Photocatalytic activity of nanoparticles was successfully enhanced by addition of multiwall carbon nanotubes (MWCNT) to make CNT/ nanocomposites by sol-gel method at ambient temperature. CNT treated by HNO3 : H2SO4 treatment (1 : 3 v/v) was mixed with nanoparticles at various molar ratios and calcination temperatures. The optimal molar ratio of CNT :  was found at 0.05 : 1 by weight. The optimal calcination condition was 400°C for 3 h. From the results, the photocatalytic activities of CNT/ nanocomposites were determined by the decolorization of 1 × 10−5 M methylene blue (MB) under visible light. CNT/ nanocomposites could enhance the photocatalytic activity and showed faster for the degradation of MB with only 90 min. The degradation efficiency of the MB solution with CNT/ nanocomposite achieved 70% which was higher than that with pristine (22%). This could be explained that CNT prevents from its agglomeration which could further enhance electron transfer in the composites. In addition, CNT/ nanocomposites had high specific surface area (202 m2/g) which is very promising for utilization as a photocatalyst for environmental applications.

1. Introduction

Titanium dioxide (TiO2) is an ideal photocatalyst for high photocatalytic activities. TiO2 can accelerate removals of organic compounds with its high stability in a chemical point of view. It is relatively cheap and easily available. Although TiO2 has several advantages, it has some hindrances to apply in the environmental field, that is, photocatalytic degradation of organic pollutants, because TiO2 is limited to work under only UV radiation (<387 nm) [1, 2]. The primary problem is the low concentration of pollutants which reduces the efficiency of TiO2. Another problem is the recombination of electron-hole pair. Therefore, many studies have been focused on how to improve the photocatalytic activity of TiO2 under visible light (>400 nm) [35].

Carbon nanotube (CNT) has been successfully used as catalyst supporting materials with properties superior to those of other regular catalyst supports like activated carbon, soot, or graphite. CNT was recently found to be able to excellently absorb some toxic gases because CNT provides large specific surface area [68]. Peining et al. [9], Cao et al. [10], and Shitole et al. [11] have reported the combined roles of CNT and TiO2. CNT and TiO2 composites showed a synergistic effect on the efficient degradation of some organic compounds. This is closely related to the enhancement of pollutant adsorptions from air and water because of the extremely high surface area of CNT and high microporous volume of TiO2. However, in the composite preparation, pristine CNT tends to lack solubility and be difficultly manipulated in any solvents, which have imposed great limitations to the use of CNT as templates to assemble diverse functional components. Therefore, to efficiently fabricate CNT based nanohybrids, it is necessary to activate the graphitic surfaces of CNT [12, 13]. Functionalization of CNT remains one of the most studied areas in CNT research fields. The most common covalent functionalization involves the addition of carbonyl and carboxyl groups via an aggressive treatment with HNO3 or a mixture of HNO3/H2SO4 acid. Covalent functionalization of CNT has been shown to be an efficient method for increasing solubility and chemical reactivity of CNT. Composite of acid-treated CNT and TiO2 was found to have higher photocatalytic activity than pristine CNT and pristine TiO2. The composite also showed a decrease of charge recombination by trapping electron in the valence band and an increase of the visible light absorption [10, 1417]. Visible light absorption of the composite could be achieved because of the reducing band gap energy of the composite [12, 17].

Typically, CNT and TiO2 composites were fabricated by sol-gel method. Sol-gel method is the common technique to synthesize TiO2 nanoparticle because it is easy to control the chemical composition and inexpensive. Sol-gel method also does not need complicated equipment [1820]. In addition, other advantages of sol-gel method are high purity, homogeneity, controllable stoichiometry, and ambient temperature preparation [2123].

