (TEM) operating at 120 kV. The supporting grids were formvar-covered, carbon-coated, 200-mesh copper grids. IR-spectra of SnO 2 nanoparticles in range 4000-400 cm -1 were recorded by using Nicolet Impact 400D FT-IR Spectrophotometer . UV-Vis Spectrophotometer Carry-100 used to record absorption spectra of synthesized SnO 2 in range of 200-500 nm. B.E.T (Brunauer-Emmett-Teller) surface area of nanoparticles was determined by using Monosorb Quantochorom.
- Catalytic Activity of Nanoparticles
The photocatalytic activity of SnO 2 nanoparticles studied in the degradation reaction of methylene blue (MB). A photocatalytic reactor system with a mercury low pressure lamp (70 W) with λ max =332 nm and light intensity 22 W/m 2 used to measure photoactivity of SnO 2 nanoparticles. The lamp and the tube were then immersed in the photoreactor cell with a light path of 3.0 cm. The photoreactor was filled with 50 ml sample contain 10.0-50.0 mg/L MB and 0.0-1.2 g/L nanoparticles of SnO 2 . The temperature of photoreactor was kept at 25 ℃ with a watercooled jacket on its outside. A magnetic stirrer applied to ensure that the suspension of the heterogeneous catalyst is uniform during the degradation. Batch experiments were also performed to study the effect of ZVT nanoparticles in degradation of MB. Dye solution (10-50 mg/L) was prepared in deionized water. A 100 mL of MB solution was poured into a 250-mL Erlenmeyer flask and 0.8 g/L of ZVT nanoparticles was added.
The degraded samples collected at regular intervals, filtered through Millipore membrane filters, and centrifuged to remove the particles. The collected samples were analyzed to measure the absorbance of dye by using a UV-Vis spectrophotometer. The decrease of absorbance value of samples at λ max of dye (625 nm) in certain time intervals shows the rate of degradation efficiency (%D) and calculated by Eq (1):
PPT Slide
Lager Image
In Eq (1), C o and C t are the initial concentration and concentration of dye at time t, respectively, and A o and A t are the initial absorbance and absorbance of dye at time t, respectively.
- Kinetic Study of Catalyzed Degradation
The simplified pseudo-first order kinetic model of Langmuir-Hinshelwood (Eq. 2) use to calculate the apparent rate constant of degradation process of dye at initial concentrations 10, 20, 30, 40 and 50 mg/L at pH 11.
PPT Slide
Lager Image
In Eq. (2), C is concentration of the dye (mg/L), t is degradation time (min), k is reaction rate constant (min -1 ), K is the adsorption coefficient of the dye onto the catalyst particles (L/mg) and kapp is the apparent rate constant (min -1 ).
The photocatalytic activity of prepared SnO 2 was also studied under sunlight irradiation and also compared to commercial SnO 2 . The recovery of catalysts and reusability of them were studied at optimum conditions. Also, the MB bleaching catalyzed by nanosized SnO 2 was studied in presence of chloride, bromide, iodide, carbonate, sulfate, phosphate, nitrate anions and magnesium and calcium cations as like a real sample.
RESULTS AND DISCUSSION
- Characterization of SnO2and Zero-valent Tin Nanoparticles
. 1 A- 1 D show the XRD patterns of SnO 2 nanoparticles that are calcined at temperatures of 300, 400, 500 and 600 ℃ in time 2 h, respectively. As seen, in all temperatures, the calcined SnO 2 particles show the diffraction peaks of (110), (101), (200), (111), (211), (220), (002), (311), (112), (301), (202) and (321) at 2q of 26.8, 33.9, 37.9, 39.0, 51.8, 54.8, 57.7, 61.8, 64.8, 66.0, 71.2 and 78.6 o , respectively. Which matches well with JCPDS card # 41-1445 and structure of the crystal is found to be Cassiterite type tetragonal of SnO 2 crystal. 10 , 11 , 15 But, the crystalinity of particles as well as the particles size increase with increasing of calcinations temperature. The XRD patterns show the decreasing of FWHM and thus increasing of particles size of SnO 2 with increasing of calcinations temperature from 300 to 600 ℃. The average crystallite size of the tin dioxide crystal calcined at 300, 400, 500 and 600 ℃ was calculated from Debye-Scherrer formula 15 and found 2.46, 3.48, 5.21 and 8.31 nm, respectively. The TEM micrograph of SnO 2 nanoparticles calcined at 500 oC is shown in . 2 that reveals the morphology and particles size. The monodispersed particles with spherical shape and size <25 nm with an equable distribution except for a little aggregated particulate, is observed in TEM image. On the other hand, the TEM photographs show that tin (IV) oxide powder is nanometer scale, which is in reasonable agreement with the results obtained from the XRD patterns.
