Document Type : Research Paper
Authors
1 Department of Chemistry, College of Science, University of Babylon, Hilla, Iraq
2 Department of Chemistry, College of Education, University of Al-Qadisiyah, Diwaniyah, Iraq
3 Department of Chemistry, College of Education, University of Al-Qadisiyah, Iraq
Abstract
Keywords
INTRODUCTION
In the near future, substantial costs are anticipated for mitigating damages caused by industrial activities and technological advancements [1]. Currently, dyes find diverse applications across various industries [2]. However, many of these dyes pose carcinogenic and mutagenic risks to humans and other organisms [3]. Malachite green, a triphenylmethane chemical structure dye, is extensively used in the aquaculture industry against external parasites, fungus, and bacteria [4]. It is also utilized in the dyeing industries for materials like silk, wool, jute, hemp, and paper [5]. Despite its effectiveness in controlling infections from bacteria, protozoa, nematodes, trematodes, and cestodes in aquaculture, malachite green is toxic and can induce liver tumors in standard organisms [6, 7]. Excessive use of malachite green, due to its detrimental environmental impact and health threats to organisms, necessitates urgent attention [8]. Conventional physicochemical methods, including chemical precipitation, solvent extraction, ion exchange resins, and others, have been employed to remove malachite green and other harmful organic compounds from water [9]. Given the molecular structure and aromatic complex of dyes, they are generally resistant to degradation by light, biological activities, oxidizing agents, and other environmental conditions [10, 11]. Consequently, traditional biological water purification systems are ineffective against dyes [12]. Moreover, these methods have disadvantages like incomplete removal of malachite green, high costs, and the need for extensive monitoring, energy, chemical consumption, and toxic sludge production [13]. This natural material exists in various forms, with Kaolin and smectite being the most commonly used in the industry. Kaolin has a platy structure resembling gold (metal leaf) with the chemical formula Al2Si2O5(OH)4, consisting of hexagonal or octagonal sheets [14]. These sheets or plates are composed of linked silicon-oxygen tetrahedra forming hexagonal rings. By repeating these rings in two dimensions, a sheet or plate is formed. Octahedral sheets are made up of silicon and aluminum units [15]. The Kaolin layer structure, is held together by hydrogen bonds between hydroxyl groups in the octahedral sheets and oxygen in the tetrahedral sheets [16]. Hydrogels, crosslinked polymers, can be synthesized either physically or chemically, contingent upon the type of polymer and the specific experimental conditions [17]. Physical crosslinking is deemed environmentally benign, owing to its independence from cross-linking agents or initiators [18]. Conversely, chemical methods, involving covalent bond formation, result in hydrogels characterized by greater stability and augmented mechanical strength [19]. Chitosan, sourced from the alkaline deacetylation of chitin (the second most plentiful natural polymer following cellulose), presents advantageous properties for material development [20]. These include biocompatibility, biodegradability, cost-effectiveness, and high reactivity attributed to Multiple functional groups [21]. Thus, chitosan Surface as a superior candidate for fabricating nanocomposite hydrogels aimed at the adsorption of MG dye [22]. The Adoption of synthetic polymers into these natural material-based hydrogels further amplifies their desired physical and chemical characteristics [23].
In aqueous solutions, hydrogel/Kaolin clay was tested for hazardous MG cation adsorption. MG removal efficiency was affected by starting MG ion concentrations, adsorbent dose, and temperature. Kinetic, mechanistic, and thermodynamic investigations were also performed to understand MG-adsorbent interactions and find the best mathematical models for adsorption. The study also reactivated the adsorbent’s surface for recurrent use during removal.
