Homework Help is Here – Start Your Trial Now!
Science
Chemistry
The arsenic in a 1.273-g sample of a pesticide was converted to H3 AsO4 by suitable treatment. The acid was then neutralized, and 42.00 mL of 0.05871 M AgNO3 was added to precipitate the arsenic quantitatively as Ag, AsO4. The excess 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 Ag+ + SCN → AgSCN(s) Find the percentage of As2 O3 in the sample. Percentage of As2 O3

The arsenic in a 1.273-g sample of a pesticide was converted to H3 AsO4 by suitable treatment. The acid was then neutralized, and 42.00 mL of 0.05871 M AgNO3 was added to precipitate the arsenic quantitatively as Ag, AsO4. The excess 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 Ag+ + SCN → AgSCN(s) Find the percentage of As2 O3 in the sample. Percentage of As2 O3

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
See similar textbooks
icon
Related questions
Question

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 = \(\frac{0.212092254 \times 100}{1.208}\) \[= 17.56\%\]
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. \[ \text{Percentage of } \text{As}_2\text{O}_3 = \boxed{\phantom{000}} \% \]
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. \[ \text{Percentage of } \text{As}_2\text{O}_3 = \boxed{\phantom{000}} \% \]
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 3 steps with 3 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Balancing of Redox Reactions
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS