Spectrophotometric Determination of Ruthenium

Larsen, R.P.; Ross, L.E.

doi:10.1021/ac60146a004

Cited by 68 publications

(24 citation statements)

References 5 publications

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“…If now we consider the equilibria (6) and (7) and that RuO 4 (OH) 2− is also a reactive species whose reactivity is similar to that of RuO 4 2− (for simplicity) then Eq. (17) leads to expression (18): (19) From the comparison between both Eqs. (18) and (19) the following relations are obtained:…”

Section: Discussionmentioning

confidence: 99%

“…Stock solutions of sodium ruthenate were prepared by adding a small quantity of the above solution to 25 cm 3 of 1 M NaOH. The purity of the solution of ruthenate ions was assessed by checking that the ratio of the absorbances at 465 and 385 nm was 2.07, corresponding to pure ruthenate [18]. The concentration of ruthenate ions was determined by measuring the absorbance at 465 nm, with its molar extinction coefficient being 1820 M −1 cm −1 [19].…”

Section: Methodsmentioning

confidence: 99%

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Kinetic study of the ruthenium(VI)‐catalyzed oxidation of benzyl alcohol by alkaline hexacyanoferrate(III)

Mucientes¹,

Santiago²,

Almena³

et al. 2002

Int J of Chemical Kinetics

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The kinetics of the Ru(VI)-catalyzed oxidation of benzyl alcohol by hexacyanoferrate(III), in an alkaline medium, has been studied using a spectrophotometric technique. The initial rates method was used for the kinetic analysis. The reaction is first order in [Ru(VI)], while the order changes from one to zero for both hexacyanoferrate(III) and benzyl alcohol upon increasing their concentrations. The rate data suggest a reaction mechanism based on a catalytic cycle in which ruthenate oxidizes the substrate through formation of an intermediate complex. This complex decomposes in a reversible step to produce ruthenium(IV), which is reoxidized by hexacyanoferrate(III) in a slow step. The theoretical rate law obtained is in complete agreement with all the experimental observations.

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Section: Discussionmentioning

confidence: 99%

Section: Methodsmentioning

confidence: 99%

Kinetic study of the ruthenium(VI)‐catalyzed oxidation of benzyl alcohol by alkaline hexacyanoferrate(III)

Mucientes¹,

Santiago²,

Almena³

et al. 2002

Int J of Chemical Kinetics

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“…After aging for 24 h this solution was found, within the limits of experimental detection, to contain only RUO:- (13).…”

Section: Preparation Of Sodium Ruthenate Solutionsmentioning

confidence: 85%

“…The solution of sodium ruthenate was separated and held at room temperature for at least 24 h to insure complete reduction to sodium ruthenate. Spectroscopic analysis of the solution showed that it did not contain detectable amounts of RuO, or RuO, (13).…”

Section: Preparation Of Sodium Ruthenate Solutionsmentioning

confidence: 99%

The oxidation of alcohols by sodium ruthenate

Lee¹,

Congson²,

Spitzer³

et al. 1984

Can. J. Chem.

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The oxidation of 2-propanol and cyclobutanol by stoichiometric amounts of sodium ruthenate has been studied. Contrary to previously published speculations, it has been found that these reactions are not initiated by traces of perruthenate present as a contaminant in the ruthenate solutions. This conclusion is supported by both the kinetic rate law for the reaction and the products obtained from the oxidation of alcohols that would be expected to react differently with [Formula: see text] and [Formula: see text].

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“…Alcohol was distilled before use, Na 2 RuO 4 was prepared by reducing RuO 4 with alkali [5] and its purity was checked by measuring the absorbance ratio at 460 and 385 nm. The ratio 2.07 is diagnostic of pure, ruthenate ion [6]. The concentration of ruthenate ion was calculated by measuring the absorbance of the solution at 460 nm with a Beckmann Spectrophotometer model-26, taking e ¼ 1820 m )1 cm )1 as its molar absorbity coefficient [7].…”

Section: Methodsmentioning

confidence: 99%

Kinetic study of ruthenium(VI) -- catalyzed oxidation of 2-methoxy- ethanol by aqueous alkaline hexacyanoferrate(III)

Veena

Behari

2007

Transition Met Chem

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The kinetics of ruthenium(VI) catalyzed oxidation of 2-methoxyethanol by hexacyanoferrate(III) ion in an aqueous alkaline medium at constant ionic strength shows zero order dependence on hexacyanoferrate(III) and first order dependence on Ru(VI). Dependence of substrate concentration shows a Michaelis -Menten type behaviour. The rate increases with the decrease in alkali concentration. A reaction mechanism involves the formation of an intermediate complex between the substrate and ruthenium(VI). This complex decomposes slowly, producing ruthenium(IV), which is reoxidized by hexacyanoferrate(III) in subsequent steps. The theoretical rate law obtained is in complete agreement with the experimental observations.

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Spectrophotometric Determination of Ruthenium

Cited by 68 publications

References 5 publications

Kinetic study of the ruthenium(VI)‐catalyzed oxidation of benzyl alcohol by alkaline hexacyanoferrate(III)

Kinetic study of the ruthenium(VI)‐catalyzed oxidation of benzyl alcohol by alkaline hexacyanoferrate(III)

The oxidation of alcohols by sodium ruthenate

Kinetic study of ruthenium(VI) -- catalyzed oxidation of 2-methoxy- ethanol by aqueous alkaline hexacyanoferrate(III)

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