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Article

Enhanced Photodegradation of p-Nitrobenzoic Acid by Binary Mixtures with Ba2+/TiO2 and MCM-41

by
Xianyuan Fan
1,2,
Hong Liu
1,2,*,
Weikun Song
3 and
Chia-Yuan Chang
4
1
Department of Resource and Environmental Engineering, Wuhan University of Science and Technology, Wuhan 430081, China
2
Hubei Key Laboratory for Efficient Utilization and Agglomeration of Metallurgic Mineral Resources, Wuhan University of Science and Technology, Wuhan 430081, China
3
China Institute of Water Resources and Hydropower Research, Beijing 100048, China
4
Department of Environment Engineering and Science, Chia Nan University of Pharmacy and Science, Tainan 71710, Taiwan
*
Author to whom correspondence should be addressed.
Materials 2021, 14(9), 2404; https://doi.org/10.3390/ma14092404
Submission received: 9 March 2021 / Revised: 22 April 2021 / Accepted: 29 April 2021 / Published: 5 May 2021
(This article belongs to the Special Issue Photocatalytic Materials for Environment Treatment and Energy Production)
Browse Figures
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Abstract

:
A novel Ba(II)/TiO2–MCM-41 composite was synthesized using binary mixtures with Ba2+/TiO2 and MCM-41, and Ba2+ as a doping ion of TiO2. The specific surface area and pore structure characterizations confirm that a mesoporous structure with a surface area of 341.2 m2/g and a narrow pore size distribution ranging from 2 to 4 nm was achieved using Ba(II)/TiO2–MCM-41. Ba(II)/TiO2 particles were synthesized into 10–15 nm particles and were well dispersed onto MCM-41. The diffraction peaks in the XRD patterns of TiO2–MCM-41 and Ba(II)/TiO2–MCM-41 were all attributed to anatase TiO2. By taking advantage of MCM-41 and Ba2+, the photocatalytic performance of Ba(II)/TiO2–MCM-41 was remarkably enhanced by suppressing its rutile phase, by lowering the band gap energy, and by facilitating the dispersion of TiO2. Therefore, the photodegradation efficiencies of p-nitrobenzoic acid (4 × 10−4 mol/L) by various photocatalysts (60 min) under UV light irradiation are arranged in the following order: Ba(II)/TiO2–MCM-41 (91.7%) > P25 (86.3%) > TiO2–MCM-41 (80.6%) > Ba(II)/TiO2 (55.7%) > TiO2 (53.9%). The Ba(II)/TiO2–MCM-41 composite was reused for five cycles and maintained a high catalytic activity (73%).

