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Article

Environment-Friendly Nanoporous Titanium Dioxide with Enhanced Photocatalytic Activity

by
Fatimah Al Qarni
1,
Nuhad A. Alomair
2,3 and
Hanan H. Mohamed
2,3,*
1
Department of Chemistry, Science College, Hafr Al Batin University, P.O. Box 1803, Hafr Al Batin 31991, Saudi Arabia
2
Department of Chemistry, Science College, Imam Abdulrahman Bin Faisal University, P.O. Box 1982, Dammam 31441, Saudi Arabia
3
Basic and Applied Research Centre, Imam Abdulrahman Bin Faisal University, P.O. Box 1982, Dammam 31441, Saudi Arabia
*
Author to whom correspondence should be addressed.
Catalysts 2019, 9(10), 799; https://doi.org/10.3390/catal9100799
Submission received: 24 August 2019 / Revised: 11 September 2019 / Accepted: 18 September 2019 / Published: 25 September 2019
(This article belongs to the Section Photocatalysis)
Browse Figures
Versions Notes

Abstract

:
Nanoporous TiO2 anatase was environment-friendly prepared using coffee husk extract (CHE) as bio-template instead of hazardous chemicals and solvents and ultrasonic waves. Caffeine and caffeic acid were found to be the main compounds in CHE to modify the morphology of TiO2. The properties of as-prepared titanium dioxide particles were determined by different characterization techniques. The results demonstrate the formation of a meso/macro-porous channel consisting of small TiO2 particles (8–10 nm). The as prepared green nanoparticles exhibited improved photocatalytic activity for the degradation of organic water pollutants with good recyclability. The enhancement in efficiency of green nanoporous TiO2 can be attributed to higher surface area and the presence of more active adsorption sites inside the pores. The current research provides for a low cost, safe, and eco-friendly way to produce efficient photocatalysts for remediation of polluted water.

Graphical Abstract

1. Introduction

Nowadays, water pollution has turned into a worldwide issue and the entire environment is aggravating as well as more diseases are caused worldwide due to water pollution [1,2]. Accordingly, water is treated in a number of traditional ways such as chemical precipitation, ion exchange, and electrochemical removal. But these procedures have huge drawbacks, as they lead to incomplete removal, require high-energy, and produce toxic materials [3,4,5,6]. Among various wastewater treatment methods, the photocatalytic process in aqueous suspension of semiconductor nanomaterials has received considerable attention in view of rapid and efficient destruction of pollutants [7,8,9,10,11]. Among various semiconductor nanomaterials, titanium dioxide (TiO2) has been a widely investigated semiconductor as the most suitable material for environmental and energy applications due to its unique properties [12]. There are many ways for the preparation of TiO2 such as the solvothermal method, hydrothermal method, sol-gel method, chemical vapor deposition, and electrodeposition. Nevertheless, these methods require high energy and hazardous materials and solvents [13,14,15,16]. Green synthesis of nanomaterials is an alternative route to physical and chemical methods that leads to environment-friendly products due to the use of non-toxic materials, and does not require high temperatures and pressure, and at a lower cost. Green synthesis may be by microorganisms, plant extracts, and plant biomass [17,18]. Therefore, using such a green and environmentally friendly method can also minimize the use of chemicals and toxic solvents. In order to control crystal growth, approaches including the use of plant extracts as reducing/oxidizing agents, stabilizers, and capping agent, have been carried out [16,17]. Chemical compounds in the plant extract play the role of bio-template producing nanomaterials with modified morphology [17]. In addition, the eco-friendly method for synthesis of nanomaterials can also be achieved by reducing the required process temperature, using microwave or ultrasonic waves [7,8,9,10,11,12,13,14,15,16,17,18]. In recent years a number of nanoparticles have been prepared using fungi, bacteria, actinomycetes, and enzymes [19,20,21,22,23] and also have been used as many plant extracts such as camellia sinensis, neem, coriandrum, ocimum sanctum, nelumbo lucifera [24,25,26]. Recently, researchers have been able to achieve the biosynthesis of nanoparticles by any part of the plant parts such as leg, leaves, roots, flowers, buds, and seeds [27]. The use of plants to produce nanoparticles has drawn attention more than the use of other biological processes as less costly, faster, non-pathogenic, and safer [28]. Due to the variety of plants, we can easily change the source of the extract and thus control the morphology and the size of the nanoparticles as needed [29]. Plant extracts are usually stable even following multi months and do not demonstrate any noticeable changes [30]. The principle phytochemicals responsible for the synthesis of nanoparticles are alkaloids, tannins, phenolic, flavones, ketones, aldehydes, terpenoids, amides, and carboxylic acid [31,32,33,34,35].
The present paper reports the results of an ongoing study on the preparation of modified titanium dioxide nanomaterials using the environment-friendly method. In this study, the chemical compounds in the plant waste, particularly coffee husk, have been exploited as bio-template to produce nanoporous TiO2 with small particle size. The as prepared green nanoporous TiO2 exhibited enhanced photocatalytic activity under UV and solar light irradiation as compared to their counterparts prepared in the absence of the plant waste extract. Hence, this study provides the simple and green method to produce porous TiO2 nanoparticles with enhanced activity for water remediation.

