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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![**Chemistry Question: Solubility of Mg(OH)₂**
Question 18 of 28
**Topic**: Solubility and pH-related Calculations
**Question**: What is the solubility of Mg(OH)₂ at a pH of 11.80?
*(Ksp for Mg(OH)₂ is 1.6 × 10⁻¹³)*
**Solution Approach**:
1. **Understanding the Solubility Product Constant (Ksp)**:
- The Ksp of a compound such as Mg(OH)₂ helps us determine its solubility in water.
- The expression for Ksp of Mg(OH)₂ is given by:
\( K_{sp} = [\text{Mg}^{2+}][\text{OH}^-]^2 \)
2. **Using the pH to find [OH⁻]**:
- Given pH = 11.80, we calculate pOH using:
\( \text{pOH} = 14 - \text{pH} = 14 - 11.80 = 2.20 \)
- From pOH, find [OH⁻]:
\([OH⁻] = 10^{-2.20} \approx 6.31 \times 10^{-3}\)
3. **Solving for [Mg²⁺]**:
- Substitute \([OH⁻]\) into the Ksp expression:
\( 1.6 \times 10^{-13} = [\text{Mg}^{2+}](6.31 \times 10^{-3})^2 \)
- Solve for \([\text{Mg}^{2+}]\):
\([\text{Mg}^{2+}] = \frac{1.6 \times 10^{-13}}{(6.31 \times 10^{-3})^2}\)
4. **Final Answer**:
- Calculate \([\text{Mg}^{2+}]\) to find the molarity, which represents the solubility of Mg(OH)₂ at the given pH.
**Calculator Interface**:
- A numeric keypad is shown for input, with options for basic operations and scientific notation (x10ⁿ).
This problem integrates concepts of equilibrium, pH, and solubility product](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2b31c76d-31c3-4f02-9c7e-c3848d4eba7b%2F280d05bb-21b4-40e1-b7a6-505c00a4c4c7%2F0xdatzi_processed.png&w=3840&q=75)
Transcribed Image Text:**Chemistry Question: Solubility of Mg(OH)₂**
Question 18 of 28
**Topic**: Solubility and pH-related Calculations
**Question**: What is the solubility of Mg(OH)₂ at a pH of 11.80?
*(Ksp for Mg(OH)₂ is 1.6 × 10⁻¹³)*
**Solution Approach**:
1. **Understanding the Solubility Product Constant (Ksp)**:
- The Ksp of a compound such as Mg(OH)₂ helps us determine its solubility in water.
- The expression for Ksp of Mg(OH)₂ is given by:
\( K_{sp} = [\text{Mg}^{2+}][\text{OH}^-]^2 \)
2. **Using the pH to find [OH⁻]**:
- Given pH = 11.80, we calculate pOH using:
\( \text{pOH} = 14 - \text{pH} = 14 - 11.80 = 2.20 \)
- From pOH, find [OH⁻]:
\([OH⁻] = 10^{-2.20} \approx 6.31 \times 10^{-3}\)
3. **Solving for [Mg²⁺]**:
- Substitute \([OH⁻]\) into the Ksp expression:
\( 1.6 \times 10^{-13} = [\text{Mg}^{2+}](6.31 \times 10^{-3})^2 \)
- Solve for \([\text{Mg}^{2+}]\):
\([\text{Mg}^{2+}] = \frac{1.6 \times 10^{-13}}{(6.31 \times 10^{-3})^2}\)
4. **Final Answer**:
- Calculate \([\text{Mg}^{2+}]\) to find the molarity, which represents the solubility of Mg(OH)₂ at the given pH.
**Calculator Interface**:
- A numeric keypad is shown for input, with options for basic operations and scientific notation (x10ⁿ).
This problem integrates concepts of equilibrium, pH, and solubility product
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