MATERIALS AND METHODS
Preparation of CS-g-P(AA)/Kaolin nanocomposite
The CS-g-P(AA)/Kaolin hydrogel nanocomposite was prepared from a series of solutions starting with the dissolution of 1.0 g of chitosan (CS) in 40 mL of 1% acetic acid, stirred using a magnetic stirrer (hotplate stirrer) for 15 minutes. Subsequently, 10 mL of acrylic acid (AA) was added, followed by varying amounts (0.5, 1, 1.5, 2 grams) of the primary material, Kaolin clay (KAOLIN), dissolved in 10 mL of distilled water with continuous stirring for 30 minutes. Additionally, a cross-linker solution of MBA was prepared by dissolving 0.05 g in 2 mL of distilled water. Then, a solution of potassium persulfate (KPS) was prepared by dissolving 0.05 g in 2 mL of distilled water with continuous stirring. Nitrogen gas was then injected for a minute, after which the prepared solution was transferred to test tubes and then to a water bath at 70°C for 2 hours to complete the reaction. The nanocomposite was then cut, washed with distilled water, and dried in an electric oven at a temperature of 70°C, as shown in Fig.1.
CS-g-P(AA)/Kaolin nanocomposite characterization
Fourier transform infrared (FTIR) spectroscopy
In attenuated reflection setting, the synthesized CS-g-P(AA)/Kaolin hydrogels’ chemical structures were checked out making use of a Range GX FTIR System (Perkin-Elmer, United States). The FTIR ranges, covering wavenumbers from 400 to 4000 cm-1, were acquired from 64 scans at a resolution of 2 cm-1.
Scanning electron microscope (SEM)
The JEOL JSM-6510LV SEM from Japan was utilized to catch the cross-sectional shape of the manufactured hydrogels. Before the SEM evaluation, the hydrogels were dried out using a lyophilizer under vacuum conditions. After drying, they were coated with platinum. The ImageJ software application was utilized to identify the ordinary sizes of pores in each group of hydrogels by analyzing 100 pores from an SEM image.
Adsorption Isotherm
In this procedure, 10 mL solutions of MG with concentrations ranging from 50 to 500 ppm were introduced into stoppered flasks containing 0.05 g of chaff. These flasks were then agitated in a thermostatically controlled water bath at a speed of 120 rpm until equilibrium was reached, which was 150 minutes for MG. These durations were sufficient to allow the adsorption process to reach equilibrium in case. Following the lapse of the equilibrium time, the suspensions were centrifuged at 6000 rpm for 20 minutes. The resultant clear supernatants were then analyzed for dye content, after suitable dilution, using a UV-visble Spectrophotometer (FAAS). Equilibrium concentrations were determined by comparing the experimental data with a pre-established calibration curve.
The equation 1 for determining the removal capacity (qe) at equilibrium is given by:
Here, qe (expressed in mg/g) represents the amount of MG adsorbed per unit mass of the adsorbent at equilibrium. Co and Ce are the initial and equilibrium concentrations of MG in the solution (in mg/L), respectively. Vsol is the volume of the solution (in Liters), and m is the mass of the adsorbent used (in grams). In this equation (2), %E represents the efficiency of adsorption in percentage. These equations are fundamental in evaluating the effectiveness of the adsorbent in removing specific dye from a solution, providing a quantitative measure of the adsorption process.
Effect of Temperature
For the thermodynamic aspect of adsorption, the experiment was replicated at different temperatures (25°C, 40°C, and 55°C) to evaluate the fundamental thermodynamic functions. This approach helps in understanding how temperature variations impact the adsorption process and allows for the calculation of thermodynamic parameters such as enthalpy, entropy, and Gibbs free energy changes.
RESULTS AND DISCUSSION
Characterization
The FTIR spectra of MG-loaded adsorbent CS-g-P(AA)/Kaolin were analyzed, as shown in Fig. 2. Compared to the surface spectra of CS-g-P(AA)/KAOLIN, a notable decrease in the broad absorption bands at 3300 and 3450 cm-1 was observed. This change in intensities, particularly in the amino and hydroxyl groups’ bands, suggests their involvement in dye sorption. This coincides with the formation of hydrogen bonds between the dye and the adsorbent surface, resulting in the disappearance of certain bands previously present on the surface within the confined region of 1600-1000 cm-1 [24,25].
The morphology of CS-g-P(AA)/Kaolin before adsorption was examined using FE-SEM, depicted in Fig. 3. The FE-SEM analysis revealed that CS-g-P(AA)/Kaolin tends to form multilayer agglomerates. Post-adsorption, the FE-SEM images showed a roughened CS-g-P(AA)/Kaolin surface with MG evenly dispersed as bright dots, indicating the presence of both CS-g-P(AA)/Kaolin and MG [26,27].
