Consider a buffer solution containing `0.1mol` each of acetic and sodium acetate in `1.0L` of solution, `0.01mol` of `NaOH` is gradually added to this buffer solution. Calculate the average buffer capacity of the solution and as well as initial and final buffer capacity. `[K_(a) = 2 xx 10^(-5)] pK_(a) = 4.7`

Explanation

To solve the problem, we will follow these steps:

### Step 1: Calculate Initial pH of the Buffer Solution
We start with a buffer solution containing 0.1 mol of acetic acid (CH₃COOH) and 0.1 mol of sodium acetate (CH₃COONa) in 1 L of solution.

Using the Henderson-Hasselbalch equation:
\[
\text{pH} = \text{pKa} + \log\left(\frac{[\text{Salt}]}{[\text{Acid}]}\right)
...