JAST
2012 March;3(1):104-112.
Published online 2012 January 26.
doi:http://dx.doi.org/10.5355/JAST.2012.104
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| Copyright ⓒ 2010 Journal of Analytical Science & Technology |
| Removal of Pb2+ ions in aqueous phase by a sodic Montmorillonite |
| Zoubida Lounis1, Smail Saddouki2, Fatiha Djafri3 |
1Institut de Maintenance et Sécurité Industrielle, Université d’Oran BP1524 El Manouer, 31000 Oran, Algérie
2Université Stambouli Moustapha, Mascara, Algérie
3Laboratoire de Chimie des Matériaux, Université d’Oran BP1524 El Manouer |
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Corresponding Author:
Zoubida Lounis ,Tel: +213556424884, Email: lounis_amira@yahoo.fr |
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ABSTRACT |
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| The sorption of Pb2+ ions in aqueous phase was carried out using sodium bentonite. The influence of the temperature and the pH on the capacity of the sorption and the percentage of the uptake of Pb2+ 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 Pb2+ 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 Pb2+ 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 |
| Keywords: pollution water, sorption, heavy metals, smectite, lead ions, Montmorillonite |
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FIGURES |
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Fig.1
XRD spectra of Algerian natural clay (Mont-morillonite) (Mt) (a:clay; f:feldspaths; q:quartz) |
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Fig.2
XRD spectra of purified Montmorillonite (* m) |
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Fig.3
SEM image of Algerian natural clays (Montmorillonite) (Mt) Amplifying: a=x6000; b=x4000; c=x4300; d=x10000; e= x33000; f=x3700 |
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Fig.4
Variation of % of removal rate of Pb2+ ions with pHi |
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Fig.5
Variation of the adsorption capacity (qe) of Pb2+ ions with pHi |
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Fig.6
Variation of % removal rate of the Pb2+ ions with time |
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Fig.7
Variation of the adsorption capacity of Pb2+ ions with time |
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Fig.8
Freundlish isotherm sorption of Pb2+ (a= 30 °C, b= 40 °C and c= 50 °C) |
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Fig.9
Langmuir isotherm sorption of Pb2+ (a= 30 °C, b= 40 °C and c= 50 °C) |
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Fig.10
Lead (Pb2+)adsorption isotherm (T= 30 °C) |
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Fig.11
Lead (Pb2+) adsorption isotherm (T= 40 °C) |
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Fig.12
Lead (Pb2+) adsorption isotherm (T= 50°C) |
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Fig.13
Effect of temperature on the adsorption of the Pb2+ (Ci = 30 mg/l) on Na-Mt |
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Fig.14
Effect of temperature on the adsorption of the Pb2+ (Ci = 40 mg/l) on Na-Mt) |
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Fig.15
Effect of temperature on the adsorption of the Pb2+ (Ci = 50 mg/l) on Na-Mt |
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TABLES |
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Table.1
Langmuir and Freundlich sorption parameters. |
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Table.2
Values of thermodynamic parameters of adsorption of Pb2+ ions on the Na-Mt |
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