# Probe Sonicated Synthesis of Bismuth Oxide (Bi2O3): Photocatalytic Application and Electrochemical Sensing of Ascorbic Acid and Lead

Authors: K. B. Kusuma; M. Manju; C. R. Ravikumar; V. G. Dileepkumar; A. Naveen Kumar; Mysore Sridhar Santosh; H. C. Ananda Murthy; K. Gurushantha
Journal: Journal of Nanomaterials
 (2022)

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## Abstract

A simple and low-cost and highly calibrated probe sonication method was used to prepare bismuth oxide nanoparticles (Bi2O3 NPs). The formation of a well-crystalline sample at the end of the product has been further calcined at 600°C for 2 hrs. The powder X-ray diffraction (PXRD) patterns of the NPs substantiated the monoclinic structure (space group P21/c), and the average crystallite size was found to be 60 nm, which was also confirmed by transmission electron microscopic (TEM) studies. Scanning electron microscopic (SEM) images depicted highly porous Bi2O3 NPs with little agglomeration. Utilizing diffused reflectance spectra (DRS) data, the energy bandgap (Eg) value of 3.3 eV was deduced for Bi2O3 NPs, and their semiconductor behavior has been confirmed. Two dyes, methylene blue (MB) and acid green (AG) were utilized for degradation studies using Bi2O3 NPs under UV light irradiation (from 0 to 120 min). The photocatalytic degradation was found to be maximum for MB (93.45%) and AR (97.80%) dyes. Cyclic voltammetric (CV) and sensor studies using the electrochemical impedance spectroscopy (EIS) were performed. The specific capacitance value of 25.5 Fg-1 was deduced from the cyclic voltammograms of the Bi2O3 electrode in 0.1 N HCl with a scan rate of 10 to 50 mV/s. From the obtained EIS data, the Bi2O3 electrode showed pseudocapacitive characteristics. The prepared electrodes also exhibited high sensitivity towards the detection of ascorbic acid and lead. Hence, sonochemically synthesized Bi2O3 NPs are possibly hopeful for excellent photocatalytic and electrochemical sensing of biomolecules.


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## Body

## 1. Introduction

With the rapid escalation of industrial activities by mankind, environmental remediation of pollutants has become an issue of global concern. Many industries such as textile, food processing, pharmaceuticals, tannery, papermaking, and electroplating are the source of dyes in the water bodies leading to the contamination of water [1, 2]. A significant amount of industrial waste is being released into the environment as the chemical industry grows, and this waste has a high likelihood of causing adverse reactions in human beings, such as immunological dysfunction and reproductive system abnormalities, as well as neurological and behavioral abnormalities. Because the therapy or cure for many diseases, such as diabetes, is still in the early stages of development, it is critical to control the living conditions associated with the disease. The monitoring of heavy metals such as lead and monitoring of the drug ascorbic acid is necessary to induce the welfare of humans as well as water bodies. As a result, the development of novel sensors for the detection of substances at trace quantities has emerged as a highly essential area of research. Electrochemical detection methods have a number of advantages over other conventional procedures. Electrochemical sensors are one of the fields that are growing at the fastest rate. Amperometric sensors use the voltage difference between a reference and an electrode to cause the oxidation or reduction of an electroactive species in a reaction [3–6]. A large number of nanometal oxides have been applied to degrade many pollutant dyes for many decades [7].There are numerous transition metal oxides such as ZnO, Mn2O3, Fe3O4, TiO2, and Fe2O3, which have been applied to degrade the plenty of dye molecules [8–11]. Each of these metal oxides exhibits good degradation efficiency, but still face serious drawbacks such as fast electron-hole recombination, agglomeration, and inefficient band gap values. Thus, to find an alternative metal oxide for the effective photocatalytic degradation, Bi2O3 has been chosen in this work due to its environmental friendly applications in solid oxide fuel cells, gas sensors, photocatalyst, energy, and medicine [12–14]. It is well known that bismuth oxide has six polymorphic forms, denoted by α-Bi2O3 (monoclinic), β-Bi2O3 (tetragonal), δ-Bi2O3 (face-centered cubic), γ-Bi2O3 (body-centered cubic), ῳ-Bi2O3 (orthorhombic), and Bi2O3 (triclinic), respectively [15, 16]. Among them, α- and δ-phases are stable both at low temperatures as well as at higher temperatures, respectively, but the others remain in a metastable phase at high temperatures Bi2O3 has a lot of peculiar physical and chemical properties, such as a wide energy gap change (from 2 to 3.96 eV), high metal oxide ion conductivity properties (1.0 s/cm), high refractive index, dielectric permittivity, addition to that, and excellent photo conductivities and photoluminescence properties [17, 18].Modified nanoelectrodes have been utilized for the determination of paracetamol in pharmaceutical preparations including electrodeposition attachment of metal nanoparticles such as Au, Ru, and Cu. In addition, fullerene and carbon nanotube-based electrodes also showed high sensitivity with a low detection limit [19, 20]. Generally, the modification of the electrode is needed for a sensitive and selective determination of overdose levels of paracetamol in whole blood or urine samples [21–23]. Bismuth oxide NP modified carbon electrode has been employed for the determination of heavy metal ions present in drinking water, mineral water, and urine samples [24, 25]. The fabrication of chemically modified nanoelectrode (CMNE) has been widely used to improve the sensitivity and selectivity of amino acids, vitamins, drugs, DNA, and many more [26–28].Many researchers have reported different methods for the synthesis of NPs, such as thermal decomposition using organic solvents which create hampers. The combustion method is one of the fast methods for the synthesis of NPs, but in the combustion method, it is difficult to control the agglomeration of the NPs. The other method for the fast and better yield is the coprecipitation method where there will be no control over the size distribution of the NPs. The probe-sonication method was proven to be the best due to its accuracy and capacity to form nanosized small particles. The synthesis of NPs by the application of ultrasonic waves exhibited various advantages like fast rate of reaction, high purity, and narrow distribution of particle sizes [29]. Several authors have reported the synthesis of many NPs through the sonochemical method.In the present work, we aimed to synthesize Bi2O3 NPs by using the probe sonication method. This method is usually applied for the preparation of nanometal oxides. This method usually differs from other traditional procedures. In recent times, this method has also been applied to prepare binary metal oxides. Probe sonicationally synthesized powdered Bi2O3 nanomaterials using Bi(NO3)3.5H2O offer many advantages like a good degree of crystallinity, well-established morphology, and high purity. After the calcination, the obtained pure powders of Bi2O3 NPs were characterized by the techniques like PXRD, FTIR, SEM, and TEM. To the best of our knowledge, no one has reported the improvement of electrocatalytic oxidation of paracetamol using nanoparticle bismuth oxide modified by graphite carbon electrode. The characterization of a known amount of Bi2O3 NPs that could catalyse the oxidation process of paracetamol in an acidic medium was investigated.