Graphical Abstract

1. Introduction

TiO2 has been extensively studied as a photocatalyst in the photodegradation of organic pollutants due to its relatively high photocatalytic activity, excellent chemical stability, and nontoxic characteristics [1,2,3,4]. However, its associated disadvantages, such as low quantum yield and relatively small surface area, as well as its difficulty being separated and retrieved from treated water, may limit its in situ application in photodegrading organic pollutants [5,6]. In addition, TiO2 nanoparticles are small but easily form an agglomerate. During the past several decades, researchers have discovered that the agglomeration of TiO2 nanoparticles and their phase transition from an anatase to a rutile form can be inhibited efficiently [4,5]. Thus, to address these issues, improvements have been conducted by using surface modification, porous material loading or blocking, and metal/nonmetal doping [7,8,9,10].
Metal doping provides a convenient method of solving the problems associated with the use of TiO2 in photodegradation [11,12,13]. Both the photophysical and the photochemical activities of TiO2 are affected by the doping of metal ion and oxide [14,15]. Transition metals (such as Cr [16], Ag [17], Fe [18], Rh [19], and V [20]) have been employed as dopants of TiO2, but the phenomenon with alkaline earth metals is understudied [21]. Kumaresan [22] prepared TiO2 nanoplates doped with Sr2+ and evaluated their photocatalytic activities using 2,4-dinitrophenol (2,4-DNP) as a target pollutant. The complete mineralization of 2,4-DNP by Sr2+-doped TiO2 nanoplates required a shorter photodegradation time than the TiO2 nanoparticles. According to Rodriguez et al. [23], the ionic radius of dopants and their electric charges are the important parameters that control stabilization of the anatase phase, and the transition temperature of the anatase–rutile process is plotted as a function of the charge of the ion times its volume. Ba2+ demonstrated the best stabilization due to its largest charge ionic volume.
Since Mobil Company successfully synthesized an MCM-41 molecular sieve (MCM-41) in 1992, MCM-41 has been widely used in catalysis, adsorption, separation, and other fields because of its large specific surface area, high porosity, narrow pore size distribution, and other beneficial characteristics [24,25,26]. Although UV and visible light are not absorbed by MCM-41 composed of SiO2, its readily accessible mesoporous frameworks and adjustable porosities are beneficial to the incorporation of metal ions [27,28]. In addition, by dispersing photocatalysts on MCM-41, the composites are provided with improved light absorption performance [28,29]. According to Dong et al. [29], the photocatalytic efficiency of Acid Red B by TiO2/MCM-41 reached 100% within 2 h.
In this study, the feasibility and role of Ba2+ as a doping ion of TiO2 were evaluated. The mesoporous MCM-41 was mechanically mixed with the Ba(II)/TiO2 composite to disperse and improve the reactive surface area of the aqueous media. The physical and chemical properties of Ba(II)/TiO2–MCM-41 were characterized by adopting a specific surface analyzer, a transmission electron microscope (TEM), X-ray photoelectron spectroscopy (XPS), X-ray diffraction (XRD), and UV-vis diffuse reflectance spectroscopy (UV-vis DRS). The photocatalytic activity and reaction rate constant of Ba(II)/TiO2–MCM-41 was evaluated by a photodegrading p-nitrobenzoic acid in an aqueous solution under UV light irradiation. The findings obtained were compared with that of the TiO2–MCM-41, Ba(II)/TiO2, TiO2, and P25. Finally, the service life and cycle times of the Ba(II)/TiO2–MCM-41 catalyst were investigated.

2. Materials and Methods

2.1. Materials and Chemicals

MCM-41, Degussa P25 (P25), was obtained from Nankai University Catalyst Co. (Tianjin, China). Tetrabutyl titanate (Ti(OBu)4), Ba(NO3)2, anhydrous alcohol, acetic acid (99.5%), and p-nitrobenzoic acid were purchased from Tianda Chemical Co. (Tianjin, China). All chemicals used in this study were of analytical grade and were used as received.

2.2. Preparation of Ba(II)/TiO2–MCM-41

2.2.1. Preparation of Ba(II)/TiO2 and TiO2

The conventional sol–gel method was employed to prepare the Ba(II)/TiO2 composite. Specifically, 0.0028 g Ba(NO3)2 was dissolved in 8.75 mL ethanol and, then 0.5 mL acetic acid (99.5%) was added. The resulting solution was stirred for 10 min at 250 rpm. Subsequently, the mixture of 8.75 mL ethanol and 7.5 mL Ti(OBu)4 was added dropwise into the solution. The mixture was continuously stirred until the gel was formed. The gel was dried at 80 °C and ground after cooling. Finally, a calcination kept at 700 °C for 2 h was carried out to obtain the Ba(II)/TiO2 composite. The mass ratio of TiO2:Ba (II) in the resulting composite was 3:0.0025. Same procedure was adopted for TiO2 preparation except for the addition of Ba(NO3)2.

2.2.2. Preparation of Mixtures with Ba(II)/TiO2 and MCM-41

The binary mixtures with Ba(II)/TiO2 and MCM-41 were prepared by a liquid phase mixing method. First, 0.0028 g Ba(NO3)2 was dissolved in 8.75 mL ethanol, after which 0.5 mL acetic acid (99.5%) was added to the solution and stirred for 10 min at 250 rpm. Subsequently, the mixture of 8.75 mL ethanol and 7.5 mL Ti(OBu)4 was added dropwise into the solution. After the solution was stirred rapidly for 30 min, 1.2 g of MCM-41 powder was mixed. Next, 3 mL of deionized water was added dropwise under vigorous stirring. The mixture was continuously stirred until the gel was formed. The gel was dried at 80 °C and then ground after cooling down. Finally, a calcination kept at 700 °C for 2 h was carried out to obtain the Ba(II)/TiO2–MCM-41 composite. The mass ratio of the Ba(II)/TiO2 to MCM-41 in the resulting composite was 3:2. The same procedure was adopted for TiO2–MCM-41 preparation, except for the addition of Ba(NO3)2.

