Effect of the Amount of Water in the Synthesis of B-TiO<sub>2</sub>: Orange II Photodegradation

May-Lozano, M.; Ramos-Reyes, G. M.; López-Medina, R.; Martínez-Delgadillo, S. A.; Flores-Moreno, J.; Hernández-Pérez, I.

doi:https://doi.org/10.1155/2014/721216

International Journal of Photochemistry

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Research Article | Open Access

Volume 2014 | Article ID 721216 | https://doi.org/10.1155/2014/721216

Effect of the Amount of Water in the Synthesis of B-TiO₂: Orange II Photodegradation

M. May-Lozano,¹G. M. Ramos-Reyes,¹R. López-Medina,¹S. A. Martínez-Delgadillo,¹J. Flores-Moreno,¹and I. Hernández-Pérez¹

Academic Editor: Shinya Maenosono

Received28 May 2014

Revised10 Aug 2014

Accepted11 Aug 2014

Published28 Aug 2014

Abstract

A series of boron-doped TiO₂ photocatalysts (2% B-TiO₂) with different water/alkoxide molar ratio were synthesized by conventional sol-gel method. The prepared samples were characterized by BET measurement, X-ray diffraction (XRD), Fourier transform infrared spectroscopy (FTIRS), and diffuse-reflectance UV-vis. The phase anatase was present, but unexpectedly a small amount of rutile phase was formed with low and excess water in the synthesis. Additionally it has been observed that the increase in the molar ratio of water significantly increases the values of band gap energy and the specific surface area. Results showed that degradation of Orange II azo dye increases with surface area, particle size, boron, and water content in photocatalysis. The boron species were introduced in the tricoordinated form.

1. Introduction

Current emission of pollutants from textile industry to different bodies of water is a serious problem, not only since this industry uses large volumes of water, but also because most of these dyes are resistant to the conventional wastewater treatment processes. Different emerging technologies have been tested to try to solve this problem; among them, the advanced oxidation processes such as heterogeneous photocatalysis employing TiO₂ have demonstrated to be the most viable alternative to eliminate several organic contaminants [1, 2]. On the other hand titanium dioxide (TiO₂) has attracted growing scientific interest due to its good chemical and photochemical stability, nontoxicity, availability, low price, or ease of synthesis. However the structural, electronic, and photocatalytic properties of TiO₂ depend on the method of synthesis, while the size, morphology, and microstructure of crystals can be controlled and modified during hydrolysis and condensation steps [2–4]; that is, the water content changes the rate of hydrolysis. In order to improve its photocatalytic activity and shift its absorption band towards the visible region, several attempts have been also made to narrow the band gap energy by doping with various metals ions [5, 6], where it is suggested that the incorporation of metal to TiO₂ structure modifies both the charge carriers recombination rate and the interfacial electron-transfer rate, as well as the generation of recombination sites or the band gap energy, depending on where these ions are located in the TiO₂ structure. On the other hand the doping of TiO2 with non metals atoms such as carbon, nitrogen or boron atoms [7–12] have shown a higher photoactivity performance under visible light irradiation. The photoreactivity of doped TiO₂ is a complex function of the dopant concentration, the energy level, the electronic configuration, the distribution of dopants, the electron donor concentration, and the light intensity [5]. Photocatalysis involves the absorption of photons by a molecule or the substrate to produce reactive electronically excited states and the photocatalysis process by TiO₂ is the generation of electron-hole pairs [5, 13]. Metal and nonmetal dopants influence the photoreactivity of TiO₂ by acting as electron and hole traps and by altering the e⁻/h⁺ pair recombination [13].

The boron (nonmetal) doping to the TiO₂ has been studied in the literature and the doping content as well as the chemical state of boron element affects much the photocatalytic activity of the photocatalyst [14–17]. Likewise, it has been found that the selectivity was improved in degradation of pollutants when boron was used to dope the TiO₂ in photocatalytic reactions.