Table 1 shows several photocatalysts fabricated by sol-gel technique, which were made of CNT/TiO2 composites and applied for photocatalytic degradations of dyes under UV and visible light radiations from opened literatures [1116, 18]. Most of the studies showed that the rate of photocatalytic activity for degradation of pollutants can be enhanced by CNT/TiO2 nanocomposites. Although many researchers studied the synthesis of TiO2 and doped it with CNT, they mostly reported the photocatalytic activities under UV light. There are very few reports studied on those photocatalytic activities under visible light with relatively low activities (degradations of dyes ~50%) [17, 18]. Thus, this study aims to improve photocatalytic activity of CNT/TiO2 nanocomposites under visible light.

For this contribution, we reported the preparation and characterizations of CNT/TiO2 nanocomposites at ambient temperature using TiBu and MWCNT as precursors. This is the first report on the precursors and ambient temperature preparation for CNT/TiO2 nanocomposites. The optimal molar ratio (CNT/TiO2) and calcination temperature were studied. FTIR, XRD, UV-vis, BET surface area analysis, and SEM were used to characterize the composites. Additionally, the photocatalytic activity of the composite photocatalysts was determined by decolorization of MB under visible light.

2. Experimental

2.1. Materials

All chemicals used were of analytical grade. Titanium butoxide (97%, Fluka), MWCNT (Nanogeneration Company, purity > 90%, average diameter 9.5 nm, and length 1.5 µm), ethanol (96%, Merck), nitric acid (65%, Merck), sulfuric acid (95–97%, Merck), hydrochloric acid (37%, Merck), and deionizer water were used for the preparation of nanocomposites. MB (UNILAB) was used for the photocatalytic experiments.

2.2. Acid Treatment of CNT

In a typical acid treatment, MWCNT was treated by nitric/sulfuric-mixed acid following the methods reported in previous works [10, 11]. MWCNT (1 g) was stirred for 10 min in HNO3 : H2SO4 mixture (1 : 3 (v/v), 40 mL). The solution was sonicated for 6 h at 70°C in an ultrasonic bath to completely disperse MWCNT in the acid solution. MWCNT was then washed with deionized water to remove any residual acid until its pH value was adjusted to be 7. Treated MWCNT was dried overnight at 100°C in an oven. Finally, the resulting carboxyl-functionalized MWCNT powders were obtained. This functionalization will enhance the solubility of MWCNT in solvents as well as the creation of chemical compatibility with TiO2 surfaces.

2.3. Preparation of CNT/TiO2 Nanocomposites

Saleh and Gupta [16] and Morales et al. [24] reported a method to prepare CNT/TiO2 nanocomposites at relatively high temperature (70–80°C) with a long time process (typically 6–8 h). In this work, CNT/TiO2 nanocomposites were synthesized by sol-gel method adapted from that method. Specially, the preparation time was shortened to be only 3 h and the preparation temperature was reduced to be at room temperature. TiBu (Ti(OC4H9)4) was used as a titanium precursor. TiBu, ethanol, H2O, and HCl were sequentially mixed as a solution. The molar ratio of TiBu : ethanol : H2O : HCl was 1 : 0.35 : 34 : 0.2. The mixture was stirred at ambient temperature for 1 h to complete the hydrolysis reaction. Acid-treated CNT was then dispersed in a solution. The solution was sonicated for 2 h at ambient temperature. The molar ratios of CNT : TiO2 used in the sol were 0.1 : 1, 0.05 : 1, and 0.03 : 1 by weight. Finally, the mixture was dried overnight at 100°C and calcined at different temperatures (300, 350, 400, or 500°C) for 3 h.