## 2. Experimental

### 2.1. Synthesis of Bismuth Oxide Nanoparticles (Bi2O3 NPs)

The synthesis of Bi2O3 NPs by probe sonication method from the precursors, bismuth nitrate pentahydrate (Bi (NO3)3.5H2O), and sodium hydroxide (NaOH) taken in the ratio of 1 : 2 was carried out with the support of ultrasound radiation. All the chemicals were used as received in analytical reagent (AR) grade. 1.0 M solution of bismuth nitrate pentahydrate (4.85 g) was added to a mixture of 5 mL of concentrated nitric acid (HNO3) and 45 mL of deionized water with continuous stirring. Then, 0.5 M solution of sodium hydroxide (1 g) was added dropwise to the above precursor solution under stirring. This solution was bombarded with high-intensity ultrasound radiation at 40°C for 1 hr by using a microprocessor unit controlled ultrasonic probe of 13 mm diameter made up of high-grade titanium alloy (model PRO-550, 20 kHz, 500 W), operated at 20% amplitude, 20 kHz frequency with 100 W theoretical power dissipation [30]. On completion of the reaction process, a light yellow precipitate was formed. Then, the solution was centrifuged and the obtained precipitate was washed with distilled water and ethanol to remove excess NaOH. The precipitate was dried in a hot air oven at 100°C for 1 hr and calcined at 600°C for 2 hrs to get greenish coloured Bi2O3 NPs.


### 2.2. Instrumentation

The structural analysis, functional group analysis, morphological studies, and optical analysis were carried out using, X-ray diffractometer (Shimadzu) (CuKα-1.541 Å) with a scan rate of 20 per minute, Perkin Elmer FTIR (Spectrum-1000) spectrometer in the range of 4000-400 cm−1, JEOL transmission electron microscopy (TEM) (JEM-2100 (accelerating voltage up to 200 kV, LaB6 filament)), and Shimadzu UV–Vis spectrophotometer model 2600 in the range of 200–800 nm, respectively. The cyclic voltammetric and impedance measurements were executed on an electrochemical analyzer CHI608E potentiostat and in a tri-electrode system.


### 2.3. Preparation of an Electrode from Carbon Paste

The working electrode was made by blending Bi2O3 NPs with graphite powder (conducting carbon) and silicon oil (binder) in the weight ratio of 15 : 70 : 15 and made into a consistent slurry by physically grinding [31, 32]. Finely grounded material was filled into a teflon cavity tube (homemade) and confirming a fitted packing and the packed carbon paste surface was then smoothened.


## 2.1. Synthesis of Bismuth Oxide Nanoparticles (Bi2O3 NPs)

The synthesis of Bi2O3 NPs by probe sonication method from the precursors, bismuth nitrate pentahydrate (Bi (NO3)3.5H2O), and sodium hydroxide (NaOH) taken in the ratio of 1 : 2 was carried out with the support of ultrasound radiation. All the chemicals were used as received in analytical reagent (AR) grade. 1.0 M solution of bismuth nitrate pentahydrate (4.85 g) was added to a mixture of 5 mL of concentrated nitric acid (HNO3) and 45 mL of deionized water with continuous stirring. Then, 0.5 M solution of sodium hydroxide (1 g) was added dropwise to the above precursor solution under stirring. This solution was bombarded with high-intensity ultrasound radiation at 40°C for 1 hr by using a microprocessor unit controlled ultrasonic probe of 13 mm diameter made up of high-grade titanium alloy (model PRO-550, 20 kHz, 500 W), operated at 20% amplitude, 20 kHz frequency with 100 W theoretical power dissipation [30]. On completion of the reaction process, a light yellow precipitate was formed. Then, the solution was centrifuged and the obtained precipitate was washed with distilled water and ethanol to remove excess NaOH. The precipitate was dried in a hot air oven at 100°C for 1 hr and calcined at 600°C for 2 hrs to get greenish coloured Bi2O3 NPs.


## 2.2. Instrumentation

The structural analysis, functional group analysis, morphological studies, and optical analysis were carried out using, X-ray diffractometer (Shimadzu) (CuKα-1.541 Å) with a scan rate of 20 per minute, Perkin Elmer FTIR (Spectrum-1000) spectrometer in the range of 4000-400 cm−1, JEOL transmission electron microscopy (TEM) (JEM-2100 (accelerating voltage up to 200 kV, LaB6 filament)), and Shimadzu UV–Vis spectrophotometer model 2600 in the range of 200–800 nm, respectively. The cyclic voltammetric and impedance measurements were executed on an electrochemical analyzer CHI608E potentiostat and in a tri-electrode system.


## 2.3. Preparation of an Electrode from Carbon Paste

The working electrode was made by blending Bi2O3 NPs with graphite powder (conducting carbon) and silicon oil (binder) in the weight ratio of 15 : 70 : 15 and made into a consistent slurry by physically grinding [31, 32]. Finely grounded material was filled into a teflon cavity tube (homemade) and confirming a fitted packing and the packed carbon paste surface was then smoothened.


