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Synthesis of Alumina-Grafted Manganese Oxide Particles Using Surfactants through Coprecipitation Method and Their Thermal Properties
Synthesis of Alumina-Grafted Manganese Oxide Particles Using Surfactants through Coprecipitation Method and Their Thermal Properties
Bulletin of the Korean Chemical Society. 2013. Dec, 34(12): 3559-3564
Copyright © 2013, Korea Chemical Society
  • Received : July 29, 2013
  • Accepted : September 05, 2013
  • Published : December 20, 2013
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About the Authors
Boseong Kwon
Jun-Hwan Park
Seong-Cheol Jang
Seong-Geun Oh

Abstract
Alumina particles were grafted onto the surface of manganese oxide particles via the coprecipitation process using surfactant and cosurfactant. The phase of Mn/Al salts (Phase I) and the phase of precipitation agent (Phase II) were prepared in aqueous surfactant solution, separately. Phase II was added into Phase I and the reaction was performed to form the precursors of composites through hydrogen bonding between Mn(OH) 2 and Al(OH) 3 prepared by the reaction of Mn/Al salts with the precipitation agent. The alumina-grafted manganese oxide particles were obtained as a final product after calcination. The concentrations of Al salt and surfactant were varied to investigate their effects on the formation and the crystallinity of composites. In addition, the crystal structure of products could be controlled by changing the calcination temperature. Through thermal analyses, it was found that the thermal stability of manganese oxide was improved by the introduction of alumina on its surface.
Keywords
Introduction
Manganese oxide particles have been applied in many industrial fields such as ion sieves, lithium-ion batteries, high density magnetic storage media, magnetic resonance imaging, drug delivery system, and catalysis due to their unique physical and chemical properties. 1 - 6 Among manganese oxide materials having different Mn oxidation states, Mn 2 O 3 is known as an inexpensive and an environmentfriendly catalyst for the decomposition of NO 7 and N 2 O 8 and the removal of organic pollutants. 9 , 10 Also, Mn 2 O 3 can be used as a precursor for cathode material (LiMn 2 O 4 ) in lithium-ion battery systems. 11 - 13
Alumina is a significant material in the fields of ceramics and catalysts because it has good thermal, chemical, and mechanical properties. 14 , 15 Due to these characteristics, alumina has been widely used as a doping or a supporting material in order to improve the properties of other substances. Xu et al . found that the electrical conductivity of silicate perovskite was enhanced by substitution of alumina into its phase. 16 Makarov and Trontelj investigated the effect of alumina addition on the current-voltage (I-V) characteristics and microstructure of (Na,Mn)-doped WO 3 ceramics. 17 Deraz prepared alumina-doped Mn/Fe oxide solids and studied their thermal behaviors and phase transformation processes. 18 Amini and co-workers synthesized aluminapolyaniline nanocomposites via a template-guided polymerization of aniline using alumina nanosheets and analyzed their conductivity and cyclic voltammetry. 19 Logar et al. fabricated alumina-TiO 2 composites through an in-situ solgel reaction of TiO 2 precursor on the surface of alumina and investigated their photocatalytic activity. 20 Kwon and coworkers studied the improvement in thermal stability of LiMn 2 O 4 cathode material in a Li-ion battery by utilizing a coating of alumina which inhibited Mn dissolution. 21
In this research, alumina-grafted Mn 2 O 3 particles were synthesized through the coprecipitation method using Mn nitrate and Al nitrate as starting materials and ammonium hydroxide as a precipitation agent. In order to control the formation and the crystallinity of alumina-Mn 2 O 3 composite particles, polyoxyethylenesorbitan monolaurate (Tween 20) and tert -butanol ( t -butanol) were used as a nonionic surfactant and a cosurfactant, respectively. In our previous works, we reported that the enhancement in crystallinity of Mn oxide and the thickness-controlled formation of Mn oxide on the surface of silica could be achieved by using a mixture of surfactant and cosurfactant. 22 , 23 In addition, the crystal structure and the degree of crystallization of composites were controlled by varying the calcination temperature from 500 ℃ to 800 ℃. The characterizations of synthesized alumina-grafted Mn2O3 particles were performed by using XRD, FE-SEM, TEM, EDS, and XPS. Moreover, the thermal properties of obtained products were analyzed with TGA and DSC in order to confirm the effect of alumina on the thermal stability of manganese oxide.
