Sodium sulfate is slowly added to a solution containing 0.0500 M Ca²+ (aq) and 0.0210 M Ag+ (aq). What will be the concentration of Ca²+ (aq) when Ag₂SO4(s) begins to precipitate? Solubility-product constants, Ksp, can be found in the chempendix. [Ca²+] = What percentage of the Ca²+ (aq) can be precipitated from the Ag+ (aq) by selective precipitation? percentage: M Ag %
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![**Educational Content: Solving Precipitation Equilibria**
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**Scenario:**
Sodium sulfate is slowly added to a solution containing 0.0500 M Ca²⁺ (aq) and 0.0210 M Ag⁺ (aq).
**Objective:**
Determine the concentration of Ca²⁺ (aq) when Ag₂SO₄(s) begins to precipitate.
**Concept:**
Solubility-product constants, \( K_{sp} \), can be referenced in the appendix or a chemistry handbook.
**Questions:**
1. Calculate \([ \text{Ca}^{2+} ]\)
- **Answer Box:** [‾‾‾‾‾‾‾‾] M
2. What percentage of the \(\text{Ca}^{2+}\) (aq) can be precipitated from the \(\text{Ag}^{+}\) (aq) by selective precipitation?
- **Answer Box:** [‾‾‾‾‾‾‾‾] %
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**Instructions:**
In solving this problem, you will need to utilize your understanding of solubility equilibria and the \( K_{sp} \) values for Ag₂SO₄. This involves writing the equilibrium expressions and solving for the concentrations at which precipitation occurs. Use these calculations to determine at which point precipitation begins and calculate percentage yield based on initial concentrations.
*Note: Ensure to consult the appendix for the necessary \( K_{sp} \) values.*
**Source:** McQuarrie, Rock, and Gallogly 4e - General Chemistry
**Publisher:** University Science Books](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F00154cd9-82c7-455b-845c-02cf21fdb65c%2F30fc03f2-183a-40fc-9652-9daa3aaba654%2Fog8opme_processed.jpeg&w=3840&q=75)
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