# Photocatalytic Degradation of 2,4-Dichlorophenol Using Nanosized Na2Ti6O13/TiO2 Heterostructure Particles

Authors: Zicong Jian; Shaobin Huang; Yongqing Zhang
Journal: International Journal of Photoenergy
 (2013)

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## Abstract

Na2Ti6O13/TiO2 composite particles were synthesized through the hydrolyzation of tetrabutyl titanate in a reverse microemulsion and characterized by thermogravimetry and differential scanning calorimetry (TG-DSC), X-ray diffraction (XRD), and scanning electron microscope (SEM). The photocatalytic property of Na2Ti6O13/TiO2 was evaluated by degradation of 2,4-dichlorophenol(2,4-DCP) under 40 W ultraviolet lamp (λ=365 nm) irradiation and compared with commercial P25-TiO2 in the same condition. The results showed that the synthesized nanobelts Na2Ti6O13/TiO2 heterostructures had typical width from 80 to 100 nm, with thickness less than 40 nm and length up to 5 μm. Such Na2Ti6O13/TiO2 nanosized particles exhibited better photocatalytic activity than that of P25-TiO2, and the degradation rate of 2,4-DCP with initial concentration of 0.02 g/L reached 99.4% at the end of 50 min.


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## Body

## 1. Introduction

Chlorophenols, as significantly harmful environmental pollutants [1–3], are of high toxicity, recalcitrance, bioaccumulation, and persistence in the environment. These compounds, which have been widely used as insecticides, bactericides, herbicides, fungicides, and wood preservative, are difficult to be biodegradated [4, 5]; thus, they are environmental residue. Chlorophenols are considered to be harmful for human health [6, 7] and have been listed as priority pollutants by the US EPA and the EU. Conventional processes [8–10], such as physical, chemical, and biological methods, are used to remove chlorophenols. These techniques, however, are difficult to degrade such refractory biodegradation organic pollutants completely. In recent years, several advanced oxidation processes (AOPs) are put forward for the degradation of chlorophenols [11, 12], including electrochemical anodic oxidation [13, 14], Fenton oxidation [15, 16], and photocatalytic oxidation [17, 18]. Such AOPs generate free radicals, which have strong oxidation capability; thus, the organic pollutants can be destructed easily. Photocatalytic oxidation is one of the AOPs widely used to degrade organic pollutants into harmless final products.The present researches focusing on the materials of photocatalytic oxidation are semiconductors included oxides [19, 20], sulfides [21], nitrides [22], and oxynitrides [23]. These semiconductors provide a promising strategy for environmental pollutants control or hydrogen generation. One of the most important photocatalysts is titanium dioxide (TiO2) [24, 25], which has been known as the most preferable photocatalyst due to its stability, nontoxicity, and low cost. However, there are disadvantages, such as low separation rate of the photoexcited electrons and holes, which lead to the limited quantum efficiency of TiO2. Therefore, many scholars have been devoted to prepare a TiO2 photocatalyst that is capable of efficient generation and separation of photoinduced electron-hole pairs. These investigations include doping with cation or anion ions, coupling TiO2 with other semiconductors [26], depositing precious metal, and so on. For example, Yu et al. synthesized novel carbon self-doped TiO2 sheets with exposed {001} facets, which exhibited an excellent absorption in the whole visible-light region, due to the exposed {001} facets which were much more reactive than the thermodynamically more stable {101} surface [27].It was reported [28, 29] that alkali titanates, general formula as A2O–nTiO2 (3≤n≤8, A = Li, Na, K), exhibited good photocatalytic activity and ion conductivity. According to Billik et al. [30], Na2Ti6O13 could be prepared by mechanochemical reaction of the TiC14–Na2SO4·10H2O–Na2CO3 mixture followed by a molten salt synthesis.The present work is based on the idea that heterostructures of Na2Ti6O13 coupling with TiO2 would perform outstanding photocatalytic properties. To our knowledge, Na2Ti6O13 is hard to be obtained at the temperature lower than 800°C. Since the costs are high and the process of crystallization is difficult to control, we proposed a simple and rapid method to obtain such heterostructures. In this paper, x-Na2Ti6O13/TiO2 (x=0, 1.0, 1.5, 2.5) composite particles were synthesized in reverse microemulsions system at room temperature and ambient pressure followed by heat treatments from 500°C to 800°C. The photocatalytic activity of these samples was evaluated and compared with the commercial P25-TiO2 on the degradation of 2,4-DCP in aqueous solution under ultraviolet light irradiation. The forming conditions of Na2Ti6O13/TiO2 heterostructures and their photocatalytic property were discussed based on characterization results.