## 3. Results and Discussion

### 3.1. Powder X-Ray Diffraction Studies

Figure1 reveals the PXRD patterns of Bi2O3 NPs synthesized by the probe sonication method and calcined at 600°C for 2 hrs. The diffraction peaks appeared at 2θ values of 24.9°, 25.8°, 27.4°, 27.9°, 33.1°, 35.2°, 37.6°, and 46.4° are correlated to (102), (002), (120), (012), (-122), (212), (112), and (041) planes which are very well indexed to monoclinic structure and in compliance with JCPDS card no. 01-076-1730 with phase group P21/c [33]. The lattice parameters were found to be; a=5.8499Å, b=8.1698Å, and c=7.5123Å and α=90°, β=112.988°, and γ=90°. From Debye-Scherrer’s formula (equation (1)), the crystallite size of Bi2O3 NPs was deduced to be in the range between 55 and 60 nm (Table 1).
(1)D=kλβcosθ,Figure 1
PXRD patterns of Bi2O3 NPs.Table 1
FWHM values, d-spacing, and Miller indices for Bi2O3.
Miller indices (hkl)2θ (degree)FWHM (degree)d-spacing (nm)Crystal size (nm)10224.90.170.4355.7800225.80.200.3752.0012027.50.130.3365.7801227.90.150.3953.13-12233.10.190.4063.1121235.20.140.3259.2111237.60.160.3560.1404146.40.210.4261.21Averagecrystallitesize=58.79nm.whereβ is full width at half maximum (FWHM) of the diffraction peak, λ is wavelength of X-ray (1.5418 Å), θ is Bragg’s angle, and k is Scherrer’s constant (0.88–0.92); the average value of 0.9 was used for the calculation.Thed-spacing can be deduced using the following equation
(2)1d2=1sin2βh2a2+k2sin2βb2+l2c2−2hlcosβac,wherea, b, and c are lattice parameters, hkl is Miller indices, and dhkl is interplanar spacing for hkl.FWHM values, crystallite sizes,d-spacing values, and Miller indices for Bi2O3 NPs obtained from the probe sonication method have been tabulated in Table 1.Various other crystal parameters such as unit cell volume (V), the number of unit cells (n), X-ray density (Dx), dislocation density (δ), microstrain (ε), stress (σ), and stacking fault were determined using PXRD data (Table 2) and following relationships [14, 21, 34]:
(3)V=a3,(4)N=43πD/2V,(5)Dx=16MNa3,(6)δ=1D2,(7)ε=βcosθ4,(8)σstress=ϵE,(9)S.F=2π2453tanθ,Table 2
Estimated structural parameters of Bi2O3 NPs prepared from probe sonication method.
Plane for Bi2O3β×10−3D (nm)d (nm)V×10−30m3n×10−21Dx×104 (kgm−3)δ×1015 (kgm−3)−2ε×10−3E (GPa)σ×108 (Pa)SF(120)0.1365.780.3320.06.478.6322.328.650119.23.410.35whereM is molecular mass, N is Avogadro’s number (6.0223×1023 particles mol−1), and E is elastic constant of the material.


### 3.2. Fourier-Transform Infrared Spectroscopy

The Fourier transform infrared (FTIR) spectrum of Bi2O3 NPs was recorded in the wavenumber range of 400–4000 cm-1 at room temperature using KBr pellets Figure 2. The appearance of two peaks at 691.5 cm-1 and 853.8 cm-1 corresponds to the metal-oxygen (Bi-O) vibration [35]. After calcination of Bi2O3 NPs at 500°C, many peaks were assumed to have disappeared because of the evaporation of most of the solvent molecules and decomposition of the organic ingredient. The additional peaks, at about 1291 cm−1 and 1247 cm-1, can be attributed to Bi3+– O2−stretching.Figure 2
FT-IR spectrum of Bi2O3 NPs.


### 3.3. SEM Analysis

SEM micrographs of Bi2O3 NPs as shown in Figures 3(a) and 3(b) approve the formation of highly porous and agglomerated nanoparticles with an irregular morphology which is possibly due to the escape of a large amount of gases during the probe sonication process [36, 37]. These NPs were found to possess active surface sites and thus they can be suitably employed for applications in electrochemical and supercapacitor devices. The EDX spectrum of Bi2O3 NPs is presented in Figure 3(c). The spectrum confirmed the presence of only Bi and O elements (Table 3) in Bi2O3 NPs confirming the purity of the NPs.Figure 3
(a) and (b) SEM images. (c) EDAX of Bi2O3 NPs.
(a)(b)(c)Table 3
Compositional data obtained from EDAX.
ElementWeight %Atomic %O K15.0969.89Bi L84.9130.11


### 3.4. TEM Analysis

The surface morphology of the synthesized Bi2O3 nanostructures was investigated using high-resolution transmission electron microscopy (HRTEM), and the morphology is depicted in Figure 4. Figures 4(a) and 4(b) show that the morphology has been slightly agglomerated, but SEM and TEM images show that the prepared Bi2O3 has a sheet shape morphology, which is consistent with previous findings [38]. It is possible that the sheet shape morphology is caused by the nature of the laminar structure. Clear fringes can be seen in Figure 4(d) with an interplanar distance of 4.57 nm, which corresponds to the plane of (120), and an interplanar distance of 5.76 nm (Figure 4(c)), which corresponds to the plane of (-122). The other planes, which are denoted by the numbers 3 and 4 in the SAED pattern of prepared Bi2O3, correspond to the planes of (112) and (041). The planes observed in the SAED pattern are in excellent agreement with the planes observed in the XRD pattern.Figure 4
(a) and (b) TEM images, (c) SAED pattern, and (d) HR-TEM of Bi2O3 NPs.
(a)(b)(c)(d)


