Benrath and Ruland1) were the earliest to investigate the oxidizing action of ceric sulfate on several substances, while Lejune3) studied the oxidizability of alcohols, aldehydes and ketones by potassium permanganate and potassium dichromate.Later Willard and Young3) observed the unreactivity of formic and acetic acids towards ceric sulfate and complicated kinetics and stoichiometry in the case of tartaric, malonic and other acids. Ross and Swain4) tried to apply the principle of the concentration cells to kinetic studies on the oxidation of oxalic acid by ceric sulfate. The work of Shorter and Hinshelwood5) concerned the oxidation of acetone6) by ceric sulfate in dilute sulfuric acid. They assumed direct reaction between trisulfato-hydroxy cerate ion {H2CeOH(SO4)3}-with enolic form of acetone. Hargreaves and Sutcliffe7), using rather high concentrations of sulfuric acid, found the rate of oxidation of formaldehyde to depend on the cubic exponent of sulfuric acid concentration, indicating tetra-sulfate ceric acid H4Ce-(SO4)4 to be the reactive species. Dodson and Black8) favored the existence of the trisulfato cerate ions Ce(SO4)32-in soulution and assumed the main reductant to be the bioxalate ion HC2O4-. Shao Minchzhou and Gorbachev') 1) A.

The oxidation of methyl alcohol by ceric perchlorate in perchloric acid solution was studied at 13, 20 and 26°C. The stoichiometry consisted of two cerie ions for the oxidation of one molecule of methanol. While the rate of disappearance of ceric ions directly depended on the concentration of ceric ions, the dependence on methanol concentration was such as to suggest a ‘broken order’: \frac−dCeivdt=\frack(Ceiv)(MeOH)1+k′(MeOH) This rate also depended on the concentration of perchloric acid in such a way that at high acidity it became independent of it. These data were explained on the basis of Duke’s mechanism for 2,3-butane diol-ceric perchlorate reaction, i. e. the oxidation of methanol by ceric ions proceeded via an intermediate complex between one Ce4+ ion and one methanol molecule. The formation of this complex was also proved independently by a spectrophotometric method. The kinetic data were further used to derive the true heat of formation of the methanol-cerate complex and the heat of hydrolysis of the cerie ions in aqueous perchloric acid.

The ultraviolet absorption spectra of hydrogen peroxide have been The at 30" for the dissociation constant of hydrogen determined in aqueous buffers of different pH by spectrophotometry. value (2.63 f 0.12) x peroxide has been derived. AQUEOUS solutions of hydrogen peroxide absorb continuously in the range 3'750-2160 A, the extinction being a maximum at 2150 A but decreasing continuously at longer

The decarboxylation of p-chlorobenzoic acid has been studied in the solvent resorcinol. The activation energy, frequency factor and free energy and entropy of activation have been calculated. It is shown that the reaction follows the SE2 mechanism.