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The molar solubility of calcium phosphate in a 0.214 M potassium phosphate solution is М.

The molar solubility of calcium phosphate in a 0.214 M potassium phosphate solution is М.

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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Ksp for calcium phosphate = 2*10^(-29)

**Problem Statement:** The molar solubility of **calcium phosphate** in a **0.214 M potassium phosphate** solution is __ M. **Explanation:** This problem involves determining the molar solubility of calcium phosphate in a solution of potassium phosphate. To solve this, consider the solubility product constant (Ksp) of calcium phosphate and the common ion effect contributed by the presence of potassium phosphate. **Key Concepts:** 1. **Calcium Phosphate** and its Dissociation: - Formula: \( \text{Ca}_3(\text{PO}_4)_2 \) - Dissociates: \( \text{Ca}_3(\text{PO}_4)_2 (s) \rightleftharpoons 3\text{Ca}^{2+} (aq) + 2\text{PO}_4^{3-} (aq) \) 2. **Potassium Phosphate** and its Contribution: - Formula: \( \text{K}_3\text{PO}_4 \) - In a 0.214 M solution of \( \text{K}_3\text{PO}_4 \), it contributes phosphate ions (\( \text{PO}_4^{3-} \)) to the solution. 3. **Common Ion Effect**: - The presence of \( \text{PO}_4^{3-} \) from the potassium phosphate will affect the solubility of calcium phosphate by shifting the equilibrium. **Calculations:** Replace the placeholder __ with the actual value (molar solubility) after performing the necessary calculations considering the Ksp value of calcium phosphate and the concentration of \( \text{PO}_4^{3-} \) from potassium phosphate. **Further Reading:** To understand the common ion effect and its influence on solubility, review sections on equilibrium, solubility products, and buffer systems in chemistry textbooks.
Transcribed Image Text:**Problem Statement:** The molar solubility of **calcium phosphate** in a **0.214 M potassium phosphate** solution is __ M. **Explanation:** This problem involves determining the molar solubility of calcium phosphate in a solution of potassium phosphate. To solve this, consider the solubility product constant (Ksp) of calcium phosphate and the common ion effect contributed by the presence of potassium phosphate. **Key Concepts:** 1. **Calcium Phosphate** and its Dissociation: - Formula: \( \text{Ca}_3(\text{PO}_4)_2 \) - Dissociates: \( \text{Ca}_3(\text{PO}_4)_2 (s) \rightleftharpoons 3\text{Ca}^{2+} (aq) + 2\text{PO}_4^{3-} (aq) \) 2. **Potassium Phosphate** and its Contribution: - Formula: \( \text{K}_3\text{PO}_4 \) - In a 0.214 M solution of \( \text{K}_3\text{PO}_4 \), it contributes phosphate ions (\( \text{PO}_4^{3-} \)) to the solution. 3. **Common Ion Effect**: - The presence of \( \text{PO}_4^{3-} \) from the potassium phosphate will affect the solubility of calcium phosphate by shifting the equilibrium. **Calculations:** Replace the placeholder __ with the actual value (molar solubility) after performing the necessary calculations considering the Ksp value of calcium phosphate and the concentration of \( \text{PO}_4^{3-} \) from potassium phosphate. **Further Reading:** To understand the common ion effect and its influence on solubility, review sections on equilibrium, solubility products, and buffer systems in chemistry textbooks.
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