### 3.5. Diffuse Reflectance Spectroscopy (DRS) Analysis

The value ofEg for Bi2O3 NPs was evaluated by using the UV–vis reflectance spectroscopy is given in Figure 5 [39]. The synthesized NPs exhibited a representative reflectance with a strong transition in the UV region corresponding to the bandgap transition of the Bi2O3 semiconductor. The Kubelka-Munk function F(R) provides the diffused reflectance as a function of absorption coefficient and can be utilized for examining the powders as given by the following equation:
(10)FR=1−R22R,Figure 5
DRS and energy bandgap spectra patterns of Bi2O3 NPs.whereR is reflectance and FR is Kubelka-Munk functions.The inset of Figure5 shows the direct bandgap energy was estimated by plotting fRhv2 vs. energy gap (eV). The optical energy gap was calculated using the Tauc relation [40], as given by the following equation.
(11)αhυ=Ahυ–Egn,wherehυ; photon energy, α; absorption coefficient (α=4πk/λ); (k; absorption index or absorbance, λ; the wavelength in nanometer), Eg; energy band gap, A; constant, n=1/2 for the allowed direct bandgap. The exponent “n” depends on the type of transition, and it may have values 1/2, 2, 3/2, and 3 corresponding to the allowed direct, allowed indirect, forbidden direct, and forbidden indirect transitions, respectively [41, 42]. The optical energy gap thus calculated for the synthesized Bi2O3 NPs is 3.3 eV and is shown in the inset of Figure 5. This resulted in the generation of higher electron-hole pairs for better photocatalytic efficiency.


### 3.6. Photocatalytic Studies

Spherical glass reactor with 176.6 cm2 surface areas and mercury vapor lamps UV light source with 125 W medium pressures were used to carry out photocatalytic experiments. The emission wavelength with the highest emission at 370 nm (UVA) in the range of 350–400 nm was utilized, and no filters were used to exclude the light of different wavelengths. In open-air conditions, at a distance of 23 cm, the light was directly irradiated onto the reaction mixture. Double distilled water was used to perform all the experiments. The experiment was conducted using 60 mg of photocatalyst sample Bi2O3 was dissolved in 250 mL of 20 ppm concentrated dye solution. Throughout the experiment, the solution was stirred continuously by using a magnetic stirrer. At definite time intervals, 5 mL of the reaction mixture was collected from the dye solution, and the catalyst particles were removed using an external magnet [43, 44].Photocatalytic activity (PCA) of the Bi2O3 NPs was assessed by photodegradation of methylene blue (MB), a cationic dye with maximum absorption at 664 nm, and acid red (AR), an anionic dye with maximum absorption at 640 nm as shown in Figures 6(a) and 6(b). Initially, the PCA experiments were carried out in the dark condition to see the photocatalytic activity for (MB) and (AG) dye using the synthesized catalysts. The dyes did not undergo any degradation, and hence, no change was observed [45, 46].Figure 6
(a) and (b) Absorption spectra of MB and AR dyes decomposition for Bi2O3 NPs.
(a)(b)As presented in Figures7(a) and 7(b) after 120 min of UV light irradiation, the photodegradation rate of MB dye (Tables 4 and 5) was found to be 93.45%, but, in the same environment, the photodegradation rate of AR dye (Tables 6 and 5) was recorded to be 97.8%. This clearly indicates that AR dye is more susceptible to decolorization than MB when exposed to UV light for 120 min. The obtained results are superior compared to the earlier published work where the dye degradation efficiencies were found to be 95.02% for Fast Red acid dye [47] and 92.3 for methylene blue dye [48]. The percentage of degradation was calculated from the following equation,
(12)%D=Co−CCo×100,where %D is photo-decolorization efficiency, Co and C are initial concentrations of the dye solutions and the residual concentration of the dye in solution after decolorization in equilibrium, respectively.Figure 7
(a) and (b) Plot ofC/Co for the decolorization of MB and AR under UV light illumination.
(a)(b)Table 4
Rate constants and kinetic studies of Bi2O3 for methylene blue (MB) decolorization under UV light irradiation.
20ppmMB+60mgBi2O3+UVlighttcc/coLog c/co-log c/co%D020100015160.8-0.096910.09691203011.250.5625-0.249880.24987743.75458.430.4215-0.37520.37520257.85606.750.3375-0.471730.47172666.25754.560.228-0.642070.64206577.2903.060.153-0.815310.81530984.71052.310.1155-0.937420.93741888.451201.310.0655-1.183761.18375993.45Rate=0.018758min−1.Table 5
List of dyes.
Name of dyeType of dyeClass of dyeStructureMol.wt (g/mol)Methylene blueBasic dyeThiazine319.9Acid redAcid dyeAzo dye400.38Table 6
Rate constants and kinetic studies of Bi2O3 for acid red (AR) decolorization under UV light irradiation.
20ppmAR+60mgBi2O3+UVlighttcc/coLog c/co-log c/co%D020100015160.8-0.096910.09691203010.80.54-0.267610.26760646457.770.3885-0.410610.41060961.15606.220.311-0.507240.5072468.9753.550.1775-0.75080.75080282.25902.810.1405-0.852320.85232485.951051.330.0665-1.177181.17717893.351200.440.022-1.657581.65757797.8Rate=0.020392min−1.Langmuir-Hinshelwood kinetic model was utilized to discuss photocatalytic degradation Kinetics of MB and AR by Bi2O3 NPs as shown in Figures 8(a) and 8(b), using the following equation.
(13)logcCo=−Kt,Figure 8
(a) and (b) Percentage decomposition of MB and AR dyes over Bi2O3 NPs.
(a)(b)whereCo is concentration of MB and AG dyes initially, C is concentration at time t, k is rate of first-order kinetics (min −1), and t is time in seconds.The slope of (logC/Co) vs. time (t) gives the rate constant K. The rate constant values for Bi2O3 NPs are 0.018758 min−1 (MB) and 0.020392 min−1 (AG). First-order kinetics was confirmed from the values calculated from the direct relationship between log C/Co and k.In Figures9(a) and 9(b), the degradation half-life was evaluated in which 50% dye degradation was observed in a time span of 37 min for (MB) and 34 min (AG). The results indicated that bismuth oxide is prominent material for the degradation of textile dye pollutants and is also useful for the removal of secondary pollutants. A novel bismuth oxide-based thin film as a photocatalyst recorded 98% degradation under UV light irradiation for 8 hours while obtaining a 73.47% COD (chemical oxygen) reduction. The photocatalytic degradation managed to degrade the smaller organic molecules that were formed during the initial stages of degradation, leaving behind the less decomposable by-products [49].Figure 9
(a) and (b) Time span of MB and AR dyes over Bi2O3 NPs.
(a)(b)


