Abstract
The sorption of Pb 2+ ions in aqueous phase was carried out using sodium Montmorillonite. The influence of the temperature and the pH on the capacity of the sorption and the percentage of the uptake of Pb 2+ ions by sodium Montmorillonite were studied. The sorption data were analysed in terms of the Freundlich and Langmuir isotherm models and the data fit the Langmuir sorption isotherm model well. Whereas, the thermodynamic parameters( the heat of adsorption Δ H°, the entropy Δ S° and the free energy ΔG°) showed that the sorption is a phenomenon of exchange cation between adsorbat /adsorbent The negative value of ΔG° indicates that the sorption of Pb 2+ ions on Na-Mt is spontaneous. The positive value of entropy ΔS° means that the disorder is at the interface solid-solution. The negative value of the heat of sorption ΔH° means that the process of elimination of Pb 2+ ions is exothermic. However, it appears that the affinity sorption of Pb +2 ions on our clay decreases with increasing the temperature as the sorption capacity.
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