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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Question
![**Question:**
Will Ag₂CO₃ (Ksp = 8.1 x 10⁻¹²) precipitate when 250.0 mL of 0.0062 M AgNO₃ and 250.0 mL of 0.0061 M Na₂CO₃ are combined?
**Explanation:**
The given problem involves the solubility product constant (Ksp) of silver carbonate (Ag₂CO₃) and whether it will precipitate under the given conditions.
1. **Identify the ions in solution:**
- When AgNO₃ dissolves in water, it dissociates into Ag⁺ and NO₃⁻ ions.
- When Na₂CO₃ dissolves in water, it dissociates into Na⁺ and CO₃²⁻ ions.
2. **Calculate the concentrations of ions:**
- **For Ag⁺:**
\[
\text{Initial concentration of Ag⁺} = 0.0062 \, M
\]
When 250 mL of 0.0062 M AgNO₃ is diluted to a total volume of 500 mL:
\[
\text{New concentration of Ag⁺} = \frac{0.0062 \, M \times 250 \, mL}{500 \, mL} = 0.0031 \, M
\]
- **For CO₃²⁻:**
\[
\text{Initial concentration of CO₃²⁻} = 0.0061 \, M
\]
When 250 mL of 0.0061 M Na₂CO₃ is diluted to a total volume of 500 mL:
\[
\text{New concentration of CO₃²⁻} = \frac{0.0061 \, M \times 250 \, mL}{500 \, mL} = 0.00305 \, M
\]
3. **Calculate the ion product (Qsp):**
\[
Q_{sp} = [Ag^+]^2 \times [CO_3^{2-}]
\]
Substituting the concentrations:
\[
Q_{sp} = (0.0031 \, M)^2 \](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2704aedc-cd59-4651-b157-0d8c71ae74f0%2F8a247505-7373-4671-9e79-0a878206b340%2Fva3h34e_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Question:**
Will Ag₂CO₃ (Ksp = 8.1 x 10⁻¹²) precipitate when 250.0 mL of 0.0062 M AgNO₃ and 250.0 mL of 0.0061 M Na₂CO₃ are combined?
**Explanation:**
The given problem involves the solubility product constant (Ksp) of silver carbonate (Ag₂CO₃) and whether it will precipitate under the given conditions.
1. **Identify the ions in solution:**
- When AgNO₃ dissolves in water, it dissociates into Ag⁺ and NO₃⁻ ions.
- When Na₂CO₃ dissolves in water, it dissociates into Na⁺ and CO₃²⁻ ions.
2. **Calculate the concentrations of ions:**
- **For Ag⁺:**
\[
\text{Initial concentration of Ag⁺} = 0.0062 \, M
\]
When 250 mL of 0.0062 M AgNO₃ is diluted to a total volume of 500 mL:
\[
\text{New concentration of Ag⁺} = \frac{0.0062 \, M \times 250 \, mL}{500 \, mL} = 0.0031 \, M
\]
- **For CO₃²⁻:**
\[
\text{Initial concentration of CO₃²⁻} = 0.0061 \, M
\]
When 250 mL of 0.0061 M Na₂CO₃ is diluted to a total volume of 500 mL:
\[
\text{New concentration of CO₃²⁻} = \frac{0.0061 \, M \times 250 \, mL}{500 \, mL} = 0.00305 \, M
\]
3. **Calculate the ion product (Qsp):**
\[
Q_{sp} = [Ag^+]^2 \times [CO_3^{2-}]
\]
Substituting the concentrations:
\[
Q_{sp} = (0.0031 \, M)^2 \
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