In this research, the effect of the amount of water on the synthesis of boron-doped TiO₂ photocatalyst by sol-gel method was studied. Few studies are on the water content during the synthesis of TiO₂ [18, 19]. Some authors have found that the higher photoactivity was shown by materials with boron content around 2-3 wt% of boron [15, 20, 21]. Moreover, the boron is a nonmetal that has been less studied doping TiO₂ and the corresponding literature is controversial [17]. According to this, the aim of this study is to find a relationship between the molar ratio water/alkoxide with structural, textural, and photoactivity properties of B-TiO₂ system and to determine the type of boron species present in this system, which can be responsible for the photoactivity.

The B-TiO₂ samples were characterized by X-ray diffraction (XRD), Brunauer-Emmett-Teller (BET) measurement, and diffuse-reflectance UV-vis spectroscopy. The study of the degradation of Orange II was carried out by UV-visible spectrophotometer.

2. Experimental

2.1. 2% B-TiO₂ Oxide Preparation

A series of 2% B-TiO₂ materials and pure TiO₂ (as reference) were prepared by sol-gel method. The B-TiO₂ catalysts were prepared to obtain a content of 2% of boron. During solids synthesis the amount of water was modified (molar ratio water/alkoxide = 0.5, 1, 4, 8, and 16) and the catalysts with different water contents were called BTiO₂-X, in which X indicates the amount of water used in the synthesis (see Table 1). The TiO₂ used as reference was called TiO₂-4 (water/alkoxide = 4). Butanol and titanium isopropoxide were used in a molar ratio alcohol/alkoxide = 10. In a three-neck flask butanol, titanium isopropoxide, and boric acid were mixed at room temperature and an appropriate amount of deionized water was added dropwise into the solution. The X = H₂O/alkoxide molar ratios used were 0.5, 1, 4, 8, or 16 and the solution was kept under stirring for 2 hours. Then, the samples were dried at 100°C in oven for 2 days and finally calcined in muffle furnace at 450°C using a heating rate of 5°C/min for 3 h. Pure TiO₂ was synthesized in the same manner as the sample with water/alkoxide = 4 content, but boric acid was not added to this material during the synthesis.

2.2. Catalysts Characterization

The structural characterization of solids was carried out by powder XRD using a Philips X’Pert diffractometer, operating in mode; samples were analyzed in the range of 20 to 80, degrees using a Cu tube Ka radiation (35 kV, 25 mA) at 2° s⁻¹ scan rate, and wavelength = 0.15405 nm. The surface areas were calculated by BET method and the pore volume was determined by the Barrett-Joiner-Halenda (BJH) method. The study was obtained on a BELSORP-max nitrogen adsorption apparatus at a temperature around 73 K. The sample was treated at 298°C before measurement. The optical properties of materials were determined using an UV-vis (Varian Cary 1 double-beam) spectrophotometer operating in the diffuse reflectance mode. The FT-IR spectroscopic measurements were carried out using a Nicolet Magna spectrophotometer and the spectra were recorded using a KBr wafer technique.

2.3. Degradation of Orange II

2.3.1. Adsorption Experiments

Degradation of Orange II dye was studied by catalytic reaction. The tests were carried out in a stirred batch reactor; it is placed inside an aluminum foil box at room temperature. In a reactor with 25 mL of Orange II solution 0.3 g of the catalyst was added, with an initial concentration of 10 mg/L of dye. The pH was monitored as a function of time and remained close to 7. Reaction monitoring is performed by a Varian Cary 1 UV-vis Spectrophotometer, which determined the amount of degraded dye and the study was carried out for 2 hours. In the quantification, the absorbance was analyzed with the wavelength of 485 nm. Likewise, in all cases, also studies were conducted without catalyst and the dye was not degraded.