2.4. Characterizations of CNT/TiO2 Nanocomposites

For physical properties, the crystallinity of CNT/TiO2 nanocomposites was studied by X-ray diffraction (XRD) (D8 Advanced Bruker Euler Cradle) using Cu Kα (λ = 0.1540 nm) as the X-ray source. The accelerating voltage and the emission current were 40 kV and 40 mA, respectively. The diffractograms were recorded in the 2θ range from 20° to 80° with the rate of 0.01°/1.5 s. The crystallite size was calculated by using the Scherrer equation. Fourier transform infrared (FTIR) spectra were recorded by a PerkinElmer System 2000 FTIR spectrometer using KBr pellets over the range of wavenumbers of 400–4000 cm−1. Brunauer-Emmett-Teller (BET) surface areas were also measured using the nitrogen adsorption method (ASAP 2010, Micromeritics Company) at 77 K. The UV-vis absorption was examined by UV-vis spectrophotometer (diffuse reflectance mode) in a range of wavelengths of 200–800 nm. Composition of CNT and TiO2 in the obtained composites was calculated from the thermogravimetric analysis (TGA) thermograms. The TGA thermograms were investigated from a TGA equipment (Pyris 1 TGA, PerkinElmer, USA). Morphological appearance of the pristine TiO2, acid-treated CNT, and CNT/TiO2 nanocomposites was obtained by a field emission scanning electron microscope (FE-SEM) (JEOL JSM-7001F).

2.5. Photodecolorization of Methylene Blue

Photocatalytic activities of CNT/TiO2 nanocomposites were studied from the removal of MB in aqueous solution. The concentration of MB used was 1 × 10−5 M. MB aqueous solution (50 mL) and CNT/TiO2 nanoparticles (0.05 g) were mixed and stirred (for 15 min) at room temperature in a reactor under a dark condition for 3 h. The decrease of MB concentration under the dark condition was then determined by UV-vis spectrometer (GENESYS 10-S, Thermo Electron Corporation) at the maximum wavelength () of 664 nm. After completed adsorption, the sample was put inside the reactor again with a new MB aqueous solution (50 mL). The visible light source, a fluorescence lamp (15 W, Philip), was turned on to study the photocatalytic activity of photocatalysts under visible irradiation. Finally, the reduction of MB concentration was recorded at a fix time interval (every 30 min).

The decolorization efficiency of MB was calculated by using [21] where and are an initial concentration and a concentration at a measuring time, respectively.

3. Results and Discussion

3.1. Acid Treatment of CNT

As mentioned above, acid treatment is one of important processes for CNT functionalization. For the preparation of CNT/TiO2 nanocomposites, the functionalization facilitates the solubility of CNT in solvents. In the first step of work, carboxyl-functionalized CNT powders were fabricated by acidic oxidation in CNT prior to using in the preparation of CNT/TiO2 nanocomposites. FTIR spectra of pristine CNT and acid-treated CNT are shown in Figure 1 (lines (a) and (b)). A broad peak at 3,400–3,600 cm−1 can be assigned to the stretching vibration of OH group of the adsorbed water. This peak could be found in all samples tested. The oxidized (acid-treated) CNT showed peaks of carbonyl and carboxyl groups at 1,650 cm−1 and 1,710 cm−1, respectively. Furthermore, the carbonyl group was confirmed by a strong peak in the C-O stretching at 1,180 cm−1 (broad band at 1,100–1,300 cm−1) [16, 24]. These indicated the presence of chemically functional groups on CNT.

To confirm the characteristics of acid-treated CNT in CNT/TiO2 nanocomposites, the nanocomposites were preliminary fabricated (CNT/TiO2 ratio at 1 : 20, calcination temperature at 400°C). FTIR spectrum of CNT/TiO2 nanocomposites also assigned the peaks of carbonyl group at 1,650 cm−1 and found the titania (Ti-O or Ti-O-Ti) bonding at 550 cm−1, as shown in Figure 1 (line (c)). This confirmed the functionalization of CNT and the functional groups remained in oxidized CNT in the obtained composites. The functional groups in CNT play a role in creating chemical compatibility of CNT with TiO2 surfaces [10, 1417].

3.2. Preparation of CNT/TiO2 Nanocomposites
3.2.1. Effect of Calcination Temperature

Acid-treated CNT was used to prepare CNT/TiO2 nanocomposites by sol-gel method at ambient temperature. The molar ratio of CNT : TiO2 was fixed at 0.05 : 1 (by weight). The composites were calcined in air at different temperatures (i.e., 300, 350, 400, and 500°C) to study the suitable calcination temperature for high-crystalline anatase titania and remained content of CNT.

