Photocatalytic activity of BiFe1-xCoxO3 for degradation of methyl orange under UV irradiation
الموضوعات : Journal of Industrial Catalysis
Razieh Khoshnood
1
,
Farid sirousi
2
1 - Department of Chemistry Faculty of Science, Islamic Azad University of Mashhad, Iran
2 - Department of Chemistry , Mashhad Branch, Islamic Azad University, Mashhad, Iran
الکلمات المفتاحية: bismuth ferrite , photocatalyst, industrial wastewater , methyl orange , sol-gel,
ملخص المقالة :
BiFeO3 (bismuth ferrite) nanoparticles are highly significant in the removal or degradation of medical pollutants and industrial wastewater due to their structural and photocatalytic properties. In this study, cobalt doped BiFeO3 nanoparticles, BiFe1-xCoxO3 (X=0.0, 0.01, 0.03, 0.05) were synthesized using the sol-gel method, and the effects of cobalt substitution on their physical properties were investigated. X-ray diffraction (XRD) spectroscopy was used for the identification and analysis of these materials, while FT-IR spectroscopy confirmed the integrity of the synthesized samples. The catalytic efficiency of BiFe1-xCoxO3 nanoparticles for the photocatalytic degradation of methyl orange, one of the primary polluting dyes in industrial wastewater, was measured using UV/Vis spectroscopy. Various parameters, including dye concentration, pH, irradiation time, and nanoparticle amount, were studied, and optimal conditions were reported. The methyl orange degradation results for a prepared 350 ml dye solution with 0.1 g catalyst and 0.5 ml hydrogen peroxide at pH = 2 over 120 minutes for (X=0.0, 0.01, 0.03, 0.05) BiFe1-xCoxO3 nanoparticles were 60.48%, 20.67%, 48.55%, and 50.42%, respectively
[1] M. Anjum, R. Miandad, M. Waqas, F. Gehany, M. Barakat, Remediation of wastewater using various nano-materials, Arabian journal of chemistry, 12 (2019) 4897-4919.
[2] P. Punia, M. Naagar, S. Chalia, R. Dhar, B. Ravelo, P. Thakur, A. Thakur, Recent advances in synthesis, characterization, and applications of nanoparticles for contaminated water treatment-A review, Ceramics International, 47 (2021) 1526-1550.
[3] A. Saghafi, R.S. Khoshnood, D.S. Khoshnoud, Z. Es’ Haghi, Magnetic properties and photocatalytic activity of Bi1-xSmxFe1-yNiyO3 nanoparticles for methyl red degradation, Reaction Kinetics, Mechanisms and Catalysis, 135 (2022) 3375-3391.
[4] M.V. Neshin, R.S. Khoshnood, D.S. Khoshnoud, Enhanced photocatalytic activity of Ni-doped BiFeO 3 nanoparticles for degradation of bromophenol blue in aqueous solutions, Reaction Kinetics, Mechanisms and Catalysis, 134 (2021) 951-970.
[5] F. Shahrab, A. Tadjarodi, Novel magnetic nanocomposites BiFeO3/Cu (BDC) for efficient dye removal, Heliyon, 9 (2023).
[6] M.V. Neshin, R.S. Khoshnood, S. Akbari, Investigation on the Photocatalytic Activity of Bromophenol Blue Using Cr-Doped BiFeO3 Nanoparticles in Aqueous Solutions by UV-Vis Spectrophotometry, Russian Journal of Physical Chemistry A, 97 (2023) 2434-2442.
[7] K. Xie, J. Fang, L. Li, J. Deng, F. Chen, Progress of graphite carbon nitride with different dimensions in the photocatalytic degradation of dyes: A review, Journal of Alloys and Compounds, 901 (2022) 163589.
[8] W. Eerenstein, N. Mathur, J.F. Scott, Multiferroic and magnetoelectric materials, nature, 442 (2006) 759-765.
[9] Y.-H. Chu, L.W. Martin, M.B. Holcomb, R. Ramesh, Controlling magnetism with multiferroics, Materials Today, 10 (2007) 16-23.
