# Efficient Photocatalytic Degradation of Rhodamine B Dye by Aligned Arrays of Self-Assembled Hydrogen Titanate Nanotubes

Authors: Sriparna Chatterjee; Avesh K. Tyagi; Pushan Ayyub
Journal: Journal of Nanomaterials
 (2014)

---

## Abstract

We show that an aligned array of hydrothermally grown, multiwalled hydrogen titanate (H2Ti3O7) nanotubes—anchored to both faces of a metallic Ti foil—acts as an efficient photocatalyst. We studied the degradation of rhodamine B dye in the presence of the nanostructured photocatalyst under UV irradiation, by monitoring the optical absorption of the dye. Rhodamine B was chosen as a representative—and particularly harmful—industrial pollutant dye. The inner and outer diameters of the H2Ti3O7 nanotubes were 5 nm and 10 nm, respectively. The nanotube array catalyst is recyclable and structurally stable. Most importantly, it shows comparable or higher photodecomposition rate constant than those of both H2Ti3O7 nanotube powder and P-25 (Degussa). The enhanced photocatalytic performance may be ascribed to the nanotube array having a superhydrophilic surface with a high accessible surface area.


---

## Body

## 1. Introduction

A prime issue in environmental remediation [1] is to remove dyes and other commercial colorants from wastewater effluents of textile mills and other dye processing units, because 15% of synthetic textile dyes are believed to get dispersed in wastewater during manufacturing and processing [2]. Among the best agents for dye degradation are wide band gap semiconductors [3], in which electron-hole pairs are formed upon photoexcitation (usually in the UV). A fraction of these get trapped in shallow defect states and are subsequently available for relatively slow, redox processes [4]. Most organic photodegradation reactions utilize the oxidizing power of holes and result in the conversion of the organic species at the interfaces into nontoxic end products. An ideal photocatalyst should be stable, inexpensive, nontoxic, and highly photoactive, and the redox potential of the H2O/OH• couple must lie within its band gap. In principle, semiconductors such as TiO2, ZnO, Fe2O3, CdS, and ZnS can all act as sensitizers for such light-induced redox processes. In practice, TiO2 (anatase) appears to be the most promising photocatalyst for the destruction of organic pollutants due to its low cost, biological and chemical stability, nonphotocorrosivity, and superior photocatalytic activity [5, 6]. Further, there are several obvious advantages of having a semiconductor photocatalyst in the nanocrystalline form, such as (a) tunability of the band gap, (b) higher specific surface area, and (c) greater availability of trap states.Photocatalytic activity has been mostly studied using spherical or equiaxed nanoparticles, in which the catalytic efficiency indeed increases with decreasing particle size [7]. However, the recovery of nanoparticulate catalysts from the solution at the end of the reaction cycle may prove to be impractical. Also, spherical nanoparticles often tend to agglomerate into larger particles, thereby reducing their catalytic activity. Considerable effort has therefore gone into the search for low cost, high activity, and easily recyclable photocatalysts based on titanium oxide [8–10]. An elegant and practical solution to the above issues would be to obtain the photocatalyst in the form of an aligned array of 1D structures anchored to a substrate. Such a catalyst would be easy to handle and not allow aggregation to occur, thus permanently providing a high interfacial area for the reactants.Among the various 1D nanostructures, nanotubes are now ubiquitous in the world of nanoscience, particularly after the discovery of noncarbon nanotubes. In particular, titanate nanotubes have attracted attention as cathodes for rechargeable Li-ion batteries [11]. However, studies of their photocatalytic properties are not only scarce but also somewhat inconclusive. Hydrogen titanate (H2Ti3O7) nanotubes have been tried out as a photocatalyst, but only with limited success. For example, Hodos et al. [12] suggested that the H2Ti3O7 nanotubes are normally photocatalytically inactive and require to be photosensitized by CdS nanoparticles. On the other hand, Amano et al. [13] claimed that though titanate crystallites with a small amount of defects show considerable photocatalytic activity—liberating oxygen from an aqueous solution of silver sulphate as well as oxidatively decomposing acetic acid—it is less than that of anatase for the liberation of H2 from methanol. From a detailed study using methylene blue as the dye, Baiju et al. [14] reported a very high surface adsorption of dye molecule with a very low dye degradation rate because of poor crystallinity—for both as-prepared and calcined titanates, in agreement with earlier findings [15]. Note that all the above studies were made withrandomly oriented (mesh-like) H2Ti3O7 nanotube samples. H2Ti3O7 nanotube meshes also show enhanced activity in the gas phase photocatalytic oxidation of ethylene [16].Here we report the first study of the photocatalytic activity of analigned array of multiwalled H2Ti3O7 nanotubes anchored to a substrate. This geometry provides comparatively greater exposure of the sample surface to the reacting environment than that of a random collection of nanotubes. We have synthesized a roughly aligned array of H2Ti3O7 nanotubes by a hydrothermal technique and studied its use for the photochemical degradation of the rhodamine B (RhB) dye under UV light exposure. The catalytic efficiency of this material has been benchmarked against a standard industrial photocatalyst (P-25). We point out that RhB is accepted as a representative dye pollutant for such studies. While most dyes are resistant to biodegradation and direct photolysis, nitrogen-containing dyes such as RhB are particularly dangerous as they undergo a natural anaerobic degradation to yield potentially carcinogenic aromatic amines [17].