Effect of Adsorbent Weight on the Adsorption process
10mL of a MG solution at a fixed concentration of 100 ppm were added to the aforementioned weights of the nanocomposite at a temperature of 20°C. The study results, as illustrated in Fig. 4, indicate that an increase in the weight of the adsorbing surface leads to an increase in the adsorption amount. This is attributed to the initial requirement of equilibrium between the adsorbate and adsorbent, ensuring all the active sites of the adsorbent are occupied, which stabilizes the adsorption process on the surface [27]. The maximum adsorption quantity is achieved at 0.05 gm, representing the adsorbent’s saturation stage. However, further increase in the adsorbent’s weight may result in an unstable dispersion of the large nanocomposite surface compared to the adsorbate (dye) quantity. Consequently, the solute’s energy overpowers the adsorption energy on the surface, leading to a decrease in the adsorbed quantity on the nanocomposite surface [28].
Adsorption isotherms
The research revealed a stronger correlation with Freundlich isotherms relative to Temkin and Langmuir isotherms, as indicated by the correlation coefficient values (R²= 0.9448 for Freundlich). This finding was distinctly illustrated in Fig. 5. Additionally, Table 1 provides the correlation coefficients and constants for each isotherm at a temperature of 25°C.
Effect of Temperature on the Adsorption Process
Temperature significantly influences the adsorption process, as changes in temperature affect the adsorptive capacity of the surface for the dye from its aqueous solution. By studying adsorption at various temperatures (10-25°C), the thermodynamic functions of the adsorption process can be understood. The results indicated that the amount of MG adsorbed on the nanocomposite surface increases with an increase in temperature, suggesting that the adsorption process is endothermic [29,30], as illustrated in Fig. 6.
This increase in adsorption with increasing temperature could be absorption into the surface will occur due to the increase in kinetic energy of the dye particles. This increase in temperature leads to a rise in the system’s entropy (ΔS), enhancing the randomness of the adsorbed dye molecules on the adsorbent surface. Consequently, the attraction forces between the dye molecules and the available active sites for adsorption on the nanocomposite surface stronger. The enthalpy change (ΔH) value is instrumental in discerning the interaction forces between the adsorbed dye molecules and the adsorbent surface. For ascertaining ΔH, a plot of the natural logarithm of the equilibrium constant (lnK) against the reciprocal of absolute temperature (1/T) is constructed, yielding a linear relationship. The slope of this graph, equating to (-ΔH/R) and intercept equating to (ΔS/R) facilitates the determination of the enthalpy value associated with the adsorption of MG on the adsorbent polymeric nanocomposite surface [31,32]. This is documented in Table 2 and illustrated in Fig. 7.
The thermodynamic functions presented in the table indicate an endothermic adsorption process, as evidenced by the positive enthalpy change (ΔH). This endothermic nature suggests the likelihood of physical bonding, particularly if ΔH is less than 40 KJ/mol. Moreover, the positive entropy change (ΔS) signifies a higher degree of disorder within the system, often associated with restricted molecular movement. Furthermore, the positive Gibbs free energy (ΔG) reinforces this understanding, confirming that the adsorption process is non-spontaneous [33,34].
CONCLUSION
The study presents a comprehensive analysis of the adsorption of MG dye using the CS-g-P(AA)/Kaolin adsorbent. FTIR and FE-SEM results demonstrate significant functional group activity and morphological changes in the adsorbent post-adsorption, indicating effective dye removal. Adsorption increases with the adsorbent weight, peaking at 0.05 gm, beyond which a decrease in efficiency is observed due to adsorbent surface saturation. The adsorption process aligns closely with Freundlich isotherms, suggesting a multilayer adsorption pattern. Additionally, the adsorption is endothermic, with increasing temperatures enhancing the process. This is supported by positive enthalpy and entropy changes, highlighting the physical nature of the adsorption. The study also underscores the importance of adsorbent-adsorbate equilibrium in optimizing the adsorption process, as well as the role of surface area and active sites in adsorbent effectiveness.
CONFLICT OF INTEREST
The authors declare that there is no conflict of interests regarding the publication of this manuscript.
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