### 3.7. Mechanism of Photocatalytic Degradation

As the solution containing photocatalyst (Bi2O3 NPs) is irradiated by visible (Vis) radiation, electrons in the valence band (VB) of the catalyst get transferred to the conduction band (CB) by creating a hole in VB (Figure 10) [46]. These holes and electrons interact with H2O and O2 to yield OH• and O2•-, respectively, and then the hydroxyl radicals interact with dye molecules to degrade to smaller molecules [50, 51]. The main steps involved in the reaction process of photocatalytic degradation under visible light irradiation are as follows:
(14)Bi2O3+hv⟶e–+h+,(15)O2+e–⟶O2,(16)OH–+h+⟶OH–,(17)OH–+O2–+Dyes⟶Decomposedproduct.Figure 10
The mechanism of MB and AR dyes decomposition for Bi2O3 NPs.It contributed towards the practicality of the synthesized Bi2O3 NPs as they could be applied in the degradation of other organic pollutants.


### 3.8. Cyclic Voltammetric Studies

In order to characterize the synthesized Bi2O3 NPs based sensor, a variety of electrochemical measurements were performed in 0.1 M HCl using lead and ascorbic acid, including cyclic voltammetry (CV) and electrochemical impedance spectroscopy (EIS) (Figure 11). For the cyclic voltammetry studies of the synthesized Bi2O3, a standard three-electrode system in 0.1 M HCl was used. Using a scan rate ranging from 10 mV/s to 50 mV/s, this process was carried out in the absence of lead and/or ascorbic acid. It has been determined that the reduction and oxidation peaks observed at potentials of -0.25 V and -0.09 V, respectively, when the potential range was varied from -0.3 to +0.1, were caused by variations in the potential range from -0.3 to +0.1. With the help of cyclic voltammograms, the specific capacitance of the electrode (Fg-1) could be calculated using the following equation,
(18)Csp=S2mk∆V.Figure 11
(a) Cyclic voltammogram of Bi2O3 NPs with different scanning rates. (b) EIS spectra with equivalent circuit of Bi2O3 NPs.
(a)(b)The area under the CV curve can be represented byS, as given in equation (18), where the mass of the material was represented by m, voltage window was represented by ΔV, and scan rate was given by k. The specific capacitance values were calculated using equation (18) and were found to be 86.6, 55.7, 36.1, 29.8, and 25.5 Fg-1, respectively, for scan rates of 10, 20, 30, 40, and 50 mV in 0.1 M HCl. It can be seen from the specific capacitance values that as the scan rate increases, the specific capacitance values decrease. This can be attributed to the fact that the ions in the electrolyte will have sufficient time to penetrate into the electrode material at a lower scan rate, whereas at a higher scan rate, the ions will simply collect on the electrode material’s outer surface [52]. This results in a decrease in the values of specific capacitance as a result of an increase in scan rate as well [53].The Nyquist plot (Figure11(b)) can be used to determine the electronic conductivity or charge transfer capacity of the prepared electrode. This plot also provides information on the capacitance behavior of the electrode. It is possible to divide the Nyquist plot into two main regions: the first denotes the high-frequency region, which provides information about the charge transfer process at the interface of electrode and/or electrolyte, which is typically seen as a semicircle [54, 55]. The other region represents the low-frequency region, which denotes the capacitance of the electrode and which was given the shape of a straight line in order to represent it accurately. The charge transfer resistance Rct was calculated from the diameter of the semicircle in the Nyquist plot [56]. When the EIS technique was used, it was possible to obtain the equivalent circuit of the system which was given in Figure 11(b) inset.The sensing capability of the synthesized nanomaterial (Bi2O3) for ascorbic acid and lead was investigated using a modified carbon paste electrode, and the obtained results were presented in Figure 12. We experimented with different concentrations of ascorbic acid/lead from 1 to 5 mM in order to better understand the sensing ability of synthesized Bi2O3. According to the results, in the absence of ascorbic acid and lead, the oxidation and reduction peaks were at -0.09 V and -0.2 V, respectively, whereas in the presence of ascorbic acid and lead, the oxidation and reduction peaks shifted to the more positive side of the potential curve [57]. After the addition of ascorbic acid, the oxidation peak at -0.09 V shifts to 0.019 V, and an additional oxidation peak appears at 0.03 V, whereas when the lead is added, the oxidation peak at -0.09 V shifts to 0.05 V. After the addition of ascorbic acid/lead, there is a complete disappearance of the reduction peak in the voltammogram (Figure 12). We can infer from the data that the synthesized material Bi2O3 can function as a good sensing material for ascorbic acid and lead, which is supported by the significant variation in the oxidation and reduction peak positions of the material. Figure 13 shows the concentration of ascorbic acid and lead vs. anodic peak current plot obtained by LSV, which also shows an increase in anodic peak current with increasing concentration of ascorbic acid and lead.Figure 12
Cyclic voltammogram of Bi2O3 NPs. Detection of (a) ascorbic acid and (b) lead concentration range 1–5 mM.
(a)(b)Figure 13
Anodic peak current vs. concentration plot using linear sweep voltammetry (LSV).


