A buffer solution contains 0.15 moles of acetic acid and 0.20 moles of potassium acetate per litre.
What would be the change in pH of the solution, if 0.5 mL of 1M HCl is added to it? Assume that the volume is unchanged. The dissociation constant of acetic acid at room temperature is `1.76 xx 10^(-5)`

Explanation

To solve the problem, we will follow these steps:

### Step 1: Calculate the initial pH of the buffer solution using the Henderson-Hasselbalch equation.

The Henderson-Hasselbalch equation is given by:

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