PPT Slide
Lager Image
(A) XRD pattern of SnO2 nanoparticles calcined at 300 ℃, (B) XRD pattern of SnO2 nanoparticles calcined at 400 ℃, (C) XRD pattern of SnO2 nanoparticles calcined at 500 ℃. (D) XRD pattern of SnO2 nanoparticles calcined at 600 ℃.
PPT Slide
Lager Image
TEM image of SnO2 nanoparticles calcined at 500 ℃.
The FT-IR spectra of SnO 2 nanoparticles ( . 3 ) show the bands of 600-700 cm -1 that are assigned to the antisymmetric Sn-O-Sn stretching mode of the surface-bridging of oxide. 16 The UV-Vis spectra of SnO 2 calcined at temperatures of 400, 500 and 600 ℃ are shown in . 4 . The red-shift in absorption edge is observed with increasing of temperature. So that, the wavelength of absorption edge is observed at 262, 268 and 275 nm for SnO 2 calcined at temperatures of 400, 500 and 600 ℃, respectively. 17 , 18
PPT Slide
Lager Image
FT-IR spectra of SnO2 calcined at 500 ℃.
PPT Slide
Lager Image
The UV-Vis spectra of SnO2 nanoparticles calcined at 400, 500 and 600 ℃ from down to up.
. 5 and 6 indicate the XRD pattern and TEM micrograph of zero-valent Sn nanoparticles, respectively. The XRD pattern show diffraction peaks that are indexed to a tetragonal cell for tin particles (JCPDS #04-0673). 19 , 20 The crystallite size of tin nanoparticles with Scherrer formula is estimated to be 16.62 nm. The TEM micrograph is also confirmed the formation of tin nanoparticles with size less of 20 nm by reduction of Sn 2+ ions by NaBH 4 at presence of Tween80. Also, the B.E.T analysis indicated that the surface area of zero-valent tin nanoparticles is 15.8 m 2 /g.
PPT Slide
Lager Image
XRD pattern of zero-valent tin nanoparticles.
PPT Slide
Lager Image
TEM image of zero-valent tin nanoparticles.
- Photocatalytic Activity of SnO2Nanoparticles
The photocatalytic activity of SnO 2 can be dependent on the preparation conditions such as time and temperature of treatment and calcination process. The effect of calcination temperature on the photocatalytic activity of SnO 2 in methylene blue degradation is shwon in . 7 . The conditions are 0.1 g/L catalyst, pH of 7 and MB of 10 mg/L. As seen, the highest photocatalytic activity is due to SnO 2 nanoparticles calcined at 500 ℃. As mentioned ( Figs. 1 A to 1 D), the crystallinity and powder size of SnO 2 nanoparticles increase with increasing of calcinations temperature. On the other hand, the band-gap energy is calculated 4.72, 4.62 and 4.50 eV for SnO 2 nanoparticles calcined at temperatures of 400, 500 and 600 ℃, respectively ( . 4 ). The band-gap energy of semiconductors is related to their photocatalytic activity for phtodegradation of pollutants. The greater of redox potential of the photogenerated electron-hole pairs is due to the larger of band-gap energy. Thus, a semiconductor exhibits more redox capacity with increase of band-gap. 21 , 22 Therefore, the most degradation for MB is seen in presence of SnO 2 calcined at 500 ℃ with band-gap energy of 4.62 eV and size of 5.21 nm. The SnO 2 calcined at 600 ℃ show the lower activity despite of having the lower bandgap energy. This decrease is related to increasing of particles size and thus the decrease of surface due to agglomeration of them in 600 ℃ temperature.
PPT Slide
Lager Image
Effect of calcination temperature (℃) on the photocatalytic activity of SnO2 nanoparticles.
PPT Slide
Lager Image
Effect of samples pH on the photocatalytic activity of SnO2 nanoparticles.