Experimental
Materials. As a manganese salt, manganese nitrate hexahydrate was obtained from Junsei Chemical Company. Aluminium nitrate nonahydrate as an aluminium salt was purchased from Yakuri Pure Chemical Company. Polyoxyethylenesorbitan monolaurate (Tween 20) and tert -butanol ( t -butanol), as a nonionic surfactant and a cosurfactant, were obtained from Sigma-Aldrich Chemical Company. As a precipitation agent, ammonium hydroxide (NH 4 OH, 25 wt % ammonia solution) was purchased from Wako Pure Chemical Industries. Acetone, used as a washing agent, was obtained from Duksan Company. All chemical reagents in this study were analytical grade and used without any further purification. The water used in all experiments was double-distilled and deionized from the Milli-Q Plus system (Millipore, France) having 18.2 MΩ·cm electrical resistivity at 25 ℃.
Synthesis of Alumina-Grafted Manganese Oxide Particles. For the formation of alumina-grafted manganese oxide (AMO) particles through the coprecipitation method, the phase of Mn/Al salts (Phase I) and the phase of precipitation agent (Phase II) were prepared in water containing surfactant and cosurfactant, separately. The Phase I included manganese nitrate hexahydrate (3000 mM), aluminium nitrate nonahydrate (0, 3, 30, 60, 300, and 600 mM), Tween 20 (0, 50, 100, and 200 mM), and t -butanol (0 and 500 mM). The Phase II consisted of ammonium hydroxide (11.59 mL) and the same concentrations of Tween 20 and t -butanol added into the Phase I. The volume ratio of Phase I to Phase II was 1:1. After the Phase II was added into the Phase I, the reaction was performed under magnetic stirring at 25 ℃ for 5 h. The formed precursors of the composites were centrifuged and washed with acetone and water several times. The obtained samples were dried in a vacuum oven at room temperature for 24 h. Then, the powders were calcined in a furnace at 700 ℃ for 6 h. Also, the calcination temperature was varied (500, 600, and 800 ℃) to control the crystal phase of AMO particles. The reason for the heat treatment of composite particles at 500 ℃ as the lowest calcination temperature in this research is that aluminium hydroxide can be transformed into alumina through calcination at 500 ℃. 24 - 29
Characterizations. The crystal structure and the crystallinity of the products were analyzed by using X-ray powder diffraction (XRD, Rigaku D/MAX-2500) from 2θ = 10° to 80° with Cu Kα radiation (λ = 1.54056 Å) measured at 40 kV and 100 mA. The morphology and the size of the particles were examined by field emission scanning electron microscopy (FE-SEM, JEOL JSM-6700F and JEOL JSM- 6701F). Before the FE-SEM analysis, the obtained powders were coated with platinum by sputtering at 15 mA for 3 min using a coating machine. For the investigation into the shape of the alumina grafted onto the surface of manganese oxide with transmission electron microscopy (TEM, JEOL JEM- 2100), a drop of sample dispersion was placed on carboncoated copper grids and dried in a drying oven at 40 ℃ for 24 h. The TEM analysis was performed at an acceleration voltage of 130 kV. Energy-dispersive X-ray spectroscopy (EDS), attached to FE-SEM, was used to confirm the chemical composition of AMO composite particles. In order to identify the chemical state of AMO composites, the analysis with X-ray photoelectron spectroscopy (XPS, Theta Probe Base System, Thermo Fisher Scientific Co.) was carried out by using Al Kα radiation as the excitation source. The binding energy of C 1s level (284.5 eV) was used as the internal reference for the data processing of XPS. The thermal analyses, with thermogravimetric analysis (TGA) and differential scanning calorimetry (DSC), were performed by using the instrument (SDT Q600, TA Instruments) in the temper temperature range from 25 ℃ to 1200 ℃, with a heating rate of 10 ℃/min, using pure nitrogen gas at a flow rate of 100 mL/ min.