## 3.1. Powder X-Ray Diffraction Studies

Figure1 reveals the PXRD patterns of Bi2O3 NPs synthesized by the probe sonication method and calcined at 600°C for 2 hrs. The diffraction peaks appeared at 2θ values of 24.9°, 25.8°, 27.4°, 27.9°, 33.1°, 35.2°, 37.6°, and 46.4° are correlated to (102), (002), (120), (012), (-122), (212), (112), and (041) planes which are very well indexed to monoclinic structure and in compliance with JCPDS card no. 01-076-1730 with phase group P21/c [33]. The lattice parameters were found to be; a=5.8499Å, b=8.1698Å, and c=7.5123Å and α=90°, β=112.988°, and γ=90°. From Debye-Scherrer’s formula (equation (1)), the crystallite size of Bi2O3 NPs was deduced to be in the range between 55 and 60 nm (Table 1).
(1)D=kλβcosθ,Figure 1
PXRD patterns of Bi2O3 NPs.Table 1
FWHM values, d-spacing, and Miller indices for Bi2O3.
Miller indices (hkl)2θ (degree)FWHM (degree)d-spacing (nm)Crystal size (nm)10224.90.170.4355.7800225.80.200.3752.0012027.50.130.3365.7801227.90.150.3953.13-12233.10.190.4063.1121235.20.140.3259.2111237.60.160.3560.1404146.40.210.4261.21Averagecrystallitesize=58.79nm.whereβ is full width at half maximum (FWHM) of the diffraction peak, λ is wavelength of X-ray (1.5418 Å), θ is Bragg’s angle, and k is Scherrer’s constant (0.88–0.92); the average value of 0.9 was used for the calculation.Thed-spacing can be deduced using the following equation
(2)1d2=1sin2βh2a2+k2sin2βb2+l2c2−2hlcosβac,wherea, b, and c are lattice parameters, hkl is Miller indices, and dhkl is interplanar spacing for hkl.FWHM values, crystallite sizes,d-spacing values, and Miller indices for Bi2O3 NPs obtained from the probe sonication method have been tabulated in Table 1.Various other crystal parameters such as unit cell volume (V), the number of unit cells (n), X-ray density (Dx), dislocation density (δ), microstrain (ε), stress (σ), and stacking fault were determined using PXRD data (Table 2) and following relationships [14, 21, 34]:
(3)V=a3,(4)N=43πD/2V,(5)Dx=16MNa3,(6)δ=1D2,(7)ε=βcosθ4,(8)σstress=ϵE,(9)S.F=2π2453tanθ,Table 2
Estimated structural parameters of Bi2O3 NPs prepared from probe sonication method.
Plane for Bi2O3β×10−3D (nm)d (nm)V×10−30m3n×10−21Dx×104 (kgm−3)δ×1015 (kgm−3)−2ε×10−3E (GPa)σ×108 (Pa)SF(120)0.1365.780.3320.06.478.6322.328.650119.23.410.35whereM is molecular mass, N is Avogadro’s number (6.0223×1023 particles mol−1), and E is elastic constant of the material.


## 3.2. Fourier-Transform Infrared Spectroscopy

The Fourier transform infrared (FTIR) spectrum of Bi2O3 NPs was recorded in the wavenumber range of 400–4000 cm-1 at room temperature using KBr pellets Figure 2. The appearance of two peaks at 691.5 cm-1 and 853.8 cm-1 corresponds to the metal-oxygen (Bi-O) vibration [35]. After calcination of Bi2O3 NPs at 500°C, many peaks were assumed to have disappeared because of the evaporation of most of the solvent molecules and decomposition of the organic ingredient. The additional peaks, at about 1291 cm−1 and 1247 cm-1, can be attributed to Bi3+– O2−stretching.Figure 2
FT-IR spectrum of Bi2O3 NPs.


## 3.3. SEM Analysis

SEM micrographs of Bi2O3 NPs as shown in Figures 3(a) and 3(b) approve the formation of highly porous and agglomerated nanoparticles with an irregular morphology which is possibly due to the escape of a large amount of gases during the probe sonication process [36, 37]. These NPs were found to possess active surface sites and thus they can be suitably employed for applications in electrochemical and supercapacitor devices. The EDX spectrum of Bi2O3 NPs is presented in Figure 3(c). The spectrum confirmed the presence of only Bi and O elements (Table 3) in Bi2O3 NPs confirming the purity of the NPs.Figure 3
(a) and (b) SEM images. (c) EDAX of Bi2O3 NPs.
(a)(b)(c)Table 3
Compositional data obtained from EDAX.
ElementWeight %Atomic %O K15.0969.89Bi L84.9130.11


## 3.4. TEM Analysis

The surface morphology of the synthesized Bi2O3 nanostructures was investigated using high-resolution transmission electron microscopy (HRTEM), and the morphology is depicted in Figure 4. Figures 4(a) and 4(b) show that the morphology has been slightly agglomerated, but SEM and TEM images show that the prepared Bi2O3 has a sheet shape morphology, which is consistent with previous findings [38]. It is possible that the sheet shape morphology is caused by the nature of the laminar structure. Clear fringes can be seen in Figure 4(d) with an interplanar distance of 4.57 nm, which corresponds to the plane of (120), and an interplanar distance of 5.76 nm (Figure 4(c)), which corresponds to the plane of (-122). The other planes, which are denoted by the numbers 3 and 4 in the SAED pattern of prepared Bi2O3, correspond to the planes of (112) and (041). The planes observed in the SAED pattern are in excellent agreement with the planes observed in the XRD pattern.Figure 4
(a) and (b) TEM images, (c) SAED pattern, and (d) HR-TEM of Bi2O3 NPs.
(a)(b)(c)(d)


## 3.5. Diffuse Reflectance Spectroscopy (DRS) Analysis

The value ofEg for Bi2O3 NPs was evaluated by using the UV–vis reflectance spectroscopy is given in Figure 5 [39]. The synthesized NPs exhibited a representative reflectance with a strong transition in the UV region corresponding to the bandgap transition of the Bi2O3 semiconductor. The Kubelka-Munk function F(R) provides the diffused reflectance as a function of absorption coefficient and can be utilized for examining the powders as given by the following equation:
(10)FR=1−R22R,Figure 5
DRS and energy bandgap spectra patterns of Bi2O3 NPs.whereR is reflectance and FR is Kubelka-Munk functions.The inset of Figure5 shows the direct bandgap energy was estimated by plotting fRhv2 vs. energy gap (eV). The optical energy gap was calculated using the Tauc relation [40], as given by the following equation.
(11)αhυ=Ahυ–Egn,wherehυ; photon energy, α; absorption coefficient (α=4πk/λ); (k; absorption index or absorbance, λ; the wavelength in nanometer), Eg; energy band gap, A; constant, n=1/2 for the allowed direct bandgap. The exponent “n” depends on the type of transition, and it may have values 1/2, 2, 3/2, and 3 corresponding to the allowed direct, allowed indirect, forbidden direct, and forbidden indirect transitions, respectively [41, 42]. The optical energy gap thus calculated for the synthesized Bi2O3 NPs is 3.3 eV and is shown in the inset of Figure 5. This resulted in the generation of higher electron-hole pairs for better photocatalytic efficiency.


