How do I calculate % in this? 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→ A SCN(s).Calculate the percentage of As2O3 (MM = 197.841 g/mol) in the original sample.

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arsenic in a 1.010 g sample of pesticide was converted to H3ASO4 by appropriate means. The acid neutralized and the arsenate precipitated quantitatively as Ag3As04 with exactly 40.00 mL of 22 M AgNO3. 3Ag* + AsO4→ Ag3AsO4 xcess Ag* was titrated with SCN , requiring 10.76 mL of 0.1000 M KSCN; the reaction being: Ag* + SCN → A SCN(s). late the percentage of As2O3 (MM = 197.841 g/mol) in the original sample.

arsenic in a 1.010 g sample of pesticide was converted to H3ASO4 by appropriate means. The acid neutralized and the arsenate precipitated quantitatively as Ag3As04 with exactly 40.00 mL of 22 M AgNO3. 3Ag* + AsO4→ Ag3AsO4 xcess Ag* was titrated with SCN , requiring 10.76 mL of 0.1000 M KSCN; the reaction being: Ag* + SCN → A SCN(s). late 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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The arsenic in a 1.010 g sample of a pesticide was converted to H3AsO4 by suitable treatment. The acid was then neutralized, and exactly 40.00 mL of 0.06222M AgNO3 was added to precipitate the arsenic quantitatively as Ag3AsO4. The excess Ag in the filtrate and in the washings from theprecipitate was titrated with 10.76 mL of 0.1000MKSCN; the reaction wasAg+ + SCN-→ AgSCN(s) Calculate the percent AsO3 in the sample.
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