## 2. Materials and Methods

### 2.1. Hydrothermal Synthesis of Multiwalled Tri-Titanate Nanotubes

A modified hydrothermal synthesis route was used to obtain self-assembled, multiwalled H2Ti3O7 nanotube arrays (NTA) on oxidized Ti foils [18]. Typically, a 30 mm × 5 mm × 25 µm Ti foil (Sigma-Aldrich, 99.9%) was first oxidized in air at 800°C for 5 h, then dipped in 35 mL of 10 M NaOH in a sealed Teflon reactor, and autoclaved at 200°C for 6 h under an autogenous pressure. After cooling down to room temperature, the foils were thoroughly washed with 1 : 10 HCl (by volume)—typically for ≈ 10–12 h—till the pH of the wash became ≈ 6.5. Finally the samples were washed with hot deionized water to remove any traces of NaCl and then dried at 70°C. The catalytic efficiency of the as-prepared H2Ti3O7 nanotube array sample was compared with that of an unsupported H2Ti3O7 nanotube powder or mesh, which was synthesized from bulk anatase powder (Sigma, 99.999%) and 10 M NaOH using a hydrothermal process [19]. The results were benchmarked by comparing with the performance of a standard TiO2-based photocatalyst: Aeroxide P-25 Degussa with an average primary particle size = 21 nm and specific surface area (BET) = 50 ± 15 m2 g−1.


### 2.2. Structural Characterization

The crystallographic phase of the as-prepared H2Ti3O7 nanotubes was investigated using a Panalytical X’Pert Pro powder X-ray diffractometer (XRD) using Cu-Kα radiation, while their microstructure was studied using an eLine field emission scanning electron microscope (FESEM) operated at 20 kV. Energy dispersive X-ray (EDX) analysis was carried out to obtain the elemental composition. The morphology and crystal structure of individual nanotubes were studied using a FEI Tecnai-20 transmission electron microscope (TEM), equipped with a LaB6 filament, and operated at 200 kV. Samples for TEM were prepared by scraping the nanotubes off the foil, dispersing in ethanol, and placing a drop of the dispersion on a Cu grid covered with a holey carbon film, which was then dried. The surface area and pore size distribution were obtained using the Brunauer-Emmet-Teller (BET) from N2 physisorption data at 77 K recorded using a Micromeritics ASAP 2020 analyzer. About 100 mg of each sample was degassed at 10−6 Torr and 100°C prior to N2 adsorption. The Barret-Joyner-Halenda (BJH) method was employed to obtain pore size distribution. Diffuse reflectance UV-visible spectra were recorded on a JASCO V-670 spectrophotometer, using BaSO4 as a reference.


### 2.3. Photocatalytic Activity

We examined the photocatalytic performance of the substrate-supported H2Ti3O7 NTA, the unsupported H2Ti3O7 nanotube powder (for comparison), the oxidized Ti foil precursor (for comparison), and P-25 powder (as a standard reference) via the photo-assisted decolorization of an aqueous solution of RhB dye under UV irradiation (λ = 365 nm) at room temperature (23 ± 2°C). Four 6W UV lamps were used as the light source. Approximately 10 mg of the H2Ti3O7 NTA sample (inclusive of the substrate) was suspended horizontally in 10 mL of 1 × 10−6 M RhB solution in a 25 mL Pyrex beaker equipped with a magnetic stirrer. The beaker was tightly covered during the experiment to prevent evaporative losses. The net volumetric loss during the full experiment was in the range of 2-3%. Before UV irradiation, the dye solution was stirred in the dark for 6 h to ensure adsorption-desorption equilibrium of the dye on the catalyst surface so that the loss of the dye due to adsorption is correctly accounted for. The zero time reading was obtained from a blank solution kept in the dark but otherwise treated similarly to the irradiated sample. During illumination, about 1 mL of the dye solution was extracted after each 30–45 minute interval, and optical absorption spectra were recorded to determine the degradation rate (decrease in absorption intensity versus irradiation time) of RhB. The test solution was returned to the beaker each time after the absorption measurement to maintain a constant catalyst: reactant ratio throughout the experiment. The characteristic optical absorption peak of RhB at 553 nm was chosen to monitor the photo-induced degradation. The procedure was repeated for a second cycle to examine the stability and applicability of H2Ti3O7 nanotube array samples for multiple uses. Blank experiments without addition of catalyst and with the catalyst in the dark were also carried out.