## 3.6. Photocatalytic Studies

Spherical glass reactor with 176.6 cm2 surface areas and mercury vapor lamps UV light source with 125 W medium pressures were used to carry out photocatalytic experiments. The emission wavelength with the highest emission at 370 nm (UVA) in the range of 350–400 nm was utilized, and no filters were used to exclude the light of different wavelengths. In open-air conditions, at a distance of 23 cm, the light was directly irradiated onto the reaction mixture. Double distilled water was used to perform all the experiments. The experiment was conducted using 60 mg of photocatalyst sample Bi2O3 was dissolved in 250 mL of 20 ppm concentrated dye solution. Throughout the experiment, the solution was stirred continuously by using a magnetic stirrer. At definite time intervals, 5 mL of the reaction mixture was collected from the dye solution, and the catalyst particles were removed using an external magnet [43, 44].Photocatalytic activity (PCA) of the Bi2O3 NPs was assessed by photodegradation of methylene blue (MB), a cationic dye with maximum absorption at 664 nm, and acid red (AR), an anionic dye with maximum absorption at 640 nm as shown in Figures 6(a) and 6(b). Initially, the PCA experiments were carried out in the dark condition to see the photocatalytic activity for (MB) and (AG) dye using the synthesized catalysts. The dyes did not undergo any degradation, and hence, no change was observed [45, 46].Figure 6
(a) and (b) Absorption spectra of MB and AR dyes decomposition for Bi2O3 NPs.
(a)(b)As presented in Figures7(a) and 7(b) after 120 min of UV light irradiation, the photodegradation rate of MB dye (Tables 4 and 5) was found to be 93.45%, but, in the same environment, the photodegradation rate of AR dye (Tables 6 and 5) was recorded to be 97.8%. This clearly indicates that AR dye is more susceptible to decolorization than MB when exposed to UV light for 120 min. The obtained results are superior compared to the earlier published work where the dye degradation efficiencies were found to be 95.02% for Fast Red acid dye [47] and 92.3 for methylene blue dye [48]. The percentage of degradation was calculated from the following equation,
(12)%D=Co−CCo×100,where %D is photo-decolorization efficiency, Co and C are initial concentrations of the dye solutions and the residual concentration of the dye in solution after decolorization in equilibrium, respectively.Figure 7
(a) and (b) Plot ofC/Co for the decolorization of MB and AR under UV light illumination.
(a)(b)Table 4
Rate constants and kinetic studies of Bi2O3 for methylene blue (MB) decolorization under UV light irradiation.
20ppmMB+60mgBi2O3+UVlighttcc/coLog c/co-log c/co%D020100015160.8-0.096910.09691203011.250.5625-0.249880.24987743.75458.430.4215-0.37520.37520257.85606.750.3375-0.471730.47172666.25754.560.228-0.642070.64206577.2903.060.153-0.815310.81530984.71052.310.1155-0.937420.93741888.451201.310.0655-1.183761.18375993.45Rate=0.018758min−1.Table 5
List of dyes.
Name of dyeType of dyeClass of dyeStructureMol.wt (g/mol)Methylene blueBasic dyeThiazine319.9Acid redAcid dyeAzo dye400.38Table 6
Rate constants and kinetic studies of Bi2O3 for acid red (AR) decolorization under UV light irradiation.
20ppmAR+60mgBi2O3+UVlighttcc/coLog c/co-log c/co%D020100015160.8-0.096910.09691203010.80.54-0.267610.26760646457.770.3885-0.410610.41060961.15606.220.311-0.507240.5072468.9753.550.1775-0.75080.75080282.25902.810.1405-0.852320.85232485.951051.330.0665-1.177181.17717893.351200.440.022-1.657581.65757797.8Rate=0.020392min−1.Langmuir-Hinshelwood kinetic model was utilized to discuss photocatalytic degradation Kinetics of MB and AR by Bi2O3 NPs as shown in Figures 8(a) and 8(b), using the following equation.
(13)logcCo=−Kt,Figure 8
(a) and (b) Percentage decomposition of MB and AR dyes over Bi2O3 NPs.
(a)(b)whereCo is concentration of MB and AG dyes initially, C is concentration at time t, k is rate of first-order kinetics (min −1), and t is time in seconds.The slope of (logC/Co) vs. time (t) gives the rate constant K. The rate constant values for Bi2O3 NPs are 0.018758 min−1 (MB) and 0.020392 min−1 (AG). First-order kinetics was confirmed from the values calculated from the direct relationship between log C/Co and k.In Figures9(a) and 9(b), the degradation half-life was evaluated in which 50% dye degradation was observed in a time span of 37 min for (MB) and 34 min (AG). The results indicated that bismuth oxide is prominent material for the degradation of textile dye pollutants and is also useful for the removal of secondary pollutants. A novel bismuth oxide-based thin film as a photocatalyst recorded 98% degradation under UV light irradiation for 8 hours while obtaining a 73.47% COD (chemical oxygen) reduction. The photocatalytic degradation managed to degrade the smaller organic molecules that were formed during the initial stages of degradation, leaving behind the less decomposable by-products [49].Figure 9
(a) and (b) Time span of MB and AR dyes over Bi2O3 NPs.
(a)(b)


## 3.7. Mechanism of Photocatalytic Degradation

As the solution containing photocatalyst (Bi2O3 NPs) is irradiated by visible (Vis) radiation, electrons in the valence band (VB) of the catalyst get transferred to the conduction band (CB) by creating a hole in VB (Figure 10) [46]. These holes and electrons interact with H2O and O2 to yield OH• and O2•-, respectively, and then the hydroxyl radicals interact with dye molecules to degrade to smaller molecules [50, 51]. The main steps involved in the reaction process of photocatalytic degradation under visible light irradiation are as follows:
(14)Bi2O3+hv⟶e–+h+,(15)O2+e–⟶O2,(16)OH–+h+⟶OH–,(17)OH–+O2–+Dyes⟶Decomposedproduct.Figure 10
The mechanism of MB and AR dyes decomposition for Bi2O3 NPs.It contributed towards the practicality of the synthesized Bi2O3 NPs as they could be applied in the degradation of other organic pollutants.