Results and Discussion
Effect of Al Salt Concentration. Since both Mn(OH) 2 and Al(OH) 3 formed by the reaction between Mn/Al salts and NH 4 OH have very low solubility in water, their precipitation occurs in aqueous solution. 15 , 30 - 36 During this precipitation process, the precursors of composites were prepared through the hydrogen bonding between Mn(OH) 2 and Al(OH) 3 . Then, alumina-manganese oxide composite particles could be obtained after the calcination of precursor powders. Figure 1 illustrates the XRD patterns of particles synthesized by varying the concentration of Al salt in the reaction medium from 0 to 300 mM. From these results, it was confirmed that Mn oxide and AMO particles, formed through calcination at 700 ℃, had the single phase of Mn 2 O 3 (JCPDS number: 41-1442). If aluminium was doped into the inside of crystal structure of manganese oxide, the pure phase of manganese oxide could not be achieved and the other peaks including Al-related characteristic peaks should be observed. However, the Al-related XRD peaks were not found. These results confirm the separate formation of Al(OH) 3 and Mn(OH) 2 and their hydrogen bonding interaction.
In addition, the characteristic peaks of alumina were not observed in any XRD patterns of AMO samples. The first reason for the absence of peaks for alumina is that the smaller amount of Al salt (0-300 mM) was used than that of Mn salt (1500 mM) in the reaction medium. The second reason is the formation of small and finely dispersed alumina particles on the surface of manganese oxide as reported in other studies. 23 , 37 , 38 Also, the crystallinity of Mn 2 O 3 (XRD intensity of (222) plane) decreased as the amount of aluminium salt increased. This indicates that the crystal growth of Mn 2 O 3 was inhibited by grafting the alumina on its surface.
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XRD patterns of particles synthesized by using different amount of Al salt: (a) 0 mM, (b) 1.5 mM, (c) 15 mM, (d) 30 mM, (e) 150 mM, and (f) 300 mM (calcination temperature: 700 ℃).
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FE-SEM images of (a) Mn2O3 and (b) AMO prepared with the addition of 300 mM Al salt (fixed parameter: 700 ℃ calcination).
Figure 2(a) and (b) represent the FE-SEM images of Mn 2 O 3 and AMO particles prepared without Al salt and with 300 mM of Al salt, respectively. When aluminium nitrate was not used, manganese oxide particles, having a larger and irregularly agglomerated structure, were formed. However, smaller and less aggregated particles were synthesized by adding Al salt 300 mM for the formation of AMO composites. This means that the prevention of crystallization of Mn 2 O 3 by alumina occurred with the addition of Al salt. These experimental results are in a good agreement with the previously mentioned XRD data. As illustrated in Figure 3(a) , the pristine Mn 2 O 3 had a smooth surface. On the other hand, it was confirmed that alumina particles were formed on the surface of manganese oxide through the addition of aluminium nitrate 300 mM ( Figure 3(b) ). From these experimental results, it was found that the concentration of aluminium salt was a significant factor in controlling the crystallinity and the size of alumina-manganese oxide composite particles.
Influences of Tween 20 and t-Butanol. In order to increase the attractive interaction of hydrogen bonding between Mn(OH) 2 and Al(OH) 3 , Tween 20 and t -butanol were used as binders. Tween 20 is a nonionic surfactant having three hydroxyl groups in its molecular structure and t -butanol is a cosurfactant inducing a dramatic decrease in the surface tension of water with surfactant. 39 Due to these properties, Tween 20 and t -butanol in aqueous solution can interact and adsorb onto the surface of hydrophobic Mn and Al hydroxides and then AMO could be more successfully synthesized than AMO prepared without surfactants as shown in Figure 3(b) and (c) . 22 , 23 , 40 Compared to Figure 3(b) , it was shown that the more amount of alumina particles were formed on the surface of smaller Mn 2 O 3 particles in Figure 3(c) . This indicates that the smaller Mn 2 O 3 was synthesized by using surfactant and cosurfactant and then alumina particles were formed on the Mn 2 O 3 surface more efficiently. Thus, the alumina particles could be introduced onto the surface of manganese oxide particles more effectively by using surfactant/cosurfactant mixture.
