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The arsenic in a 1.208-g sample of a pesticide was converted to H3 AsO4 by suitable treatment. The acid was then neutralized, and 44.00 mL of 0.05854 M AgNO, was added to precipitate the arsenic quantitatively as Ag3 AsO4. The excess Ag* in the filtrate and in the washings from the precipitate was titrated with 9.69 mL of 0.1000 M KSCN, and the reaction was Ag+ + SCN¯ → AgSCN(s) Find the percentage of As2 O3 in the sample. Percentage of As2O3 =

The arsenic in a 1.208-g sample of a pesticide was converted to H3 AsO4 by suitable treatment. The acid was then neutralized, and 44.00 mL of 0.05854 M AgNO, was added to precipitate the arsenic quantitatively as Ag3 AsO4. The excess Ag* in the filtrate and in the washings from the precipitate was titrated with 9.69 mL of 0.1000 M KSCN, and the reaction was Ag+ + SCN¯ → AgSCN(s) Find the percentage of As2 O3 in the sample. Percentage of As2O3 =

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter16: Principles Of Chemical Reactivity: The Chemistry Of Acids And Bases
Section16.6: Types Of Acid-base Reactions
Problem 2RC: 2. Equal amounts (moles) of acetic acid(aq) and sodium sulfite, Na2SO3(aq), are mixed. The resulting...
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The arsenic in a 1.208-g sample of a pesticide was converted to H₃AsO₄ by suitable treatment. The acid was then neutralized, and 44.00 mL of 0.05854 M AgNO₃ was added to precipitate the arsenic quantitatively as Ag₃AsO₄. The excess Ag⁺ in the filtrate and in the washings from the precipitate was titrated with 9.69 mL of 0.1000 M KSCN, and the reaction was \[ \text{Ag}^+ + \text{SCN}^- \rightarrow \text{AgSCN(s)} \] Find the percentage of As₂O₃ in the sample. Percentage of As₂O₃ = \(\boxed{\phantom{3%}}\)%
Transcribed Image Text:The arsenic in a 1.208-g sample of a pesticide was converted to H₃AsO₄ by suitable treatment. The acid was then neutralized, and 44.00 mL of 0.05854 M AgNO₃ was added to precipitate the arsenic quantitatively as Ag₃AsO₄. The excess Ag⁺ in the filtrate and in the washings from the precipitate was titrated with 9.69 mL of 0.1000 M KSCN, and the reaction was \[ \text{Ag}^+ + \text{SCN}^- \rightarrow \text{AgSCN(s)} \] Find the percentage of As₂O₃ in the sample. Percentage of As₂O₃ = \(\boxed{\phantom{3%}}\)%
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