Sorption behavior of cesium and strontium ions on mixtures of clay sorbents.

Yanagi, Tadashi; Watanabe, Mieko; Yamamoto, Koichiro

doi:10.3327/jnst.26.861

Cited by 10 publications

(4 citation statements)

References 1 publication

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“…The increase of Sr sorption with increasing pH was not simple, showing moderate increase in acidic and neutral pH regions and larger increase in alkaline pH region, which suggested two sorption mechanisms or two sorption sites. Similar tendency of Sr sorption was observed in the literature [6,12]. Cation-exchange reactions have been considered a predominant mode of Sr sorption onto bentonite because of experimental data showing the reversibility of sorption, competing sorption with other cations, etc.…”

Section: Resultssupporting

confidence: 76%

Sorption and diffusion behaviours of strontium in sodium-type bentonite bed

2006

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Sorption and diffusion of Sr were examined using a typical Japanese bentonite. The experimental results showed that Sr sorption on the bentonite had linear relationship between the equilibrium Sr concentration and Sr sorption amount, i.e., Henry's type of sorption, in wide initial Sr concentration from 1.1 × 10 -9 to 1.1 × 10 -4 mol L -1 at pH 10. The Sr sorption also indicated pH dependence in pH range between 2 and 12. Sorption modelling calculation indicated that cationexchange reactions contributed to Sr sorption in the pH range studied and a surface complexation reaction was predominant above pH 8. Diffusion of Sr in loosely compacted bentonite bed was described by pore and surface diffusion and surface complexation of Sr. Chemical-transport calculations reproduce the diffusion data at pH 5 using the cation-exchange parameters obtained in the analysis of the batch sorption experiment.

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Section: Resultssupporting

confidence: 76%

Sorption and diffusion behaviours of strontium in sodium-type bentonite bed

2006

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“…Sr(II) sorption on various minerals has been widely studied due to the abundant presence of Sr(II) in nuclear waste repositories. Most studies concluded that Sr-(II) is partitioned at solid/water interfaces via ion-exchange reactions (16)(17)(18), and the adsorbed Sr(II) is characterized as a weak, outer-sphere complex (19). XAS studies of Sr(II) on silica surfaces have also been conducted to probe the coordination structure of adsorbed Sr(II) (20).…”

Section: Resultsmentioning

confidence: 99%

Bridging the Gap between Macroscopic and Spectroscopic Studies of Metal Ion Sorption at the Oxide/Water Interface: Sr(II), Co(II), and Pb(II) Sorption to Quartz

Chen

Coleman

Katz

2005

Environ. Sci. Technol.

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Metal sorption mechanisms were investigated for strontium, cobalt, and lead using sodium chloride, sodium nitrate, and sodium perchlorate as background electrolytes and quartz as the adsorbent. Spectroscopic analyses of concentrated sorption samples were evaluated for their ability to provide insight into the controlling sorption process for more dilute systems. For strontium, outersphere complexes identified using X-ray absorption spectroscopy (XAS) of concentrated samples were consistent with macroscopic sorption data collected in more dilute systems. XAS results indicated that cobalt formed a new solid phase upon sorption to silica. Macroscopic studies of cobalt sorption supported the spectroscopic data for total cobalt concentrations of 10 -5 M, regardless of the background electrolyte composition or concentration. At a lower total cobalt concentration (10 -7 M), adsorption appeared to be the prevailing mechanism of cobalt removal. Spectroscopic results suggested that lead adsorbed as an inner-sphere complex on silica. The decrease of lead removal with increasing chloride concentration was attributed to competition with aqueous lead-chloride complexes, based on thermodynamic calculations.

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“…These radionuclides comprise an infinitesimally small volume or mass fraction of the wastes, and their separation from nontoxic salts (e.g., NaOH, NaNO 3 ) will dramatically ease the handling of the wastes. Materials that have been used for the separation of cesium include clays ( , ), zeolites ( − ), phosphotungstates (), silicotitanates (), Al 2 O 3 (), and various hexacyanoferrates (HCFs). Of those, Cu, Co, and Ni HCFs have been most widely employed ( − ).…”

Section: Introductionmentioning

confidence: 99%

Separation of Cesium from High Ionic Strength Solutions Using a Cobalt Hexacyanoferrate-Modified Graphite Electrode

Green-Pedersen

Korshin

1999

Environ. Sci. Technol.

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Graphite electrodes modified with cobalt hexacyanoferrate (CoHCF) were used to investigate the feasibility of electrochemically (EC) controlled ion exchange for separation and transfer of Cs from high sodium wastes. A thin layer of CoHCF was formed on the graphite substrate. The surface CoHCF phase was highly selective to Cs + in the presence of overwhelmingly higher concentrations of Na + and K + . Cs + was incorporated into the electrode at 0 V and expelled at +1.0 V. X-ray photoelectron spectroscopy (XPS) confirmed the EC control of the cesium flux and its association with the Fe oxidation state in the CoHCF phase. There was a good correlation between the electric charge passed through the electrode and the amount of Cs incorporated or released. The maximum share of charge associated with Cs + incorporation is ca. 40%. The performance of the electrode was stable in the range of pH from 1 to 11, but it deteriorated at pH > 11. The CoHCF electrodes performed well in multicycle processes of Cs separation and transfer, but the impact of non-EC-controlled cation exchange and carryover by the porous substrate were also significant.

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Sorption behavior of cesium and strontium ions on mixtures of clay sorbents.

Cited by 10 publications

References 1 publication

Sorption and diffusion behaviours of strontium in sodium-type bentonite bed

Sorption and diffusion behaviours of strontium in sodium-type bentonite bed

Bridging the Gap between Macroscopic and Spectroscopic Studies of Metal Ion Sorption at the Oxide/Water Interface: Sr(II), Co(II), and Pb(II) Sorption to Quartz

Separation of Cesium from High Ionic Strength Solutions Using a Cobalt Hexacyanoferrate-Modified Graphite Electrode

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