**Problem:**If a buffer solution is 0.130 M in a weak acid (\(K_a = 5.80 \times 10^{-5}\)) and 0.560 M in its conjugate base, what is the pH of the buffer? Show your work.**Explanation:**To find the pH of a buffer solution, you can use the Henderson-Hasselbalch equation:\[ \text{pH} = \text{pK}_a + \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right) \]Where:- \([\text{A}^-]\) is the concentration of the conjugate base.- \([\text{HA}]\) is the concentration of the weak acid.- \(\text{pK}_a = -\log(K_a)\).1. Calculate \(\text{pK}_a\):\[ \text{pK}_a = -\log(5.80 \times 10^{-5}) \]2. Use the Henderson-Hasselbalch equation:\[ \text{pH} = \text{pK}_a + \log \left( \frac{0.560}{0.130} \right) \]Substitute the values and solve for pH to determine the answer.

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Answered: (2) 12. If a buffer solution is 0.130 M…

(2) 12. If a buffer solution is 0.130 M in a weak acid (Ka = 5.80 x 10-5) and 0.560 Min its conjugate base, what is the pH of the buffer? Show your work.

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

**Problem:**

If a buffer solution is 0.130 M in a weak acid (\(K_a = 5.80 \times 10^{-5}\)) and 0.560 M in its conjugate base, what is the pH of the buffer? Show your work.

**Explanation:**

To find the pH of a buffer solution, you can use the Henderson-Hasselbalch equation:

\[ \text{pH} = \text{pK}_a + \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right) \]

Where:
- \([\text{A}^-]\) is the concentration of the conjugate base.
- \([\text{HA}]\) is the concentration of the weak acid.
- \(\text{pK}_a = -\log(K_a)\).

1. Calculate \(\text{pK}_a\):

\[ \text{pK}_a = -\log(5.80 \times 10^{-5}) \]

2. Use the Henderson-Hasselbalch equation:

\[ \text{pH} = \text{pK}_a + \log \left( \frac{0.560}{0.130} \right) \]

Substitute the values and solve for pH to determine the answer.

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