Oxidation Of Tartaric Acid Research Articles

One-step three-electron oxidation of tartaric and glyoxylic acids by chromium(VI) in the absence and presence of manganese(II)

Kinetics of the initial stages of oxidation of tartaric acid (TA) in the absence and presence of manganese(II) ions have been studied spectrophotometrically. The rate of the induction was slow and then gradually increased with increasing [TA] and/or [HClO4]. The reaction followed third-order kinetics; first-order with respect to each of [TA], [HClO4] and [CrVI]. The kinetic and manganese(II) effect studies are consistent with a one-step three-electron mechanism (CrVI → CrIII without passing through CrIV as an intermediate) in which a termolecular complex is formed between TA, MnII and HCrO4−. In order to obtain further insight, oxidation of glyoxylic acid (GA), an oxidation product of TA, was also studied under the similar conditions. Details of the process are discussed.

Kinetic and mechanistic aspects for the tartaric acid oxidation by vanadium(V) in sulfuric acid medium

Tartaric acid oxidation by vanadium(V) in sulfuric acid medium was investigated spectrophotometrically at 760 nm and 30°C by appearance of the vanadium(IV), as vanadyl. The reaction rate was determined under pseudo-first-order conditions with an excess of hydroxyacid over the oxidant concentration. The oxidation showed a first-order dependence with respect to vanadium(V) concentration and fractional orders with respect to tartaric acid and sulfuric acid concentrations, with no control and with constant ionic strength. The reaction rate is enhanced by an increase of ionic strength, and slightly reduced by a decrease of the dielectric constant of the medium. The activation parameters were calculated based on the rate constants determined in the 293 to 313 K interval. The proposed oxidation mechanisms and the derived rate laws are consistent with the experimental rate laws. © 1998 John Wiley & Sons, Inc. Int J Chem Kinet: 30: 55–61, 1998.

Effect of acrylamide concentration on the kinetics of oxidation of tartaric acid by cerium(IV) in sulfuric-perchloric acid media

The kinetics of oxidation of tartaric acid by Ce(IV) in the absence and presence of acrylamide has been investigated spectrophotometrically in aqueous H2SO4−HClO4 media at a constant ionic strength 2.0M and 25°C. Oxidation of tartaric acid in both cases was first order with respect to Ce(IV). Kinetic data showed that the reaction involves the formation of an unstable complex and an intermediate free radical. The activation parameters were calculated to be E a =91.3±0.4 kJ-mol−1, ΔSΔ=20.2±1.0 J-mol−1-K−1, ΔHΔ=88.8±0.4 kJ-mol−1. A polymerization mechanism is discussed.

Kinetics and mechanisms of oxidations by metal ions. Part VI. Oxidation of α-hydroxy acids by cerium(IV) in aqueous nitric acid

The kinetics of oxidation of glycolic, malic, tartaric, and citric acids by cerium(IV) ammonium nitrate were investigated in 0.006 mol dm−3 nitric acid. The reaction was catalysed by H+ in the range 0.006–0.016 mol dm−3 at constant [Formula: see text] (0.02 mol dm−3). The pseudo first-order rate constant kobs was independent of [CeIII] (0.0004–0.002 mol dm−3). The proposed mechanism is based on the assumption that the formation of the precursor Ce(IV) – α-hydroxy acid complex precedes its rate controlling disproportionation, which is assisted by a proton, possibly due to the formation of the activated state [H+—CeIV – HA]≠ (where CeIV is the reactive cerium(IV) species and HA is the α-hydroxy acid). The free radical R1R2ĊOH produced in the rate controlling step further reacts with a number of Ce(IV) molecules in the fast step to yield the final oxidation product. The activation parameters for the rate controlling step could be evaluated only in the oxidation of tartaric acid.