## 2.1. Hydrothermal Synthesis of Multiwalled Tri-Titanate Nanotubes

A modified hydrothermal synthesis route was used to obtain self-assembled, multiwalled H2Ti3O7 nanotube arrays (NTA) on oxidized Ti foils [18]. Typically, a 30 mm × 5 mm × 25 µm Ti foil (Sigma-Aldrich, 99.9%) was first oxidized in air at 800°C for 5 h, then dipped in 35 mL of 10 M NaOH in a sealed Teflon reactor, and autoclaved at 200°C for 6 h under an autogenous pressure. After cooling down to room temperature, the foils were thoroughly washed with 1 : 10 HCl (by volume)—typically for ≈ 10–12 h—till the pH of the wash became ≈ 6.5. Finally the samples were washed with hot deionized water to remove any traces of NaCl and then dried at 70°C. The catalytic efficiency of the as-prepared H2Ti3O7 nanotube array sample was compared with that of an unsupported H2Ti3O7 nanotube powder or mesh, which was synthesized from bulk anatase powder (Sigma, 99.999%) and 10 M NaOH using a hydrothermal process [19]. The results were benchmarked by comparing with the performance of a standard TiO2-based photocatalyst: Aeroxide P-25 Degussa with an average primary particle size = 21 nm and specific surface area (BET) = 50 ± 15 m2 g−1.


## 2.2. Structural Characterization

The crystallographic phase of the as-prepared H2Ti3O7 nanotubes was investigated using a Panalytical X’Pert Pro powder X-ray diffractometer (XRD) using Cu-Kα radiation, while their microstructure was studied using an eLine field emission scanning electron microscope (FESEM) operated at 20 kV. Energy dispersive X-ray (EDX) analysis was carried out to obtain the elemental composition. The morphology and crystal structure of individual nanotubes were studied using a FEI Tecnai-20 transmission electron microscope (TEM), equipped with a LaB6 filament, and operated at 200 kV. Samples for TEM were prepared by scraping the nanotubes off the foil, dispersing in ethanol, and placing a drop of the dispersion on a Cu grid covered with a holey carbon film, which was then dried. The surface area and pore size distribution were obtained using the Brunauer-Emmet-Teller (BET) from N2 physisorption data at 77 K recorded using a Micromeritics ASAP 2020 analyzer. About 100 mg of each sample was degassed at 10−6 Torr and 100°C prior to N2 adsorption. The Barret-Joyner-Halenda (BJH) method was employed to obtain pore size distribution. Diffuse reflectance UV-visible spectra were recorded on a JASCO V-670 spectrophotometer, using BaSO4 as a reference.


## 2.3. Photocatalytic Activity

We examined the photocatalytic performance of the substrate-supported H2Ti3O7 NTA, the unsupported H2Ti3O7 nanotube powder (for comparison), the oxidized Ti foil precursor (for comparison), and P-25 powder (as a standard reference) via the photo-assisted decolorization of an aqueous solution of RhB dye under UV irradiation (λ = 365 nm) at room temperature (23 ± 2°C). Four 6W UV lamps were used as the light source. Approximately 10 mg of the H2Ti3O7 NTA sample (inclusive of the substrate) was suspended horizontally in 10 mL of 1 × 10−6 M RhB solution in a 25 mL Pyrex beaker equipped with a magnetic stirrer. The beaker was tightly covered during the experiment to prevent evaporative losses. The net volumetric loss during the full experiment was in the range of 2-3%. Before UV irradiation, the dye solution was stirred in the dark for 6 h to ensure adsorption-desorption equilibrium of the dye on the catalyst surface so that the loss of the dye due to adsorption is correctly accounted for. The zero time reading was obtained from a blank solution kept in the dark but otherwise treated similarly to the irradiated sample. During illumination, about 1 mL of the dye solution was extracted after each 30–45 minute interval, and optical absorption spectra were recorded to determine the degradation rate (decrease in absorption intensity versus irradiation time) of RhB. The test solution was returned to the beaker each time after the absorption measurement to maintain a constant catalyst: reactant ratio throughout the experiment. The characteristic optical absorption peak of RhB at 553 nm was chosen to monitor the photo-induced degradation. The procedure was repeated for a second cycle to examine the stability and applicability of H2Ti3O7 nanotube array samples for multiple uses. Blank experiments without addition of catalyst and with the catalyst in the dark were also carried out.