XRD patterns of acid-treated CNT (heat-treated at 400°C), TiO2 nanoparticles (calcined at 400°C), and CNT/TiO2 nanocomposites (calcined at various calcination temperatures) are shown in Figure 2. It was observed that the strong peaks of CNT powders at angles (2θ) of 25.8° and 42.7° can be assigned to C(002) and C(100) diffractions [25]. For calcined TiO2 nanoparticles and CNT/TiO2 nanocomposites, the peaks appearing at 25.80°, 37.80°, 48.18°, 54.09°, 55.10°, and 62.70° can be assigned to crystalline planes of (101), (004), (200), (105), (211), and (204) which clearly confirmed the anatase TiO2 phase [24]. These peaks correspond to the Joint Committee on Powder Diffraction Standards (JCPDS) Card File number 21-1272 [26, 27]. The peak of CNT/TiO2 nanocomposites at 25.80°, which corresponds to the C(002) reflection of CNT, overlaps the anatase (101) TiO2 reflection. Therefore, the anatase phase was the major crystal in CNT/TiO2 nanocomposites.

For comparison of various calcination temperatures, it could be observed that the intensity and the sharpness peak were increased when the samples were calcined at higher temperatures. This indicates higher crystallinity of TiO2 calcined at higher temperatures. Moreover, because the calcination was carried out in air, CNT can be easier oxidized at higher temperature [2830]. The TGA thermogram of CNT (the result is not shown here), which was investigated under oxygen condition, revealed the significant weight loss around 500–600°C. This evidence also supports the increasing intensity and the sharpness of peaks at higher calcination temperature. Therefore, the calcinations at 500°C show the highest intensity.

The crystallite size of TiO2 anatase in CNT/TiO2 nanocomposites was estimated from Scherrer’s equation which is shown in Table 2. It was observed that the crystallite size of TiO2 nanoparticles calcined at 400°C was 30.2 nm which is larger than that of CNT/TiO2 nanocomposites calcined at 400°C (27.7 nm). For CNT/TiO2 nanocomposites, the crystallite size was found to increase with increasing calcination temperature (i.e., 22.2 nm at 300°C and 33.3 nm at 500°C).

UV-vis spectra of CNT, TiO2 nanoparticles, and CNT/TiO2 nanocomposites calcined at various temperatures were showed in Figure 3. TiO2 shows light absorption under UV region (200–400 nm), while CNT can absorb light in both UV and visible regions (200–700 nm). For CNT/TiO2 nanocomposites calcined at temperatures 300–400°C, the UV-vis absorption spectra are similar to CNT. The absorption intensities in the visible region of CNT/TiO2 nanocomposites calcined at temperatures 300–400°C are lower than that of CNT. The higher calcination temperatures, the lower visible region intensity, could be observed. The absorption in visible region dramatically decreased when the composites were calcined at 500°C. This revealed the degradation of CNT, which corresponds to the result from XRD as explained above.

Band gap energy of CNT, TiO2 nanoparticles, and CNT/TiO2 nanocomposites calcined at various temperatures was estimated from the UV absorption edges from UV-vis spectra using cut-off adsorption edges [31, 32]. The results of calculation are shown in Table 2. It is well known that the band gap of TiO2 is around 3.2 eV [25, 27, 28]; the band gap energy of TiO2 shown in Table 2 is 2.8 eV. The lower band gap of TiO2 is because some organic compounds did not completely burn out at the calcination temperature of 400°C. It was observed that the absorption wavelength of CNT/TiO2 nanocomposites showed lower band gaps compared with pristine TiO2 because of the presence of CNT. The composites which were calcined at different temperatures in the range of 300°C–400°C demonstrated similar UV absorption edge at 755–760 nm, equivalent to band gap energy of about 1.6 eV. The calcination temperature at 500°C showed the absorption band edge at 750 nm (band gap = 1.7 eV). This is because of some degradation of CNT. This band gap of the composites obtained is narrower than the reported CNT/TiO2 nanocomposites prepared by different sol-gel method (2.31 eV) [27] and hydrothermal (2.84 eV) [11]. The narrow band gap benefits to the composites that can absorb light in visible region make the photocatalyst able to be used in the visible irradiation.