## 2. Materials and Methods

### 2.1. Preparation of Na2Ti6O13/TiO2 Composite Particles

The nanostructured Na2Ti6O13/TiO2 photocatalyst was synthesized by a microemulsion approach. The n-hexanol (chemically pure, CP) was considered as both the oil phase and the cosurfactant, and cetyltrimethylammonium bromide (CTAB) (CP) was chosen as the surfactant. Sodium hydroxide (CP) solution with specific molar concentration of 0, 1.0, 1.5, and 2.5 mol/L, respectively, acted as the water phase.Stock solutions ofn-hexanol and CTAB with a quality ratio of 2 : 1 were mixed under stirring. Sodium hydroxide solution was added drop-wise to the glass vial containing the mixtures aforementioned, and the mass of sodium hydroxide solution was 10% of the bulk quality. After stirring for 60 min, a steady microemulsion was obtained. A desired amount of Ti(OBut)4 (CP) was injected into the microemulsion. The resultant suspension was stirred for 120 min until it became milk white. In the system, the quality ratio of CTAB to Ti(OBut)4 was 2.5 : 1. The solid products were separated in a centrifuge at 4000 r min−1 and washed with anhydrous ethanol (AP) to remove the organic compounds and surfactants from the particles and dried in an oven at 105°C for 12 h. The obtained precursors were calcined for 3 h at 500, 600, 700, and 800°C, respectively. The final products were milled before characterization. Samples were labeled as x-Na2Ti6O13/TiO2, where x=0, 1.0, 1.5, and 2.5 mol/L was the molar concentration of NaOH. All the products were synthesized at room temperature and ambient pressure without thermal treatment, if not otherwise stated.


### 2.2. Characterization of Na2Ti6O13/TiO2 Composite Particles

X-ray powder diffraction (XRD) patterns were recorded on a Bruker D8 ADVANCE X-ray diffractometer with Cu Kα radiation (λ=0.15406 nm) at a high voltage of 40 kV with a step of 0.02°. The particle size and morphology were observed on a field emission scanning electron microscope (FESEM, LEO 1530 VP, Germany). The TG analysis of precursors was measured by an STA449c/1/41G thermal analyzer (Netzsch, Germany).


### 2.3. Photocatalytic Studies

The photocatalytic reaction was conducted in a 200 mL cylindrical glass vessel fixed in the XPA photochemical reactor (Nanjing Xujiang Machine-electronic Plant). The XPA reactor consists of a magnetic stirrer, quartz cool trap, and a condenser to keep the reaction temperature steady and to prevent the evaporation of water. A 40 W Hg lamp (365 nm) was used as the UV light source. 2,4-Dichlorophenol (2,4-DCP) with certain concentration(0.02 g/L) was used as reactant.Prior to illumination, various quantities of photocatalyst powder were dispersed in 200 mL reaction solution and stirred in the dark for 30 min in order to obtain an optimally dispersed system and to ensure complete adsorption/desorption equilibration. Subsequently, the Hg lamp was turned on, and the catalysts began to decompose 2,4-DCP.During the course of illumination, 1.0 mL of suspensions was withdrawn periodically from the reactor and filtered (Millipore Millex25 0.45 mm membrane filter) previously to HPLC measurements.The concentrations of 2,4-DCP were monitored with a high performance liquid chromatography (HLPC, Shimadzu, Japan) equipped with a UV detector (SPD-10AV) and a Symmetry C18 column (250 mm × 4.6 mm). Mobile phase: methanol (HPLC grade) and water (80 : 20, volume); flow rate: 1.0 mL/min; injection volume: 20μL; absorbance detection: 284 nm. The concentration of the remaining 2,4-DCP was measured by its area of characteristic peak (A). The degradation ratio (X) of the reactant was calculated using X(%)=100(A0-At)/A0.