## 3. Results and Discussion

### 3.1. Structure and Morphology

We have earlier reported a detailed, electron microscopic study of each stage of the growth of the H2Ti3O7 nanotube array [18], the significant steps of which are as follows. It is important to note that the oxidized Ti foil (precursor) actually consists of a central, virtually unoxidized Ti layer sandwiched between layers of TiO2 (rutile). During hydrothermal treatment, nascent nanotubes were first detected at the Ti/TiO2 interface. This indicates that the Ti-rich core layer acts as a substrate for the growth of the tri-titanate nanotube array, whereas the surrounding oxide (rutile) layers serve as the source material. Complete dissolution of the rutile phase takes about six hours, and the resulting 1D H2Ti3O7 nanostructures grow to a length of about 45–50 µm on either side of the central Ti foil. High resolution TEM studies of the nature of the nanotube walls indicate that the tube formation takes place by a “scrolling” of the multilayer nanosheets. Hydrothermal treatment for 6 h completely converts the rutile layers to a monoclinic, tri-titanate (H2Ti3O7) phase, as shown by their respective X-ray diffractograms (Figures 1(a) and 1(b), resp.). Figure 1(c) shows the XRD pattern of free H2Ti3O7 nanotube powder dispersed on a glass substrate. Unlike the substrate-attached H2Ti3O7, which is partially oriented along [200], the nanotube powder is unoriented. EDX spectra (not shown here) indicate the presence of only Ti and O, and no sodium was detected. Cross-sectional SEM images recorded at a tilt angle of 89° (Figure 2(a)) clearly show that the H2Ti3O7 phase actually consists of a brush-like array of 1D structures (with an average length ≈45 µm on both sides) growing outwards from the central, metallic Ti layer. A plan view SEM (Figure 2(b)) shows that these unagglomerated, roughly parallel 1D structures provide an extremely high effective surface area. A typical TEM image (Figure 2(c)), obtained by dispersing a sample of the scraped material on a Cu grid, confirms that each 1D structure is a hollow, multiwalled nanotube with approximate inner and outer diameters of 5 nm and 10 nm, respectively. The XRD pattern of the H2Ti3O7 phase indicates a preferential alignment of the nanotubes along the (200) axis.Figure 1
X-ray diffraction patterns of the (a) precursor oxidized Ti foil showing the pure rutile phase of TiO2, (b) aligned H2Ti3O7 nanotube array showing preferential growth along <200> direction of the monoclinic tri-titanate phase, and (c) free H2Ti3O7 nanotube powder.(a) Cross-sectional FE-SEM image of the oxidized Ti foil after hydrothermal treatment of 6 h, showing formation of 1D nanostructure array on both sides of the central metal rich oxide layer. (b) Plan view of the same sample from one side. (c) HR-TEM image of a few nanotubes broken off from the same sample.
(a)
(b)
(c)Figure3 shows the typical nitrogen adsorption-desorption isotherm obtained from an aligned array of H2Ti3O7 nanotubes. The nature of the hysteresis in the isotherm at a high relative pressure (p/p0) range (Type IV-IUPAC) indicates the mesoporous character of the sample [20]. The inflection observed at p/p0~0.9 may be attributed to the porous structure of the sample, consistent with the SEM micrographs. The BET surface area of the substrate-attached sample used for the experiments is not very high (22.7 m2/g) due to the mass contributed by the substrate (central Ti-rich layer) to which the nanowires are anchored. The BET surface area for the rutile-coated precursor foil is only 0.1430 m² g−1, and no hysteresis loop is observed for this sample. Thus, the conversion from the rutile layer to the H2Ti3O7 NTA is accompanied by a 150-fold increase in the specific surface area. Expectedly, the specific surface area offree H2Ti3O7 nanotubes (with the same dimensions as the substrate-attached ones) was found to be in much higher (230–250 m² g−1) [16].Figure 3
Nitrogen adsorption-desorption isotherm of an aligned array of H2Ti3O7 nanotubes.


### 3.2. Diffused Reflectance UV-Visible Spectroscopy

The diffuse reflectance spectrum of the H2Ti3O7 NTA shows a distinct blue shift with respect to the oxidized Ti foil precursor (Figure 4). The band gap was calculated for both systems from the optical spectra using the equation, Eband-gap=hc/λint⁡, where “h” is Plank’s constant, “c” is the velocity of light, and “λint⁡” is the wavelength corresponding to the intersection of the extension of linear part of the spectrum and thex-axis. The calculated band gap for the H2Ti3O7 nanotube sample is 3.4 eV, while that for the oxidized Ti precursor is 2.9 eV.Figure 4
Diffuse reflectance optical spectra of oxidized Ti (rutile) foil and H2Ti3O7 nanotube array.