3.2.2. Effect of CNT/TiO2 Molar Ratio

CNT/TiO2 nanocomposites with various molar ratios of CNT to TiO2 were fabricated. The composites calcined at 400°C. CNT/TiO2 molar ratio was varied at 0.10 : 1, 0.05 : 1, and 0.03 : 1. It should be noted that, in the preparation of the composite (61.5 mL), the weight of TiO2 precursor (TiBu) was fixed at 6.5 g for all samples, while the amount of CNT added was varied corresponding to the molar ratios.

Figure 4 shows XRD patterns of the nanocomposites at various molar ratios compared with acid-treated CNT and TiO2 nanoparticles calcined at 400°C. It was observed that, at the fixed amount of TiO2, increasing composition of CNT resulted in decreases of peak intensity and sharpness. This could be attributed to the obstruction in crystallization of TiO2 if higher amount of CNT is added to TiO2 precursor during sol-gel process.

The crystallite sizes of the composites at various CNT/TiO2 molar ratios were estimated as shown in Table 3. It was obviously seen that, at the fixed amount of TiO2, increasing composition of CNT resulted in decrease of crystallite size of TiO2. This indicates the heterogeneous nucleation in CNT for the formation of anatase TiO2 particles.

UV-vis spectra of samples are shown in Figure 5. All CNT/TiO2 nanocomposites at various CNT : TiO2 molar ratios could enhance the UV light sensitivity of anatase TiO2 and increase the absorption capacity for visible light irradiation. At higher composition of CNT, relatively higher intensity of UV-vis spectra could be observed. For comparison, band gap energy of CNT/TiO2 nanocomposites at various CNT/TiO2 molar ratios was calculated as shown in Table 3. It can be seen that higher composition of CNT resulted in lower band gap energy.

3.3. Morphology and Surface Properties of CNT/TiO2 Nanocomposites

To investigate the morphology and surface properties of CNT/TiO2 nanocomposites, the nanocomposites at CNT/TiO2 ratio of 0.05 : 1 were fabricated and calcined (400°C). Specific surface areas of CNT, TiO2 nanoparticles, and CNT/TiO2 nanocomposites were characterized by BET method, where the result is shown in Table 4. The surface areas of TiO2 and CNT were 79 and 218 m2/g, respectively. With adding small amount of CNT in TiO2 as nanocomposites, the surface area of TiO2 was increased to 202 m2/g. This observation indicated that the composites have relatively high surface for chemical reactions.

Figure 6 depicts FE-SEM images showing the morphology and microstructure of CNT, TiO2, and CNT/TiO2 nanocomposites. It could be observed that, in CNT/TiO2 nanocomposites, even the weight ratio of CNT to TiO2 is very low, but the characteristic morphology of CNT in nanocomposites was obviously observed (Figure 6(c)). The dispersion of TiO2 nanoparticles on the surface of CNT could be confirmed in the image. However, some part of TiO2 aggregates could be observed in the images, due to high composition of TiO2 in the composites.

3.4. Photodecolorization of MB

The effects of calcination temperature and CNT/TiO2 molar ratio of CNT/TiO2 nanocomposites were confirmed by the photocatalytic activity for MB degradation under visible light irradiation.