## 2.1. Preparation of Na2Ti6O13/TiO2 Composite Particles

The nanostructured Na2Ti6O13/TiO2 photocatalyst was synthesized by a microemulsion approach. The n-hexanol (chemically pure, CP) was considered as both the oil phase and the cosurfactant, and cetyltrimethylammonium bromide (CTAB) (CP) was chosen as the surfactant. Sodium hydroxide (CP) solution with specific molar concentration of 0, 1.0, 1.5, and 2.5 mol/L, respectively, acted as the water phase.Stock solutions ofn-hexanol and CTAB with a quality ratio of 2 : 1 were mixed under stirring. Sodium hydroxide solution was added drop-wise to the glass vial containing the mixtures aforementioned, and the mass of sodium hydroxide solution was 10% of the bulk quality. After stirring for 60 min, a steady microemulsion was obtained. A desired amount of Ti(OBut)4 (CP) was injected into the microemulsion. The resultant suspension was stirred for 120 min until it became milk white. In the system, the quality ratio of CTAB to Ti(OBut)4 was 2.5 : 1. The solid products were separated in a centrifuge at 4000 r min−1 and washed with anhydrous ethanol (AP) to remove the organic compounds and surfactants from the particles and dried in an oven at 105°C for 12 h. The obtained precursors were calcined for 3 h at 500, 600, 700, and 800°C, respectively. The final products were milled before characterization. Samples were labeled as x-Na2Ti6O13/TiO2, where x=0, 1.0, 1.5, and 2.5 mol/L was the molar concentration of NaOH. All the products were synthesized at room temperature and ambient pressure without thermal treatment, if not otherwise stated.


## 2.2. Characterization of Na2Ti6O13/TiO2 Composite Particles

X-ray powder diffraction (XRD) patterns were recorded on a Bruker D8 ADVANCE X-ray diffractometer with Cu Kα radiation (λ=0.15406 nm) at a high voltage of 40 kV with a step of 0.02°. The particle size and morphology were observed on a field emission scanning electron microscope (FESEM, LEO 1530 VP, Germany). The TG analysis of precursors was measured by an STA449c/1/41G thermal analyzer (Netzsch, Germany).


## 2.3. Photocatalytic Studies

The photocatalytic reaction was conducted in a 200 mL cylindrical glass vessel fixed in the XPA photochemical reactor (Nanjing Xujiang Machine-electronic Plant). The XPA reactor consists of a magnetic stirrer, quartz cool trap, and a condenser to keep the reaction temperature steady and to prevent the evaporation of water. A 40 W Hg lamp (365 nm) was used as the UV light source. 2,4-Dichlorophenol (2,4-DCP) with certain concentration(0.02 g/L) was used as reactant.Prior to illumination, various quantities of photocatalyst powder were dispersed in 200 mL reaction solution and stirred in the dark for 30 min in order to obtain an optimally dispersed system and to ensure complete adsorption/desorption equilibration. Subsequently, the Hg lamp was turned on, and the catalysts began to decompose 2,4-DCP.During the course of illumination, 1.0 mL of suspensions was withdrawn periodically from the reactor and filtered (Millipore Millex25 0.45 mm membrane filter) previously to HPLC measurements.The concentrations of 2,4-DCP were monitored with a high performance liquid chromatography (HLPC, Shimadzu, Japan) equipped with a UV detector (SPD-10AV) and a Symmetry C18 column (250 mm × 4.6 mm). Mobile phase: methanol (HPLC grade) and water (80 : 20, volume); flow rate: 1.0 mL/min; injection volume: 20μL; absorbance detection: 284 nm. The concentration of the remaining 2,4-DCP was measured by its area of characteristic peak (A). The degradation ratio (X) of the reactant was calculated using X(%)=100(A0-At)/A0.


