Sn Iv and Hg H can be titrated amperometrically with tetraphenylarsonium chloride using the dropping mercury electrode as the indicator electrode. Procedures are given and the limitations of the method are discussed.The use of tetraphenylarsonium chloride (denoted as TPAC) as a reagent in the indirect determination of mercuric, stannic, cadmium, and zinc ions has been described by Willard and Smith (1). These determinations involve formation of insoluble tetraphenylarsonium salts of the chloro-complexes of the metal ions and subsequent determination of the excess TPAC by potentiometric titration with iodine (2).Certain features of the reactions of TPAC with stannic and mercuric chlorocomplexes suggest their use in amperometric titrations. First, attainment of equilibrium is rapid. Second, the precipitates have a low solubility. Third, both mercuric and stannie ions yield suitable diffusion currents.The amperometric titration permits a direct determination of the metal ions and represents a considerable saving in time over the indirect method.
DETERMINATION OF STANNIC [ONThis determination of tin is based on the reactionCurrent before the end point is derived from the stannic-stannous wave, which is catalyzed by TPAC (3). In 3N hydrochloric acid, the current may be measured at -0.3 volt vs. S.C.E.Because tin must be in the form of the hexachlorostannate complex to react with tetraphenylarsonium ion, a certain lower limit of chloride concentration is indicated for the titration. Furthermore, the acidity must be high enough to prevent hydrolysis of the hexachloro-complex. If both the acidity and chloride concentrations are less than 2N, quantitative precipitation does not occur and the attainment of equilibrium is slow. If the concentration of chloride is 2-4M, good precipitation lines and precision are 1 Manuscript received December 14, 1950. 231 obtained even when the concentration of hydrogen ion is as low as IN. Above 4M chloride, the points on the precipitation line are not linearly related; in particular, currents obtained in the beginning of the precipitation are less than theoretical, but closer to the end point the current approaches the expected values. For best results, the chloride concentration should be maintained at approximately 3-4M.The effects of variation in hydrogen-ion concentration are not as marked as the effects associated with chloride variations. In mixtures containing 2-3M chloride which are 1N in acid the results are slightly higher and the titration curves are not as well defined as in 2N acid. In 5N acid the results tend to be a little low. The best range of acidity is between two and four normal. This acidity can be lowered to 1N without seriously affecting the results, at a total chloride concentration of 2-3N.
Procedure