2.3.2. Photocatalytic Degradation of Orange II

The same conditions of the catalytic reaction were used, but in this case a UV lamp was placed at the top of the reactor. The reactor was irradiated by the UV light at wavelength 365 nm (lamp power 5 W). Likewise, tests were conducted without catalyst and the dye was not degraded. The pH of solution was 7 and no significant modification of the pH was observed during the experiments. Figure 1 shows the photocatalytic reaction system, which is illustrated as the degradation is carried out using a UV lamp. The UV lamp is placed above the reactor and the reaction was maintained under moderate stirring.

3. Results and Discussion

3.1. Textural Analysis

Figure 2 and Table 1 present the textural properties of BTiO₂-X samples; these results show that the average pore diameter of BTiO₂-X samples was increased with increasing the water content in the synthesis, and a similar behavior occurs with the specific surface area and the pore volume, except the sample with a molar ratio of 16% (Figure 2). The surface area of the TiO₂ without boron (TiO₂-4) is larger than the sample containing boron (BTiO₂-4, see Table 1). The decrease in the specific areas and the pore diameters due to the presence of boron is known in the literature [22]. Štengl et al. [22] found that the specific surface area from the BET had tendency to decrease with increasing content of boron and the pore size distribution indicated conversion from micropores to mesopores with increasing amount of boron, but samples with the highest content of boron became microporous. The size of the pore diameter is different between the sample without boron (TiO₂-4, 30.1 nm) and the sample with boron (BTiO₂-4, 7.1 nm); there is a decrease, which can be attributed to the particle size (see XRD section). There is a strong dependence between the dimensions of the particles and the pore diameters [23]; smaller particles lead to small pores. Figure 2 shows the pore volume of BTiO₂-X samples; the pore volume increases with higher water concentrations in the synthesis.

The particles with different size have different surface area and pore volume [2, 23]. A greater amount of water during the synthesis leads to increase of hydrolysis and condensation allowing an increase in the formation of Ti–O–B and Ti–O–Ti groups [16]. The changes in surface area and pore volume of BTiO₂-X samples are related to the size of the particles or the largest number of particles formed. The specific surface area and anatase phase are important in the photocatalysis of TiO₂ [4]. Therefore, the greater specific surface area for the B-TiO₂ with high water concentration in the synthesis is due to the formation of larger pore volume between aggregated particles (Figure 2).

3.2. XRD

Figure 3 shows the XRD patterns of the solids. In the case of TiO₂-4 only well-defined diffractions of anatase phase (JPCDS 21-1272) can be seen in the pattern at = 25.4° (101), 38.0° (004), 48.2° (200), 54.1° (105), 55.1° (211), 62.8° (204), 68.9° (116), 70.3° (220), and 75.2° (205); the number in the parenthesis indicates the hkl values [24]. The XRD powder patterns of the week rutile phase (JPCDS 21-1276) at = 27.4° (110), 36.1° (101), and 41.2° (122) appeared in BTiO₂-0.5 and BTiO₂-16 with different ratio of water/alkoxide (Figure 3). The weight fractions were calculated from the relative intensities of the strongest peaks for anatase (101) and rutile (110). The average crystal size is presented in Table 2 calculated from the strongest diffraction peak at = 25.4° in the (101) reflection using the Scherrer equation: where is the wavelength of the Cu K radiation used (1.542 Å), is the full width at half maximum of the diffraction angle considered, is the shape factor (0.89), and is the angle of diffraction.

The relative intensity of the peaks of BTiO₂-X samples is weakened and broadened compared with those of the TiO₂ [25] (Figure 3). No crystalline phase assigned to B₂O₃ could be found in any B-TiO₂ catalysts because the concentration of B₂O₃ is so low or the boron species in all samples are highly dispersed on TiO₂ support [26]. As it is well known, sol-gel method is an easy route to obtain high purity nanosized TiO₂ at mild synthesis conditions. It has been well established that the photoactivity of TiO₂ is correlated with its crystallinity and particle size. It can be clearly observed that the crystallinity of these BTiO₂-X samples is different. Table 2 shows that the BTiO₂-4 has the smallest particle size (11 nm) which indicated that the water in the synthesis would generate a distortion in the crystalline structure. These results indicate that the boron acted as an inhibitor for the growth of the anatase nanoparticles, because pure TiO₂ has larger particle size (TiO₂-4 = 14 nm).