3.4.1. Effect of Calcination Temperature

The photocatalytic activity of CNT/TiO2 nanocomposites calcined at various temperatures is presented in Figure 7. In this experiment, the molar ratio of CNT/TiO2 was fixed at 0.05 : 1. To eliminate the decolorization of MB by adsorption and study only the decolorization by photocatalysis, the adsorption of MB under a dark condition was carried out. The decrease of MB concentration under the dark condition was determined for 3 h. After completed adsorption, the sample was placed inside the reactor again with a new MB solution; then the photocatalytic activity of photocatalysts under visible light irradiation was performed.

The dye adsorption behavior of CNT/TiO2 nanocomposites is shown in Figure 7(a). For comparison, the acid-treated CNT and TiO2 nanoparticles with the equal amount of each component in the composites were also tested (e.g., CNT/TiO2 composites = 0.05 g, CNT = 0.0024 g, and TiO2 = 0.0476 g). Even CNT was used as less amount compared with TiO2; the MB adsorption of CNT was higher than TiO2, because of remarkably higher surface of CNT. The MB adsorption of CNT/TiO2 nanocomposites was higher than those of acid-treated CNT and TiO2, because of higher weight amount of composites compared with the pristine ones. From various calcination temperatures, it was found that composites calcined at lower temperatures showed higher MB adsorption. This result is in correspondence with TGA thermogram of CNT that shows decomposition at high temperature as described above.

In order to consider the decolorization of MB under visible irradiation by photocatalytic properties of CNT without any effect of adsorption, adsorption equilibrium of MB on CNT was studied. CNT has significantly high surface, so it takes longer time to reach the adsorption equilibrium of MB on CNT compared with TiO2 [16]. It was found that the adsorption equilibrium of MB on CNT was 12 h (4 cycles of 3 h adsorption). Therefore, the photocatalytic performance of CNT was investigated under visible irradiation after the 12-h dye adsorption.

After 3 h adsorption of MB in dark condition (except for CNT, adsorption = 12 h), the photocatalytic degradation of MB under visible irradiation was studied (Figure 7(b)). Decolorization of MB with CNT showed different behavior from that in the adsorption step, because dye molecules were mostly adsorbed in dark condition after 12 h adsorption. TiO2 nanoparticles showed photocatalytic behavior under visible light irradiation with higher decolorization of MB compared with that in the dark condition. The MB degradation on CNT/TiO2 nanocomposites (from all calcination temperatures) was higher than that on pristine TiO2 particles. This is because of the advantage of CNT for visible light adsorption. In addition, the important role of CNT was as a transporting channel of electron to TiO2 nanoparticles [26, 27, 29, 30].

For comparison of various calcinations, it can be observed that the photocatalytic activity increased with increasing calcination temperatures from 300°C to 400°C because of more crystallinity of TiO2 (see Figure 2) with the presence of CNT (confirmed by TGA). At too high calcination temperature, that is, 500°C, the photocatalytic activity was the lowest compared with other CNT/TiO2 due to the degradation of CNT during the calcination. From this result, the optimal calcinations temperature which provided the highest photocatalytic activity was 400°C. At this temperature, the composites have a good composition and interfacial contacts between CNT and anatase TiO2.

3.4.2. Effect of CNT/TiO2 Molar Ratio

Figure 8 shows photocatalytic degradations of CNT, TiO2, and CNT/TiO2 nanocomposites (calcined at 400°C) at various molar ratios of CNT : TiO2 compared with a blank (MB without any photocatalyst). Figure 8(a) showed the dye adsorption in the dark condition. At CNT : TiO2 ratio of 0.10 : 1, the highest adsorption performance was observed due to its high CNT content.

After reaching the adsorption equilibrium in dark conditions, the photocatalytic activity of MB degradation under visible light irradiation was examined in Figure 8(b). It was observed that CNT/TiO2 nanocomposites at CNT : TiO2 ratio of 0.05 : 1 showed the highest photocatalytic activity efficiency (70% at 90 min) compared with other ratios as summarized in Table 5. The photocatalytic activity of the nanocomposites at CNT : TiO2 ratio of 0.05 : 1 was also higher than pristine TiO2 nanoparticles and CNT.

