“…The presence of carboxylate groups, main chelating groups of metallic species, can be evidenced by the band near 1620 cm À1 with observed stretching of CH bonds near to 2925 cm À1 [24].…”
Section: Infrared Spectroscopymentioning
confidence: 97%
“…Therefore, 50 mL aliquots of the solutions of prepared metals at different pH levels were added to falcon-type tubes containing 100.00 mg of humin samples. The tubes were kept in a mechanical shaker at a temperature of 25 AE 3 C. After reaching the contact times, the solutions were filtered using a system equipped with membrane filters with a pore size of 0.45 mm, and the potentially toxic metals were determined by inductively coupled argon plasma atomic emission spectroscopy (ICP-OES) [24]. The Cu 2+ , Cr 3+ , Pb 2+ , Cd 2+ and Ni 2+ concentrations adsorbed in the humin were then calculated based on the difference between the initial and final concentrations of the solution, using Eq.…”
Section: Studies Of the Adsorption Between Ptm And Humin: Ph Effectmentioning
“…The presence of carboxylate groups, main chelating groups of metallic species, can be evidenced by the band near 1620 cm À1 with observed stretching of CH bonds near to 2925 cm À1 [24].…”
Section: Infrared Spectroscopymentioning
confidence: 97%
“…Therefore, 50 mL aliquots of the solutions of prepared metals at different pH levels were added to falcon-type tubes containing 100.00 mg of humin samples. The tubes were kept in a mechanical shaker at a temperature of 25 AE 3 C. After reaching the contact times, the solutions were filtered using a system equipped with membrane filters with a pore size of 0.45 mm, and the potentially toxic metals were determined by inductively coupled argon plasma atomic emission spectroscopy (ICP-OES) [24]. The Cu 2+ , Cr 3+ , Pb 2+ , Cd 2+ and Ni 2+ concentrations adsorbed in the humin were then calculated based on the difference between the initial and final concentrations of the solution, using Eq.…”
Section: Studies Of the Adsorption Between Ptm And Humin: Ph Effectmentioning
“…However, since the y-intercept (C i ) is not equal to zero, it implies that this mechanism does not solely limit the overall adsorption process. The rate-limiting step maybe a complex combination of chemisorption and intraparticle transport [65].…”
“…However, the y-intercept C i is not equal to zero, which implies that this mechanism does not solely limit the overall adsorption process. The rate-limiting step may be a complex combination of chemisorption and intraparticle transport [17].…”
The current study focused on the equilibrium, kinetics, and thermodynamics of Basic Fuchsin dye adsorption from aqueous solution using mussel shells as an adsorbent. Optimum adsorption conditions were identified by varying the solution pH, adsorbent dose, initial dye concentration, and contact time. Equilibrium data were fitted by the Langmuir, Freundlich and Dubinin-Radushkevich isotherm models, and a pseudo-second-order model best described the kinetics. Thermodynamic data showed that Basic Fuchsin dye adsorption onto mussel shells was a feasible, spontaneous and endothermic process. Statistical analysis was performed using the Chi-square (χ 2) and mean square error (MSE) test methods to evaluate the best fit of the model to the experimental data. The adsorption of Basic Fuchsin by calcined mussel shells indicates their potential application as an adsorbent for the removal of dyes from aqueous solutions.
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