2. Results and Discussion

2.1. Characterization

2.1.1. Characterization of Coffee Husk Extract

CHE was analyzed by UV-vis absorption and FTIR spectra (see Figure 1a,b, respectively). UV-vis absorption spectroscopy measurement of CHE with absorption in the range 200–400 nm shows two peaks, one peak at 275 nm attributed to caffeine and the peak at 320 nm attributed to caffeic acid [36,37]. The results indicate the presence of polyphenolic, caffeic acid and caffeine which act as bio-template forming porous TiO2 nanoparticles.
FTIR spectrum of the as obtained CHE show broad absorption peak from 3600 to 3200 cm−1 which can be assigned to –OH in polyphenolic compounds in CHE. The carbonyl C=O stretching vibration appears at 1700 cm−1 in infrared spectrum of the free caffeine. A peak occurs at 1655 cm−1 of (C=O) and (C=C) in free caffeine [38]. The quadratal CN stretching in imidazole ring appears at 1403 cm−1 of the caffeine. The vibrations of free caffeine appear at 2900, 1700, 1683, 1456 and the broad bands at 1284–973, 925 cm−1.

2.1.2. Characterization of TiO2 Nanomaterials

Figure 2 shows the XRD patterns of chemically as well as green prepared TiO2 nanoparticles. XRD of both TiO2 samples shows the diffractions peaks at 25.28°, 37.93°, 48.37°, 53.89°, 55.29°, 62.73°, 69.00°, and 75.37° for anatase phase (JCPDS no. 21–1272) [39]. Moreover, the intensities diffraction peak decreases and becomes broader for green TiO2 nanoparticles indicating smaller particle size [40]. The crystallite size of the as prepared TiO2 nanomaterials has been determined from the XRD data using the Scherrer equation to be 16 and 7.5 nm respectively, for chemically as well as green prepared TiO2 nanoparticles, respectively.
The morphological features of chemically as well as green prepared TiO2 nanoparticles have been determined by SEM and TEM measurements. SEM images TiO2 sample prepared in presence and in absence of CHE are Figure 3a–c. It was found that, while agglomeration of TiO2 particles was observed for the TiO2 sample prepared without CHE (Figure 3a), the macro porous structure with pore size of range 1.3–1.6 μm was observed for the TiO2 sample prepared with CHE (Figure 3b,c). The diameter of the TiO2 particles was noticed to be smaller for green TiO2 nanoparticles (8–10 nm) (Figure 4b) as compared to chemically prepared TiO2 (Figure 4a). The TEM results were found to be in good agreement with the XRD measurements.
Figure 5a,b shows the Raman and FTIR spectra of the as synthesized nanomaterials. The Raman spectra of the TiO2 samples prepared with and without CHE show the characteristic peaks of pure anatase phase. The band at 390 cm−1 is assigned to B1g. The bands at 510 and 620 cm−1 are assigned to A1g and the band at 140 cm−1 is assigned to Eg, which are all related to the anatase phase [41]. As shown in the inset of Figure 7a, no apparent peaks of carbon have been observed, confirming that, carbon did not dope into the TiO2 lattice in both TiO2 samples. The FTIR spectrum of TiO2 nanomaterials prepared with and without CHE present similar FTIR spectra with peak around 450 cm−1 assigned to stretching vibration of Ti–O–Ti bonds. The broad band at 3428 cm−1 can be ascribed to the –OH stretching vibration of the adsorbed water molecules on TiO2 surface and the peak around 1630 cm−1 is attributed to the bending vibrations of –OH [42]. The FTIR results indicated no adsorption of the plant extract compounds on TiO2 surface after calcination at 773 K.
The UV-vis diffuse reflectance measurements (Figure 6a) show that both TiO2 samples can only absorb UV light and reflect most light in the visible region. The band gap energy has been estimated using the Kubelka–Munk relation [43]. The band gap energy of nanomaterials prepared with and without CHS was estimated to be 3.21 eV and 3.16 eV, respectively. A slight increase in the band gap energy of the TiO2 sample prepared with CHE was observed which can be attributed to the smaller particle size [44]. Figure 6b shows the N2 adsorption–desorption measurements of the samples. The adsorption–desorption isotherms of both samples can be assigned to typical H3 hysteresis loop. The BET surface area of the samples revealed that TiO2 prepared with CHE exhibited larger surface area of about 147.15 m2/g compared to TiO2 nanoparticles prepared without CHE (53.96 m2/g) (Table 1), which can be readily attributed to the porous structure as well as the small particle size of the green TiO2 particles prepared with CHE.