[10] S. Kalikeri, V. Shetty Kodialbail, Auto-combustion synthesis of narrow band-gap bismuth ferrite nanoparticles for solar photocatalysis to remediate azo dye containing water, Environmental Science and Pollution Research, 28 (2021) 12144-12152.
[11] م. درح, ث. خشنود, ث. خشنود, داود, اسحاقی, زرین, تخریب فتوکاتالیستی رنگ آزوروبین در محلول های آبی با استفاده از نانوپودرهای بیسموت فریت, شیمى کاربردى روز, 18 (2023) 107-122.
[12] K. Mathankumar, M. Sukumar, C.S. Dash, M. Sundararajan, M. Ubaidullah, A.M. Al-Enizi, A. Sutha, M. Kausar Raza, J. Arockia Dhanraj, D. Kumar, Facile synthesis, characterization, catalytic and photocatalytic activity of multiferroic BiFeO3 perovskite nanoparticles, [1] M. Anjum, R. Miandad, M. Waqas, F. Gehany, M. Barakat, Remediation of wastewater using various nano-materials, Arabian journal of chemistry, 12 (2019) 4897-4919.
[2] P. Punia, M. Naagar, S. Chalia, R. Dhar, B. Ravelo, P. Thakur, A. Thakur, Recent advances in synthesis, characterization, and applications of nanoparticles for contaminated water treatment-A review, Ceramics International, 47 (2021) 1526-1550.
[3] A. Saghafi, R.S. Khoshnood, D.S. Khoshnoud, Z. Es’ Haghi, Magnetic properties and photocatalytic activity of Bi1-xSmxFe1-yNiyO3 nanoparticles for methyl red degradation, Reaction Kinetics, Mechanisms and Catalysis, 135 (2022) 3375-3391.
[4] M.V. Neshin, R.S. Khoshnood, D.S. Khoshnoud, Enhanced photocatalytic activity of Ni-doped BiFeO 3 nanoparticles for degradation of bromophenol blue in aqueous solutions, Reaction Kinetics, Mechanisms and Catalysis, 134 (2021) 951-970.
[5] F. Shahrab, A. Tadjarodi, Novel magnetic nanocomposites BiFeO3/Cu (BDC) for efficient dye removal, Heliyon, 9 (2023).
[6] M.V. Neshin, R.S. Khoshnood, S. Akbari, Investigation on the Photocatalytic Activity of Bromophenol Blue Using Cr-Doped BiFeO3 Nanoparticles in Aqueous Solutions by UV-Vis Spectrophotometry, Russian Journal of Physical Chemistry A, 97 (2023) 2434-2442.
[7] K. Xie, J. Fang, L. Li, J. Deng, F. Chen, Progress of graphite carbon nitride with different dimensions in the photocatalytic degradation of dyes: A review, Journal of Alloys and Compounds, 901 (2022) 163589.
[8] W. Eerenstein, N. Mathur, J.F. Scott, Multiferroic and magnetoelectric materials, nature, 442 (2006) 759-765.
[9] Y.-H. Chu, L.W. Martin, M.B. Holcomb, R. Ramesh, Controlling magnetism with multiferroics, Materials Today, 10 (2007) 16-23.
[10] S. Kalikeri, V. Shetty Kodialbail, Auto-combustion synthesis of narrow band-gap bismuth ferrite nanoparticles for solar photocatalysis to remediate azo dye containing water, Environmental Science and Pollution Research, 28 (2021) 12144-12152.
[11] م. درح, ث. خشنود, ث. خشنود, داود, اسحاقی, زرین, تخریب فتوکاتالیستی رنگ آزوروبین در محلول های آبی با استفاده از نانوپودرهای بیسموت فریت, شیمى کاربردى روز, 18 (2023) 107-122.
[12] K. Mathankumar, M. Sukumar, C.S. Dash, M. Sundararajan, M. Ubaidullah, A.M. Al-Enizi, A. Sutha, M. Kausar Raza, J. Arockia Dhanraj, D. Kumar, Facile synthesis, characterization, catalytic and photocatalytic activity of multiferroic BiFeO3 perovskite nanoparticles, Journal of Inorganic and Organometallic Polymers and Materials, 32 (2022) 3476-3487.
