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Chemistry · EQUILIBRIUM
हिन्दीA buffer solution contains \( 0.1\text{ M} \) weak acid HA (\( \text{p}K_a = 4.74 \)) and \( 1.0\text{ M} \) of its conjugate base \( \text{A}^- \). What is the pH of this buffer solution?
Correct answer · Option 2
\( 5.74 \)
Explanation
By Henderson-Hasselbalch equation: \( \text{pH} = \text{p}K_a + \log\frac{[\text{Salt}]}{[\text{Acid}]} = 4.74 + \log(\frac{1.0}{0.1}) = 4.74 + 1 = 5.74 \).
