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.
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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.
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.
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