Anode name origin

Faraday, in 1834, was the first to encounter Kolbe-electrolysis, when he studied the electrolysis of an aqueous acetate solution [1], However, it was Kolbe, in 1849, who recognized the reaction and applied it to the synthesis of a number of hydrocarbons [2]. Thereby the name of the reaction originated. Later on Wurtz demonstrated that unsymmetrical coupling products could be prepared by coelectrolysis of two different alkanoates [3]. Difficulties in the coupling of dicarboxylic acids were overcome by Crum-Brown and Walker, when they electrolysed the half esters of the diacids instead [4]. This way a simple route to useful long chain l,n-dicarboxylic acids was developed. In some cases the Kolbe dimerization failed and alkenes, alcohols or esters became the main products. The formation of alcohols by anodic oxidation of carboxylates in water was called the Hofer-Moest reaction [5]. Further applications and limitations were afterwards foimd by Fichter [6]. Weedon extensively applied the Kolbe reaction to the synthesis of rare fatty acids and similar natural products [7]. Later on key features of the mechanism were worked out by Eberson [8] and Utley [9] from the point of view of organic chemists and by Conway [10] from the point of view of a physical chemist. In Germany [11], Russia [12], and Japan [13] Kolbe electrolysis of adipic halfesters has been scaled up to a technical process. 

Tafel s original work in 1905 was concerned with organic reactions and H2 evolution at electrodes, and Eq. (1) was written as an empirical representation of the behavior he first observed. A particular value o b = RT/2F has come to be associated specifically with Tafel s name for the behavior of the cathodic H2 evolution reaction (h.e.r.) when under kinetic control by the recombination of two (adsorbed) H atoms following their discharge from or H2O in a prior step. Such kinetic behavior of the h.e.r. is observed under certain conditions at active Pt electrodes and in anodic CI2 evolution at Pt. (We note here, in parentheses, that an alternative origin for a Tafel slope of RT/2F for the h.e.r. at Pt has been discussed by Breiter and by Schuldiner in terms of a quasiequilibrium diffusion potential for H2 diffusing away from a very active Pt electrode at which H2 supersaturation arises). 

Electrophoresis on paper using a single buffer was applied to bile acid separation by Biserte et al. (41). The buffer system was made up of 30 ml of pyridine and 100 ml of glacial acetic acid in 5 liters of water. The pW was 3.9. In this system, cholic, glycocholic, taurocholic, and taurochenodeoxycholic acids were attracted toward the anode at rates increasing in the order named. Curiously, free deoxycholic acid remained at the origin. The locations of the bile acids on the paper were found by spraying with phosphomolybdic acid. Results with various animal biles were reported. 

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