2.3. Characterizations

The X-ray diffraction (XRD) measurements for the Ba-doped and the undoped TiO2–MCM-41 powders were conducted by an X-ray diffractometer (max-IIIA, Rigaku D, Japan). The specific surface area of the N2 adsorption–desorption isotherm and the pore parameters were measured using an Autosorb-1-MP/LP analyzer (Quantachrome instruments, Tallahassee, FL, USA). A morphological analysis was carried out by an H-9500 transmission electron microscope (Hitachi, Hitachi, Japan). The UV-vis absorption spectrum and the absorbance (λ = 270 nm) of p-nitrobenzoic acid at different photodegradation times were obtained using a UV-2550 spectrophotometer (Shimadzu, Tokyo, Japan). The UV-vis diffuse reflectance spectra of the Ba(II)/TiO2–MCM-41 were also obtained by using UV-2550 with the aid of a solid module. The surface chemical compositions and oxidation states were examined using an X-ray photoelectron spectrometer (Escalab 250Xi, Thermo Fisher Scientific, Waltham, MA, USA).

2.4. Photocatalytic Activity Measurement

Photodegradation of p-nitrobenzoic acid by different photocatalysts was conducted in a reactor equipped with a 300 W high-pressure mercury lamp emitting UV irradiation mainly in the range of 250–400 nm [30]. The photocatalyst was dispersed into the p-nitrobenzoic acid (4 × 10−4 mol/L, pH = 4.0 ± 0.1) aqueous solution at a dose of 0.5 g/L, and the mixture was stirred at 200 rpm for 60 min. At given time intervals, a 10 mL suspension was withdrawn and centrifuged, and the supernatant was used to determine the concentration of p-nitrobenzoic acid after UV irradiation.
The photodegradation efficiency of p-nitrobenzoic acid can be expressed as follows:
η = (C0 − C)/C0 × 100% = (A0 − A)/A0 × 100%
where C0 and A0 are the initial concentration and the absorbency of p-nitrobenzoic acid, respectively, and where C and A are the concentration and absorbency of p-nitrobenzoic acid after photodegradation time (t), respectively.

3. Results

3.1. BET Specific Surface Area and Pore Parameters

The pore size distribution and the N2 adsorption–desorption isotherms of the Ba(II)/TiO2–MCM-41 are shown in Figure 1. It was found that the Ba(II)/TiO2–MCM-41 composite exhibits a narrow pore size distribution of 2–4 nm with a characteristic peak at 2.71 nm.
The BET (Brunauer-Emmett-Teller) specific surface area (SBET) and the pore parameters of TiO2, MCM-41, TiO2–MCM-41, and Ba(II)/TiO2–MCM-41 are presented in Table 1. The SBET of the Ba(II)/TiO2–MCM-41 composite was 341.2 m2·g−1, and this was found to be lower than that of MCM-41 (805.8 m2·g−1) due to loading of Ba(II)/TiO2 onto the surface of MCM-41 but was much higher than that of TiO2 (65.8 m2·g−1). The large SBET of Ba(II)/TiO2–MCM-41 could enhance the contact with organic molecules and increase the adsorption of water and hydroxyl. The adsorbed water and hydroxyl may react with the photoexcited holes on the surface of Ba(II)/TiO2–MCM-41 to generate hydroxyl radicals. In addition, the mesoporous structure and high pore volume (0.357 cm3/g) of the Ba(II)/TiO2–MCM-41 composite allowed for rapid diffusion of the reactants and products during the photocatalytic reaction. These properties of Ba(II)/TiO2–MCM-41 are beneficial to the photodegradation of organic contaminants.