The photocatalytic activity of a semiconductor is related to the pH of samples and dosage of it. The effects of pH and amount of SnO 2 nanoparticles are indicated in . 8 and 9 , respectively. The . 8 shows the increasing of photocatalytic activity of SnO 2 nanoparticels with increasing of samples pH. The increasing of pH is due to increase hydroxyl ions concentration to react with the holes and formation hydroxyl radicals. Also, the adsorption of MB molecules with positive charge is occurred on the surface of catalyst in basic solutions because the negative charge of SnO 2 with pH of isoelectric point of 3.5. 22 However, the degradation of MB is inhibited when the pH is greater than 11. Because the hydroxyl ions compete with dye molecules in adsorption on the surface of catalyst. 23 , 24 Degradation efficiency at presence of 0.1, 0.5, 0.8, 1.0 and 1.2 g/L is obtained 78.6, 88.7, 93.5, 89.1 and 84.2, respectively. As seen, the optimized value of SnO 2 nanoparticles is 0.8 g/L. The active sites and density of particles in the area of illumination are increased with increasing of concentration of catalyst in the photodegradation process. 25 , 26 But, at higher catalyst loading of 0.8 g/L, the activated particles deactivate by agglomeration. Also, the decrease of radiation penetration and increase of radiation scattering occur at higher catalyst loading.
Because the influence of many factors and even their mutual effects, the heterogeneous photocatalysis reaction is complicated process. However, the pseudo-first-order rate equation of Langmuir–Hinshelwood (Eq. 2) is used to determine the apparent rate constant, kapp , of MB photodegradation catalyzed by SnO 2 nanoparticles. 27 The apparent rate constants are obtained at range of 10-50 mg/L of methylene blue and collected in 1 . The regression coefficients ( R 2 ) of Langmuir-Hinshelwood kinetic model also indicated in 1 . As seen, the apparent rate constant decrease with increasing of the initial concentration of MB. The decrease of apparent rate constant is due from two reasons: i) increasing the probability of absorption of photons by pollutant molecules and decrease to reach of them to surface of catalyst, ii) increasing of pollutant molecules adsorbed on the surface of catalyst and decrease the active sites to generate of radicals. 28 , 29
The apparent rate constants (kapp, min-1) and regression coefficients (R2) of methylene blue degradation catalyzed by SnO2and zaro-valent Sn nanoparticles calcined at 500 ℃
PPT Slide
Lager Image
The apparent rate constants (kapp, min-1) and regression coefficients (R2) of methylene blue degradation catalyzed by SnO2 and zaro-valent Sn nanoparticles calcined at 500 ℃
Photocatalytic activity of prepared SnO 2 nanoparticles studied also under sunlight irradiation in optimized conditions. The degradation efficiency of MB was 92.7% in time 150 min with apparent rate constant of 21.6×10 -3 min -1 . As a result, the prepared tin (IV) oxide shows photocatalytic activity under sunlight irradiation as well UV-irradation.
The photocatalytic activity of SnO 2 nanoparticles investigated in presence of ions of Ca 2+ , Mg 2+ , Cl - , Br - , I - , CO 3 2- , NO 3 - , SO 4 2- and PO 4 3- with concentration of 1000 mg/L as real samples. The effect of each ion on the nanosized SnO 2 activity is shown in . 9 . However, the photocatalytic activity of SnO 2 nanoparticles diminished in a real sample contains cations and anions. This reduction is due to scavenger effect of active radicals by cations and anions. 4
PPT Slide
Lager Image
The effect of several ions on the photocatalytic activity of SnO2 nanoparticles.
Also, the catalytic activity of tin dioxide nanoparticles is compared to commercially SnO 2 with purity of 99.7%. The degradation of 63.4% of MB is obtained at presence of commercially SnO 2 powder. This reduction of degradation efficiency can be due to difference of surface area and band-gap of SnO 2 nanoparticles and SnO 2 powder. So that, B.E.T (Brunauer-Emmett-Teller) surface area of prepared nanoparticles is obtained 258.3 m 2 /g in comparison of 132.6 m 2 /g of SnO 2 powder. The reusability of SnO 2 nanoparticles studied in four-cycles. In each cycle, the nanoparticles separated, washed with water and ethanol and dried at 80 ℃ and used in next cycles. The D% values obtained 97.0, 93.7, 89.7 and 82.6% in order of four-cycles.
