The differential titration of sulfite and thiosulfate ions with mercuric chloride (HgCl
2) solution has been studied by short-circuited amperometry using a rotating platinum wire electrode (1000 rpm) as the indicator and SCE as the reference electrode.
Sulfite and thiosulfate ions, respectively, from Hg-(SO
3)
22- and Hg(S
2O
3)
22- quantitatively at pH 78. But, in the presence of large excess of formaldehyde to sulfite ion, Hg(SO
3)
22- is not formed. On the basis of these phenomena, sulfite or thiosulfate ion in their mixture is determined differentially. To prevent air oxidation of sulfite ion, glycerin is added to
ca. 5 (v/v) % in the sodium sulfite solution. The recommended procedure is as follows: To a sample solution,
ca. 10 ml of 1 M KNO
3 and
ca. 10 ml of 0.2% gelatin are added. The solution is adjusted to pH 78 with the diluted perchloric acid or sodium hydroxide. The solution is diluted to 100 ml with deaerated water. The sample solution is titrated amperometrically with (0.050.0005) M HgCl
2 standard solution by Pt rotating electrode (1000 rpm) at
ca. 20°C. The concentration of sum of sulfite and thiosulfate ions is found by this titration.
The second sample solution, to which 2 ml of 1 M formaldehyde is added, is titrated with HgCl
2 standard solution, then the concentration of thiosulfate ion is found. The sulfite ion can be determined from the difference of the two concentrations. The whole titration procedure requires about 10 minutes. Each ion of sulfite and thiosulfate can be determined at the concentration range of
ca. 5×10
-5 M10
-2M and the relative errors are
ca. ±3%, even in the case of lower concentration (5×10
-5 M). Sulfate, carbonate, chloride, azide, nitrite and chlorate ions in the concentration ranges up to 100 times of the mixture of sulfite and thiosulfate ions do not interfere the determination. It is an advantage of this method that the titration is applicable to the solution containing oxidation reduction substances such as nitrite and chlorate ions.
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