3.2. TEM Images

The TEM images of MCM-41 and Ba(II)/TiO2–MCM-41 are shown in Figure 2. As shown in Figure 2a, the MCM-41 is characterized by a highly ordered structure with a uniform aperture. Figure 2b shows that the Ba(II)/TiO2 particles are well dispersed on the surface of the MCM-41, and this may be attributed to the fact that MCM-41 is a mesoporous material with a pore size of 3.15 nm (as shown in Table 1). In addition, the Ba(II)/TiO2 particles are too large (5–15 nm) to enter the pores of the MCM-41. As a result, the Ba(II)/TiO2–MCM-41 composite exhibits less regularity in pore structure. However, the mesoporous structure is still maintained.

3.3. XPS Analyses

Figure 3 presents a typical survey spectrum of Ti 2p, O 1s, and Si 2p. It can be observed that Ti and O show the strongest peaks, as expected since they make up the crystal lattice of TiO2. Unfortunately, the characteristic peak of Ba was not observed, which may be due to the low content of Ba in the Ba(II)/TiO2–MCM-41 composite. In order to determine the chemical state of Ti/Si in the composite, the high-resolution XPS spectra of Ti, Si, and O were analyzed separately, as shown in Figure 4. The XPS spectra of the Ti 2p spin orbit components were located at bonding energies of 458.8 and 464.3 eV, thus corresponding to Ti 2p3/2 and Ti 2p1/2, respectively. The strongest peak is the Ti 2p3/2, and this corresponds with tetravalent Ti4+. These results are in accordance with that in the literature [31,32].
The XPS spectrum of the Si 2p includes two peaks located at 102.8 and 102.2 eV that are attributed to the Si–O–Si and Ti–O–Si linkages [33]. This evidence confirms that Ti4+ in a titania octahedral lattice can be replaced by Si4+, and vice versa [34,35]. The XPS spectrum of the O 1s comprises several peaks in the regions from 528 to 537 eV. The strong peaks of O 1s appear at 529.8 and 533.2 eV and are ascribed to oxygen in the Ti–O–Ti linkage of the TiO2 and OH groups in Ti–OH and Si–OH bonding, respectively. The peak arising at 530.7 eV belongs to Ti–O–Si bonds, and this could be due to the coordination of Ti and Si atoms in the matrix surface [32].

3.4. XRD Analyses

The XRD patterns of MCM-41, TiO2, TiO2–MCM-41, and Ba(II)/TiO2–MCM-41 are shown in Figure 5. The peaks at 2θ = 5.7° (Figure 5b) and 23.0° (Figure 5a) are characteristic of MCM-41, as reported elsewhere [28,29,36,37]. The diffraction peaks of the anatase phase and rutile phase appear simultaneously in the diffraction pattern of TiO2. There are ten obvious rutile characteristic peaks (2θ = 27.5°, 36.1°, 39.3°, 41.2°, 44.1°, 54.2°, 56.8°, 64.2°, 69.0°, and 69.9°), while only two anatase characteristic peaks can be observed. However, the XRD pattern of TiO2–MCM-41 shows an opposite situation, with all of the diffraction peaks being attributed to the anatase phases. It was reported that TiO2 will be transformed from an anatase phase to a rutile phase when the calcination temperature is higher than 600 °C [29]. The TiO2 in TiO2–MCM-41 still exists in an anatase phase under 700 °C calcination for 2 h in the present study, and this may be caused by the formation of a Ti–O–Si bond between the Ti (Ⅳ) and Si (Ⅳ). In other words, the loading of TiO2 onto the surface of MCM-41 inhibits the phase transformation of TiO2 at higher calcination temperatures.
The doping of Ba2+ into TiO2–MCM-41 has no obvious effect on crystal structure, except that the diffraction peak intensity of the anatase phase is slightly higher. This is because the radius of Ba2+ (134 pm) is larger than that of Ti4+ (61 pm) and close to the radius of O2− (140 pm). The anatase structure is more open than the rutile structure, and large substituting groups can be more easily accommodated in this structure than in a rutile structure [23]. As a result, the anatase crystalline structure is more difficult to transform into a rutile structure.
The calculated diffraction patterns of the Ba(II)/TiO2–MCM-41 composite were analyzed using the Scherrer equation to infer the crystallite size, ≈33.5 nm. The particle size measured via TEM is smaller (10–15 nm) than that deduced from the Scherrer formula (≈33.5 nm, Figure 2b) because the fusion of the neighboring tiny particles caused substantial overestimation of the primary particles, as suggested recently by Weidenthaler [38].

