The arsenic in a 1.223-g sample of a pesticide was converted to H3AsO4 by suitable treatment. The acid was then neutralized, and 40.00 mL 0.07891 M AgNO3 was added to precipitate the arsenic quantitatively as Ag3AsO4. The excess Ag+ in the filtrate and washings from the precipitate was titrated with 11.27 mL of 0.1000 M KSCN; the reaction was Ag+ + SCN- → AgSCN(s) Calculate the percent As2O3 in the sample.
The arsenic in a 1.223-g sample of a pesticide was converted to H3AsO4 by suitable treatment. The acid was then neutralized, and 40.00 mL 0.07891 M AgNO3 was added to precipitate the arsenic quantitatively as Ag3AsO4. The excess Ag+ in the filtrate and washings from the precipitate was titrated with 11.27 mL of 0.1000 M KSCN; the reaction was Ag+ + SCN- → AgSCN(s) Calculate the percent As2O3 in the sample.
Chapter16: Applications Of Neutralization Titrations
Section: Chapter Questions
Problem 16.48QAP
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The arsenic in a 1.223-g sample of a pesticide was converted to H3AsO4 by suitable treatment. The acid was then neutralized, and 40.00 mL 0.07891 M AgNO3 was added to precipitate the arsenic quantitatively as Ag3AsO4. The excess Ag+ in the filtrate and washings from the precipitate was titrated with 11.27 mL of 0.1000 M KSCN; the reaction was
Ag+ + SCN- → AgSCN(s)
Calculate the percent As2O3 in the sample.
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