[13] B. Harikumar, M.K. Okla, I.A. Alaraidh, A. Mohebaldin, W. Soufan, M.A. Abdel-Maksoud, M. Aufy, A.M. Thomas, L.L. Raju, S.S. Khan, Robust visible light active CoNiO2–BiFeO3–NiS ternary nanocomposite for photo-fenton degradation of rhodamine B and methyl orange: Kinetics, degradation pathway and toxicity assessment, Journal of Environmental Management, 317 (2022) 115321.
[14] A.D. Mahboob, R.S. Khoshnood, D.S. Khoshnoud, Photocatalytic degradation of bisacodyl using Fe3O4@CuO core-shell nanocomposite in aqueous solutions, Nano scale, 8 (2022) 153-166.
[15] E. Mahmoudi Doroh, R. Sanavi Khoshnood, D. Sanavi Khoshnoud, Z. Esʹhaghi, Synthesis and kinetic study of the photocatalytic efficiency of Bi1− xDyxFeO3 nanoparticles in the removal of Ponceau 4R dye, Reaction Kinetics, Mechanisms and Catalysis, 136 (2023) 2751-2767.
[16] M. Shakil, U. Inayat, N. Khalid, M. Tanveer, S. Gillani, N. Tariq, A. Shah, A. Mahmood, A. Dahshan, Enhanced structural, optical, and photocatalytic activities of Cd–Co doped Zn ferrites for degrading methyl orange dye under irradiation by visible light, Journal of Physics and Chemistry of Solids, 161 (2022) 110419.
[17] S. Ruby, D.R. Rosaline, S. Inbanathan, K. Anand, G. Kavitha, R. Srinivasan, A. Umar, H. Hegazy, H. Algarni, Sunlight-driven photocatalytic degradation of methyl orange based on bismuth ferrite (BiFeO3) heterostructures composed of interconnected nanosheets, Journal of nanoscience and nanotechnology, 20 (2020) 1851-1858.
[18] R.S. Khoshnood, D.S. Khoshnoud, Structural, magnetic, and photocatalytic properties in Bi0. 83− x La0. 17Y x FeO3 nanoparticles, Applied Physics A, 125 (2019) 750.
Original Research Paper
Journal of Industrial Catalysis Vol. 1, No. 2, 2024, 43-49. |
Photocatalytic activity of BiFe1-xCoxO3 for degradation of methyl orange under UV irradiation
Razieh Sanavi Khoshnood *1. Farid Sirousi1
1Department of Chemistry , Mashhad Branch, Islamic Azad University, Mashhad, Iran
* Corresponding author E-mail: rskhoshnood@yahoo.com
Received 3 February 2025; accepted 27 May 2025
Abstract
BiFeO3 (bismuth ferrite) nanoparticles are highly significant in the removal or degradation of medical pollutants and industrial wastewater due to their structural and photocatalytic properties. In this study, cobalt doped BiFeO3 nanoparticles, BiFe1-xCoxO3 (X=0.0, 0.01, 0.03, 0.05) were synthesized using the sol-gel method, and the effects of cobalt substitution on their physical properties were investigated. X-ray diffraction (XRD) spectroscopy was used for the identification and analysis of these materials, while FT-IR spectroscopy confirmed the integrity of the synthesized samples. The catalytic efficiency of BiFe1-xCoxO3 nanoparticles for the photocatalytic degradation of methyl orange, one of the primary polluting dyes in industrial wastewater, was measured using UV/Vis spectroscopy. Various parameters, including dye concentration, pH, irradiation time, and nanoparticle amount, were studied, and optimal conditions were reported. The methyl orange degradation results for a prepared 350 ml dye solution with 0.1 g catalyst and 0.5 ml hydrogen peroxide at pH = 2 over 120 minutes for BiFe1-xCoxO3 (X=0.0, 0.01, 0.03, 0.05) nanoparticles were 60.48%, 20.67%, 48.55%, and 50.42%, respectively.