3.5. UV-Vis Diffuse Reflectance Spectra

The UV-visible diffuse reflectance spectra of TiO2, TiO2–MCM-41, Ba(II)/TiO2–MCM-41, and P25 are presented in Figure 6. The Ba(II)/TiO2–MCM-41 composite exhibited a higher absorbance than the other photocatalysts in the UV light range. Moreover, the absorption spectra of Ba(II)/TiO2–MCM-41 is slightly shifted to the visible light range. According to the equation Eg = 1240/λ (where λ is the wavelength edge of the absorption band) [39], the band gaps energy of TiO2, TiO2–MCM-41, P25, and Ba(II)/TiO2–MCM-41 were calculated as 3.26, 3.22, 3.21, and 3.19 eV, respectively. The decrease in band gap energy increased the number of photogenerated electrons and holes to participate in the photocatalytic reaction. This resulted in an improvement in the photocatalytic activity of Ba(II)/TiO2–MCM-41.

3.6. Photodegradation of p-Nitrobenzoic Acid

The photocatalytic reactivity of the Ba(II)/TiO2–MCM-41 composite was evaluated by the photodegradation of p-nitrobenzoic acid under UV light irradiation and compared with that of TiO2–MCM-41, Ba(II)/TiO2, TiO2, and P25 (shown in Figure 7a). Moreover, the photodegradation efficiency of p-nitrobenzoic acid under only UV irradiation (without photocatalyst) and the adsorption efficiency of MCM-41 and Ba(II)/TiO2–MCM-41 on p-nitrobenzoic acid without irradiation were also tested (shown in Figure 7b). The photodegradation efficiencies of all photocatalysts are as follows: Ba(II)/TiO2–MCM-41 > P25 > TiO2–MCM-41 > Ba(II)/TiO2 > TiO2. The highest photocatalytic activity belongs to Ba(II)/TiO2–MCM-41, with a photodegradation efficiency of 91.7% at 60 min. The following photodegradation efficiencies, 86.3%, 80.6%, 55.7%, and 53.9%, were achieved by P25, TiO2–MCM-41, Ba(II)/TiO2, and TiO2, respectively. These results indicate that the photocatalytic activity of TiO2 is enhanced by the addition of MCM-41 and by doping Ba(II), hence the higher photocatalytic activity than that of P25.
Due to the contributions of both photocatalysis and the adsorption towards the removal of p-nitrobenzoic acid, the adsorption ability of Ba(II)/TiO2-MCM-41 and MCM-41 were characterized in a dark condition (no irradiation) as shown in Figure 7b. The adsorption efficiency of Ba(II)/TiO2–MCM-41 after 60 min was mainly due to the MCM-41.
MCM-41 prevented the anatase from transforming into a low activity rutile phase, and the mesoporous structure and facilitated dispersion of MCM-41 allowed for rapid contact and diffusion of the reactants and products. The lower band gap energy of Ba(II)/TiO2–MCM-41 accelerated the generation of photogenerated electrons and holes in the photocatalytic reaction, and consequently assisted with the improvement in the photocatalytic activity of Ba(II)/TiO2–MCM-41.
The photodegradation kinetics of p-nitrobenzoic acid can be described by the zero order equation as follows:
C 0 − C = kt
where C0 and C are the initial concentration and the residue concentration after irradiation of p-nitrobenzoic acid solution, respectively; t is the time for irradiation (min); and k is the kinetic rate constant obtained from the slope of the linear graph illustrated in Figure 8. All graphs are linear, with a coefficient of determination (R2) greater than 0.99. The reaction rate constants (k) and R2 are summarized in Table 2.
Among various photocatalysts, the reaction rate constant of the Ba(II)/TiO2–MCM-41 is the highest value of 0.00631 mmol·L−1·min−1. Therefore, the mesoporous structure and facilitated dispersion of the Ba(II)/TiO2/MCM-41 allowed for rapid contact and diffusion of the reactants and products, which consequently enhanced the efficiency and reaction rate of the photocatalytic reaction.
In addition to the photocatalytic activity, stability was another important issue for their practical application. The recycling test for the photocatalysis of p-nitrobenzoic acid are shown in Figure 9. In our experiment, the stability of the Ba(II)/TiO2–MCM-41 composite was evaluated by performing the cycling experiments under the same conditions. With the reuse time increasing, the photocatalytic activity of p-nitrobenzoic acid demonstrated no obvious reduction. The Ba(II)/TiO2–MCM-41 composite reused for five cycles maintained a high catalytic activity (about 73%). This result indicated that the Ba(II)/TiO2–MCM-41 composite exhibited an excellent recycle performance.