The results of XRD show that water content has the greatest effect on the particle size and crystal phase of B-TiO₂. The obtained XRD patterns showed that with the excess amount of water (BTiO₂-16) used in the synthesis the particle size increased, and peaks became more evident and could result in more –OH groups on the surface of nanoparticles. Increasing the water content, the hydrolysis occurs more quickly and much more Ti–O–Ti, Ti–O–B, or Ti–O–H groups are produced. The intensity of the XRD peaks increases with increasing water content in the synthesis, and then this indicates an increase in the crystal phase (anatase).

In similar synthesis conditions regularly pure anatase phase is obtained, but unexpectedly rutile phase was formed. This study found that the rutile phase was present when the particle size is large (BTiO₂-0.5 and BTiO₂-16, see Table 2). This suggests that low and excessive water additive caused a phase transition for the synthesized BTiO₂-16 (Figure 3). Results are consistent with studies where rutile is obtained by thermal methods or boron doped [16, 26, 27], where the rutile has a significant increase when there is an increase in the crystal size (Table 2). The formation of rutile at low water concentration synthesis (BTiO₂-0.5) could be because few groups Ti–O–Ti are formed during the initial synthesis; possibly the bonds Ti–O–Ti are formed during drying or calcination. Moreover, the formation of rutile with excess water in the synthesis (BTiO₂-16) is explained by a structural rearrangement of the catalyst. The anatase to rutile rearrangement involves breaking of two of the six Ti–O bonds in anatase [13]. During the temperature treatment the water excess causes the Ti–O–Ti network to weaken and this facilitates the Ti–O bond breaking and a consequent structural rearrangement to more stable rutile phase. The water in excess is lost by evaporation of solid, leaving behind oxygen vacancies, which accelerates the Ti–O bond breaking and crystallite growth. In this case, boron is certainly helping in the process of rutile formation.

With low water molar ratios (0.5 to 4) the particle size decreases, whereas it increases with a water excess (8–16) (Table 2). The lattice parameters and are affected with possible transitions of the crystal phases (Table 2). Sample BTiO₂-4 prepared with a stoichiometric ratio of water (4H₂O : 1 alkoxide) is slightly distorted as indicated by its parameter (9.42 Å) which is the closest to the data reported for the anatase ( Å) [13].

3.3. Bandgap Determination

UV-vis DRS spectra of BTiO₂-X photocatalysts are shown in Figure 4. The estimates band gap was obtained from extrapolation of the linear region of the Kubelka-Munk transformation of the UV-vis absorption spectra , as shown in Figure 4.

A relevant property to the photocatalytic activity of a semiconductor is its energy band configuration, the photons with energy equal to or higher than the band gap (Eg) promote formation of electron-hole pairs and the redox capabilities of excited-state electrons and holes. The band gaps of the BTiO₂-X samples are presented in Table 2. The band gap energies ( values) suggest a decrease in the intrinsic band gap of B doped TiO₂ [28]. Thus boron incorporation into TiO₂ lattice alters the electronic structure leading to the appearance of intermediate energy level [29, 30]. The band gap energy of BTiO₂-X catalysts is lower than the pure TiO₂ (3.16 eV, ca 380 nm) making it hardly absorbed in visible light region [31–33]. When the TiO₂ surface was modified with the boron ions, adsorption in the visible region increased, and therefore the number of photogenerated electrons and holes increased [34]. With the increase of water in the synthesis the band gap increases (Figure 4). However, when there is an excess of water (BTiO₂-16) the band gap decreases probably due to the formation of large particle size. Figure 4 (top left) shows a marked inverse relationship between particle size and ; it means that particles with larger sizes lead to lower energies, which are in good agreement with the quantum confinement effect.

