Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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This was what was done before with the values in order of the prompt: 1.208 g, 44.00 mL, 0.05854 M, 9.69 mL, 0.1000 M KSCN. It was wrong, but this is a different set.
![**Step 1**
Moles of As = ½ moles of As₂O₃
Moles of As atoms = moles of H₃AsO₄ = moles of Ag₃AsO₄
3 moles of AgNO₃ reacts with 1 mole of H₃AsO₄
Moles of AgNO₃ = moles of SCN⁻
---
**Step 2**
Initial moles of AgNO₃ = \(\frac{44.0}{1000} \times 0.05854 = 0.00257576\)
Moles of AgNO₃ used in Ag₃AsO₄ formation
\[= 0.00257576 - \frac{9.69}{1000 \times 0.1} \]
\[= 0.00160676 \text{ moles} \]
Moles of H₃AsO₄ = \(\frac{0.00160676}{3} = 5.355867 \times 10^{-4}\)
Moles of As₂O₃ = \(2 \times 5.355867 \times 10^{-4}\)
\[= 0.001071173\]
Mass of As₂O₃ = \(0.001071173 \times 198\)
\[= 0.212092254 \text{ g}\]
% of As₂O₃ in the mixture = \(\frac{0.212092254 \times 100}{1.208}\)
\[= 17.56\%\]](https://content.bartleby.com/qna-images/question/2bafa3d4-8362-4eaf-b0f1-0c492e72839c/e6446f18-c52c-49db-aaad-fbf31e88d7ad/ao9na45_processed.png)
Transcribed Image Text:**Step 1**
Moles of As = ½ moles of As₂O₃
Moles of As atoms = moles of H₃AsO₄ = moles of Ag₃AsO₄
3 moles of AgNO₃ reacts with 1 mole of H₃AsO₄
Moles of AgNO₃ = moles of SCN⁻
---
**Step 2**
Initial moles of AgNO₃ = \(\frac{44.0}{1000} \times 0.05854 = 0.00257576\)
Moles of AgNO₃ used in Ag₃AsO₄ formation
\[= 0.00257576 - \frac{9.69}{1000 \times 0.1} \]
\[= 0.00160676 \text{ moles} \]
Moles of H₃AsO₄ = \(\frac{0.00160676}{3} = 5.355867 \times 10^{-4}\)
Moles of As₂O₃ = \(2 \times 5.355867 \times 10^{-4}\)
\[= 0.001071173\]
Mass of As₂O₃ = \(0.001071173 \times 198\)
\[= 0.212092254 \text{ g}\]
% of As₂O₃ in the mixture = \(\frac{0.212092254 \times 100}{1.208}\)
\[= 17.56\%\]
![The arsenic in a 1.273-g sample of a pesticide was converted to \( \text{H}_3\text{AsO}_4 \) by suitable treatment. The acid was then neutralized, and 42.00 mL of 0.05871 M \( \text{AgNO}_3 \) was added to precipitate the arsenic quantitatively as \( \text{Ag}_3\text{AsO}_4 \). The excess \( \text{Ag}^+ \) in the filtrate and in the washings from the precipitate was titrated with 9.58 mL of 0.1000 M KSCN, and the reaction was
\[
\text{Ag}^+ + \text{SCN}^- \rightarrow \text{AgSCN}(s)
\]
Find the percentage of \( \text{As}_2\text{O}_3 \) in the sample.
\[ \text{Percentage of } \text{As}_2\text{O}_3 = \boxed{\phantom{000}} \% \]](https://content.bartleby.com/qna-images/question/2bafa3d4-8362-4eaf-b0f1-0c492e72839c/e6446f18-c52c-49db-aaad-fbf31e88d7ad/8d56uvef_processed.png)
Transcribed Image Text:The arsenic in a 1.273-g sample of a pesticide was converted to \( \text{H}_3\text{AsO}_4 \) by suitable treatment. The acid was then neutralized, and 42.00 mL of 0.05871 M \( \text{AgNO}_3 \) was added to precipitate the arsenic quantitatively as \( \text{Ag}_3\text{AsO}_4 \). The excess \( \text{Ag}^+ \) in the filtrate and in the washings from the precipitate was titrated with 9.58 mL of 0.1000 M KSCN, and the reaction was
\[
\text{Ag}^+ + \text{SCN}^- \rightarrow \text{AgSCN}(s)
\]
Find the percentage of \( \text{As}_2\text{O}_3 \) in the sample.
\[ \text{Percentage of } \text{As}_2\text{O}_3 = \boxed{\phantom{000}} \% \]
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