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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![**Calculating pH of a Buffer Solution**
A solution contains **0.285 M sodium acetate** and **5.55×10^-2 M acetic acid**.
The pH of this solution is **__________**.
**Explanation:**
To calculate the pH of this buffer solution, you can use the Henderson-Hasselbalch equation:
\[ \text{pH} = \text{p}K_\text{a} + \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right) \]
Where,
- \( \text{p}K_\text{a} \) is the negative log of the acid dissociation constant of the weak acid.
- \([\text{A}^-]\) is the concentration of the conjugate base (sodium acetate, in this case).
- \([\text{HA}]\) is the concentration of the weak acid (acetic acid, in this case).
For acetic acid:
\[ \text{p}K_a \approx 4.76 \]
\[ \text{pH} = 4.76 + \log \left( \frac{0.285}{5.55 \times 10^{-2}} \right) \]
Fill in the blank box with the calculated pH value after you perform the computation.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F03ba95c9-584b-483d-8f8a-8f0f9c4c55b7%2Fd2652136-921d-4fdf-b964-2818a1f6fc07%2F86zifce_processed.png&w=3840&q=75)
Transcribed Image Text:**Calculating pH of a Buffer Solution**
A solution contains **0.285 M sodium acetate** and **5.55×10^-2 M acetic acid**.
The pH of this solution is **__________**.
**Explanation:**
To calculate the pH of this buffer solution, you can use the Henderson-Hasselbalch equation:
\[ \text{pH} = \text{p}K_\text{a} + \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right) \]
Where,
- \( \text{p}K_\text{a} \) is the negative log of the acid dissociation constant of the weak acid.
- \([\text{A}^-]\) is the concentration of the conjugate base (sodium acetate, in this case).
- \([\text{HA}]\) is the concentration of the weak acid (acetic acid, in this case).
For acetic acid:
\[ \text{p}K_a \approx 4.76 \]
\[ \text{pH} = 4.76 + \log \left( \frac{0.285}{5.55 \times 10^{-2}} \right) \]
Fill in the blank box with the calculated pH value after you perform the computation.
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