3.4. FT-IR of B-TiO₂

Figure 5 shows FT-IR spectra of BTiO₂-X photocatalysts. For samples, the bands at 1398 cm⁻¹ can be ascribed to the vibration of tricoordinated interstitial boron (in the form of B³⁺) [20, 27] and the band at 1640 cm⁻¹ is assigned to the stretching of hydroxyl groups and the bending vibration of H₂O adsorbed on the surface of the samples. In the IR spectra of the samples, another small peak appears at 1280 cm⁻¹ which can be ascribed to the stretching vibration of the B–O bonds of boroxol rings [27].

Results reveal that boron is introduced into the titania framework in the form of B–O–Ti bond, corresponding to tricoordinated interstitial boron. The results indicate that the boron species are introduced in the tricoordinated form mainly with high amounts of water used in the synthesis. This indicates that boron is more easily trapped into the titania framework when hydrolysis is favored. The peak at 1640 cm⁻¹ which is related to vibration of water also increases, because larger amount of water in the synthesis results in the formation of higher content of hydroxyl groups in the samples.

3.5. Adsorption Study

The catalytic activity of the BTiO₂-X catalysts for the degradation of Orange II was evaluated without UV irradiation. In all catalysts, the Orange II concentration decreases slightly, indicating that the degradation of Orange II is very limited. The presence of the catalyst without light does not allow an efficient degradation of the dye. In the catalysts, the concentration of water during the synthesis of BTiO₂-X was not a critical factor in the degradation of the dye. The low activity is present in all of the catalysts with or without boron. Figure 6(d*) displays the Orange II concentration as a function of the reaction time of the BTiO₂-4 catalyst without visible light. The activity of other catalysts (BTiO₂-X and TiO₂-4) was very similar.

3.6. Photocatalytic Test

The photocatalytic activity of the B-TiO₂ catalyst for the degradation of Orange II was evaluated with a reactor irradiated by UV light at wavelength 365 nm. Figure 6 displays the Orange II concentration as a function of the reaction time. It can be seen that increasing the amount of water in the synthesis promotes an increase in the Orange dye degradation. An exception is the catalyst BTiO₂-16, where this catalyst with more water shows different behavior (Figure 6(f)). The BTiO₂-8 (e) after 2 hours of reaction showed a slightly higher activity than BTiO₂-16. Also, Figure 6 shows a comparison between the BTiO₂-4 (d) and TiO₂ (TiO₂-4 (a)) photocatalysts, which were synthesized with the same amount of water. BTiO₂-4 photocatalyst containing boron has greater activity than TiO₂-4, which is the catalyst without boron. The above results confirm that the photocatalysis is favored with the boron content and the increase of water in the synthesis. The tricoordinated interstitial boron could also play an important role in the catalytic degradation (see Figure 5). Heterogeneous photocatalysis followed the first order kinetics for Orange II degradation (Figure 7). Kinetics of Orange II photodegradation shows that the photocatalytic activity increases when the molar ratio of water increases from 0.5 to 16. According to the overall results of our investigation, we have found that a high specific surface area and the presence of the anatase phase of TiO₂ are indispensable in the photodegradation of Orange II but are not the only determinant factors; on the contrary, it is important to note that the photocatalytic behavior of B-TiO₂ system can be explained more appropriately, not only considering the values of , but also taking into consideration the type of electronic states induced by the addition of boron. Additionally, it is important to consider that the incorporation of nonmetallic dopants, such as boron, occupying interstitial sites in the anatase TiO₂ structure, can generate reduced Ti³⁺ species, which can act as traps for electrons or holes. As expected, several parameters are related to the photoactivity of the B-TiO₂ nanoparticles, so additional characterization studies are in progress in our laboratory.