### 3.3. Photocatalytic Activity

The photocatalytic activities of the aligned H2Ti3O7 NTA, the unsupported H2Ti3O7 nanotube powder, the oxidized Ti foil precursor, and P-25 powder (as a standard reference) were estimated by studying the photo-induced degradation of the 553 nm absorption peak of rhodamine B as the colored contaminant. A time evolution study of the absorption spectrum of RhB solution exposed to UV light in the presence of the H2Ti3O7 NTA (Figure 5(a)) clearly shows a steady extinction of the absorption maximum of RhB with increasing UV exposure time, till it virtually disappears after 10 h of exposure. After a similar period in the presence of the precursor Ti oxide foil (with the same dimensions as that of the NTA anchored to the Ti foil), there was only a marginal change in the RhB absorption profile (Figure 5(b)).Time dependence of the optical absorption spectrum of rhodamine B dye solution in presence of the H2Ti3O7 nanotube array (a) and the (precursor) oxidized Ti foil (b).
(a)
(b)The catalytic performance of the H2Ti3O7 NTA was quantitatively benchmarked by carrying out the same reaction with (a) unsupported H2Ti3O7 nanotube powder and (b) a standard photocatalyst such as P-25, which is a mixture of nanocrystalline rutile and anatase. For this, it is essential to have a fairly accurate knowledge of the mass of the H2Ti3O7 nanotubes anchored to the substrate. We found that the mass of nanorods physically scraped off from the surface was subject to some degree of inaccuracy because either the nanotubes were not completely removed, or a part of the substrate also tended to get scraped off. A relatively more accurate method is to estimate the number of nanotubes per unit area from a statistically significant number of SEM images and calculate the total mass per unit area of substrate by assuming theoretical density of H2Ti3O7 (3.163 g/cm3). By scaling appropriately to the size of the experimental nanotube array sample (30 mm × 5 mm) and assuming nanotubes of uniform inner and outer diameter growing outwards from both faces of the Ti substrate, we obtained the total mass of the H2Ti3O7 nanotubes per sample with an estimated error of ±10%.In each case, the time evolution of the optical absorption was used to calculate the photodecomposition rate for identical masses of the H2Ti3O7 NTA and the comparison samples. Figure 6 shows that the normalized absorption C/C0 (C = concentration at time t, C0 = initial concentration) decays exponentially with time, which implies that the photodecomposition is a first order reaction. The calculated rate constant was the highest (0.002 min−1) for the supported H2Ti3O7 NTA sample. In comparison, the corresponding rate constant is 0.001 min−1 for P-25 and 0.0003 min−1 for the H2Ti3O7 nanotube mesh. We point out that the specific surface area of the P-25 Degussa powder (as per the specification sheet) is 50 ± 15 m2/g, which is in between the values for the substrate-attached HTO sample and for free H2Ti3O7 nanotubes (see Section 3.1). However, it is well-known that the high photocatalytic activity of P-25 arisesmainlyfrom reasons other than high surface area. P-25 is a mixed phase system containing atypically small rutile crystallites intermeshed with anatase crystallites. Charges produced on rutile by visible light are stabilized through rapid electron transfer to lower energy anatase lattice trapping sites. Thus, rutile acts as an antenna that extends the photoactivity into visible wavelengths and the structural arrangement of biphasic TiO2 crystallites creates catalytic “hot spots” at the rutile-anatase interface [21]. Thus, a direct quantitative comparison of P-25 and HTO nanotubes based on surface area alone would be inaccurate. However, our rate constant data (Figure 6) indicates at least that the dye degradation rate of the H2Ti3O7 NTA photocatalyst compares very favorably with standard commercial photocatalysts.Figure 6
Photocatalytic degradation curves for H2Ti3O7 nanorod array (filled circles), P-25 Degussa (half-filled circles), and H2Ti3O7 nanoparticles (open circles), where C/C0 = normalized absorption. The corresponding rate constants are also shown.Additional control experiments were performed to confirm the photocatalytic efficiency off the H2Ti3O7 NTA. The time dependence of the RhB solution concentration was monitored (i) on being exposed to UV irradiationwithout the H2Ti3O7 NTA and (ii) in presence of the H2Ti3O7 NTA butwithout UV irradiation. Almost no change in the RhB concentration was observed during either case, thereby confirming that both the H2Ti3O7 photocatalystand the UV light are necessary for the efficient degradation of RhB. Earlier studies [14, 15] had reported that the rate of surface adsorption of dye (in the dark) on H2Ti3O7 nanotubes is faster than the rate of dye degradation under UV light. But our study clearly shows that the rate of dye degradation under UV is much faster than the surface adsorption in the dark. This may be ascribed to the much larger effective surface area of the nanotube array catalyst and possibly also to the greater crystallinity of the sample.Our study has also established the following important issues. While several earlier authors—such as Hodos et al. [12]—had suggested that “undoped tri-titanate nanotubes failed to act as photocatalysts” and need to be sensitized with CdS, we have shown clear evidence of strong photocatalytic activity in this materialwhen in the form of an array. One of the few papers that reported significant photocatalytic activity in H2Ti3O7 nanofibers [9] also found the activity to be measurably enhanced when the nanofibers were decorated with anatase nanoparticles. Zheng et al. have recently reported the synthesis of hydrogenated anatase nanotube powder by heating pristine H2Ti3O7 nanotubes in H2 atmosphere [22]. They suggest that the hydrogenated TiO2 nanotube surface shows better photocatalytic activity than bare TiO2 nanorods and P-25. The rate constant of this sample for H2-production is 3.8 times higher than that of P-25 and 3.2 times that of bare TiO2 nanorods. The enhanced photocatalytic activity is ascribed to improved visible light absorption and efficient separation of photogenerated excitons by the surface Ti–H bonds.It is instructive to compare the degradation rate for the sulforhodamine dye by the H2Ti3O7 nanofiber mesh [9] with that for the rhodamine B by H2Ti3O7 nanotube arrays, reported here. An extrapolation of the data in [9] indicates that the dye concentration falls to 50% in ≈ 200 min, while in the present study it is found to fall to 50% in ≈ 300 min. Hence, an (roughly) aligned nanotube array, anchored to a substrate, is an extremely effective structure from the point of view of catalysis. Significantly, the surface of the HTO nanotube array has a strong affinity for aqueous media. In fact, the surface exhibits superhydrophilic behavior to an approaching water drop, which is sucked up rapidly on contact (see video clip: Supplementary Material 1 available online at http://dx.doi.org/10.1155/2014/328618). Further, on recycling the H2Ti3O7  NTA catalyst, we found almost no change in the crystal structure and overall morphology—as confirmed by XRD and TEM observations (not shown here). The catalytic activity decays slightly on recycling (with 0.001 < k < 0.002) but does not fall below the performance of P-25.


