Adsorption of lead and cadmium ions from aqueous solution to the montmorillonite/water interface

Barbier, F; Duc, G.; Petit‐Ramel, M.

doi:10.1016/s0927-7757(99)00501-4

Cited by 244 publications

(157 citation statements)

References 13 publications

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“…First, we need to obtain the surface population of MG on the PSS before the addition of clay, N(t < 0). The MG concentration before the addition of the clay particles is 10 µM, and the PSS particle density is 3.3 × 10 10 particles/cm 3 . Using the adsorption equilibrium constant, 4.23 × 10 6 M -1 , obtained from the adsorption isotherm of MG on PSS particles, we calculated that N(t < 0) is 1.47 × 10 5 per PSS.…”

Section: Transfer Kinetics Of Mg From Pss To Clay Particlesmentioning

confidence: 99%

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In Situ Studies of Molecular Transfer between Microparticles by Second-Harmonic Generation

2001

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We have demonstrated that second-harmonic generation (SHG) can be used to investigate the in situ transfer of molecules between colloidal microparticles. The transfer kinetics of organic cations, malachite green (MG) initially adsorbed on to spherical polystyrene sulfate (PSS) microparticles, to disk-shaped clay particles in aqueous solution was obtained. The surface population of MG on the PSS particles during the transfer process can be measured in real time. In the present studies, the adsorption free energy and the number of adsorption sites were found from the adsorption isotherm measured by the SHG method (Wang, H.; Yan, E. C. Y.; Liu, Y.; Eisenthal, K. B. J. Phys. Chem. B 1998, 102, 4446). The kinetics of transfer was observed to depend linearly on the particle density of clay. The observed transfer was biexponential with decay times of 17 ( 1 s and 217 ( 4 s for the case of a clay particle density of 3 × 10 9 /cm 3 . This method was further applied to study the transfer of MG between PSS microparticles. At a PSS density of 4 × 10 8 /cm 3 , the decay time was 40 s. Because of the coherent nature of the SHG signal, the transfer kinetics can be obtained in situ by the SHG method. A kinetic model is used to describe the transfer process from which the desorption and adsorption rate constants of MG from and onto PSS particles were obtained.

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Section: Transfer Kinetics Of Mg From Pss To Clay Particlesmentioning

confidence: 99%

“…A 1.5 mL of plain PSS particles is injected to a 1.5 mL MG-PSS solution. The diameter of the PSS particles is 1.0 µ, and the particle density is 4 × 10 8 /cm 3 . The MG total concentration is 0.06 µM at t g 0.…”

Section: Transfer Kinetics Of Mg Between Pss Particlesmentioning

confidence: 99%

In Situ Studies of Molecular Transfer between Microparticles by Second-Harmonic Generation

2001

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“…Various studies on the adsorptivity of Mont have been reported and studies of adsorption of inorganic ions, such as Pb and Cd, and organic compounds, such as amines and pyrazines, have been conducted (Abollino et al, 2003;Barbier et al, 2000;Ogawa et al, 1989Ogawa et al, , 1991Theng, 1974). Cesium adsorptivity, in particular, has been receiving much attention in recent years.…”

Section: Introductionmentioning

confidence: 99%

Influence of hydrophilicity on adsorption of caffeine onto montmorillonite

Yamamoto

Shiono

Yoshimura

et al. 2017

Adsorption Science & Technology

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Some types of montmorillonite containing different interlayer ions were prepared and the changes in the interlayer spacings, the hydrophilicity, and the characteristics of adsorption of caffeine in solution were observed. Ion exchange treatments were performed using Li, Na, K, Rb, Cs, Mg, Ca, Sr, or Ba. As a result, Li-and Na-type montmorillonite showed larger interlayer distance (1.31-1.53 nm), than K, Rb, and Cs-type montmorillonite (1.23-1.26 nm). In the measurement of hydrophilicity using a pulse NMR-based particle interface analyzer, Li-and Na-type montmorillonite showed higher hydrophilicity. In addition, K Lang , which indicates the interaction with caffeine, was 0.25-0.32 l/mmol, which is lower than K-, Rb-, and Cs-type montmorillonite (1.14-1.60 l/mmol). It is possible that adsorption of water molecules inhibits caffeine from adsorbing. Because of the difficulty of exchange between caffeine and water molecules in interlayer of the Li-and Na-type montmorillonite, the interaction with caffeine decreased. Alternatively, another possibility is that when highly hydrophilic montmorillonite retains many water molecules, the caffeine adsorption sites are blocked by water molecules. In either case, hydrophilicity has a large influence on the adsorption of caffeine onto montmorillonite.

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“…Manning and Goldberg (1997) studied the stability of Arsenic at the clay mineral-water interface. Barbier et al (2000) showed that Pb 2+ and Cd 2+ could be eliminated from aqueous solution efficiently by montmorillonate. However when most of these naturally occurring materials were used no further treatment followed.…”

Section: Introductionmentioning

confidence: 99%

Cobalt and zinc removal from aqueous solution by chemically treated bentonite

et al. 2007

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Natural bentonite was treated by hydrochloric, nitric, and phosphoric acids followed by washing with sodium hydroxide in order to enhance its adsorption capacity. The sample that treated with hydrochloric acid followed by further treatment with NaOH showed the highest cation exchange capacity with a value of 51.20 meq/100 g. The zero-point of charge for this sample was found to be 4.50. Adsorption isotherms for both cobalt and zinc were fitted using Langmuir, Freundlich, and Redlich-Peterson and showed an adsorption capacity of 138.1 mg Co 2+ and 202.6 mg Zn 2+ per gram of treated sample.

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Adsorption of lead and cadmium ions from aqueous solution to the montmorillonite/water interface

Cited by 244 publications

References 13 publications

In Situ Studies of Molecular Transfer between Microparticles by Second-Harmonic Generation

In Situ Studies of Molecular Transfer between Microparticles by Second-Harmonic Generation

Influence of hydrophilicity on adsorption of caffeine onto montmorillonite

Cobalt and zinc removal from aqueous solution by chemically treated bentonite

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