Oxidation of thiocyanate by alkaline ferricyanide
- 50 Downloads
Oxidation of KSCN by alkaline K3Fe(CN)6 in presence of osmic acid has been studied quantitatively. The reaction proceeds at a measurable rate at ordinary temperature but is accelerated on refluxing the system on a water bath for a short time. The stoichiometry of the redox process suggests the formation of cyanate and sulphate as the products of oxidation. The quantity of thiocyanate is calculated by estimating the ferrocyanide formed and the ferricyanide consumed in terms of Ce(SO4)2 and Na2S2O3 respectively. A kinetic study of the above reaction is under investigation.
KeywordsOxidation Sulphate Physical Chemistry Analytical Chemistry Inorganic Chemistry
Unable to display preview. Download preview PDF.
- 1.Gleu, K.: Z. analyt. Chem. 95, 305 (1933).Google Scholar
- 2.Hess, L.: Arch. Pharmac. Ber. dtsch. pharmaz. Ges. 33, 178 (1923).Google Scholar
- 3.Hofmann, K. A.: Ber. dtsch. chem. Ges. 45, 3329 (1912); c. f. 79, 259 (1930).Google Scholar
- 4.Hofmann, K. A., G. Ehrhart u. G. Schneider: Ber. dtsch. chem. Ges. 46, 1657 (1913).Google Scholar
- 5.Smith, G. F., and C. A. Getz: Ind. Engng. Chem., anal. Edit. 10, 304 (1938).Google Scholar
- 6.Stamm, H.: Angew. Chem. 4, 791 (1934); c. f. 115, 3. (1938/39).Google Scholar
- 7.Vogel, A. I.: A Text-Book of Quantitative Inorganic Analysis, p. 305, London: Longmans, Green and Co., 1951.Google Scholar
- 8.Vogel, A. I.: A Text-Book of Quantitative Inorganic Analysis, p. 356, London: Longmans, Green and Co., 1951.Google Scholar
- 9.Willard, H. H., and Ph. Young: J. Amer. chem. Soc. 50, 1322 (1928); c. f. Z. 79, 360 (1930).Google Scholar