- Catalytic Activity of Zero-valent Tin Nanoparticles
The use of zero-valent metal particles such as Sn for decontamination of common soil and water contaminants has been the subject of many studies. 30 Synthesis of zerovalent tin (ZVT) nanoparticles was achieved by reaction NaBH 4 and SnCl 2 according to the following equation:
PPT Slide
Lager Image
The bleaching of MB solution studied at presence of 0.8 g/L of ZVT nanoparticles and pH 11 like as the optimum conditions in photodegradation reaction. The pseudo firstorder rate constants ( kapp ) of MB degradation by ZVT nanoparticles are calculated using Eq. (2) and indicated in 1 . As seen, the rate constants of MB degradation catalyzed by SnO 2 photocatalyst and ZVT nanoparticles are near to each other. The MB degradation is obtained 97.8 and 92.1% in presence of SnO 2 and Sn nanoparticles, respectively, in duration of 150 min. Thus, reactivity of ZVT nanoparticles in MB degradation process is comparable with photocatalytic activity of SnO 2 nanoparticles in photodegradation reaction of dye in spite of different in degradation mechanism. The holes and electrons are produced by SnO 2 semiconductor under irradiation and the formation of hydroxyl radicals particularly in basic solution apply as an active species in degradation of MB. 31 While, zero-valent tin is a strong reducing agent in basic solutions with Eo =-0.91 and -0.93 V for Sn(II) to Sn(0) and Sn(IV) to Sn(II), respectively (Eq. 4). Furthermore, the most important factor that influences on kapp is the surface area of the zero-valent metal. 32
PPT Slide
Lager Image
This means that it can act as an electron donor that due to reduction of MB molecules in basic solution. The methylene blue is a redox indicator with blue color in oxidized form and colorless in reduced form. The reduction of MB is occurred in acidic solutions and this reduction is due to reduction of absorbance at λ max of it in visible region. While, in basic solution (pH=11) and in presence of ZVT nanoparticles, the MB molecules degrade and the reduction of absorbance in wavelength ranges of 200-300 and 600-700 nm is observed in UV-Vis spectra similar to variations of MB absorption spectra in photodegradation reaction. Thus, Sn (0) nanoparticles as well SnO 2 nanoparticles in photodegradation could be due to destruction of a dye pollutant such as MB.
CONCLUSION
The activity of SnO 2 as a photocatalyst is dependent on the calcinations temperature, dosage of it and pH of samples. Because, the calcinations temperature influence on the band-gap energy and size of particles. The zero-valent tin as reducing agent can be due to degradation of methylene blue in basic solution. In the same conditions of nanoparticles (0.8 g/L of catalyst) and sample pH of 11, the SnO 2 nanoparticles and zero-valent Sn nanoparticles show similar and attractive activity in degradation of methylene blue as a dye pollutant.
References
Robert D. 2007 Catal. Today 122 20 -    DOI : 10.1016/j.cattod.2007.01.060
Jing L. , Fu H. , Wang B. , Wang D. , Xin B. , Li S. , Sun J. 2006 Appl. Catal., B: Environ. 62 282 -    DOI : 10.1016/j.apcatb.2005.08.012
Jing L. , Wang D. , Wang B. , Li S. , Xin B. , Fu H. , Sun J. 2006 J. Mol. Catal., A: Chem. 244 193 -    DOI : 10.1016/j.molcata.2005.09.020
Augugliaro V. , Litter M. , Palmisano L. , Sori J. 2006 J. Photochem. Photobiol. C 7 127 -    DOI : 10.1016/j.jphotochemrev.2006.12.001