2.2. Photocatalytic Performance

Photocatalytic performance of the as prepared nanomaterials has been evaluated for the degradation MB dye. The change in MB concentration was determined from UV-vis absorbance measurements. The absorbance of MB with λmax 668 nm was found to decrease gradually with irradiation (Figure 7a,b).
The photocatalytic degradation efficiency for MB degradation is shown in Figure 7c. Slow degradation was shown when TiO2 (ethanol) nanomaterial is used as a catalyst, while more efficient degradation was obtained in presence of TiO2 (CHE).
Since phenol frequently exists in industry effluents and is difficult to be degraded due to the stability of the benzene ring, the photocatalytic degradation of phenol was of interest. The degradation of phenol was monitored using the UV-vis absorbance measurement in the wavelength range (200–400 nm) (Figure 8a,b) with two characteristic bands at 210 nm and 269 nm. Upon irradiation in the presence of TiO2 nanoparticles, a gradual decrease in intensity of phenol absorbance was observed, confirming the decrease in phenol concentration. Figure 8c shows the photocatalytic degradation efficiency for phenol degradation using various TiO2 nanomaterials. Noticeable photocatalytic improvement has been achieved when TiO2 (CHE) was used as the catalyst.
The kinetics of MB and phenol degradation have been also investigated by plotting –ln (C/C0) with time. Linear correlation for MB and phenol degradation was obtained for all samples which fit well with the pseudo first-order model (Figure 7d and Figure 8d, respectively) and the apparent rate constant k’ (min−1) has been estimated and the data have been gathered in Table 2. It was found that, the observed rate constant of photocatalytic degradation of MB in the presence of TiO2 (CHE) is around 2 times higher than that in the presence of TiO2 (ethanol). In addition, the photocatalytic degradation of phenol in the presence of TiO2 (CHE) is three times higher than that when used TiO2 (ethanol) (Table 2).
The improvement of the photocatalytic performance of TiO2 (CHE) can be attributed to increasing the surface area as well as the active adsorption sites inside the pores, leading to increased accessibility for the organic pollutant and therefore enhancing photocatalytic performance.
The recyclability of the green TiO2 has been studied for 3 cycles of photocatalytic degradation of MB (20 mg L−1). Ninety-eight percent of MB was degraded even after the 3rd cycle, indicating the stability and recyclability of green nanoporous TiO2 photocatalyst (Figure 9).

3. Experimental

3.1. Preparation of Coffee Husk Extract

Coffee husk of Arabian coffee obtained from the western province, Saudi Arabia were washed several times with distilled water to remove the dust particles on their surface then dried in air. The dried husk was grinded to obtain fine powder. Twenty (20) g of coffee husk was boiled with 400 mL of distilled water for 30 min, then allowed to cool down slightly and finally filtered to obtain a clear brown solution of coffee husk extract (CHE) (Figure 10). It can be kept in a dark bottle in the fridge for further use.

3.2. Synthesis of TiO2 Nanoparticles Using CHE

Two hundred (200) mL of the CHE solution was placed in a conical flask. Five (5) mL of titanium tetraisopropoxide (TTIP) was drop-wise added to the CHE solution under ultrasonic waves. The obtained suspension was stirred overnight. After that, solid TiO2 nanoparticles were separated and washed 3 times by centrifuge. Then, dried in the oven at 70 °C and finally calcined at 500 °C for 1 h (Figure 11). For comparison, TiO2 nanoparticles were prepared in absence of CHE, in typical synthesis, 5 mL of (TTIP) in 15 mL ethanol was drop-wise added to ethanol/water solution (1:1) under continuous stirring for overnight. The TiO2 nanoparticles were separated and washed 3 times by centrifuge and denoted as (TiO2 ethanol).

