An electrolytic process for the production of potassium or sodium bromate using a pure lead peroxide anode has been operated successfully. A concentrated bromate solution was electrolyzed continuously at a cathode of stainless steel with an anodic current density of 20 amp/dm2 at 70°C; current efficiency, about 90%; anode consumption about 50–60 mg/K amp‐hr. Pure crystalline bromate could be obtained by cooling the cell effluent at room temperature.

The anodes used in this study were platinum, gold, palladium, lead dioxide, and graphite. The normal Kolbe process, the formation of ethane (and methane) and carbon dioxide, can be realized at a potential higher than 2.0v (vs. SCE) in both methanol and glacial acetic acid. In methanol, only platinum and gold seem to be suitable for realizing the process. In glacial acetic acid, however, all of the anodes except graphite can be used successfully for the same process. Another process, the formation of methyl acetate, occurs in both solvents at graphite in the potential range 1.4–2.0v. A side reaction observed in methanol at palladium, graphite, and lead dioxide was the formation of formaldehyde (and methyl formate in case of lead dioxide) which occurs at potentials as low as 1.2v.

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A tentative mechanism or hydrocarbon formation is proposed which, by combining the usual mechanism of pinacol and isopropanol formation, will contribute to one clarification of the over-all electrode process of acetone reduction. CH3CH3 CH3 CH3

Current-potential curves of the electrolytic oxidation of chlorate were determined polarographically using a platinum microanode. The nature of the polarogram thus obtained was quite different from that of the usual oxidation-reduction process. Two potential stages were found; the lower one is believed to be the potential of oxygen evolution and the higher one the potential of perchlorate formation. Probably the limiting current for the oxidation of water could also be seen in the polarogram.Electrolysis of chlorate solution at definite anodic potentials corresponding to the higher stage of the polarogram was carried out in order to confirm the results of the polarographic study. From these experiments, it was clear that the first step of perchlorate formation was probably the discharge of chlorate ion at higher potential than that of oxygen evolution.NTRODUCTION"