4. Conclusions

This study investigated the physical and chemical properties of TiO2 doping with Ba2+ and mixing with MCM-41 as well as the photocatalytic activity of the Ba(II)/TiO2–MCM-41 composite in the photodegrading p-nitrobenzoic acid under UV light irradiation. It was found that the BET specific surface area of Ba(II)/TiO2–MCM-41 (341.2 m2·g−1) is much larger than that of TiO2 (65.8 m2·g−1). The TEM spectra showed that the TiO2 and Ba(II)/TiO2 particles were synthesized into 10–15 nm particles and well dispersed onto the MCM-41. The XPS spectra showed the formation of Ti–O–Si bonds in Ba(II)/TiO2–MCM-41, which inhibited the transformation of TiO2 from an anatase phase to a rutile phase. As a result, all of the diffraction peaks in the XRD patterns of TiO2–MCM-41 and Ba(II)/TiO2–MCM-41 were attributed to the anatase TiO2. Among the five photocatalysts (TiO2, Ba(II)/TiO2, TiO2–MCM-41, Ba(II)/TiO2–MCM-41, and P25), the photocatalytic performance of Ba(II)/TiO2–MCM-41 was remarkably enhanced by suppressing the rutile phase, by lowering the band gap energy, and by facilitating the dispersion of TiO2 by using the advantages of MCM-41 and Ba2+. The efficiency of the photodegrading p-nitrobenzoic acid (4 × 10−4 mol/L) under UV light irradiation by Ba(II)/TiO2–MCM-41 reached 91.7% at 60 min. The Ba(II)/TiO2–MCM-41 composite was reused for five cycles and maintained a high catalytic activity, thus indicating that the Ba(II)/TiO2–MCM-41 composite exhibited an excellent recycle performance.

Author Contributions

H.L., X.F., W.S. and C.-Y.C. conceived and designed the methodology; X.F. and W.S. performed the experiment and prepared the composite materials; H.L and C.-Y.C. analyzed the data. All authors evaluated and discussed the results and wrote the paper together. All authors have read and agreed to the published version of the manuscript.

Funding

This research was funded by the Key Project of Natural Science Foundation of China (grant No. 41230638).

Institutional Review Board Statement

Not applicable.

Informed Consent Statement

Not applicable.

Data Availability Statement

All relevant data presented in the article are stored according to institutional requirements and, as such, are not available online. However, all data used in this manuscript can be made available upon request to the authors.

Acknowledgments

Many thanks goes to the Open Fund of Hubei Key Laboratory for Efficient Utilization and Agglomeration of Metallurgic Mineral Resources from Wuhan University of Science and Technology (2017zy008).

Conflicts of Interest

The authors declare no conflict of interest.

