8. The arsenic in a 1.010 g sample of pesticide was converted to H3ASO4 by appropriate means. The acidwas neutralized and the arsenate precipitated quantitatively as Ag3AsO4 with exactly 40.00 mL of0.06222 M AgNO3.3Ag* + AsO4 → Ag3AsO4The excess Ag* was titrated with SCN", requiring 10.76 mL of 0.1000 M KSCN; the reaction being:Ag* + SCN- → AgSCN(s).Calculate the percentage of As2O3 (MM = 197.841 g/mol) in the original sample.

Molarity is defined as moles of solute upon the volume in litre

The arsenic in a 1.010 g sample of pesticide was converted to H3ASO4 by appropriate means. The acid was neutralized and the arsenate precipitated quantitatively as Ag3AsO4 with exactly 40.00 mL of 0.06222 M AgNO3. 3Ag* + AsO4¯ → A33ASO4 The excess Ag* was titrated with SCN¯, requiring 10.76 mL of 0.1000 M KSCN; the reaction being: Ag* + SCN- → AgSCN(s). Calculate the percentage of AS2O3 (MM = 197.841 g/mol) in the original sample.

The arsenic in a 1.010 g sample of pesticide was converted to H3ASO4 by appropriate means. The acid was neutralized and the arsenate precipitated quantitatively as Ag3AsO4 with exactly 40.00 mL of 0.06222 M AgNO3. 3Ag* + AsO4¯ → A33ASO4 The excess Ag* was titrated with SCN¯, requiring 10.76 mL of 0.1000 M KSCN; the reaction being: Ag* + SCN- → AgSCN(s). Calculate the percentage of AS2O3 (MM = 197.841 g/mol) in the original sample.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter13: Titrations In Analytical Chemistry

Section: Chapter Questions

Problem 13.22QAP

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