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TEM images of products calcined at 700 ℃: (a) Mn2O3, (b) AMO formed through the addition of 300 mM Al salt, and (c) AMO synthesized by using 300 mM Al salt, 200 mM Tween 20, and 500 mM t-butanol.
As shown in Figure 4 , compared with the XRD intensity of (222) plane of AMO synthesized without Tween 20 and t -butanol, the peak intensity decreased by 3.5% and 9.6%, respectively, with an increase of the amount of Tween 20 in the reaction solution (50 mM and 100 mM). When 200 mM of Tween 20 was used, the lowest XRD intensity was observed (decrease by 46.3%). This indicates that more and smaller alumina particles inducing the inhibition of crystal growth of Mn 2 O 3 were grafted onto the surface of Mn 2 O 3 particles as the amount of Tween 20 was increased. However, characteristic peaks of Mn 3 O 4 (JCPDS number: 24- 0734) were found in the XRD data of AMO formed by using 100 mM and 200 mM of Tween 20. From these results, it was found that the calcination of samples at 700 ℃ was not enough for the phase transformation from Mn 3 O 4 phase into Mn 2 O 3 phase when the AMO particles were prepared by using Tween 20 100 mM and 200 mM with t -butanol 500 mM. Therefore, the calcination temperature was varied to obtain the pure phase of AMO composites.
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XRD patterns of AMO composite particles obtained by using various concentrations of Tween 20: (a) 0 mM, (b) 50 mM, (c) 100 mM, and (d) 200 mM (fixed parameters: Al salt (300 mM), t-butanol (500 mM), and 700 ℃ calcination). When Tween 20 was not used, t-butanol (500 mM) was not added into the reaction medium.
Effect of Calcination Temperature. Figure 5 shows the XRD patterns of AMO composite particles synthesized with variations of calcination temperatures from 500 ℃ to 800 ℃ at fixed amounts of Al salt (300 mM), Tween 20 (200 mM), and t -butanol (500 mM). The crystal structure of manganese oxide materials can be controlled efficiently by changing the temperature of the heat treatment. 41 The single phase of Mn 3 O 4 or the mixed phase of Mn 2 O 3 and Mn 3 O 4 was observed from 500 ℃ to 700 ℃ calcination. In this range of calcination temperature, the XRD intensity of Mn 3 O 4 phase decreased and the crystallinity of Mn 2 O 3 phase increased as the temperature of heat treatment increased. However, the formation of a pure Mn 2 O 3 phase could be accomplished through the calcination of AMO composite particles at 800 ℃. These results were attributed to the existence of a plentiful amount of Tween 20 and t -butanol in the composites. In other words, the higher calcination temperature was needed to remove the entire amount of organic materials. The chemical composition of AMO composite particles prepared by using Al salt (300 mM), Tween 20 (200 mM), and t -butanol (500 mM) through calcination at 800 ℃ was investigated by using EDS ( Figure 6 ). Peaks of Mn and Al were observed clearly and the atomic ratio of Mn to Al in the synthesized products was 34.23:9.65. Also, the chemical states of Mn and Al in the composites were analyzed by using XPS as illustrated in Figure 7 . As shown in the Mn 2p spectrum, the binding energies of Mn 2p 1/2 and Mn 2p 3/2 were 655.78 eV and 643.89 eV, respectively ( Figure 7(a) ). These values are higher than those of pristine Mn 2 O 3 (653.7 eV and 641.9 eV). 42 This increase in the binding energy of Mn 2p was caused by the interaction between manganese oxide and alumina during the synthetic process. 43 In addition, a higher binding energy of Al 2p (75.83 eV), compared to that in the pure Al 2 O 3 (74.60 eV), was observed in the Al 2p spectrum ( Figure 7(b) ). 44 This shift is attributed to the fine dispersion of alumina on the surface of manganese oxide particles. 45 From these results, it is clear that alumina particles were grafted onto the surface of Mn oxide particles successfully.
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XRD patterns of AMO composites calcined at (a) 500 ℃, (b) 600 ℃, (c) 700 ℃, and (d) 800 °C℃. The concentrations of Al salt, Tween 20, and t-butanol were 300 mM, 200 mM, and 500 mM, respectively.