## 3.1. Structure and Morphology

We have earlier reported a detailed, electron microscopic study of each stage of the growth of the H2Ti3O7 nanotube array [18], the significant steps of which are as follows. It is important to note that the oxidized Ti foil (precursor) actually consists of a central, virtually unoxidized Ti layer sandwiched between layers of TiO2 (rutile). During hydrothermal treatment, nascent nanotubes were first detected at the Ti/TiO2 interface. This indicates that the Ti-rich core layer acts as a substrate for the growth of the tri-titanate nanotube array, whereas the surrounding oxide (rutile) layers serve as the source material. Complete dissolution of the rutile phase takes about six hours, and the resulting 1D H2Ti3O7 nanostructures grow to a length of about 45–50 µm on either side of the central Ti foil. High resolution TEM studies of the nature of the nanotube walls indicate that the tube formation takes place by a “scrolling” of the multilayer nanosheets. Hydrothermal treatment for 6 h completely converts the rutile layers to a monoclinic, tri-titanate (H2Ti3O7) phase, as shown by their respective X-ray diffractograms (Figures 1(a) and 1(b), resp.). Figure 1(c) shows the XRD pattern of free H2Ti3O7 nanotube powder dispersed on a glass substrate. Unlike the substrate-attached H2Ti3O7, which is partially oriented along [200], the nanotube powder is unoriented. EDX spectra (not shown here) indicate the presence of only Ti and O, and no sodium was detected. Cross-sectional SEM images recorded at a tilt angle of 89° (Figure 2(a)) clearly show that the H2Ti3O7 phase actually consists of a brush-like array of 1D structures (with an average length ≈45 µm on both sides) growing outwards from the central, metallic Ti layer. A plan view SEM (Figure 2(b)) shows that these unagglomerated, roughly parallel 1D structures provide an extremely high effective surface area. A typical TEM image (Figure 2(c)), obtained by dispersing a sample of the scraped material on a Cu grid, confirms that each 1D structure is a hollow, multiwalled nanotube with approximate inner and outer diameters of 5 nm and 10 nm, respectively. The XRD pattern of the H2Ti3O7 phase indicates a preferential alignment of the nanotubes along the (200) axis.Figure 1
X-ray diffraction patterns of the (a) precursor oxidized Ti foil showing the pure rutile phase of TiO2, (b) aligned H2Ti3O7 nanotube array showing preferential growth along <200> direction of the monoclinic tri-titanate phase, and (c) free H2Ti3O7 nanotube powder.(a) Cross-sectional FE-SEM image of the oxidized Ti foil after hydrothermal treatment of 6 h, showing formation of 1D nanostructure array on both sides of the central metal rich oxide layer. (b) Plan view of the same sample from one side. (c) HR-TEM image of a few nanotubes broken off from the same sample.
(a)
(b)
(c)Figure3 shows the typical nitrogen adsorption-desorption isotherm obtained from an aligned array of H2Ti3O7 nanotubes. The nature of the hysteresis in the isotherm at a high relative pressure (p/p0) range (Type IV-IUPAC) indicates the mesoporous character of the sample [20]. The inflection observed at p/p0~0.9 may be attributed to the porous structure of the sample, consistent with the SEM micrographs. The BET surface area of the substrate-attached sample used for the experiments is not very high (22.7 m2/g) due to the mass contributed by the substrate (central Ti-rich layer) to which the nanowires are anchored. The BET surface area for the rutile-coated precursor foil is only 0.1430 m² g−1, and no hysteresis loop is observed for this sample. Thus, the conversion from the rutile layer to the H2Ti3O7 NTA is accompanied by a 150-fold increase in the specific surface area. Expectedly, the specific surface area offree H2Ti3O7 nanotubes (with the same dimensions as the substrate-attached ones) was found to be in much higher (230–250 m² g−1) [16].Figure 3
Nitrogen adsorption-desorption isotherm of an aligned array of H2Ti3O7 nanotubes.


