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6. Consider the following separation scheme; Solution containing Ag*, Pb2+, and Cu2+ Add HNO3, so pH=1 Add H,S; Heat X Y (aq)» Pb+ (aq) NaCl (aq) Zag) Boil solution Q(aq a. What is present in the precipitate at (X)? b. Which cation will precipitate next if you continue adding H,S to the above solution? c. Assuming X has been removed, what are the identities of Q, W,Y and Z after the solution has been boiled?

6. Consider the following separation scheme; Solution containing Ag*, Pb2+, and Cu2+ Add HNO3, so pH=1 Add H,S; Heat X Y (aq)» Pb+ (aq) NaCl (aq) Zag) Boil solution Q(aq a. What is present in the precipitate at (X)? b. Which cation will precipitate next if you continue adding H,S to the above solution? c. Assuming X has been removed, what are the identities of Q, W,Y and Z after the solution has been boiled?

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...
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## Separation Scheme Analysis ### Diagram Description: The diagram represents a chemical separation process involving a solution containing \( \text{Ag}^+, \text{Pb}^{2+}, \text{and Cu}^{2+} \). The process involves adding \(\text{HNO}_3\) to achieve a pH of 1, followed by the addition of \(\text{H}_2\text{S}\) and the application of heat. This results in the separation into different precipitates and solutions, labeled as follows: - **\(X(s)\):** A solid precipitate initially formed. - **\(Y(aq)\):** Aqueous phase containing \(\text{Pb}^{2+}\). - Further addition of \(\text{NaCl}\) leads to: - **\(W(s)\):** Another solid precipitate. - **\(Z(aq)\):** Aqueous solution. - Boiling results in: - **\(Q(aq)\):** Further separated aqueous solution. ### Questions: a. **What is present in the precipitate at \(X\)?** b. **Which cation will precipitate next if you continue adding \(\text{H}_2\text{S}\) to the above solution?** c. **Assuming \(X\) has been removed, what are the identities of \(Q\), \(W\), \(Y\), and \(Z\) after the solution has been boiled?** d. **How do you confirm the identity of each cation in the above solution?** e. **What is the minimum concentration of sulfide ion required for 0.15 \text{ M Ag}^+\) solution to form a precipitate?** \((K_{sp} \ \text{Ag}_2\text{S} = 6 \times 10^{-51})\)
Transcribed Image Text:## Separation Scheme Analysis ### Diagram Description: The diagram represents a chemical separation process involving a solution containing \( \text{Ag}^+, \text{Pb}^{2+}, \text{and Cu}^{2+} \). The process involves adding \(\text{HNO}_3\) to achieve a pH of 1, followed by the addition of \(\text{H}_2\text{S}\) and the application of heat. This results in the separation into different precipitates and solutions, labeled as follows: - **\(X(s)\):** A solid precipitate initially formed. - **\(Y(aq)\):** Aqueous phase containing \(\text{Pb}^{2+}\). - Further addition of \(\text{NaCl}\) leads to: - **\(W(s)\):** Another solid precipitate. - **\(Z(aq)\):** Aqueous solution. - Boiling results in: - **\(Q(aq)\):** Further separated aqueous solution. ### Questions: a. **What is present in the precipitate at \(X\)?** b. **Which cation will precipitate next if you continue adding \(\text{H}_2\text{S}\) to the above solution?** c. **Assuming \(X\) has been removed, what are the identities of \(Q\), \(W\), \(Y\), and \(Z\) after the solution has been boiled?** d. **How do you confirm the identity of each cation in the above solution?** e. **What is the minimum concentration of sulfide ion required for 0.15 \text{ M Ag}^+\) solution to form a precipitate?** \((K_{sp} \ \text{Ag}_2\text{S} = 6 \times 10^{-51})\)
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