## 3. Results and Discussion

### 3.1. Characterization of Na2Ti6O13/TiO2 Composite Particles

The TG-DSC curves for 1.5-Na2Ti6O13/TiO2 precursor are shown in Figure 1. The TG results indicate that the sample lost weight slowly from 25 to 80°C, which could be attributed to the volatilization of physically absorbed oil phase and water. There is a sharp weight loss from 80 to 270°C due to the evaporation of water and the desorption of hexanol (boiling point 156°C), and this is supported by the exothermic peak at 119°C in the DSC curve. As the temperature increases from 270 to 320°C, the sample exhibits further and faster weight loss, which corresponds to the burning of residual surfactant, and this could be explained well by an exothermic peak detected in the DSC curve at 272°C. Beyond 320°C, the curve becomes almost flat, implying that the weight of the precursor has little changed. Combining with the DSC curve, phase transition may be the mainly occurring at this process.Figure 1
TG-DSC curves of 1.5-Na2Ti6O13/TiO2 precursor.The DSC curve of the precursor shows two main exothermic peaks: one of which is the evaporation of water and oil phase, and the other is the decomposition of surfactant as discussed earlier. Three endothermic peaks appear at 341, 406, and 566°C, which could be ascribed to the crystallization of TiO2 from amorphous to anatase, and from anatase to rutile, and the crystallization of Na2Ti6O13, respectively.The typical SEM images of 1.5-Na2Ti6O13/TiO2 are presented in Figure 2. As can be seen in Figure 2(a), the 1.5-Na2Ti6O13/TiO2 precursor without heat treatment is amorphous and bonding loosely, appearing to be large and bubbles-like, which might reflect the situation of the water droplet in the microemulsion. While the precursors were calcined at 500 or 600°C, the loose bubbles-like structures break into small particles, and the diameter was less than 100 nm. Comparing with Figures 2(b) and 2(c), particles calcined at 600°C dispersed better than that at 500°C. Subcircular and well-crystallized particles with diameter of around 50 nm were obtained in Figure 2(c). Combining with XRD pattern, it can be known that the precursors were dehydrated and they would be transformed into the crystalline anatase and Na2Ti6O13, under calcinations at 500 and 600°C, respectively.SEM image of Na2Ti6O13/TiO2 composite particles. (a) 1.5-Na2Ti6O13/TiO2 precursor; (b) 1.5-Na2Ti6O13/TiO2 calcined at 500°C; (c) 1.5-Na2Ti6O13/TiO2 calcined at 600°C; (d) 1.5-Na2Ti6O13/TiO2 calcined at 700°C; (e) 1.5-Na2Ti6O13/TiO2 calcined at 800°C.
(a)
(b)
(c)
(d)
(e)The SEM micrographs of Na2Ti6O13 powders calcined at 700 and 800°C are shown in Figures 2(d) and 2(e). The belt-like morphology of the product calcined at 700°C is well documented in the SEM image shown in Figure 2(d). Na2Ti6O13 nanobelts have typical width from 80 to 100 nm, thickness less than 40 nm, and length up to 5 μm. The phase of the obtained sample was supported by XRD. It is also found that the nanobelts were fractured under calcination at 800°C, though the fragments have higher degree of crystallinity, as shown obviously in Figure 2(e).Figure3 shows the XRD patterns of 1.5-Na2Ti6O13/TiO2 precursor and the composite particles which were calcined for 3 h at 500, 600, 700, and 800°C, respectively. As can be seen, no characteristic diffraction peaks are observed from the pattern of precursor, indicating that the precursor is amorphous. The XRD pattern of 1.5-Na2Ti6O13/TiO2 calcined at 500°C shows a strong peak at 2θ=25.34° and a weak one at 2θ=27.50°, implying that TiO2 is crystallized as the anatase and rutile phase coexistence after calcined at 500°C. Curves of 1.5-Na2Ti6O13/TiO2 calcined at 600–800°C show that Na2Ti6O13 could be obtained by calcining the microemulsion-resulted precursor at relatively low temperature (<800°C). The pattern of 1.5-Na2Ti6O13/TiO2 calcined at 600°C shows the characteristic diffraction peak of both rutile and Na2Ti6O13; however, the samples calcined at 700, and 800°C have no characteristic diffraction peak of TiO2.Figure 3
XRD pattern of 1.5-Na2Ti6O13/TiO2 composite particles: (a) 1.5-Na2Ti6O13/TiO2 precursor; (b) 1.5-Na2Ti6O13/TiO2 calcined at 500°C; (c) 1.5-Na2Ti6O13/TiO2 calcined at 600°C; (d) 1.5-Na2Ti6O13/TiO2 calcined at 700°C; (e) 1.5-Na2Ti6O13/TiO2 calcined at 800°C.Although the formation mechanisms of the titanate nanobelts are still under debate, we believe that the formation of Na2Ti6O13 nanobelts may be affected by the crystallite size or chemical activity of the precursor and the condition of crystallization. In our work, the precursor is considered to be Ti(OH)4. Under heat treatment, –OH from the surface of Ti(OH)4 combined with each other to produce H2O and –O–Ti–bond. With the calcined temperature increase and the existence of Na+, more –OH were removed and Na–O–Ti–bonds were formed, which means that Na2Ti6O13 were formed. As it was supported by SEM and XRD, at the temperature of 600°C, the crystallization of Na2Ti6O13 which are the prerequisites for the nanobelts formation was obtained. According to Dominko et al. [31], Na2Ti6O13 crystallizes in a monoclinic crystalline structure with continuous tunnel channels along c axis (Figure 4). Such tunnel channels suppressed the possible delamination into sheets or nanotubes [30].Figure 4
Schematic representation of the crystal structure of Na2Ti6O13 along a-axis [31] (octahedral: Ti–O6; spheres: Na).In a word, the amorphous precursor forms anatase and rutile phase at 500°C, and the anatase phase transits into rutile phase at 600°C; meanwhile, Na2Ti6O13 crystal formed. However, when the temperature is higher than 600°C, no TiO2 exists. Thus, the optimum temperature for heterostructure particles is 600°C.


### 3.2. Degradation Activities of Na2Ti6O13/TiO2

In this investigation, 2,4-dichlorophenol(2,4-DCP) was chosen as a representative model pollutant (C0=20 mg/L, 200 mL) to study the adsorption and photocatalytic activity of the Na2Ti6O13/TiO2 composite particles (10 mg) under UV-light (40 W Hg lamp) irradiation and the results can be seen in Figure 5. The degradation efficiency of 2,4-DCP increased with time. After 50 min UV-light irradiation, the degradation rate reached 99.4%, 96.0%, 83%, and 56.2%, by the photocatalyst synthesized in 1.5, 1.0, 0, and 2.5 mol/L sodium hydroxide solution, respectively, while the commercial P25 has the degradation rate of 76.9%, and the degradation rate of 11.5% was obtained without any photocatalysts.Figure 5
Effects of ratio of Na2Ti6O13/TiO2 calcined at 600°C: (a) 1.5-Na2Ti6O13/TiO2; (b) 1.0-Na2Ti6O13/TiO2; (c) 0-Na2Ti6O13/TiO2; (d) commercial P25; (e) 2.5-Na2Ti6O13/TiO2; (f) blank.The different molar ratios of Na2Ti6O13/TiO2 have significant differences in photoactivity. While the ratio raises from 0 to 1.5, the degradation rate raises obviously; however, the 2.5 sample has the weakest activity. The sample of 1.5-Na2Ti6O13/TiO2 has the best efficiency for decomposing 2,4-DCP, which is about 1.3 times higher than commercial P25. Thus, 1.5-Na2Ti6O13/TiO2 was chosen as the standard photocatalyst.Figure6 shows the photoactivity of 1.5-Na2Ti6O13/TiO2 calcined at different temperatures. After 50 min UV-light irradiation, the degradation rate reached 99.4%, 83.8%, 56.3%, and 37.2%, by the photocatalyst calcined at 600, 500, 700, and 800°C, respectively. The commercial P25 has the degradation rate of 76.9%, and the blank experiment showed the degradation rate of 11.5%.Figure 6
Effects of calcined temperature of 1.5-Na2Ti6O13/TiO2: (a) 600°C (b) 500°C; (c) commercial P25; (d) 700°C; (e) 800°C; (f) blank.Combining with SEM and XRD characterization, the temperature of calcinations determines the crystal line, the morphology, and the components of the photocatalyst. At 500°C the component of the photocatalyst mainly is TiO2. Such photocatalyst formed by anatase and rutile exhibits a general photoactivity. At 600°C Na2Ti6O13/TiO2 heterostructure formed and the particles were well crystalline. These microstructures improve the separation efficiency of photogenerated electrons and holes, increase the contact area, and allow more efficient transport for the reactant molecules to get to the active sites on the framework walls, enhance the adsorption of light, and reduce the reflection of light. Therefore, the photocatalytic activity was enhanced.In order to observe the photo degradation process of 2,4-DCP, the concentrations of possible intermediates, such as phenol, 4-CP, and 2-CP, were measured with HPLC. Figure7 represents these three intermediates generation from the system. It is clear that 2,4-DCP was not completely mineralized and was residue as phenol and chlorophenol; meanwhile, the concentration of phenol is much higher than 4-CP and 2-CP. After 40 min photoreaction, the concentration of these three intermediates reduced obviously, indicating that Na2Ti6O13/TiO2 heterostructure is capable of degrading phenol and chlorophenol.Figure 7
Variation of (a) phenol; (b) 4-CP; (c) 2-CP concentration during the photo degradation.


## 3.1. Characterization of Na2Ti6O13/TiO2 Composite Particles

The TG-DSC curves for 1.5-Na2Ti6O13/TiO2 precursor are shown in Figure 1. The TG results indicate that the sample lost weight slowly from 25 to 80°C, which could be attributed to the volatilization of physically absorbed oil phase and water. There is a sharp weight loss from 80 to 270°C due to the evaporation of water and the desorption of hexanol (boiling point 156°C), and this is supported by the exothermic peak at 119°C in the DSC curve. As the temperature increases from 270 to 320°C, the sample exhibits further and faster weight loss, which corresponds to the burning of residual surfactant, and this could be explained well by an exothermic peak detected in the DSC curve at 272°C. Beyond 320°C, the curve becomes almost flat, implying that the weight of the precursor has little changed. Combining with the DSC curve, phase transition may be the mainly occurring at this process.Figure 1
TG-DSC curves of 1.5-Na2Ti6O13/TiO2 precursor.The DSC curve of the precursor shows two main exothermic peaks: one of which is the evaporation of water and oil phase, and the other is the decomposition of surfactant as discussed earlier. Three endothermic peaks appear at 341, 406, and 566°C, which could be ascribed to the crystallization of TiO2 from amorphous to anatase, and from anatase to rutile, and the crystallization of Na2Ti6O13, respectively.The typical SEM images of 1.5-Na2Ti6O13/TiO2 are presented in Figure 2. As can be seen in Figure 2(a), the 1.5-Na2Ti6O13/TiO2 precursor without heat treatment is amorphous and bonding loosely, appearing to be large and bubbles-like, which might reflect the situation of the water droplet in the microemulsion. While the precursors were calcined at 500 or 600°C, the loose bubbles-like structures break into small particles, and the diameter was less than 100 nm. Comparing with Figures 2(b) and 2(c), particles calcined at 600°C dispersed better than that at 500°C. Subcircular and well-crystallized particles with diameter of around 50 nm were obtained in Figure 2(c). Combining with XRD pattern, it can be known that the precursors were dehydrated and they would be transformed into the crystalline anatase and Na2Ti6O13, under calcinations at 500 and 600°C, respectively.SEM image of Na2Ti6O13/TiO2 composite particles. (a) 1.5-Na2Ti6O13/TiO2 precursor; (b) 1.5-Na2Ti6O13/TiO2 calcined at 500°C; (c) 1.5-Na2Ti6O13/TiO2 calcined at 600°C; (d) 1.5-Na2Ti6O13/TiO2 calcined at 700°C; (e) 1.5-Na2Ti6O13/TiO2 calcined at 800°C.
(a)
(b)
(c)
(d)
(e)The SEM micrographs of Na2Ti6O13 powders calcined at 700 and 800°C are shown in Figures 2(d) and 2(e). The belt-like morphology of the product calcined at 700°C is well documented in the SEM image shown in Figure 2(d). Na2Ti6O13 nanobelts have typical width from 80 to 100 nm, thickness less than 40 nm, and length up to 5 μm. The phase of the obtained sample was supported by XRD. It is also found that the nanobelts were fractured under calcination at 800°C, though the fragments have higher degree of crystallinity, as shown obviously in Figure 2(e).Figure3 shows the XRD patterns of 1.5-Na2Ti6O13/TiO2 precursor and the composite particles which were calcined for 3 h at 500, 600, 700, and 800°C, respectively. As can be seen, no characteristic diffraction peaks are observed from the pattern of precursor, indicating that the precursor is amorphous. The XRD pattern of 1.5-Na2Ti6O13/TiO2 calcined at 500°C shows a strong peak at 2θ=25.34° and a weak one at 2θ=27.50°, implying that TiO2 is crystallized as the anatase and rutile phase coexistence after calcined at 500°C. Curves of 1.5-Na2Ti6O13/TiO2 calcined at 600–800°C show that Na2Ti6O13 could be obtained by calcining the microemulsion-resulted precursor at relatively low temperature (<800°C). The pattern of 1.5-Na2Ti6O13/TiO2 calcined at 600°C shows the characteristic diffraction peak of both rutile and Na2Ti6O13; however, the samples calcined at 700, and 800°C have no characteristic diffraction peak of TiO2.Figure 3
XRD pattern of 1.5-Na2Ti6O13/TiO2 composite particles: (a) 1.5-Na2Ti6O13/TiO2 precursor; (b) 1.5-Na2Ti6O13/TiO2 calcined at 500°C; (c) 1.5-Na2Ti6O13/TiO2 calcined at 600°C; (d) 1.5-Na2Ti6O13/TiO2 calcined at 700°C; (e) 1.5-Na2Ti6O13/TiO2 calcined at 800°C.Although the formation mechanisms of the titanate nanobelts are still under debate, we believe that the formation of Na2Ti6O13 nanobelts may be affected by the crystallite size or chemical activity of the precursor and the condition of crystallization. In our work, the precursor is considered to be Ti(OH)4. Under heat treatment, –OH from the surface of Ti(OH)4 combined with each other to produce H2O and –O–Ti–bond. With the calcined temperature increase and the existence of Na+, more –OH were removed and Na–O–Ti–bonds were formed, which means that Na2Ti6O13 were formed. As it was supported by SEM and XRD, at the temperature of 600°C, the crystallization of Na2Ti6O13 which are the prerequisites for the nanobelts formation was obtained. According to Dominko et al. [31], Na2Ti6O13 crystallizes in a monoclinic crystalline structure with continuous tunnel channels along c axis (Figure 4). Such tunnel channels suppressed the possible delamination into sheets or nanotubes [30].Figure 4
Schematic representation of the crystal structure of Na2Ti6O13 along a-axis [31] (octahedral: Ti–O6; spheres: Na).In a word, the amorphous precursor forms anatase and rutile phase at 500°C, and the anatase phase transits into rutile phase at 600°C; meanwhile, Na2Ti6O13 crystal formed. However, when the temperature is higher than 600°C, no TiO2 exists. Thus, the optimum temperature for heterostructure particles is 600°C.