Liotta L. F. , Gruttadauria M. , Di Carlo G. , Perrini G. , Librando V. 2009 J. Hazard. Mater. 162 588 -    DOI : 10.1016/j.jhazmat.2008.05.115
Pouretedal H. R. , Norozi A. , Keshavarz M. H. , Semnani A. 2009 J. Hazard. Mater. 162 674 -    DOI : 10.1016/j.jhazmat.2008.05.128
Pouretedal H. R. , Eskandari H. , Keshavarz M. H. , Semnani A. 2009 Acta Chim. Slov. 56 353 -
Wang H. , Baek S. , Lee J. , Lim S. 2009 Chem. Eng. J. 146 355 -    DOI : 10.1016/j.cej.2008.06.016
Dhage S. R. , Gaikwad S. P. , Samuel V. , Ravi V. 2004 Bull. Mater. Sci. 27 221 -    DOI : 10.1007/BF02708509
Kandjani A. E. , Salehpoor P. , Tabrizi M. F. , Arefian N. A. , Vaezi M. R. 2010 Mater. Sci.-Poland 28 377 -
Balan L. , Schneider R. , Billaud D. , Ghanbaj J. 2005 Mater. Lett. 59 1080 -    DOI : 10.1016/j.matlet.2004.12.010
Lee K. T. , Jung Y. S. , Oh S. M. 2003 J. Am. Chem. Soc. 125 5652 -    DOI : 10.1021/ja0345524
Bottani C. E. , Li Bassi A. , Tanner B. K. , Stella A. , Tognini P. , Cheyssac P. , Kofman R. 2001 Mater. Sci. Eng., C, Biomim. Mater., Sens. Syst. 15 41 -    DOI : 10.1016/S0928-4931(01)00214-4
Depero L. E. , Bontempi E. , Sangaletti L. , Pagliara S. 2003 J. Chem. Phys. 118 1400 -    DOI : 10.1063/1.1531074
Krishnakumar T. , Jayaprakash R. , Parthibavarman M. , Phani A. R. , Singh V. N. , Mehta B. R. 2009 Mater. Lett. 63 896 -    DOI : 10.1016/j.matlet.2009.01.032
Anandan K. , Rajendran V. 2010 J. Non-Oxide Glasses 2 83 -
Zhang M. , An T. , Hu X. , Wang C. , Sheng G. , Fu J. 2004 Appl. Catal., A 260 215 -    DOI : 10.1016/j.apcata.2003.10.025
Jiang L. , Sun G. , Zhou Z. , Sun S. , Wang Q. , Yan S. , Li H. , Tian J. , Guo J. , Zhou B. , Xin Q. 2005 J. Phys. Chem. B 109 8774 -    DOI : 10.1021/jp050334g
Zhao Y. , Zhang Z. , Dang H. 2003 Mater. Sci. Eng. A 359 405 -    DOI : 10.1016/S0921-5093(03)00395-2
Noh M. , Kim Y. , Kim M. G. , Lee H. , Kim H. , Kwon Y. , Lee Y. , Cho J. 2005 Chem. Mater. 17 3320 -    DOI : 10.1021/cm0504337
Gu F. , Wang S. F. , Leu M. K. , Qi Y. X. , Zhou G. J. , Xu D. , Yuan D. R. 2003 Inorg. Chem. Commun. 6 882 -    DOI : 10.1016/S1387-7003(03)00135-7
Rodriguez-Santiago V. , Fedkin M. V. , Wesolowski D. J. , Rosenqvist J. , Lvov S. N. 2009 Langmuir 25 8101 -    DOI : 10.1021/la900611u
Pouretedal H. R. , Hosseini M. 2010 Acta Chim. Slov. 57 415 -
Pouretedal H.R. , Kadkhodaie A. 2010 Chin. J. Catal. 31 1328 -    DOI : 10.1016/S1872-2067(10)60121-0
Nezamzadeh-Ejhieh A. , Hushmandrad S. 2010 Appl. Catal., A 388 149 -    DOI : 10.1016/j.apcata.2010.08.042
Nezamzadeh-Ejhieh A. , Salimi Z. 2010 Appl. Catal., A 390 110 -    DOI : 10.1016/j.apcata.2010.09.038
Wang K. , Zhang J. , Lou L. , Yang S. , Chen Y. 2004 J. Photochem. Photobiol. A 165 201 -    DOI : 10.1016/j.jphotochem.2004.03.025
Pouretedal H. R. , Keshavarz M. H. 2010 J. Alloys Comp. 501 130 -    DOI : 10.1016/j.jallcom.2010.04.058
Kudo A. , Niishiro R. , Iwase A. , Kato H. 2007 Chem. Phys. 339 104 -    DOI : 10.1016/j.chemphys.2007.07.024
Lin C. J. , Liou Y. H. , Lo S. L. 2009 Chemosphere 74 314 -    DOI : 10.1016/j.chemosphere.2008.08.046
Hoffmann M. R. , Martin S. T. , Choi W. , Bahnemannt D. W. 1995 Chem. Rev. 95 69 -    DOI : 10.1021/cr00033a004
Satapanajaru T. , Chompuchan C. , Suntornchot P. , Pengthamkeerati P. 2011 Desalination 266 218 -    DOI : 10.1016/j.desal.2010.08.030