Keywords: bismuth ferrite – photocatalyst – industrial wastewater – methyl orange – sol-gel
1. Introduction
Water is the most essential and fundamental resource for the human population worldwide. People need water for drinking, cooking, washing, agricultural irrigation, and various socio-economic activities. However, only about 1% of water is suitable for human consumption[1]. Each year, more than 3.5 million people lose their lives due to waterborne diseases. Treating contaminated water can help alleviate these concerns, making clean and accessible water available[2]. Lately, the discharge of industrial organic dye molecules has emerged as one of the major environmental pollutants among thousands of wastewater contaminants[3]. Industries such as textiles, paper, and rubber produce significant volumes of these pollutants, which are characterized by toxicity, low biodegradability, and harmful effects on human health and environmental sustainability. These pollutants have been identified as carcinogenic agents, intensifying their hazardous nature[4]. Given the rising environmental concerns, research groups are increasingly focused on exploring methods to remove and reduce the presence of vibrant dyes in wastewater[5, 6]. Methyl orange is an anionic dye with an azo structure that is easily absorbed by the skin and accumulates in the body, as shown in Figure 1. The azo group (N=N) can cause allergic
reactions upon skin contact, toxicity through inhalation and ingestion, low degradability, and harmful effects on aquatic life. Therefore, the development of new materials for the removal of such dyes has gained attention over the past decade.
Fig. 1. Chemical structure of methyl orange
Advancements in science and technology have paved the way for the use of photocatalytic degradation as a viable mechanism for removing dye molecules from contaminated water sources[7]. Bismuth ferrite (BiFeO3), with its rhombohedral perovskite structure, is an important and versatile material due to its diverse properties and applications. BiFeO3 exhibits various interesting properties, such as multiferroic nature due to its magnetic and ferroelectric behavior at room temperature, thermodynamic stability, superconducting and redox behavior, excellent chemical stability, and more[8, 9]. Photocatalysis is an advanced oxidation process that is widely used for the degradation of various pollutants. Bismuth ferrite (BiFeO3) is extensively utilized for the degradation of organic pollutants under UV/Vis light[10, 11]. The unique properties of BiFeO3 make it an effective photocatalyst for the degradation of organic pollutants. Extensive research efforts have been devoted to leveraging the diverse capabilities of BiFeO3 for efficient and sustainable photocatalysis[12, 13]. In the removal of pollutants, photocatalysis finds its application in the degradation of contaminants in industrial wastewater and can serve as a cost-effective treatment process[14]. Due to its exceptional efficiency, minimal byproduct production, relatively economical nature, and simple operational methods, it is widely recognized as a highly sustainable approach[6, 15]. Among various ferrite materials, cobalt ferrite has garnered significant interest. Cobalt ferrite is preferred over other ferrites due to its high chemical stability, soft magnetic behavior, superior electromagnetic performance, and hardness[16, 17]. In this study a series of cobalt doped bismuth ferrite (BiFeO₃) nanostructures were synthesized via the sol-gel method to evaluate their photocatalytic efficiency for degrading hazardous dyes under UV/Vis light irradiation. Photocatalytic experiments demonstrated that methyl orange (MO) was effectively degraded within 120 minutes. This finding highlights the potential of BiFeO₃ as a promising candidate for the degradation of various organic pollutants. Bismuth ferrite (BiFeO₃) is considered one of the most attractive and promising photocatalysts due to its high oxidative potential and excellent chemical stability[4, 18]. By incorporating cobalt into its structure, the material was investigated through UV/Vis spectroscopy for the removal of methyl orange dye from industrial wastewater. The effects of various operational parameters, including irradiation time, dye concentration, pH, catalyst dosage, and hydrogen peroxide (H₂O₂) concentration, were systematically studied, and the optimal conditions for efficient photocatalysis were determined. 2- Experimental 2-1- Chemicals Iron(III) nitrate nonahydrate (99%), bismuth(III) nitrate pentahydrate (99%), methyl orange, and tartaric acid (99%) were obtained from MERCK. Cobalt(II) nitrate (98%) was sourced from FLUKA, nitric acid (65%) was provided by RIEDEL-DEHA, and hydrogen peroxide 37% Neutron was also obtained.
