Hydrolysis Constant of Quadrivalent Cerium from Spectrometric Measurements.

Offner, H. G.; Skoog, Douglas A.

doi:10.1021/ac60243a015

Cited by 33 publications

(16 citation statements)

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“…McAuley and Amzad [33] determined K h to be 0.2 ± 0.02 mol dm -3 at 25°C, which is compared well with the values of 0.18 (25°C) and 0.11 (5°C), reported by Offner and Skoog [34]. However, the value of K h determined kinetically in this work is 0.5 mol dm -3 , which agreed well with these values.…”

Section: Discussionsupporting

confidence: 90%

Kinetics and Mechanism of Uncatalyzed and Ag (I) Catalyzed Oxidation of Hydroxylysine by Cerium (IV) in Acid Medium

Mathur¹,

Yadav²,

Devra³

2013

J Phys Chem Biophys

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Section: Discussionsupporting

confidence: 90%

Kinetics and Mechanism of Uncatalyzed and Ag (I) Catalyzed Oxidation of Hydroxylysine by Cerium (IV) in Acid Medium

Mathur¹,

Yadav²,

Devra³

2013

J Phys Chem Biophys

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“…5). Skoog, 1966;Heidt & Smith, 1943;Steemer & Lourier, 1976;Wiberg & Ford, 1968;Danessi, 1967;Noyes & Garner, 1936). Their results can be summarized as follows:…”

Section: Effect Of Equilibration Period On Adsorption and Fixation Ofmentioning

confidence: 99%

The adsorption of quadrivalent cerium by kaolinite

1984

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A B S T R A C T:The adsorption of cerium(IV) by both natural and Na-exchanged kaolinite from aqueous solutions of ceric ammonium nitrate was studied in equilibrium systems. Cerium may be adsorbed either as a monomeric species or as a polymeric hydroxy cation. The species adsorbed depends on the concentration of cerium in the stock solution, the age of this solution prior to the preparation of the equilibrium system and on the equilibration period. Adsorbed cations undergo polymerization on the surface of the kaolinite; the resulting polymeric species forms strong bonds with the clay surface--it is not desorbed by sulphuric acid--and may be considered fixed. Adsorption of cerium reaches a maximum in solutions containing 0.15 M sulphuric acid.Very little is known about the adsorption of lanthanides by clay minerals, although this process seems to be important in the geochemical cycle of these elements. Recently, the adsorption of a few lanthanides by montmorillonite was investigated by Bruque et al. (1980( ) and Miller et al. (1982( , 1983. The present communication deals with the mechanism of adsorption of cerium by kaolinite. EXPERIMENTAL MaterialsNatural kaolinite from Maktesh-Ramon, Israel, was manually ground using an agate pestle and mortar and the fraction passing an 80-mesh (0.177 mm) sieve was used. Na-kaolinite was prepared by dispersing 1 g of natural kaolinite:in 25 ml M NaC1 and, after a 24-h equilibration period, the excess NaCI was removed by repeated washing with distilled water, followed by centrifugation, until no chloride was detected. The exchangeable sodium content of the Na-kaolinite was 0.03 mEq Na/g clay. Equilibrium systemsThree stock solutions containing 0.1, 0.01 and 0.001 M ceric ammonium nitrate were used for the preparation of equilibrium systems. The cerium salt was dissolved either in distilled water or in aqueous solutions of sulphuric acid. Adsorption was carried out in equilibrium systems containing 1 g clay. Various amounts between 0.5 and 10.0 ml of each of the stock solutions of cerium(IV) were added. The suspension was diluted to 12.0 ml by adding distilled water. Some of the series of equilibrium systems were prepared from fresh and others from aged stock solutions. Equilibration periods ranged from 30 min to 1984 The Mineralogical Society

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“…The simplest way to explain this is to assume that the following three hypotheses are valid simultaneously. ( i ) One species alone largely predominates between the monomeric ones (including the unhydrolyzed solvated ion); (ii) One species alone largely predominates between the dimeric ones; (iii) The number y of OHgroups bound to the dimeric (20) in accordance with the above hypothesis, from equations (12), (13), and (19a), equation (21) is obtained where the left-hand…”

Section: Resultsmentioning

confidence: 73%

On the formal potential of the cerium(IV)–cerium(III) couple at –5 °C in 6.5 mol kg^–1HClO₄

Zingales¹

1990

J. Chem. Soc., Dalton Trans.

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Hydrolysis Constant of Quadrivalent Cerium from Spectrometric Measurements.

Cited by 33 publications

References 3 publications

Kinetics and Mechanism of Uncatalyzed and Ag (I) Catalyzed Oxidation of Hydroxylysine by Cerium (IV) in Acid Medium

Kinetics and Mechanism of Uncatalyzed and Ag (I) Catalyzed Oxidation of Hydroxylysine by Cerium (IV) in Acid Medium

The adsorption of quadrivalent cerium by kaolinite

On the formal potential of the cerium(IV)–cerium(III) couple at –5 °C in 6.5 mol kg^–1HClO₄

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Hydrolysis Constant of Quadrivalent Cerium from Spectrometric Measurements.

Cited by 33 publications

References 3 publications

Kinetics and Mechanism of Uncatalyzed and Ag (I) Catalyzed Oxidation of Hydroxylysine by Cerium (IV) in Acid Medium

Kinetics and Mechanism of Uncatalyzed and Ag (I) Catalyzed Oxidation of Hydroxylysine by Cerium (IV) in Acid Medium

The adsorption of quadrivalent cerium by kaolinite

On the formal potential of the cerium(IV)–cerium(III) couple at –5 °C in 6.5 mol kg–1HClO4

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On the formal potential of the cerium(IV)–cerium(III) couple at –5 °C in 6.5 mol kg^–1HClO₄