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EDS spectrum of AMO prepared by using Al salt (300 mM), Tween 20 (200 mM), and t-butanol (500 mM) (calcination temperature: 800 ℃).
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XPS data of AMO composite particles synthesized by using Al salt (300 mM), Tween 20 (200 mM), and t-butanol (500 mM) through calcination at 800 ℃: (a) Mn 2p spectrum and (b) Al 2p spectrum.
Thermal Properties of the Synthesized Products. For the verification of the effect of alumina on the thermal properties of manganese oxide, thermal analyses were used. TGA and DSC thermograms of the pristine Mn 2 O 3 and the AMO powders are shown in Figure 8(a) and (b) , respectively. From 25 ℃ to 1200 ℃, the weight loss of Mn 2 O 3 particles was 5.53 wt % and its endothermic peak was found at approximately 815 ℃, which corresponds to the thermal decomposition of Mn 2 O 3 . 46 On the other hand, in the case of AMO composite particles, 6.2 wt % of weight loss was observed and thermal decomposition appeared around 855 ℃. The decreased amount of Mn 2 O 3 during the heating of the sample was similar to that of AMO. However, the shift of thermal decomposition temperature was obvious when alumina particles were introduced onto the surface of manganese oxide particles. This indicates that the thermal stability of Mn 2 O 3 was enhanced by grafting alumina onto its surface. 47 Thus, the improvement in the thermal stability of Mn 2 O 3 could be achieved by the immobilization of finely dispersed alumina particles on the surface of Mn 2 O 3 using surfactant and cosurfactant.
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TGA data (dotted line) and DSC data (solid line) of (a) Mn2O3 calcined at 700 ℃ and (b) AMO calcined at 800 ℃. The AMO was synthesized with Al salt (300 mM), Tween 20 (200 mM), and t-butanol (500 mM).
Conclusion
In summary, alumina-grafted manganese oxide composite particles were synthesized successfully through the coprecipitation process involving hydrogen bonding between Mn(OH) 2 and Al(OH) 3 and heat treatment at different temperatures. By adding Al salt into the reaction medium, the crystal growth of manganese oxide was inhibited and the formation of alumina on its surface was observed. Also, the introduction of alumina onto the surface of manganese oxide could be controlled effectively by using Tween 20 and t -butanol as a surfactant and a cosurfactant. However, a single phase of Mn 3 O 4 or a mixed phase of Mn 2 O 3 and Mn 3 O 4 appeared when large amounts of surfactant and cosurfactant were used. Through the change of calcination temperature, the controls in the crystal phase and the degree of crystallization of products could be achieved. Furthermore, the thermal decomposition temperature of Mn 2 O 3 particles was increased from 815 ℃ to 855 ℃ when the alumina particles were introduced onto their surface via a surfactants-mediated reaction in the coprecipitation process. This result means that the enhancement in the thermal stability of Mn 2 O 3 could be accomplished by grafting alumina particles onto the Mn 2 O 3 surface using surfactant/cosurfactant mixture. Also, it indicates that the prepared Al 2 O 3 -grafted Mn 2 O 3 with the improved thermal stability can be used as an advanced material in various fields. For example, it is expected that the Mn dissolution from LiMn 2 O 4 which is a cathode material of lithium rechargeable batteries at high temperature may be decreased by using the Al 2 O 3 -Mn 2 O 3 composite as a precursor of LiMn 2 O 4 . This may result in the enhancement of the electrochemical performance of batteries.
Acknowledgements
This work was supported by the New & Renewable Energy Program of the Korea Institute of Energy Technology Evaluation and Planning (KETEP) grant funded by the Korea government Ministry of Trade, Industry & Energy (No. 20113010010030).