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Materials 14 02404 g001 550
Figure 1. Pore size distribution of Ba(II)/TiO2–MCM-41 and TiO2–MCM-41.
Figure 1. Pore size distribution of Ba(II)/TiO2–MCM-41 and TiO2–MCM-41.
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Materials 14 02404 g002 550
Figure 2. TEM images of MCM-41 (a) and Ba(II)/TiO2/MCM-41 (b).
Figure 2. TEM images of MCM-41 (a) and Ba(II)/TiO2/MCM-41 (b).
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Materials 14 02404 g003 550
Figure 3. XPS survey spectra of the Ba(II)/TiO2–MCM-41 composite.
Figure 3. XPS survey spectra of the Ba(II)/TiO2–MCM-41 composite.
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Materials 14 02404 g004a 550Materials 14 02404 g004b 550
Figure 4. High-resolution XPS spectra of the Ba/TiO2–MCM-41composite for Ti 2p (a), O 1s (b), and Si 2p (c).
Figure 4. High-resolution XPS spectra of the Ba/TiO2–MCM-41composite for Ti 2p (a), O 1s (b), and Si 2p (c).
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Figure 5. XRD patterns of MCM-41—1, TiO2—2, TiO2–MCM-41—3, and Ba(II)/TiO2–MCM-41—4 scanned at wide angle (a) and low angle (b).
Figure 5. XRD patterns of MCM-41—1, TiO2—2, TiO2–MCM-41—3, and Ba(II)/TiO2–MCM-41—4 scanned at wide angle (a) and low angle (b).
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Materials 14 02404 g006 550
Figure 6. UV-vis diffuse reflectance spectra of Ba(II)/TiO2–MCM-41—a, P25—b, TiO2–MCM-41—c, and TiO2—d.
Figure 6. UV-vis diffuse reflectance spectra of Ba(II)/TiO2–MCM-41—a, P25—b, TiO2–MCM-41—c, and TiO2—d.
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Figure 7. Photodegradation efficiencies of p-nitrobenzoic acid by different photocatalysts under (a) UV irradiation and (b) no irradiation (reaction conditions: C0 = 4 × 10−4 mol/L, dosage of material = 0.5 g/L, initial pH = 4.0 ± 0.1).
Figure 7. Photodegradation efficiencies of p-nitrobenzoic acid by different photocatalysts under (a) UV irradiation and (b) no irradiation (reaction conditions: C0 = 4 × 10−4 mol/L, dosage of material = 0.5 g/L, initial pH = 4.0 ± 0.1).
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Figure 8. Zero order models for the photodegradation of p-nitrobenzoic acid by various photocatalysts.
Figure 8. Zero order models for the photodegradation of p-nitrobenzoic acid by various photocatalysts.
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Figure 9. Recycling test for the photocatalysis of p-nitrobenzoic acid by Ba(II)/TiO2–MCM-41 (reaction conditions: C0 = 4×10-4 mol/L, dosage of material = 0.5 g/L, reaction time: t = 60 min, initial pH = 4.0 ± 0.1).
Figure 9. Recycling test for the photocatalysis of p-nitrobenzoic acid by Ba(II)/TiO2–MCM-41 (reaction conditions: C0 = 4×10-4 mol/L, dosage of material = 0.5 g/L, reaction time: t = 60 min, initial pH = 4.0 ± 0.1).
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Table
Table 1. SBET and pore parameters of different materials.
Table 1. SBET and pore parameters of different materials.
SamplesSpecific Surface Area
(m2·g−1)		Average Pore Size
(nm)		Pore Volume
(mL·g−1)
TiO265.83.750.207
MCM-41805.83.150.811
TiO2–MCM-41358.82.750.429
Ba(II)/TiO2–MCM-41341.22.710.357
Table
Table 2. Reaction rate constant (k) and correlation coefficient (R2) of various photocatalysts.
Table 2. Reaction rate constant (k) and correlation coefficient (R2) of various photocatalysts.
Photocatalystsk (mmol·L−1·min−1)R2
TiO20.003600.999
Ba(II)/TiO20.003770.999
P250.005930.997
TiO2–MCM-410.005440.998
Ba(II)/TiO2–MCM-410.006310.998
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Fan, X.; Liu, H.; Song, W.; Chang, C.-Y. Enhanced Photodegradation of p-Nitrobenzoic Acid by Binary Mixtures with Ba2+/TiO2 and MCM-41. Materials 2021, 14, 2404. https://doi.org/10.3390/ma14092404

AMA Style

Fan X, Liu H, Song W, Chang C-Y. Enhanced Photodegradation of p-Nitrobenzoic Acid by Binary Mixtures with Ba2+/TiO2 and MCM-41. Materials. 2021; 14(9):2404. https://doi.org/10.3390/ma14092404

Chicago/Turabian Style

Fan, Xianyuan, Hong Liu, Weikun Song, and Chia-Yuan Chang. 2021. "Enhanced Photodegradation of p-Nitrobenzoic Acid by Binary Mixtures with Ba2+/TiO2 and MCM-41" Materials 14, no. 9: 2404. https://doi.org/10.3390/ma14092404

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