2-2- Instruments
Samples were prepared in the form of solid discs. The vibrational spectrum (FT-IR) of the samples was analyzed and recorded using the spectrophotometer (Avatar 370 FT-IR, Thermo Nicolet) in the range of 400-4000 cm⁻¹. The analysis of crystalline structures and material identification was conducted using X-ray diffraction (XRD) with the Philips Analytical X-Ray B.V. model. The oven (Pars Azma Co) was used for drying samples, while the furnace (SCI FINETECH) was utilized for drying samples at higher temperatures. Solutions were stirred and heated using a magnetic stirrer (Heidolph MR Hei), and pH measurements were performed with a pH meter (MetRoHM). A digital balance (Sartorius) with an accuracy of 0.0001 grams was employed for weighing materials. For analyzing the concentration of methyl orange dye in this study, a UV-Vis spectrophotometer (Varian, Cary Bio50) was used. Additionally, a photochemical device equipped with a 250-watt mercury lamp was utilized for irradiating the samples and monitoring changes in the solution.
2-3- Synthesis of BiFeO3 and BiFe1-xCoxO3 Compounds by the sol-gel method
2-3-1- Synthesis of BiFeO3
Bismuth ferrite (BiFeO₃) was synthesized using the sol-gel method, utilizing bismuth nitrate (Bi(NO₃)₃·5H₂O) and iron(III) nitrate (Fe(NO₃)₃·9H₂O) as the precursor materials. The synthesis procedure consisted of several key steps to form the perovskite structure of BiFeO₃. Initially, the required amounts of bismuth nitrate and iron(III) nitrate were accurately weighed and dissolved in either ethylene glycol or distilled water. The solution was stirred continuously to ensure homogeneity. Once the precursors were completely dissolved, acetic acid was added dropwise to the solution to adjust the pH. The pH was carefully controlled to facilitate the formation of a gel. Upon successful pH adjustment, the solution was heated to induce gelation. The heating process promoted the transformation of the solution into a gel-like substance. Following gel formation, the material was dried at 100°C to remove the solvent, leaving behind a solid gel precursor.The dried gel was then subjected to calcination at 600°C for 4 hours. This high-temperature treatment allowed the crystallization of BiFeO₃. After the calcination process, the sample was allowed to cool to room temperature, resulting in the formation of BiFeO₃.
2-3-2 Synthesis of BiFe1-xCoxO3
BiFe1-xCoxO3 nanoparticles (X=0.01, 0.03, 0.05) were synthesized through the sol-gel process, utilizing tartaric acid for the preparation of the photocatalyst nanoparticles. To synthesize the BiFe1-xCoxO3 compound, 20 milliliters of deionized distilled water was added to a beaker and heated to 60 degrees Celsius. After that, nitric acid was added, and once it dissolved, bismuth nitrate (2.52 grams – 5H2O), iron(III) nitrate (1.99 grams – 9H2O), and cobalt nitrate in amounts of (0.01, 0.05, 0.07) were added. Once the salts were completely dissolved, tartaric acid (1.5 grams) was introduced to form a yellowish-brown homogeneous solution. By adding ammonia , the solution turned lemon-yellow, and the pH reached 3. The solution was placed in an oven at 80 degrees Celsius, with the temperature increased by 20 degrees Celsius every 8 hours until it reached 120 degrees. After that, the temperature was raised by 10 degrees Celsius every 30 minutes and maintained at 200 degrees for 2 hours. The powdered materials were transferred to a crucible and placed in a furnace at 400 degrees Celsius for 3 hours. The cooled materials were then washed with acid, and the crucible was returned to the furnace at 650 degrees Celsius for 4 hours before being analyzed using X-ray diffraction (XRD).
2-4- Photocatalytic Experiment Method
The photocatalytic activity of BiFeO3 and BiFe1-xCoxO3 (X= 0.00, 0.01, 0.03, 0.05) nanoparticles were evaluated in an aqueous solution of methyl orange under mercury lamp irradiation. The first step involved calibration to determine the initial concentration of methyl orange, and a concentration of 3 mg L⁻¹ was selected for the experiments. Next, 300 ml of methyl orange at a concentration of 3 mg L⁻¹ was transferred into a 600 ml beaker. After adding H₂O₂ and the Nano catalyst to the beaker, various pH levels were adjusted using NaOH and HCl. In the next step, the beaker was placed inside the photoreactor (a chemical reactor device that brings photons, the photocatalyst, and reactants into contact). The solution was stirred at 750 rpm under dark conditions for 30 minutes. Every 20 minutes, 3 ml of the solution was drawn with a pipette and transferred to a centrifuge tube. To settle the suspended photocatalyst particles, the mixture was centrifuged at 4000 rpm for 10 minutes, and the absorbance spectrum of the solution was recorded using a UV-Vis spectrophotometer. The mercury lamp in the photochemical reactor was switched on to initiate the photocatalytic process. At predetermined time intervals, the absorbance of the methyl orange solution was measured at its maximum wavelength of 461 nm. The photocatalytic degradation efficiency was calculated using Equation 1, based on the percentage reduction in dye concentration, where 𝐶0 and Ct represent the initial concentration and the concentration at a given irradiation time (0–120 minutes), respectively.
