A solution that contains 0.67 MHZ and 0.98 M NaZ has a pH of 5.38. What is Ką for HZ? Use scientific notation for your answer like this: 10,000 = 1*10^4. Type your answer...
A solution that contains 0.67 MHZ and 0.98 M NaZ has a pH of 5.38. What is Ką for HZ? Use scientific notation for your answer like this: 10,000 = 1*10^4. Type your answer...
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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![**Problem Statement:**
A solution that contains 0.67 M HZ and 0.98 M NaZ has a pH of 5.38. What is Kₐ for HZ?
**Instructions:**
Use scientific notation for your answer like this: 10,000 = 1*10^4.
**Answer Input:**
[Type your answer...]
**Explanation:**
This problem requires calculating the acid dissociation constant (Kₐ) for the acid HZ in the given solution. The concentration of HZ and its conjugate base NaZ, along with the pH of the solution, are provided.
1. **Determine [H⁺]:**
- Use the pH to calculate the concentration of hydrogen ions:
\[ \text{[H⁺]} = 10^{-\text{pH}} \]
2. **Use the Henderson-Hasselbalch Equation:**
- The equation is:
\[ \text{pH} = \text{pKₐ} + \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right) \]
- Rearrange to find pKₐ:
\[ \text{pKₐ} = \text{pH} - \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right) \]
3. **Convert pKₐ to Kₐ:**
- Use the relation:
\[ \text{Kₐ} = 10^{-\text{pKₐ}} \]
4. **Express Kₐ in Scientific Notation.**
Utilize the instructions and input your calculated Kₐ value in the text box using scientific notation as shown.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6512cb2f-6b19-463a-b51b-739ff268c6f0%2Fbe57bb00-1f77-4207-8a2d-9137e05a65e6%2Ffc1unyi_processed.png&w=3840&q=75)
Transcribed Image Text:**Problem Statement:**
A solution that contains 0.67 M HZ and 0.98 M NaZ has a pH of 5.38. What is Kₐ for HZ?
**Instructions:**
Use scientific notation for your answer like this: 10,000 = 1*10^4.
**Answer Input:**
[Type your answer...]
**Explanation:**
This problem requires calculating the acid dissociation constant (Kₐ) for the acid HZ in the given solution. The concentration of HZ and its conjugate base NaZ, along with the pH of the solution, are provided.
1. **Determine [H⁺]:**
- Use the pH to calculate the concentration of hydrogen ions:
\[ \text{[H⁺]} = 10^{-\text{pH}} \]
2. **Use the Henderson-Hasselbalch Equation:**
- The equation is:
\[ \text{pH} = \text{pKₐ} + \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right) \]
- Rearrange to find pKₐ:
\[ \text{pKₐ} = \text{pH} - \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right) \]
3. **Convert pKₐ to Kₐ:**
- Use the relation:
\[ \text{Kₐ} = 10^{-\text{pKₐ}} \]
4. **Express Kₐ in Scientific Notation.**
Utilize the instructions and input your calculated Kₐ value in the text box using scientific notation as shown.
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