4. Conclusions

BET results indicated that specific surface area increased with increasing water content in the synthesis of BTiO₂-X and the powders calcined at 450°C had anatase phase. However, the samples with low and high ratio of water have some content of rutile. The results showed that large amounts of water increase the crystal size and excessive water in the preparation causes a phase transition from anatase to rutile. Increasing water content in the synthesis increases the crystal phase (anatase) and the band gap energies. With the increase of water in the synthesis the band gap increases and the band gap decreases due to the presence of large particle size. The photocatalytic activity of BTiO₂-X powders for the degradation of Orange II increased with increasing water in the synthesis. It is noteworthy that the specific surface area and particle size of BTiO₂-X nanoparticles were dominant factors controlling the photocatalytic activity. As reported in recent times, the results indicate that the boron content improves photocatalytic activity. It is also necessary to mention that boron is more easily trapped inside the TiO₂ when there is more water in the synthesis (in the form of B³⁺).

Conflict of Interests

The authors declare that there is no conflict of interests regarding the publication of this paper.

Acknowledgment

Ricardo López acknowledges the support provided by CONACYT (206771) to perform a postdoctoral fellowship at UAM-A, as well as support for the project CONACYT (CB-201169786-Y).

References

N. Xu, Z. Shi, Y. Fan, J. Dong, J. Shi, and M. Z. C. Hu, “Effects of particle size of TiO₂ on photocatalytic degradation of methylene blue in aqueous suspensions,” Industrial and Engineering Chemistry Research, vol. 38, no. 2, pp. 373–379, 1999.
View at: Publisher Site | Google Scholar
K. Natarajan, T. S. Natarajan, H. C. Bajaj, and R. J. Tayade, “Photocatalytic reactor based on UV-LED/TiO₂ coated quartz tube for degradation of dyes,” Chemical Engineering Journal, vol. 178, pp. 40–49, 2011.
View at: Publisher Site | Google Scholar
H. Lee, M. Choi, Y. Kye, M. An, and I. M. Lee, “Control of particle characteristics in the preparation of TiO₂ nano particles assisted by microwave,” Bulletin of the Korean Chemical Society, vol. 33, no. 5, pp. 1699–1702, 2012.
View at: Publisher Site | Google Scholar
E. Kim, D. S. Kim, and B. Ahn, “Synthesis of Mesoporous TiO₂ and its application to photocatalytic activation of methylene blue and E. coli,” Bulletin of the Korean Chemical Society, vol. 30, no. 1, pp. 193–198, 2009.
View at: Publisher Site | Google Scholar
R. J. Tayade, H. C. Bajaj, and R. V. Jasra, “Photocatalytic removal of organic contaminants from water exploiting tuned bandgap photocatalysts,” Desalination, vol. 275, no. 1–3, pp. 160–165, 2011.
View at: Publisher Site | Google Scholar
R. J. Tayade, R. G. Kulkarni, and R. V. Jasra, “Transition metal ion impregnated mesoporous TiO₂ for photocatalytic degradation of organic contaminants in water,” Industrial and Engineering Chemistry Research, vol. 45, no. 15, pp. 5231–5238, 2006.
View at: Publisher Site | Google Scholar
H. Irie, Y. Watanabe, and K. Hashimoto, “Carbon-doped anatase TiO₂ powders as a visible-light sensitive photocatalyst,” Chemistry Letters, vol. 32, no. 8, pp. 772–773, 2003.
View at: Publisher Site | Google Scholar
