2. Dr. Dahm has a 0.4 M solution of nitrous acid. If he takes 3 mL of this solution and dilutes it to 100 mL calculate the pH of the new solution. (assume that no dissociation takes place until the new solution is made.) Ka = 4.6´ 10-4 HNO₂(aq) + H₂O(1) NO₂ (aq) H,O*(aq) +
2. Dr. Dahm has a 0.4 M solution of nitrous acid. If he takes 3 mL of this solution and dilutes it to 100 mL calculate the pH of the new solution. (assume that no dissociation takes place until the new solution is made.) Ka = 4.6´ 10-4 HNO₂(aq) + H₂O(1) NO₂ (aq) H,O*(aq) +
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter16: Spontaneity, Entropy, And Free Energy
Section: Chapter Questions
Problem 100CWP: Consider the dissociation of a weak acid HA (Ka = 4.5 103) in water: HA(aq)H+(aq)+A-(aq) Calculate...
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![### Problem Statement
Dr. Dahm has a 0.4 M solution of nitrous acid. If he takes 3 mL of this solution and dilutes it to 100 mL, calculate the pH of the new solution. Assume that no dissociation takes place until the new solution is made. The dissociation constant, \( K_a \), for nitrous acid is \( 4.6 \times 10^{-4} \).
### Chemical Reaction
\[ \text{HNO}_2(aq) + \text{H}_2\text{O}(l) \rightarrow \text{H}_3\text{O}^+(aq) + \text{NO}_2^-(aq) \]
### Explanation
1. **Dilution Calculation:**
- Initial concentration (\( C_i \)) = 0.4 M
- Initial volume (\( V_i \)) = 3 mL
- Final volume (\( V_f \)) = 100 mL
Use the dilution formula:
\[
C_f = \frac{C_i \times V_i}{V_f}
\]
Calculate the new concentration (\( C_f \)) after dilution.
2. **pH Calculation:**
- Use the dissociation constant (\( K_a \)) to find the concentration of \( \text{H}_3\text{O}^+ \).
- Calculate the pH using:
\[
\text{pH} = -\log [\text{H}_3\text{O}^+]
\]
The task involves using chemical equilibrium concepts to find the pH of the solution after dilution.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4ef19cdf-d917-4e85-90d1-e182276b5042%2F89a38fb4-230b-49c5-acbf-645b7b54aacd%2Fqe3zzdd_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Problem Statement
Dr. Dahm has a 0.4 M solution of nitrous acid. If he takes 3 mL of this solution and dilutes it to 100 mL, calculate the pH of the new solution. Assume that no dissociation takes place until the new solution is made. The dissociation constant, \( K_a \), for nitrous acid is \( 4.6 \times 10^{-4} \).
### Chemical Reaction
\[ \text{HNO}_2(aq) + \text{H}_2\text{O}(l) \rightarrow \text{H}_3\text{O}^+(aq) + \text{NO}_2^-(aq) \]
### Explanation
1. **Dilution Calculation:**
- Initial concentration (\( C_i \)) = 0.4 M
- Initial volume (\( V_i \)) = 3 mL
- Final volume (\( V_f \)) = 100 mL
Use the dilution formula:
\[
C_f = \frac{C_i \times V_i}{V_f}
\]
Calculate the new concentration (\( C_f \)) after dilution.
2. **pH Calculation:**
- Use the dissociation constant (\( K_a \)) to find the concentration of \( \text{H}_3\text{O}^+ \).
- Calculate the pH using:
\[
\text{pH} = -\log [\text{H}_3\text{O}^+]
\]
The task involves using chemical equilibrium concepts to find the pH of the solution after dilution.
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