## 3.2. Degradation Activities of Na2Ti6O13/TiO2

In this investigation, 2,4-dichlorophenol(2,4-DCP) was chosen as a representative model pollutant (C0=20 mg/L, 200 mL) to study the adsorption and photocatalytic activity of the Na2Ti6O13/TiO2 composite particles (10 mg) under UV-light (40 W Hg lamp) irradiation and the results can be seen in Figure 5. The degradation efficiency of 2,4-DCP increased with time. After 50 min UV-light irradiation, the degradation rate reached 99.4%, 96.0%, 83%, and 56.2%, by the photocatalyst synthesized in 1.5, 1.0, 0, and 2.5 mol/L sodium hydroxide solution, respectively, while the commercial P25 has the degradation rate of 76.9%, and the degradation rate of 11.5% was obtained without any photocatalysts.Figure 5
Effects of ratio of Na2Ti6O13/TiO2 calcined at 600°C: (a) 1.5-Na2Ti6O13/TiO2; (b) 1.0-Na2Ti6O13/TiO2; (c) 0-Na2Ti6O13/TiO2; (d) commercial P25; (e) 2.5-Na2Ti6O13/TiO2; (f) blank.The different molar ratios of Na2Ti6O13/TiO2 have significant differences in photoactivity. While the ratio raises from 0 to 1.5, the degradation rate raises obviously; however, the 2.5 sample has the weakest activity. The sample of 1.5-Na2Ti6O13/TiO2 has the best efficiency for decomposing 2,4-DCP, which is about 1.3 times higher than commercial P25. Thus, 1.5-Na2Ti6O13/TiO2 was chosen as the standard photocatalyst.Figure6 shows the photoactivity of 1.5-Na2Ti6O13/TiO2 calcined at different temperatures. After 50 min UV-light irradiation, the degradation rate reached 99.4%, 83.8%, 56.3%, and 37.2%, by the photocatalyst calcined at 600, 500, 700, and 800°C, respectively. The commercial P25 has the degradation rate of 76.9%, and the blank experiment showed the degradation rate of 11.5%.Figure 6
Effects of calcined temperature of 1.5-Na2Ti6O13/TiO2: (a) 600°C (b) 500°C; (c) commercial P25; (d) 700°C; (e) 800°C; (f) blank.Combining with SEM and XRD characterization, the temperature of calcinations determines the crystal line, the morphology, and the components of the photocatalyst. At 500°C the component of the photocatalyst mainly is TiO2. Such photocatalyst formed by anatase and rutile exhibits a general photoactivity. At 600°C Na2Ti6O13/TiO2 heterostructure formed and the particles were well crystalline. These microstructures improve the separation efficiency of photogenerated electrons and holes, increase the contact area, and allow more efficient transport for the reactant molecules to get to the active sites on the framework walls, enhance the adsorption of light, and reduce the reflection of light. Therefore, the photocatalytic activity was enhanced.In order to observe the photo degradation process of 2,4-DCP, the concentrations of possible intermediates, such as phenol, 4-CP, and 2-CP, were measured with HPLC. Figure7 represents these three intermediates generation from the system. It is clear that 2,4-DCP was not completely mineralized and was residue as phenol and chlorophenol; meanwhile, the concentration of phenol is much higher than 4-CP and 2-CP. After 40 min photoreaction, the concentration of these three intermediates reduced obviously, indicating that Na2Ti6O13/TiO2 heterostructure is capable of degrading phenol and chlorophenol.Figure 7
Variation of (a) phenol; (b) 4-CP; (c) 2-CP concentration during the photo degradation.


## 4. Conclusions

Nanobelts Na2Ti6O13/TiO2 heterostructure particles were synthesized in an n-hexanol/CTAB/sodium hydroxide solution reverse microemulsion. The samples were investigated by TG-DSC, XRD, and SEM. The results show that such belt-like photocatalyst has typical width from 80 to 100 nm, thickness of less than 40 nm, and length up to 5 μm. The photocatalytic activity of photocatalysts synthesized by 1.5 mol/L sodium hydroxide solution and calcined at 600°C for 3 h gave the greatest degradation rate towards 2,4-DCP. In summary, it was proved that the heterostructure particles had higher photocatalytic activity than the common TiO2.



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*Source: 606291-2013-05-30.xml*