References
Aronson B. J. , Blanford C. F. , Stein A. 2000 J. Phys. Chem. B 104 449 -    DOI : 10.1021/jp9920343
Ammundsen B. , Paulsen J. 2001 Adv. Mater. 13 943 -    DOI : 10.1002/1521-4095(200107)13:12/13<943::AID-ADMA943>3.0.CO;2-J
Chang Y. Q. , Xu X. Y. , Luo X. H. , Chen C. P. , Yu D. P. 2004 J. Cryst. Growth 264 232 -    DOI : 10.1016/j.jcrysgro.2003.11.117
Gilad A. A. , Walczak P. , McMahon M. T. , Na H. B. , Lee J. H. , An K. , Hyeon T. , Zijl P. C. M. V. , Bulte J. W. M. 2008 Magn. Reson. Med. 60 1 -    DOI : 10.1002/mrm.21622
Shin J. , Anisur R. M. , Ko M. K. , Im G. H. , Lee J. H. , Lee I. S. 2009 Angew. Chem.Int. Edit. 48 321 -    DOI : 10.1002/anie.200802323
Fu X. , Feng J. , Wang H. , Ng K. M. 2009 Nanotechnology 20 375601 (9pp) -    DOI : 10.1088/0957-4484/20/37/375601
Yamashita T. , Vannice A. 1996 J. Catal. 163 158 -    DOI : 10.1006/jcat.1996.0315
Imamura S. , Shono M. , Okamoto N. , Hamada A. , Ishida S. 1996 Appl. Catal. AGen. 142 279 -    DOI : 10.1016/0926-860X(96)00095-6
Yang Z. , Zhang Y. , Zhang W. , Wang X. , Qian Y. , Wen X. , Yang S. 2006 J. Solid State Chem. 179 679 -    DOI : 10.1016/j.jssc.2005.11.028
Cao J. , Zhu Y. , Shi L. , Zhu L. , Bao K. , Liu S. , Qian Y. 2010 Eur. J. Inorg. Chem. 2010 1172 -    DOI : 10.1002/ejic.200901116
Guo S. , Zhang S. , He X. , Pu W. , Jiang C. , Wan C. 2008 J. Electrochem. Soc. 155 A760 -    DOI : 10.1149/1.2965635
Guo H.-J. , Li X.-H. , Wang Z.-X. , Peng W.-J. , Cao X. , Li H.-F. 2009 J. Power Sources 189 95 -    DOI : 10.1016/j.jpowsour.2008.10.099
Wang Y. , Shao X. , Xu H. , Xie M. , Deng S. , Wang H. , Liu J. , Yan H. 2013 J. Power Sources 226 140 -    DOI : 10.1016/j.jpowsour.2012.10.077
Uyeda R. 1991 Prog. Mater. Sci. 35 1 -    DOI : 10.1016/0079-6425(91)90004-D
Park J.-Y. , Oh S.-G. , Paik U. , Moon S.-K. 2002 Mater. Lett. 56 429 -    DOI : 10.1016/S0167-577X(02)00517-7
Xu Y. , McCammon C. , Poe B. T. 1998 Science 282 922 -    DOI : 10.1126/science.282.5390.922
Makarov V. O. , Trontelj M. 2000 Eur. Ceram. Soc. 20 747 -    DOI : 10.1016/S0955-2219(99)00194-6
Deraz N.-A. M. 2003 Thermochim. Acta 401 175 -    DOI : 10.1016/S0040-6031(02)00564-6
Nabid M. R. , Golbabaee M. , Moghaddam A. B. , Mahdavian A. R. , Amini M. M. 2009 Polym. Compos. 30 841 -    DOI : 10.1002/pc.20628
Logar M. , Kocjan A. , Dakskobler A. 2012 Mater. Res. Bull. 47 12 -    DOI : 10.1016/j.materresbull.2011.10.017
Kim W.-K. , Han D.-W. , Ryu W.-H. , Lim S.-J. , Kwon H.-S. 2012 Electrochim. Acta 71 17 -    DOI : 10.1016/j.electacta.2012.03.090
Park J.-H. , Kwon B. , Oh S.-G. 2012 Chem. Lett. 41 1317 -    DOI : 10.1246/cl.2012.1317
Park J.-H. , Oh S.-G. 2011 Colloid Surf. A-Physicochem. Eng. Asp. 390 199 -    DOI : 10.1016/j.colsurfa.2011.09.028