## 3.2. Diffused Reflectance UV-Visible Spectroscopy

The diffuse reflectance spectrum of the H2Ti3O7 NTA shows a distinct blue shift with respect to the oxidized Ti foil precursor (Figure 4). The band gap was calculated for both systems from the optical spectra using the equation, Eband-gap=hc/λint⁡, where “h” is Plank’s constant, “c” is the velocity of light, and “λint⁡” is the wavelength corresponding to the intersection of the extension of linear part of the spectrum and thex-axis. The calculated band gap for the H2Ti3O7 nanotube sample is 3.4 eV, while that for the oxidized Ti precursor is 2.9 eV.Figure 4
Diffuse reflectance optical spectra of oxidized Ti (rutile) foil and H2Ti3O7 nanotube array.


## 3.3. Photocatalytic Activity

The photocatalytic activities of the aligned H2Ti3O7 NTA, the unsupported H2Ti3O7 nanotube powder, the oxidized Ti foil precursor, and P-25 powder (as a standard reference) were estimated by studying the photo-induced degradation of the 553 nm absorption peak of rhodamine B as the colored contaminant. A time evolution study of the absorption spectrum of RhB solution exposed to UV light in the presence of the H2Ti3O7 NTA (Figure 5(a)) clearly shows a steady extinction of the absorption maximum of RhB with increasing UV exposure time, till it virtually disappears after 10 h of exposure. After a similar period in the presence of the precursor Ti oxide foil (with the same dimensions as that of the NTA anchored to the Ti foil), there was only a marginal change in the RhB absorption profile (Figure 5(b)).Time dependence of the optical absorption spectrum of rhodamine B dye solution in presence of the H2Ti3O7 nanotube array (a) and the (precursor) oxidized Ti foil (b).
(a)
(b)The catalytic performance of the H2Ti3O7 NTA was quantitatively benchmarked by carrying out the same reaction with (a) unsupported H2Ti3O7 nanotube powder and (b) a standard photocatalyst such as P-25, which is a mixture of nanocrystalline rutile and anatase. For this, it is essential to have a fairly accurate knowledge of the mass of the H2Ti3O7 nanotubes anchored to the substrate. We found that the mass of nanorods physically scraped off from the surface was subject to some degree of inaccuracy because either the nanotubes were not completely removed, or a part of the substrate also tended to get scraped off. A relatively more accurate method is to estimate the number of nanotubes per unit area from a statistically significant number of SEM images and calculate the total mass per unit area of substrate by assuming theoretical density of H2Ti3O7 (3.163 g/cm3). By scaling appropriately to the size of the experimental nanotube array sample (30 mm × 5 mm) and assuming nanotubes of uniform inner and outer diameter growing outwards from both faces of the Ti substrate, we obtained the total mass of the H2Ti3O7 nanotubes per sample with an estimated error of ±10%.In each case, the time evolution of the optical absorption was used to calculate the photodecomposition rate for identical masses of the H2Ti3O7 NTA and the comparison samples. Figure 6 shows that the normalized absorption C/C0 (C = concentration at time t, C0 = initial concentration) decays exponentially with time, which implies that the photodecomposition is a first order reaction. The calculated rate constant was the highest (0.002 min−1) for the supported H2Ti3O7 NTA sample. In comparison, the corresponding rate constant is 0.001 min−1 for P-25 and 0.0003 min−1 for the H2Ti3O7 nanotube mesh. We point out that the specific surface area of the P-25 Degussa powder (as per the specification sheet) is 50 ± 15 m2/g, which is in between the values for the substrate-attached HTO sample and for free H2Ti3O7 nanotubes (see Section 3.1). However, it is well-known that the high photocatalytic activity of P-25 arisesmainlyfrom reasons other than high surface area. P-25 is a mixed phase system containing atypically small rutile crystallites intermeshed with anatase crystallites. Charges produced on rutile by visible light are stabilized through rapid electron transfer to lower energy anatase lattice trapping sites. Thus, rutile acts as an antenna that extends the photoactivity into visible wavelengths and the structural arrangement of biphasic TiO2 crystallites creates catalytic “hot spots” at the rutile-anatase interface [21]. Thus, a direct quantitative comparison of P-25 and HTO nanotubes based on surface area alone would be inaccurate. However, our rate constant data (Figure 6) indicates at least that the dye degradation rate of the H2Ti3O7 NTA photocatalyst compares very favorably with standard commercial photocatalysts.Figure 6
Photocatalytic degradation curves for H2Ti3O7 nanorod array (filled circles), P-25 Degussa (half-filled circles), and H2Ti3O7 nanoparticles (open circles), where C/C0 = normalized absorption. The corresponding rate constants are also shown.Additional control experiments were performed to confirm the photocatalytic efficiency off the H2Ti3O7 NTA. The time dependence of the RhB solution concentration was monitored (i) on being exposed to UV irradiationwithout the H2Ti3O7 NTA and (ii) in presence of the H2Ti3O7 NTA butwithout UV irradiation. Almost no change in the RhB concentration was observed during either case, thereby confirming that both the H2Ti3O7 photocatalystand the UV light are necessary for the efficient degradation of RhB. Earlier studies [14, 15] had reported that the rate of surface adsorption of dye (in the dark) on H2Ti3O7 nanotubes is faster than the rate of dye degradation under UV light. But our study clearly shows that the rate of dye degradation under UV is much faster than the surface adsorption in the dark. This may be ascribed to the much larger effective surface area of the nanotube array catalyst and possibly also to the greater crystallinity of the sample.Our study has also established the following important issues. While several earlier authors—such as Hodos et al. [12]—had suggested that “undoped tri-titanate nanotubes failed to act as photocatalysts” and need to be sensitized with CdS, we have shown clear evidence of strong photocatalytic activity in this materialwhen in the form of an array. One of the few papers that reported significant photocatalytic activity in H2Ti3O7 nanofibers [9] also found the activity to be measurably enhanced when the nanofibers were decorated with anatase nanoparticles. Zheng et al. have recently reported the synthesis of hydrogenated anatase nanotube powder by heating pristine H2Ti3O7 nanotubes in H2 atmosphere [22]. They suggest that the hydrogenated TiO2 nanotube surface shows better photocatalytic activity than bare TiO2 nanorods and P-25. The rate constant of this sample for H2-production is 3.8 times higher than that of P-25 and 3.2 times that of bare TiO2 nanorods. The enhanced photocatalytic activity is ascribed to improved visible light absorption and efficient separation of photogenerated excitons by the surface Ti–H bonds.It is instructive to compare the degradation rate for the sulforhodamine dye by the H2Ti3O7 nanofiber mesh [9] with that for the rhodamine B by H2Ti3O7 nanotube arrays, reported here. An extrapolation of the data in [9] indicates that the dye concentration falls to 50% in ≈ 200 min, while in the present study it is found to fall to 50% in ≈ 300 min. Hence, an (roughly) aligned nanotube array, anchored to a substrate, is an extremely effective structure from the point of view of catalysis. Significantly, the surface of the HTO nanotube array has a strong affinity for aqueous media. In fact, the surface exhibits superhydrophilic behavior to an approaching water drop, which is sucked up rapidly on contact (see video clip: Supplementary Material 1 available online at http://dx.doi.org/10.1155/2014/328618). Further, on recycling the H2Ti3O7  NTA catalyst, we found almost no change in the crystal structure and overall morphology—as confirmed by XRD and TEM observations (not shown here). The catalytic activity decays slightly on recycling (with 0.001 < k < 0.002) but does not fall below the performance of P-25.