Methyl Orange Degradation (%)= 
Equation 1 - Percentage Degradation of Methyl Orange
2-5- Preparation of Methyl Orange Solution
A specified amount of methyl orange was diluted to volume in a flask, transferred to a beaker, and a certain amount of BiFeO₃ adsorbent was added. Then, 0.5 ml of hydrogen peroxide was added, and finally, the solution was tested under various parameters.
The increase in H₂O₂ volume resulted in a higher generation of electron–hole pairs and reactive species. Notably, the photodegradation efficiency of Methyl Orange was significantly enhanced, primarily due to the increased formation of hydroxyl (OH) radicals on the surface of BiFeO3or doped BiFeO3, as described by the following equation 2:
Equation 2 - Photocatalytic mechanism of Methyl Orange degradation via electron–hole pair separation and hydroxyl radical formation on BiFeO₃ catalysts.
This catalytic mechanism efficiently suppresses the recombination of photogenerated electron–hole pairs, thereby enhancing the overall photocatalytic performance in the degradation of Methyl Orange .
3- Results and discussion
The degradation of methyl orange dye was measured and tested under the influence of irradiation time, pH, and nanoparticle amount, and then the optimized values were reported.
3-2-Effect of time
A specified amount of the prepared methyl orange solution was poured into a beaker, an appropriate number of nanoparticles was added, and after adding H₂O₂, the pH was adjusted. The prepared solution was transferred to the photochemical apparatus, and the degradation rate was measured at different times and reported in Figure 2.
Fig. 2. Effect of different time intervals (30, 60, 90, 120 minutes) on the degradation of methyl orange dye under experimental conditions of 300 ml of methyl orange solution with a concentration of 3 mg L⁻¹, 0.1 g of nanoparticles, and 0.5 ml of hydrogen peroxide at pH = 2.
3-3- Effect of pH
The effect of pH on the degradation of methyl orange was investigated at pH levels of 2, 3, and 4. In this stage, after transferring the prepared methyl orange solution to a beaker, a specified number of nanoparticles was added, followed by a defined quantity of H₂O₂. Finally, the optimized pH value was reported in Figure 3. Based on the investigations conducted, pH = 2 was reported as the optimal pH, as the degradation rate decreased at pH levels higher than , And the photocatalytic degradation efficiency of methyl orange decreases at higher pH values.
Fig.3. Effect of different pH levels (2, 3, 4) on the degradation of methyl orange dye under experimental conditions of 300 ml of methyl orange solution with a concentration of 3 mg L⁻¹, 1 g of nanoparticles, and 0.5 ml of hydrogen peroxide under UV-Vis irradiation.
3-4-Effect of nanoparticle dose
In Fig.4 the impact of nanoparticle amount on degradation shows that degradation is very minimal in the absence of nanoparticles. Following the investigation and testing of the influence of nanoparticle quantity on methyl orange degradation, an optimal dose of 0.1 g was reported. Given the similar photocatalytic degradation performance observed at 100 mg and 150 mg of catalyst, the lower dosage (100 mg) was preferred for economic efficiency. The solution exhibits turbidity at catalyst dosages exceeding 150 mg.
Fig.4 Effect of different nanoparticle amounts (0.01 g, 0.03 g, 0.05 g) on the degradation of methyl orange dye under experimental conditions of 300 ml of methyl orange solution with a concentration of 3 mg L⁻¹, 0.5 ml of hydrogen peroxide, and at pH = 2.
