Data analysis
The resulting equilibrium data were modeled using Langmuir, Freundlich models. The linearized form of Langmuir equations [6] expressed as Ce/qe=Ce/qm+1/KLqm (2)
Where qe is the equlibrium adsorption capacity of ions on the adsorbent(mg/g) Ce is the equlibrium ions concentration in solution (mg/L), qm is the maximum capacity of the adsorbent (mg/g) and KL ,the Langmuir adsorption constant (L/mg). The linearized form of Freundlich equation is expressed as [6] log qe=log KF + (1/n) log Ce (3) (4)
Where equilibrium capacity (qe) and Ce are defined as above, KF is the Freundlich constant (L/mg) and n is the heterogeneity factor. The qe was increased with increasing concentrations until reaching equilibrium. The adsorption isotherm data for the surfactant were …show more content…
The optimum adsorbent concentration obtained as 0.75 g/L. The fig 6 shows the percentage removal of surfactant with various adsorbent dosage. As the adsorbent dosage increases the efficiency of adsorption also increases, which could be due to availability of more active sites in the adsorbent. A further increase in adsorbent dosage did not show much increase in the removal of surfactant, and it remains constant.
D. Effect of initial SDS concentration
Optimization of initial SDS concentration was done by varying the concentration of SDS as 5, 10, 15, 20, 25 mg/L. The optimum SDS concentration is obtained as 10 mg/L. The fig 7 shows the variation of percentage removal of surfactant with various SDS concentration. The percentage of SDS removal decreases with increase of initial SDS concentration. The reason behind this is the pores for adsorption reduces after a higher values of SDS concentration. When the all the pores of adsorbent was filled further adsorption will not takes place.
E. Langmuir
The resulting equilibrium data were modeled using Langmuir, Freundlich models. The linearized form of Langmuir equations [6] expressed as Ce/qe=Ce/qm+1/KLqm (2)
Where qe is the equlibrium adsorption capacity of ions on the adsorbent(mg/g) Ce is the equlibrium ions concentration in solution (mg/L), qm is the maximum capacity of the adsorbent (mg/g) and KL ,the Langmuir adsorption constant (L/mg). The linearized form of Freundlich equation is expressed as [6] log qe=log KF + (1/n) log Ce (3) (4)
Where equilibrium capacity (qe) and Ce are defined as above, KF is the Freundlich constant (L/mg) and n is the heterogeneity factor. The qe was increased with increasing concentrations until reaching equilibrium. The adsorption isotherm data for the surfactant were …show more content…
The optimum adsorbent concentration obtained as 0.75 g/L. The fig 6 shows the percentage removal of surfactant with various adsorbent dosage. As the adsorbent dosage increases the efficiency of adsorption also increases, which could be due to availability of more active sites in the adsorbent. A further increase in adsorbent dosage did not show much increase in the removal of surfactant, and it remains constant.
D. Effect of initial SDS concentration
Optimization of initial SDS concentration was done by varying the concentration of SDS as 5, 10, 15, 20, 25 mg/L. The optimum SDS concentration is obtained as 10 mg/L. The fig 7 shows the variation of percentage removal of surfactant with various SDS concentration. The percentage of SDS removal decreases with increase of initial SDS concentration. The reason behind this is the pores for adsorption reduces after a higher values of SDS concentration. When the all the pores of adsorbent was filled further adsorption will not takes place.
E. Langmuir