## 4. Conclusions

We have demonstrated that an aligned array of crystalline hydrogen titanate nanotubes acts as an effective and recyclable photocatalyst for the degradation of organic dye molecules such as rhodamine B. This is in contrast to previous studies on the same nanotubes in the form of a powder or mesh, which generally exhibited poor photocatalytic activity, if at all. In the present case, the fact that theself-supported nanotubes are permanently attached to both faces of a large area Ti foil (which can easily be as large as 10 cm × 10 cm) leads to the following obvious advantages when used as a nanocatalyst. (1)High surface area: in the roughly aligned array, the nanotubes maintain a minimum separation, thus ensuring a higher surface area (and better catalytic activity) than in a nanotube mesh. The unique structure—with the nanotubes growing out ofboth faces of the central Ti foil—leads to a further doubling of the exposed surface of the catalyst. (2)Superhydrophilic surface:the superhydrophilic nature of the nanotube array surface promotes rapid contact with water-soluble reactants. (3)Minimal agglomeration: being anchored at one end, the chances of nanotubes agglomerating over prolonged use are minimal. A regeneration of the catalyst by heating is a practical possibility in this case, while spherical nanoparticles would be prone to thermal aggregation. (4)High efficiency:the photodecomposition rate constant for the supported H2Ti3O7 nanotube array catalyst is comparable to or higher than those of both H2Ti3O7 nanotube powder and P-25 (Degussa). (5)Ease of handling: the central Ti foil acts as a holder for the nanotubes, making it simple to introduce and remove them from a liquid reaction bath for subsequent regeneration and reuse.In summary, we have presented substantial data to suggest that well-crystallized, substrate-anchored H2Ti3O7 nanotube arrays—synthesized by a simple hydrothermal method—should prove to be extremely useful in important, large scale, environmental applications such as the removal of organic contaminants from wastewater with high efficiency and stability and recyclability.



---

*Source: 328618-2014-04-15.xml*