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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![**Title: Completing the Solubility Constant Expression for Nickel(II) Hydroxide**
**Introduction:**
Understanding solubility products is key in predicting the solubility of compounds in solutions. Here, we explore the solubility constant expression for Nickel(II) Hydroxide, Ni(OH)₂.
**Objective:**
Complete the solubility constant expression for Ni(OH)₂.
**Expression:**
\[ K_{sp} = [ \text{Ni}^{2+} ][ \text{OH}^- ]^2 \]
**Explanation:**
1. **Solubility Product Constant (Ksp):**
- **Ksp** is the equilibrium constant for a solid substance dissolving into its ions in a solution.
2. **Ni(OH)₂ Dissolution:**
- When Ni(OH)₂ dissolves, it dissociates as follows:
\[ \text{Ni(OH)}_2(s) \rightleftharpoons \text{Ni}^{2+}(aq) + 2 \text{OH}^-(aq) \]
3. **Expression Components:**
- \([ \text{Ni}^{2+} ]\): Concentration of nickel ions.
- \([ \text{OH}^- ]^2\): Concentration of hydroxide ions raised to the power of 2, reflecting stoichiometry.
**Practice Questions:**
1. Calculate the Ksp for a saturated solution of Ni(OH)₂ if \([ \text{Ni}^{2+} ] = 1.0 \times 10^{-6} \, \text{M} \) and \([ \text{OH}^- ] = 2.0 \times 10^{-6} \, \text{M} \).
2. Explain how changes in pH affect the solubility of Ni(OH)₂.
**Conclusion:**
By understanding the components and calculations involved in determining the solubility product constant, students can predict and manipulate the solubility of compounds like Nickel(II) Hydroxide in various solutions.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa60cc6ce-11de-444a-af29-e9eb1b50e640%2F69bde657-38d8-4420-be64-f20b07e74909%2F4h6bhrw_processed.png&w=3840&q=75)
Transcribed Image Text:**Title: Completing the Solubility Constant Expression for Nickel(II) Hydroxide**
**Introduction:**
Understanding solubility products is key in predicting the solubility of compounds in solutions. Here, we explore the solubility constant expression for Nickel(II) Hydroxide, Ni(OH)₂.
**Objective:**
Complete the solubility constant expression for Ni(OH)₂.
**Expression:**
\[ K_{sp} = [ \text{Ni}^{2+} ][ \text{OH}^- ]^2 \]
**Explanation:**
1. **Solubility Product Constant (Ksp):**
- **Ksp** is the equilibrium constant for a solid substance dissolving into its ions in a solution.
2. **Ni(OH)₂ Dissolution:**
- When Ni(OH)₂ dissolves, it dissociates as follows:
\[ \text{Ni(OH)}_2(s) \rightleftharpoons \text{Ni}^{2+}(aq) + 2 \text{OH}^-(aq) \]
3. **Expression Components:**
- \([ \text{Ni}^{2+} ]\): Concentration of nickel ions.
- \([ \text{OH}^- ]^2\): Concentration of hydroxide ions raised to the power of 2, reflecting stoichiometry.
**Practice Questions:**
1. Calculate the Ksp for a saturated solution of Ni(OH)₂ if \([ \text{Ni}^{2+} ] = 1.0 \times 10^{-6} \, \text{M} \) and \([ \text{OH}^- ] = 2.0 \times 10^{-6} \, \text{M} \).
2. Explain how changes in pH affect the solubility of Ni(OH)₂.
**Conclusion:**
By understanding the components and calculations involved in determining the solubility product constant, students can predict and manipulate the solubility of compounds like Nickel(II) Hydroxide in various solutions.
Expert Solution
Step 1: Definition
Solubility product constant, Ksp of an electrolyte is defined as a product of the molar concentration of all its ions in a saturated solution each raised to the power equal to the number of ions produced on dissolution of 1 molecule of an electrolyte
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