4-Investigation of the Structure of the Synthesized Photocatalyst
In this study, BiFe1-xCoxO3 nanoparticles from the family of double perovskite oxides were synthesized using the sol-gel technique and characterized by X-ray diffraction (XRD) spectroscopy. Additionally, the FT-IR spectrum (Fourier-transform infrared spectroscopy) of these oxides confirmed the structural integrity of the synthesized material. The investigation of the properties of BiFe1-xCoxO3 in the removal of methyl orange dye yielded satisfactory results.
4-1-Characterization by XRD
The X-ray diffraction (XRD) patterns for the samples of BiFeO3 and BiFe1-xCoxO3 (X=0.0, 0.01, 0.03, 0.05) are presented in Figures 5 and 6 as follows:
Fig.5. X-ray diffraction (XRD) pattern for BiFeO3.
As can be observed, the diffraction peaks located at (2θ=22-32-40-46-51-57)̊ are attributed to the rhombohedral perovskite phase, with the peak at 2θ = 32° being the primary and characteristic peak of BiFeO3. The XRD pattern for the samples of BiFe1-xCoxO3 is shown in Figure5.
Fig. 6. X-ray diffraction (XRD) pattern for BiFe1-xCoxO3, shown from up to down for (X=0.01, 0.03, 0.05).
The data given in Fig. 6 show that in all the spectrum, the main peaks of the pure bismuth ferrite compound are observed. The presence of cobalt ions in place of Fe³⁺ acts as an inhibitor, leading to a reduction in crystal size. The results in Figure 3, which display the XRD patterns of BiFeO3 and BiFe1-xCoxO3, indicate that with an increase in cobalt ion concentration, the intensity of the main peak increases. Additionally, as the cobalt ion concentration increases, the main peak transitions from broadening to becoming sharper
The FT-IR spectra for the BiFeO3 and BiFe1-xCoxO3 (X=0.01,0.03,0.05) samples are shown in Figures 7 and 8. The peak observed at 3400 cm⁻¹ corresponds to the vibration of the OH group, which is broadened due to hydrogen bonding.
Fig. 7. FT-IR spectrum of BiFeO3
Fig. 8. Vibrational FT-IR spectra of samples with cobalt concentrations of 0.01, 0.03, and 0.05.
Selected previous studies are summarized in the table below:
Table 1 : Some previous studies
5. Conclusion
In this study, BiFe1-xCoxO3 nanoparticles (X = 0.0, 0.01, 0.03, 0.05) were synthesized via the sol-gel method and evaluated as photocatalysts for the degradation of methyl orange dye. The effects of cobalt doping in the BiFeO3 structure were shown to be rather different for structural characteristics and photocatalytic performance of the nanoparticles. XRD analysis verified the development of a rhombohedral perovskite phase and indicated that increasing cobalt concentration resulted in improved intensity and sharpness of the main peak, together with a decrease in crystal size. Photocatalytic evaluations under optimal conditions (pH = 2, dye concentration of 3 mg/L, 0.1 g of catalyst, and 120 minutes of UV-A irradiation) revealed that the highest degradation efficiency of 60.48% was achieved with the undoped sample. However, cobalt doping at various levels resulted in reduced photocatalytic activity. This reduction may be attributed to increased particle size, alterations in electronic properties, and a decrease in several active surface sites. This study highlights that while cobalt doping reduces the photocatalytic performance, it provides opportunities for fine-tuning the structural and optical properties of nanoparticles. Further optimization of the chemical composition and synthesis parameters could pave the way for the development of advanced photocatalytic materials for environmental applications, particularly in the removal of organic pollutants.
Catalyst | Source | pH | Time (min) | %RE | Ref |
CuO | Sunlight | 2 | 30 | 98.9 | [19] |
SiO2 | UV | 7 | 90 | 95 | [20] |
TiO₂ | UV | 2 | 45 | 98 | [21] |
Fe₂O₃ | Visible | 3 | 120 | 99 | [22] |
This Work | UV-A | 2 | 120 | 60.4 | - |
Fig. 9. UV-Vis spectrum at λmax = 461 nm showing the effect of time on the removal of methyl orange dye using BiFe1-xCoxO3 (X = 0.01, 0.03, 0.05) at pH = 2.
References
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