The composites with CNT/TiO2 ratio of 0.05 : 1 showed faster photodegradation than that of 0.03 : 1 because of higher composition of CNT for light adsorption. Addition of CNT to form the composites with higher ratio of CNT/TiO2 (0.10 : 1) did not further increase the MB degradation rate because too high content of CNT causes much light adsorption which could reduce the light intensity on the most composites in the deeper position of solution. This evidence was also reported in the literature [20].

Only a few researchers previously reported on the photocatalytic activity of organic pollutants under visible light irradiation [12, 17]. As shown in Table 1, the previously reported efficiency of photocatalytic degradation under visible irradiation was not relatively high (60% within 120 min). In this work, CNT/TiO2 nanocomposites showed much better photocatalytic degradation efficiency (70% within 90 min) due to small band gap and high surface area of CNT, which could support photocatalytic reactivity of TiO2.

3.5. Mechanism of Photodecolorization of MB with CNT/TiO2 Nanocomposites

The reaction of the photodecolorization of MB under visible irradiation can be described as the schematic illustration in Figure 9. The mechanism in this illustration is quite different from previous reports [23, 3032]. CNT/TiO2 nanocomposites were attacked by photon from visible light which are subjected to band gap excitation (>380 nm, visible region); they undergo electron-hole pair production and charge separation. Photoinduced electrons (e) from CNT are easily transferred to the conduction band of TiO2 [29]. Detailed mechanism is shown in Simultaneously, the positively charged hole (h+) from CNT reacted with the adsorbed water (H2O) and OH group and produced radicals. At the same time, electrons from TiO2 reacted with O2 and produce radical ions that are able to degrade MB. The reaction for describing the photoreduction of CNT/TiO2 nanocomposites can be summarized in

It can be proposed here that the role of CNT can be illustrated by injecting electrons into TiO2 conduction band under visible irradiation, triggering their formation of very reactive radicals such as superoxide radical ion () and hydroxyl radicals (), which are then responsible for the degradation of the organic compounds [2629].

The mechanism of MB oxidation is that the excited state from visible light of MB injects an electron into the conduction band of TiO2 as shown in (6) and (7). Consequently, MB is converted into a cationic dye radical ion (MB+) that further takes part in the photodegradation reaction. MB is totally degraded and mineralized after the photodegradation reaction by and radicals as shown in the last two formulas

4. Conclusions

Photocatalytic activity of TiO2 nanoparticle was successfully enhanced by addition of CNT to make CNT/TiO2 nanocomposites. Acid-treated CNT was mixed with TiO2 nanoparticles at various molar ratios and calcined at various temperatures. The optimal molar ratio of CNT : TiO2 was 0.05 : 1 by weight. The optimal calcination condition was 400°C for 3 h. The degradation efficiency of the MB solution with CNT/TiO2 nanocomposite under visible light irradiation achieved 70% within 90 min which was higher than that with pristine TiO2. CNT has lower band gap compared with pristine TiO2, resulting in better light absorption of the composites in visible region. In addition, CNT/TiO2 nanocomposites had high specific surface area which is very promising for utilization as a photocatalyst for environmental applications. In comparison with the previous studies reported on fabrication of CNT/TiO2 photocatalysts by sol-gel method, this work proposes a short time and low-energy preparation process which is in line with green chemistry concept. In addition, this work is the first report for highest degradation efficiency of MB under visible light irradiation until 70% within 90 min. These two important roles of CNT together lead to enhancing photocatalytic activity.

Conflict of Interests

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


The authors would like to express their gratitude to Research and Researchers for industries (RRi), the Thailand Research Fund (TRF); Perfect Solution and Consultancy Co., Ltd.; the Joint Graduate School of Energy and Environment (JGSEE), King Mongkut’s University of Technology Thonburi; Center for Energy Technology and Environment, Ministry of Education Thailand; and Nanotec-KMUTT Center of Excellence on Hybrid Nanomaterials for Alternative Energy for financial supports.