## 3.8. Cyclic Voltammetric Studies

In order to characterize the synthesized Bi2O3 NPs based sensor, a variety of electrochemical measurements were performed in 0.1 M HCl using lead and ascorbic acid, including cyclic voltammetry (CV) and electrochemical impedance spectroscopy (EIS) (Figure 11). For the cyclic voltammetry studies of the synthesized Bi2O3, a standard three-electrode system in 0.1 M HCl was used. Using a scan rate ranging from 10 mV/s to 50 mV/s, this process was carried out in the absence of lead and/or ascorbic acid. It has been determined that the reduction and oxidation peaks observed at potentials of -0.25 V and -0.09 V, respectively, when the potential range was varied from -0.3 to +0.1, were caused by variations in the potential range from -0.3 to +0.1. With the help of cyclic voltammograms, the specific capacitance of the electrode (Fg-1) could be calculated using the following equation,
(18)Csp=S2mk∆V.Figure 11
(a) Cyclic voltammogram of Bi2O3 NPs with different scanning rates. (b) EIS spectra with equivalent circuit of Bi2O3 NPs.
(a)(b)The area under the CV curve can be represented byS, as given in equation (18), where the mass of the material was represented by m, voltage window was represented by ΔV, and scan rate was given by k. The specific capacitance values were calculated using equation (18) and were found to be 86.6, 55.7, 36.1, 29.8, and 25.5 Fg-1, respectively, for scan rates of 10, 20, 30, 40, and 50 mV in 0.1 M HCl. It can be seen from the specific capacitance values that as the scan rate increases, the specific capacitance values decrease. This can be attributed to the fact that the ions in the electrolyte will have sufficient time to penetrate into the electrode material at a lower scan rate, whereas at a higher scan rate, the ions will simply collect on the electrode material’s outer surface [52]. This results in a decrease in the values of specific capacitance as a result of an increase in scan rate as well [53].The Nyquist plot (Figure11(b)) can be used to determine the electronic conductivity or charge transfer capacity of the prepared electrode. This plot also provides information on the capacitance behavior of the electrode. It is possible to divide the Nyquist plot into two main regions: the first denotes the high-frequency region, which provides information about the charge transfer process at the interface of electrode and/or electrolyte, which is typically seen as a semicircle [54, 55]. The other region represents the low-frequency region, which denotes the capacitance of the electrode and which was given the shape of a straight line in order to represent it accurately. The charge transfer resistance Rct was calculated from the diameter of the semicircle in the Nyquist plot [56]. When the EIS technique was used, it was possible to obtain the equivalent circuit of the system which was given in Figure 11(b) inset.The sensing capability of the synthesized nanomaterial (Bi2O3) for ascorbic acid and lead was investigated using a modified carbon paste electrode, and the obtained results were presented in Figure 12. We experimented with different concentrations of ascorbic acid/lead from 1 to 5 mM in order to better understand the sensing ability of synthesized Bi2O3. According to the results, in the absence of ascorbic acid and lead, the oxidation and reduction peaks were at -0.09 V and -0.2 V, respectively, whereas in the presence of ascorbic acid and lead, the oxidation and reduction peaks shifted to the more positive side of the potential curve [57]. After the addition of ascorbic acid, the oxidation peak at -0.09 V shifts to 0.019 V, and an additional oxidation peak appears at 0.03 V, whereas when the lead is added, the oxidation peak at -0.09 V shifts to 0.05 V. After the addition of ascorbic acid/lead, there is a complete disappearance of the reduction peak in the voltammogram (Figure 12). We can infer from the data that the synthesized material Bi2O3 can function as a good sensing material for ascorbic acid and lead, which is supported by the significant variation in the oxidation and reduction peak positions of the material. Figure 13 shows the concentration of ascorbic acid and lead vs. anodic peak current plot obtained by LSV, which also shows an increase in anodic peak current with increasing concentration of ascorbic acid and lead.Figure 12
Cyclic voltammogram of Bi2O3 NPs. Detection of (a) ascorbic acid and (b) lead concentration range 1–5 mM.
(a)(b)Figure 13
Anodic peak current vs. concentration plot using linear sweep voltammetry (LSV).


## 4. Conclusions

To summarize, in this research, we have used a well-known probe sonication approach for the synthesis of Bi2O3 nanoparticles that is low in cost and highly calibrated. The produced nanoparticles were submitted to a number of different characterization procedures in order to gain a better understanding of their crystal structure, as well as their morphological and optical characteristics. It was discovered from the optical properties of the Bi2O3 nanoparticles have a bandgap of 3.3 eV, which makes them excellent for the degradation of dyes when exposed to ultraviolet radiation. The SEM, TEM, and HRTEM analyses revealed that the nanoparticles are highly porous materials with a small agglomeration. MB and AR dyes were both subjected to degradation under ultraviolet (UV) radiation in the presence of the catalyst, and it was observed that the degradation of MB and AR dyes was 93.45% and 97.80%, respectively, and that the results were quite impressive. In the electrochemical investigations, it was discovered that the produced nanomaterial has the ability to detect several heavy metals as well as the ascorbic acid medication. The specific capacitance of the sample was calculated to be 25.5 Fg-1 in 0.1 N HCl, according to the results of the experiment. Hence, Bi2O3 nanoparticles can be used as bifunctional materials for degradation and for sensing applications.



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