A saturated solution of Ca(OH)2 at 20 °C has a concentration of 0.0233 M. What is the Ksp for calcium hydroxide solution at 20 °C? Ksp (Ca(OH)2) = [? ] × 10[?] Coefficient (green) Exponent (yellow) Enter
A saturated solution of Ca(OH)2 at 20 °C has a concentration of 0.0233 M. What is the Ksp for calcium hydroxide solution at 20 °C? Ksp (Ca(OH)2) = [? ] × 10[?] Coefficient (green) Exponent (yellow) Enter
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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![### Solubility Product Constant Calculation for Calcium Hydroxide
#### Problem Statement:
A saturated solution of \( \text{Ca(OH)}_2 \) at 20°C has a concentration of 0.0233 M.
**Question:** What is the \( K_{sp} \) for calcium hydroxide solution at 20°C?
#### Explanation:
To calculate the solubility product constant (\( K_{sp} \)) for calcium hydroxide:
1. **Dissociation of \( \text{Ca(OH)}_2 \):**
\[
\text{Ca(OH)}_2 \rightleftharpoons \text{Ca}^{2+} + 2\text{OH}^-
\]
2. **Solubility and Ion Concentration:**
Let the solubility of \( \text{Ca(OH)}_2 \) be S M. Therefore,
\[
[\text{Ca}^{2+}] = S = 0.0233 \, \text{M}
\]
and
\[
[\text{OH}^-] = 2S = 2 \times 0.0233 = 0.0466 \, \text{M}
\]
3. **Expression for \( K_{sp} \):**
\[
K_{sp} = [\text{Ca}^{2+}][\text{OH}^-]^2
\]
Substituting the values,
\[
K_{sp} = (0.0233) \times (0.0466)^2
\]
4. **Calculation:**
Calculate the value:
\[
K_{sp} = 5.07 \times 10^{-5}
\]
5. **Representation:**
\[
K_{sp (\text{Ca(OH)}_2)} = [ \text{5.07} ] \times 10^{-5}
\]
**Interactive Component:**
- **Coefficient (green):** Enter `5.07`
- **Exponent (yellow):** Enter `-5`
- **Enter Button:** Click to verify your answer.
This exercise helps in understanding the concept of solubility product constants, the dissociation of compounds in solutions, and applying stoichiometric conversions to find the necessary ion concentrations](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F81a43bbd-f504-4d06-af9d-cc35582a0d5e%2Fcb6e9e71-22b7-4825-8499-0d6ded42045a%2Fvv5jakf_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Solubility Product Constant Calculation for Calcium Hydroxide
#### Problem Statement:
A saturated solution of \( \text{Ca(OH)}_2 \) at 20°C has a concentration of 0.0233 M.
**Question:** What is the \( K_{sp} \) for calcium hydroxide solution at 20°C?
#### Explanation:
To calculate the solubility product constant (\( K_{sp} \)) for calcium hydroxide:
1. **Dissociation of \( \text{Ca(OH)}_2 \):**
\[
\text{Ca(OH)}_2 \rightleftharpoons \text{Ca}^{2+} + 2\text{OH}^-
\]
2. **Solubility and Ion Concentration:**
Let the solubility of \( \text{Ca(OH)}_2 \) be S M. Therefore,
\[
[\text{Ca}^{2+}] = S = 0.0233 \, \text{M}
\]
and
\[
[\text{OH}^-] = 2S = 2 \times 0.0233 = 0.0466 \, \text{M}
\]
3. **Expression for \( K_{sp} \):**
\[
K_{sp} = [\text{Ca}^{2+}][\text{OH}^-]^2
\]
Substituting the values,
\[
K_{sp} = (0.0233) \times (0.0466)^2
\]
4. **Calculation:**
Calculate the value:
\[
K_{sp} = 5.07 \times 10^{-5}
\]
5. **Representation:**
\[
K_{sp (\text{Ca(OH)}_2)} = [ \text{5.07} ] \times 10^{-5}
\]
**Interactive Component:**
- **Coefficient (green):** Enter `5.07`
- **Exponent (yellow):** Enter `-5`
- **Enter Button:** Click to verify your answer.
This exercise helps in understanding the concept of solubility product constants, the dissociation of compounds in solutions, and applying stoichiometric conversions to find the necessary ion concentrations
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