3.3. Characterization

XRD measurements were performed using Shimadzu’s-XRD Powder diffractometer (xrd-700, Maxima, Shimadzu, Kyoto, Japan) with a Cu radiation source, at a scanning speed of 2 min−1, 40 kV tube voltage, and 30 mA tube current. FTIR measurements were recorded on IR AFFINITY-1 Shimadzu (Shimadzu, Kyoto, Japan) by Fourier transform and KBr (Potassium Bromide) pellets were used to obtain the absorption spectra in infrared region for the CHE as well as nanomaterials. Raman spectroscopy was conducted on iHR320 with CCD detector, HORIBA at 632 nm excitation wavelength, DXR Raman Microscope, DXR 532 nm Laser. SEM images were taken using Hitachi S-4700 (Hitachi, Žatec, Czech Republic) using the following parameters: acceleration voltage = 20 kV, working distance about 10 mm and spot size 3. The powder specimens were mounted onto a metallic stub with a double-sided adhesive tape. Images were captured at different magnifications. For transmission electron microscopy (TEM), the powder was dispersed in ethanol, sonicated for 5 min and deposited onto TEM grid having carbon support film. The grids were dried before mounting into the TEM. A TEM, FEI, Morgagni, Czec Republic at 80 kV was used to record the images. The UV-vis diffuse reflectance measurements were performed on Shimadzu UV4100 spectrometer (Shimadzu, Kyoto, Japan) and UV-vis absorption measurements were recorded on UV-vis Spectrophotometer-UVD-3200 (LABOMED, Los Angeles, CA, USA).

3.4. Photocatalytic Activity

The photocatalytic performance of the green as well as chemically synthesized TiO2 nanoparticles has been evaluated for photocatalytic degradation of methylene blue (MB) as model pollutant under solar light irradiation. The photocatalytic activity was further evaluated for the photocatalytic mineralization of phenol under solar light irradiation. The photocatalytic experiments were carried out using solar simulator (SLB-300A, 300 W). The amount of the degraded organic pollutant (MB or phenol) was evaluated from UV-vis spectroscopic measurement before and during illumination.

4. Conclusions

Nanoporous TiO2 has been synthesized using plant waste extract (CHE). The properties of produced green nanomaterials were well determined using diverse characterization techniques. SEM and TEM analysis revealed that the produced green nanomaterials have macroporous/mesoporous structures composed of small-sized TiO2 particles and narrow particle distribution. The as synthesized green porous TiO2 nanomaterials showed enhanced photocatalytic performance under UV and solar light irradiation for degradation of organic dyes and phenol. The enhanced photocatalytic activity of the green TiO2 can be attributed to higher surface area and the presence of more active adsorption sites inside the pores leading to increased accessibility for the organic pollutant and therefore enhancing photocatalytic activity. The results demonstrate the efficiency of CHE as bio-template to produce porous TiO2 nanoparticles with enhanced photocatalytic activity.

Author Contributions

Conceptualization, H.H.M.; Methodology, H.H.M.; Validation, F.A.Q., N.A.A. and H.H.M.; Formal Analysis, F.A.Q. and H.H.M.; Investigation, F.A.Q. and H.H.M.; Data Curation, F.A.Q. and H.H.M.; Writing-Original Draft Preparation, H.H.M. and F.A.Q.; Writing-Review & Editing, H.H.M.; Supervision, H.H.M. and N.A.A.

Funding

This research received no external funding.

Acknowledgments

The authors acknowledge Imam Abdulrahman Bin Faisal University for supporting this work. The authors acknowledge Institution of Research and Medical Consultations (IRMC) for SEM and TEM measurements. Department of Chemistry-College of Science-King Fahd University of Petroleum and Minerals is gratefully acknowledged for Raman measurements.

Conflicts of Interest

The authors declare that they have no competing interests.

References

  1. Chaudhry, F.N.; Malik, M.F. Factors Affecting Water Pollution: A Review. J. Ecosyst. Ecography 2017, 7, 6–8. [Google Scholar]
  2. Site, A.D. Factors affecting sorption of organic compounds in natural sorbent/water systems and sorption coefficients for selected pollutants. A review. J. Phys. Chem. Ref. Data 2001, 30, 187–439. [Google Scholar] [CrossRef]
  3. Eccles, H. Treatment of metal-contaminated wastes: Why select a biological process? Trends Biotechnol. 1999, 17, 462–465. [Google Scholar] [CrossRef]
  4. Muller-Karger, F.E.; McClain, C.R.; Richardson, P.L. The dispersal of the Amazon’s water. Nature 1988, 333, 56–59. [Google Scholar] [CrossRef]
  5. Schalscha, B.E.; Ahumada, T.I. Heavy metals in rivers and soils of central Chile. Water Sci. Technol. 1998, 37, 251–255. [Google Scholar] [CrossRef]
  6. Fu, F.; Wang, Q. Removal of heavy metal ions from wastewaters: A review. J Environ. Manag. 2011, 92, 407–418. [Google Scholar] [CrossRef]
  7. Mohamed, H.H. Sonochemical synthesis of ZnO hollow microstructure/reduced graphene oxide for enhanced sunlight photocatalytic degradation of organic pollutants. J. Photochem. Photobiol. A 2018, 353, 401–408. [Google Scholar] [CrossRef]
  8. Mohamed, H.H.; Alomair, N.A.; Bahnemann, D.W. Kinetic and mechanistic features on the reaction of stored TiO2 electrons with Hg (II), Pb (II) and Ni (II) in aqueous suspension. Arab. J. Chem. 2016, in press. [Google Scholar] [CrossRef]
  9. Mohamed, H.H. Rationally designed Fe2O3/GO/WO3 Z-Scheme photocatalyst for enhanced solar light photocatalytic water remediation. J. Photochem. Photobiol. A 2019, 378, 74–84. [Google Scholar] [CrossRef]
  10. Mohamed, H.H.; Alsanea, A.A.; Alomair, N.A.; Akhtar, S.; Bahnemann, D.W. ZnO@ porous graphite nanocomposite from waste for superior photocatalytic activity. Environ. Sci. Pollut. Res. 2019, 26, 12288–12301. [Google Scholar] [CrossRef]
  11. Mohamed, H.H.; Alsanea, A.A. TiO2/Carbon Dots Decorated Reduced Graphene Oxide Composites from Waste Car Bumper and TiO2 Nanoparticles for Photocatalytic Applications. Arab. J. Chem. 2018, in press. [Google Scholar] [CrossRef]
  12. Mohamed, H.H.; Dillert, R.; Bahnemann, D.W. TiO2 nanoparticles as electron pools: Single- and multi-step electron transfer processes. J. Photochem. Photobiol. A Chem. 2012, 245, 9–17. [Google Scholar] [CrossRef]
  13. Su, C.; Hong, B.-Y.; Tseng, C.-M. Sol–gel preparation and photocatalysis of titanium dioxide. Catal. Today 2004, 96, 119–126. [Google Scholar] [CrossRef]
  14. Lakshmi, B.B.; Patrissi, C.J.; Martin, C.R. Sol−Gel Template Synthesis of Semiconductor Oxide Micro- and Nanostructures. Chem. Mater. 1997, 9, 2544–2550. [Google Scholar] [CrossRef]
  15. Chen, X.; Mao, S.S. Titanium dioxide nanomaterials: Synthesis, properties, modifications and applications. Chem. Rev. 2007, 107, 2891–2959. [Google Scholar] [CrossRef] [PubMed]
  16. Youssef, T.E.; Mohamed, H.H. Synthesis and photophysicochemical properties of novel mononuclear rhodium(III) phthalocyanines. Polyhedron 2011, 30, 2045–2050. [Google Scholar] [CrossRef]
  17. Alomair, N.; Mohamed, H.H.; Alomair, N. Green synthesis of ZnO hollow microspheres and ZnO/rGO nanocomposite using red rice husk extract and their photocatalytic performance. Mater. Res. Express 2018, 5, 095012. [Google Scholar] [CrossRef]
  18. Mohamed, H.H.; Alomair, N.A.; Akhtar, S.; Youssef, T.E. Eco-friendly synthesized α-Fe2O3/TiO2 heterojunction with enhanced visible light photocatalytic activity. J. Photochem. Photobiol. A Chem. 2019, 382, 111951. [Google Scholar] [CrossRef]
  19. Ahmed, S.; Ahmad, M.; Swami, B.L.; Ikram, S. A review on plants extract mediated synthesis of silver nanoparticles for antimicrobial applications: A green expertise. J. Adv. Res. 2016, 7, 17–28. [Google Scholar] [CrossRef]
  20. Hunagund, S.M.; Desai, V.R.; Barretto, D.A.; Pujar, M.S.; Kadadevarmath, J.S.; Vootla, S.; Sidarai, A.H. Photocatalysis effect of a novel green synthesis gadolinium doped titanium dioxide nanoparticles on their biological activities. J. Photochem. Photobiol. A Chem. 2017, 346, 159–167. [Google Scholar] [CrossRef]
  21. Saravanan, M.; Gopinath, V.; Chaurasia, M.K.; Syed, A.; Ameen, F.; Purushothaman, N. Green synthesis of anisotropic zinc oxide nanoparticles with antibacterial and cytofriendly properties. Microb. Pathog. 2018, 115, 57–63. [Google Scholar] [CrossRef]
  22. Mohamed, H.H.; Hammami, I.; Baghdadi, H.A.; Al-Jameel, S.S. Multifunctional TiO2 microspheres-rgo as highly active visible light photocatalyst and antimicrobial agent. Mater. Express 2018, 8, 345–352. [Google Scholar] [CrossRef]
  23. Lengke, M.; Southam, G. Bioaccumulation of gold by sulfate-reducing bacteria cultured in the presence of gold(I)-thiosulfate complex. Geochim. Cosmochim. Acta 2006, 70, 3646–3661. [Google Scholar] [CrossRef]
  24. Mukherjee, P.; Ahmad, A.; Mandal, D.; Senapati, S.; Sainkar, S.R.; Khan, M.I.; Parishcha, R.; Ajaykumar, P.V.; Alam, M.; Kumar, R.; et al. Fungus-Mediated Synthesis of Silver Nanoparticles and Their Immobilization in the Mycelial Matrix: A Novel Biological Approach to Nanoparticle Synthesis. Nano Lett. 2001, 1, 515–519. [Google Scholar] [CrossRef]
  25. Holmes, J.D.; Smith, P.R.; Richardson, D.J.; Russell, D.A.; Sodeau, J.R. Energy-dispersive X-ray analysis of the extracellular cadmium sulfide crystallites of Klebsiella aerogenes. Arch. Microbiol. 1995, 163, 143–147. [Google Scholar] [CrossRef] [PubMed]
  26. Willner, I.; Basnar, B.; Willner, B. Nanoparticle-enzyme hybrid systems for nanobiotechnology. FEBS J. 2007, 274, 302–309. [Google Scholar] [CrossRef]
  27. Begum, N.A.; Mondal, S.; Basu, S.; Laskar, R.A.; Mandal, D. Biogenic synthesis of Au and Ag nanoparticles using aqueous solutions of Black Tea leaf extracts. Colloids Surf. B Biointerfaces 2009, 71, 113–118. [Google Scholar] [CrossRef]
  28. Philip, D. Biosynthesis of Au, Ag and Au-Ag nanoparticles using edible mushroom extract. Spectrochim. Acta Part A Mol. Biomol. Spectrosc. 2009, 73, 374–381. [Google Scholar] [CrossRef]
  29. Narayanan, K.B.; Sakthivel, N. Coriander leaf mediated biosynthesis of gold nanoparticles. Mater. Lett. 2008, 62, 4588–4590. [Google Scholar] [CrossRef]
  30. Husen, A.; Siddiqi, K.S. Phytosynthesis of nanoparticles: Concept, controversy and application. Nanoscale Res. Lett. 2014, 9, 229. [Google Scholar] [CrossRef]
  31. Shankar, S.; Rai, A.; Ahmad, A.; Sastry, M. Rapid synthesis of Au, Ag, and bimetallic Au core–Ag shell nanoparticles using Neem (Azadirachta indica) leaf broth. J. Colloid Interface Sci. 2004, 275, 496–502. [Google Scholar] [CrossRef] [PubMed]
  32. Shukla, R.C.; Tandon, P.K.; Singh, S.B. Removal of Arsenic(III) from Water with Clay-Supported Zerovalent Iron Nanoparticles Synthesized with the Help of Tea Liquor. Ind. Eng. Chem. Res. 2013, 52, 10052–10058. [Google Scholar]
  33. Huang, L.; Weng, X.; Chen, Z.; Megharaj, M.; Naidu, R. Synthesis of iron-based nanoparticles using oolong tea extract for the degradation of malachite green. Spectrochim. Acta Part A Mol. Biomol. Spectrosc. 2014, 117, 801–804. [Google Scholar] [CrossRef] [PubMed]
  34. Roopan, S.M.; Bharathi, A.; Prabhakarn, A.; Rahuman, A.A.; Velayutham, K.; Rajakumar, G.; Padmaja, R.D.; Lekshmi, M.; Madhumitha, G. Efficient phyto-synthesis and structural characterization of rutile TiO2 nanoparticles using Annona squamosa peel extract. Spectrochim. Acta Part A Mol. Biomol. Spectrosc. 2012, 98, 86–90. [Google Scholar] [CrossRef] [PubMed]
