Equilibrium, Kinetic, and Thermodynamic Study of The Adsorption of Cu(II) From Aqueous Solution Using Activated Carbon Derived From Acacia

The mechanism of adsorption behavior of thermally activated carbon prepared from Acacia (AAC) for copper ions from aqueous solutions has been investigated at optimum conditions of removal in a batch system. The experimental data were analyzed by the Langmuir, Freundlich, Timken, and Dubinin- Zaverina-Radushkevich adsorption isotherm models of adsorption. The characteristic parameters for each isotherm and related coefficients of determination have been determined. Thermodynamic parameters have also been evaluated. The kinetics of the sorption were analyzed using the Simple First Order, pseudo-first-order, pseudo-second-order, and Intra-Particle Diffusion kinetic models. Kinetic parameters, rate constants, equilibrium sorption capacities, and related coefficient of determination for each kinetic model were calculated and discussed. It was shown that the adsorption of copper could be described by the pseudo-second-order model, and it has been found that the adsorption process was feasible, spontaneous, and endothermic, suggesting that the adsorption process is presumably chemisorption. The AAC investigated in this study showed good potential for the removal of copper from aqueous solutions. So, the present study shows the feasibility of the practical use of AAC as a low-cost, and natural material adsorbent for the effective removal of Cu(II) ions from aqueous solutions as an alternative to existing commercial adsorbents.