Kinetics and Mechanism of Acid Bromate Oxidation of Tartaric Acid

Kinetics and Mechanism of Acid Bromate Oxidation of Tartaric Acid

Kinetics and mechanism of oxidation of tartaric acid by bromate ions and an heterogeneous oscillation reaction of tartaric acid

The kinetics and mechanism of oxidation of tartaric acid by bromate ions in sulphuric acid solutions have been studied. As the relation between the concentration of H3O+ ions and the reaction rate constant indicates, the species involved in the reaction are protonized bromate ions (HBrO3) and tartaric acid molecules. Their interaction is of dipole-dipole nature, as borne out by measurements of the rate constant in dependence on the dielectric constant and on the ionic strength. The activation parameters and the stoichiometry of the reaction have been evaluated. An oscilation behaviour is observed in the presence of a Mn(II) catalyst if bromine is removed from the system constantly. The concentration ranges in which the oscillations occur have been established. Bromine is shown to play a major part in the heterogeneous oscillation system.

Kinetic Study of Oxidation of Tartaric Acid by Acid Permanganate

Kinetic Study of Oxidation of Tartaric Acid by Acid Permanganate

Kinetic Study of Oxidation of Tartaric Acid by Acid Permanganate

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A Versatile kinetics demonstration

The oxidation of tartaric acid by hydrogen peroxide in the presence of cobalt chloride catalyst provides a reaction that can be used in a variety of kinetics demonstrations.

Investigation on the Kinetics and Mechanism of the Reaction Between Potassium Peroxodisulphate and Tartaric Acid

AbstractThe kinetics of tartaric acid oxidation by peroxodisulphate ion has been studied to elucidate the mechanism of oxidation. Uncommon to many peroxodisulphate reactions it shows a variation in order. It is found to progress bimolecularly in the beginning and unimolecularly till completion. H+ ion and O2 gas accelerate the reaction. Some observations with change of surface revealed that area/volume ratio Influences the rate of reaction. In order to explain the observed data the chain mechanism has been proposed and rate expressions have been derived to explain the change of order from two to one.

Kinetic Studies of the Oxidation of Tartaric Acid by Ammoniacal Silver Nitrate

Kinetic Studies of the Oxidation of Tartaric Acid by Ammoniacal Silver Nitrate

Identification of the tartaric acid oxidation products in the tartaric acid accelerated reaction between uranium (IV) and thallium (III)

When tartaric acid is oxidized by thallium (III) in the presence of uranium (IV), it is converted to glyoxal (C 2H 2O 2) and carbon dioxide. If sufficient thallium (III) is present all of the tartaric acid is oxidized. In the absence of uranium (IV) tartaric acid is oxidized only very slowly, but in the presence of uranium (IV) its oxidation rate is comparable to the rate of oxidation of uranium (IV) itself. It appears that U(IV)-tartaric acid complexes form which facilitate both the oxidation of tartaric acid and uranium (IV).

Kinetics of the Oxidation of Tartaric Acid by Vanadium (V)

Kinetics of the Oxidation of Tartaric Acid by Vanadium (V)

Kinetics of Oxidation of Tartaric Acid by Ceric Sulphats in Aqueous Sulphuric Acid

Kinetics of Oxidation of Tartaric Acid by Ceric Sulphats in Aqueous Sulphuric Acid

Kinetics of Oxidation of Tartaric Acid by Ceric Sulphats in Aqueous Sulphuric Acid

Kinetics of Oxidation of Tartaric Acid by Ceric Sulphats in Aqueous Sulphuric Acid

Kinetics of the Oxidation of Tartaric Acid by Chromic Acid

Kinetics of the Oxidation of Tartaric Acid by Chromic Acid

Kinetics of the Oxidation of Tartaric Acid by Ce(IV) Sulphate

Kinetics of the Oxidation of Tartaric Acid by Ce(IV) Sulphate

Kinetics of the Oxidation of Tartaric Acid by Chromic Acid

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Dosage de l'acide tartrique et des tartrates par le tétracétate de plomb

It was found, that in a medium of 80% acetic acid, in the presence of potassium acetate the oxidation of tartaric acid by lead(IV)-acetate takes place quantitatively. In the indirect determination of tartaric acid and tartrates, an excess of lead(IV)-acetate is used, allowing 30 min for the reaction to take place. The remaining reagent is then determined by potentiometric titration with a volumetric hydroquinone solution.

CCLXXXVIII.—The oxidation of tartaric acid by solutions of silver salts

CCLXXXVIII.—The oxidation of tartaric acid by solutions of silver salts