  35. Sundrarajan, M.; Gowri, S. Green synthesis of titanium dioxide nanoparticles by nyctanthes arbor-tristis leaves extract. Chalcogenide Lett. 2011, 8, 447–451. [Google Scholar]
  36. Souto, U.T.D.C.P.; Barbosa, M.F.; Dantas, H.V.; de Pontes, A.S.; da Silva Lyra, W.; Diniz, P.H.G.D.; Araújo, M.C.U.; da Silva, E.C. Identification of adulteration in ground roasted coffees using UV-Vis spectroscopy and SPA-LDA. LWT Food Sci. Technol. 2015, 63, 1037–1041. [Google Scholar]
  37. Suhandy, D.; Yulia, M. Peaberry coffee discrimination using UV-visible spectroscopy combined with SIMCA and PLS-DA. Int. J. Food Prop. 2017, 20 (Supp. 1), S331–S339. [Google Scholar] [CrossRef]
  38. Srivastava, S.K.; Singh, V.B. Ab initio and DFT studies of the structure and vibrational spectra of anhydrous caffeine. Spectrochim. Acta Part A Mol. Biomol. Spectrosc. 2013, 115, 45–50. [Google Scholar] [CrossRef]
  39. Sutradhar, P.; Saha, M.; Maiti, D. Microwave synthesis of copper oxide nanoparticles using tea leaf and coffee powder extracts and its antibacterial activity. J. Nanostruct. Chem. 2014, 4, 4–9. [Google Scholar] [CrossRef]
  40. Sharma, R.; Bisen, D.P.; Shukla, U.; Sharma, B.G. X-ray diffraction: A powerful method of characterizing nanomaterials. Recent Res. Sci. Technol. 2012, 4, 77–79. [Google Scholar]
  41. Ohsaka, T.; Izumi, F.; Fujiki, Y. Raman spectrum of anatase, TiO2. J. Raman Spectrosc. 1978, 7, 321–324. [Google Scholar] [CrossRef]
  42. Mohamed, H.H. Biphasic TiO2 microspheres/reduced graphene oxide for effective simultaneous photocatalytic reduction and oxidation processes. Appl. Catal. A Gen. 2017, 541, 25–34. [Google Scholar] [CrossRef]
  43. López, R.; Gómez, R. Band-gap energy estimation from diffuse reflectance measurements on sol–gel and commercial TiO2: A comparative study. J. Sol Gel Sci. Technol. 2012, 61, 1. [Google Scholar] [CrossRef]
  44. Singh, M.; Goyal, M.; Devlal, K. Size and shape effects on the band gap of semiconductor compound nanomaterials. J. Taibah Univ. Sci. 2018, 12, 470–475. [Google Scholar] [CrossRef] [Green Version]
Catalysts 09 00799 g001 550
Figure 1. (a) UV-vis spectrum and (b) FTIR of the coffee husk extract (CHE).
Figure 1. (a) UV-vis spectrum and (b) FTIR of the coffee husk extract (CHE).
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Figure 2. XRD patterns of the as synthesized nanomaterials.
Figure 2. XRD patterns of the as synthesized nanomaterials.
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Figure 3. SEM micrographs of the as synthesized TiO2 nanomaterials prepared without CHE (a) and with CHE (b,c).
Figure 3. SEM micrographs of the as synthesized TiO2 nanomaterials prepared without CHE (a) and with CHE (b,c).
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Figure 4. TEM micrographs of the as synthesized TiO2 nanomaterials prepared without CHE (a) and with CHE (b).
Figure 4. TEM micrographs of the as synthesized TiO2 nanomaterials prepared without CHE (a) and with CHE (b).
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Figure 5. Raman spectra (a) and FTIR spectra (b) of the as synthesized TiO2 nanomaterials. The inset of (a) shows the enlargement for the area of carbon.
Figure 5. Raman spectra (a) and FTIR spectra (b) of the as synthesized TiO2 nanomaterials. The inset of (a) shows the enlargement for the area of carbon.
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Figure 6. UV-vis diffuse reflectance spectra of the as synthesized TiO2 nanomaterials (a), N2 adsorption-desorption isotherms of the as synthesized nanomaterials (b).
Figure 6. UV-vis diffuse reflectance spectra of the as synthesized TiO2 nanomaterials (a), N2 adsorption-desorption isotherms of the as synthesized nanomaterials (b).