Sivaraj Ch. , Reddy B. P. , Rao B. R. , Rao P. K. 1986 Appl. Catal. 24 25 -    DOI : 10.1016/S0166-9834(00)81255-5
Agrafiotis C. , Tsetsekou A. 2000 J. Eur. Ceram. Soc. 20 815 -    DOI : 10.1016/S0955-2219(99)00218-6
Chuah G. K. , Jaenicke S. , Xu T. H. 2000 Microporous Mesoporous Mater. 37 345 -    DOI : 10.1016/S1387-1811(99)00277-2
Shaheen W. M. , Hong K. S. 2002 Thermochim. Acta 381 153 -    DOI : 10.1016/S0040-6031(01)00652-9
Mercury J. M. R. , Pena P. , Aza A. H. D. , Sheptyakov D. , Turrillas X. 2006 J. Am. Ceram. Soc. 89 3728 -    DOI : 10.1111/j.1551-2916.2006.01191.x
Hollingbery L. A. , Hull T. R. 2010 Thermochim. Acta 509 1 -    DOI : 10.1016/j.tca.2010.06.012
Jang Y.-I. , Wang H. , Chiang Y.-M. 1998 J. Mater. Chem. 8 2761 -    DOI : 10.1039/a806653a
Anilkumar M. , Ravi V. 2005 Mater. Res. Bull. 40 605 -    DOI : 10.1016/j.materresbull.2005.01.009
Gibot P. , Laffont L. 2007 J. Solid State Chem. 180 695 -    DOI : 10.1016/j.jssc.2006.11.024
Liu D. , Garcia B. B. , Zhang Q. , Guo Q. , Zhang Y. , Sepehri S. , Cao G. 2009 Adv. Funct. Mater. 19 1015 -    DOI : 10.1002/adfm.200801515
Varma H. K. , Warrier K. G. K. , Damodaran A. D. 1990 Ceram. Int. 16 73 -    DOI : 10.1016/0272-8842(90)90075-Q
Li J.-G. , Ikegami T. , Lee J.-H. , Mori T. , Yajima Y. 2000 J. Eur. Ceram. Soc. 20 2395 -    DOI : 10.1016/S0955-2219(00)00116-3
Gregory J. , Duan J. 2001 Pure Appl. Chem. 73 2017 -    DOI : 10.1351/pac200173122017
Yu J. C. , Li G. , Wang X. , Hu X. , Leung C. W. , Zhang Z. 2006 Chem. Commun. 2717 -
Xue M. , Huang L. , Wang J.-Q. , Wang Y. , Gao L. , Zhu J.-H. , Zou Z.-G. 2008 Nanotechnology 19 185604 (8pp) -    DOI : 10.1088/0957-4484/19/18/185604
Rosen M. J. 2004 Surfactants and Interfacial Phenomena 3rd ed. John Wiley & Sons, Inc. Hoboken, New Jersey, U.S.A.
Esaka Y. , Kobayashi M. , Ikeda T. , Kano K. 1996 J. Chromatogr. A 736 273 -    DOI : 10.1016/0021-9673(95)01361-X
Chen H. , He J. 2008 J. Phys. Chem. C 112 17540 -    DOI : 10.1021/jp806160g
Strohmeier B. R. , Hercules D. M. 1984 J. Phys. Chem. 88 4922 -    DOI : 10.1021/j150665a026
Kapteijn F. , Langeveld A. D. V. , Moulijn J. A. , Andreini A. , Vuurman M. A. , Turek A. M. , Jehng J.-M. , Wachs I. E. 1994 J. Catal. 150 94 -    DOI : 10.1006/jcat.1994.1325
Chen M. , Wang X. , Yu Y. H. , Pei Z. L. , Bai X. D. , Sun C. , Huang R. F. , Wen L. S. 2000 Appl. Surf. Sci. 158 134 -    DOI : 10.1016/S0169-4332(99)00601-7
Wan H. , Li D. , Dai Y. , Hu Y. , Liu B. , Dong L. 2010 J. Mol. Catal. AChem. 332 32 -    DOI : 10.1016/j.molcata.2010.08.016
Xie X. , Liu W. , Zhao L. , Huang C. 2010 J. Solid State Electrochem. 14 1585 -    DOI : 10.1007/s10008-009-0987-y
Fu L. J. , Liu H. , Li C. , Wu Y. P. , Rahm E. , Holze R. , Wu H. Q. 2006 Solid State Sci. 8 113 -    DOI : 10.1016/j.solidstatesciences.2005.10.019