S. Yang and L. Gao, “New method to prepare nitrogen-doped titanium dioxide and its photocatalytic activities irradiated by visible light,” Journal of the American Ceramic Society, vol. 87, no. 9, pp. 1803–1805, 2004.
View at: Publisher Site | Google Scholar
H. Liu and L. Gao, “(Sulfur, nitrogen)-codoped rutile-titanium dioxide as a visible-light-activated photocatalyst,” Journal of the American Ceramic Society, vol. 87, no. 8, pp. 1582–1584, 2004.
View at: Publisher Site | Google Scholar
S. U. M. Khan, M. Al-Shahry, and W. B. Ingler Jr., “Efficient photochemical water splitting by a chemically modified n-TiO₂,” Science, vol. 297, no. 5590, pp. 2243–2245, 2002.
View at: Publisher Site | Google Scholar
T. Umebayashi, T. Yamaki, H. Itoh, and K. Asai, “Band gap narrowing of titanium dioxide by sulfur doping,” Applied Physics Letters, vol. 81, no. 3, pp. 454–456, 2002.
View at: Publisher Site | Google Scholar
J. C. Yu, W. Ho, Z. Jiang, and L. Zhang, “Effects of F- doping on the photocatalytic activity and microstructures of nanocrystalline TiO₂ powders,” Chemistry of Materials, vol. 14, no. 9, pp. 3808–3816, 2002.
View at: Publisher Site | Google Scholar
A. L. Linsebigler, G. Lu, and J. T. Yates Jr., “Photocatalysis on TiO₂ surfaces: principles, mechanisms, and selected results,” Chemical Reviews, vol. 95, no. 3, pp. 735–758, 1995.
View at: Publisher Site | Google Scholar
A. C. Pierre, Introduction to Sol-Gel Processing, Kluwer Academic Publishers, 2002.
E. Grabowska, A. Zaleska, J. W. Sobczak, M. Gazda, and J. Hupka, “Boron-doped TiO₂: characteristics and photoactivity under visible light,” Procedia Chemistry, vol. 1, no. 2, pp. 1553–1559, 2009.
View at: Google Scholar
D. Chen, D. Yang, Q. Wang, and Z. Jiang, “Effects of boron doping on photocatalytic activity and microstructure of titanium dioxide nanoparticles,” Industrial and Engineering Chemistry Research, vol. 45, no. 12, pp. 4110–4116, 2006.
View at: Publisher Site | Google Scholar
W. Zhang, X. Li, G. Jia et al., “Preparation, characterization, and photocatalytic activity of boron and lanthanum co-doped TiO₂,” Catalysis Communications, vol. 45, pp. 144–147, 2014.
View at: Google Scholar
C. C. Wang and J. Y. Ying, “Sol-gel synthesis and hydrothermal processing of anatase and rutile titania nanocrystals,” Chemistry of Materials, vol. 11, no. 11, pp. 3113–3120, 1999.
View at: Google Scholar
X. Ding, Z. Qi, and Y. He, “Effect of hydrolysis water on the preparation of nano-crystalline titania powders via a sol-gel process,” Journal of Materials Science Letters, vol. 14, no. 1, pp. 21–22, 1995.
View at: Publisher Site | Google Scholar
W. Zhang, B. Yang, and J. Chen, “Effects of calcination temperature on preparation of boron-doped TiO₂ by sol-gel method,” International Journal of Photoenergy, vol. 2012, Article ID 528637, 8 pages, 2012.
View at: Publisher Site | Google Scholar
W. Zhang, X. Pei, B. Yang, and H. He, “Effects of boron content and calcination temperature on properties of B-TiO₂ photocatalyst prepared by solvothermal method,” Journal of Advanced Oxidation Technologies, vol. 17, no. 1, pp. 66–72, 2014.
View at: Google Scholar
V. Štengl, V. Houškova, S. Bakardjieva, and N. Murafa, “Photocatalytic activity of boron-modified titania under UV and visible-light illumination,” ACS Applied Materials and Interfaces, vol. 2, no. 2, pp. 575–580, 2010.
View at: Publisher Site | Google Scholar