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Figure 7. (a,b) UV-vis absorption spectra of an aqueous solution of MB during solar light illumination in the presence of the as synthesized TiO2 (ethanol) and TiO2 (CHE), respectively; (c) efficiency of the photocatalytic degradation of MB as the variation of C/C0 with irradiation time in the presence of various nanomaterials; (d) linear plots of – ln C/C0 vs. time for the experimental data in Figure 7c.
Figure 7. (a,b) UV-vis absorption spectra of an aqueous solution of MB during solar light illumination in the presence of the as synthesized TiO2 (ethanol) and TiO2 (CHE), respectively; (c) efficiency of the photocatalytic degradation of MB as the variation of C/C0 with irradiation time in the presence of various nanomaterials; (d) linear plots of – ln C/C0 vs. time for the experimental data in Figure 7c.
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Figure 8. (a,b) UV-vis absorption spectra of an aqueous solution of phenol during solar light illumination in the presence of the as synthesized TiO2 (Ethanol) and TiO2 (CHE), respectively; (c) efficiency of the photocatalytic degradation of MB as the variation of C/C0 with irradiation time in the presence of various nanomaterials; (d) linear plots of –ln C/C0 vs. time for the experimental data in Figure 8c.
Figure 8. (a,b) UV-vis absorption spectra of an aqueous solution of phenol during solar light illumination in the presence of the as synthesized TiO2 (Ethanol) and TiO2 (CHE), respectively; (c) efficiency of the photocatalytic degradation of MB as the variation of C/C0 with irradiation time in the presence of various nanomaterials; (d) linear plots of –ln C/C0 vs. time for the experimental data in Figure 8c.
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Figure 9. Recyclability of the as prepared green TiO2 in the photocatalytic degradation of MB.
Figure 9. Recyclability of the as prepared green TiO2 in the photocatalytic degradation of MB.
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Figure 10. Schematic representation of preparation of coffee husk extract (CHE).
Figure 10. Schematic representation of preparation of coffee husk extract (CHE).
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Figure 11. Schematic representation of preparation of porous TiO2 nanoparticles.
Figure 11. Schematic representation of preparation of porous TiO2 nanoparticles.
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Table
Table 1. The surface area and the porous parameters of the as prepared nanomaterials.
Table 1. The surface area and the porous parameters of the as prepared nanomaterials.
NanomaterialBET (m2/g)Pore Volume (cc/g)Pore Size (nm)
TiO2 (Ethanol)53.962.49 × 10−29.24 × 102
TiO2 (CHE)147.155.54 × 10−27.53 × 102
Table
Table 2. Kinetic parameters obtained from first order fitting the experimental points of Figure 7 and Figure 8.
Table 2. Kinetic parameters obtained from first order fitting the experimental points of Figure 7 and Figure 8.
NanomaterialReactantk’ (min−1)R2
TiO2 (Ethanol)MB0.0120.99
TiO2 (Ethanol)Phenol0.00150.97
TiO2 (CHE)MB0.0230.99
TiO2 (CHE)Phenol0.00520.99

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Al Qarni, F.; Alomair, N.A.; Mohamed, H.H. Environment-Friendly Nanoporous Titanium Dioxide with Enhanced Photocatalytic Activity. Catalysts 2019, 9, 799. https://doi.org/10.3390/catal9100799

AMA Style

Al Qarni F, Alomair NA, Mohamed HH. Environment-Friendly Nanoporous Titanium Dioxide with Enhanced Photocatalytic Activity. Catalysts. 2019; 9(10):799. https://doi.org/10.3390/catal9100799

Chicago/Turabian Style

Al Qarni, Fatimah, Nuhad A. Alomair, and Hanan H. Mohamed. 2019. "Environment-Friendly Nanoporous Titanium Dioxide with Enhanced Photocatalytic Activity" Catalysts 9, no. 10: 799. https://doi.org/10.3390/catal9100799

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