Using Henderson-Hasselbach Equation, show the change in pH of the buffer solution in part B when added with 0.1 M HCl and the change in pH when added with 0.1 M NaOH. Compare calculated results with experimental results.

The Henderson-Hasselbalch equation is given by:

\[
\text{pH} = \text{pKa} + \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right)
\]

Where:
- \(\text{pH}\) is the pH of the buffer solution.
- \(\text{pKa}\) is the dissociation constant of the weak acid.
- \([\text{A}^-]\) is the concentration of the conjugate base.
- \([\text{HA}]\) is the concentration of the weak acid.

To calculate the change in pH after adding 0.1 M HCl or 0.1 M NaOH to the buffer solution, follow these steps:

### 1. **Determine the initial pH of the buffer

Explore how to calculate the change in pH of a buffer solution when 0.1 M HCl or NaOH is added using the Henderson-Hasselbalch equation. Compare the theoretical calculations with experimental results. Suitable for undergraduate chemistry students.

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