A. Weibel, R. Bouchet, F. Boulc'h, and P. Knauth, “The big problem of small particles: a comparison of methods for determination of particle size in nanocrystalline anatase powders,” Chemistry of Materials, vol. 17, no. 9, pp. 2378–2385, 2005.
View at: Publisher Site | Google Scholar
B. I. Stefanov, Z. Topalian, C. G. Granqvist, and L. Österlund, “Acetaldehyde adsorption and condensation on anatase TiO₂: influence of acetaldehyde dimerization,” Journal of Molecular Catalysis A: Chemical, vol. 381, pp. 77–88, 2014.
View at: Google Scholar
X. Wang, M. Blackford, K. Prince, and R. A. Caruso, “Preparation of boron-doped porous titania networks containing gold nanoparticles with enhanced visible-light photocatalytic activity,” ACS Applied Materials and Interfaces, vol. 4, no. 1, pp. 476–482, 2012.
View at: Publisher Site | Google Scholar
P. Carmichael, D. Hazafy, D. S. Bhachu, A. Mills, J. A. Darr, and I. P. Parkin, “Atmospheric pressure chemical vapour deposition of boron doped titanium dioxide for photocatalytic water reduction and oxidation,” Physical Chemistry Chemical Physics, vol. 15, pp. 16788–16794, 2013.
View at: Google Scholar
N. Feng, A. Zheng, Q. Wang et al., “Boron environments in B-doped and (B, N)-codoped TiO₂ photocatalysts: a combined solid-state NMR and theoretical calculation study,” Journal of Physical Chemistry C, vol. 115, no. 6, pp. 2709–2719, 2011.
View at: Publisher Site | Google Scholar
A. Zaleska, J. W. Sobczak, E. Grabowska, and J. Hupka, “Preparation and photocatalytic activity of boron-modified TiO₂ under UV and visible light,” Applied Catalysis B: Environmental, vol. 78, no. 1-2, pp. 92–100, 2008.
View at: Publisher Site | Google Scholar
C.-H. Wei, X.-H. Tang, J.-R. Liang, and S.-Y. Tan, “Preparation, characterization and photocatalytic activities of boron- and cerium-codoped TiO₂,” Journal of Environmental Sciences, vol. 19, no. 1, pp. 90–96, 2007.
View at: Publisher Site | Google Scholar
C. Yu, J. C. Yu, W. Zhou, and K. Yang, “WO₃ coupled P-TiO₂ photocatalysts with mesoporous structure,” Catalysis Letters, vol. 140, no. 3-4, pp. 172–183, 2010.
View at: Publisher Site | Google Scholar
N. Lu, X. Quan, J. Li, S. Chen, H. Yu, and G. Chen, “Fabrication of boron-doped TiO₂ nanotube array electrode and investigation of its photoelectrochemical capability,” The Journal of Physical Chemistry C, vol. 111, no. 32, pp. 11836–11842, 2007.
View at: Publisher Site | Google Scholar
Y. Wu, M. Xing, and J. Zhang, “Gel-hydrothermal synthesis of carbon and boron co-doped TiO₂ and evaluating its photocatalytic activity,” Journal of Hazardous Materials, vol. 192, no. 1, pp. 368–373, 2011.
View at: Publisher Site | Google Scholar
A. Zaleska, E. Grabowska, J. W. Sobczak, M. Gazda, and J. Hupka, “Photocatalytic activity of boron-modified TiO₂ under visible light: The effect of boron content, calcination temperature and TiO₂ matrix,” Applied Catalysis B Environmental, vol. 89, no. 3-4, pp. 469–475, 2009.
View at: Publisher Site | Google Scholar
N. O. Gopal, H. Lo, and S. Ke, “Chemical state and environment of boron dopant in B,N-codoped anatase TiO₂ nanoparticles: an avenue for probing diamagnetic dopants in TiO₂ by electron paramagnetic resonance spectroscopy,” Journal of the American Chemical Society, vol. 130, no. 9, pp. 2760–2761, 2008.
View at: Publisher Site | Google Scholar

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Copyright © 2014 M. May-Lozano et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

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