Question

In an acidic buffer, if the ratio of base to acid concentration is increased by 100 times, then find the increase in pH of the buffer solution.

• A. 1
• B. 2
• C. 0
• D. 4

Hint:

The Henderson-Hasselbalch equation illustrates how the pH of a buffer solution depends on the ratio of conjugate base to acid. A tenfold increase in this ratio results in a pH increase of 1 unit.

Answer 1

The Correct Option is B

Per the Henderson-Hasselbalch equation: \[ \text{pH} = \text{pKa} + \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right) \] A 100-fold increase in the ratio \(\frac{[\text{A}^-]}{[\text{HA}]} \) leads to: \[ \Delta \text{pH} = \log(100) = 2 \] Consequently, the pH elevates by 2 units. Conclusion: A tenfold increase in the base-to-acid concentration ratio results in a 2-unit pH rise in the buffer. % Quicktip