Question:
Equal volumes of 0.5 N acetic acid and 0.5 N sodium acetate are mixed. What is the pH of resultant solution?
(\( \text{p}K_a \) of acetic acid = 4.75)
Equal volumes of 0.5 N acetic acid and 0.5 N sodium acetate are mixed. What is the pH of resultant solution?
(\( \text{p}K_a \) of acetic acid = 4.75)
(\( \text{p}K_a \) of acetic acid = 4.75)
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If concentrations of acid and conjugate base are equal, then \( \text{pH} = \text{p}K_a \).
Updated On: Jan 6, 2026
- 4.85
- 4.65
- 4.75
- 7.0
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The Correct Option is C
Solution and Explanation
This is a buffer solution of a weak acid and its salt in equal concentrations.
Use Henderson-Hasselbalch equation:
\[ \text{pH} = \text{p}K_a + \log \left( \frac{[\text{Salt}]}{[\text{Acid}]} \right) = 4.75 + \log(1) = 4.75 \]
Use Henderson-Hasselbalch equation:
\[ \text{pH} = \text{p}K_a + \log \left( \frac{[\text{Salt}]}{[\text{Acid}]} \right) = 4.75 + \log(1) = 4.75 \]
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