Two buffer, (X) and (Y) of pH `4.0` and `6.0` respectively are prepared from acid HA and the salt NaA. Both the buffers are `0.50` M in HA. What would be the pH of the solution obtained by mixing equal volumes of the two buffers ? `(K_(HA)=1.0xx10^(-5))`

Explanation

To find the pH of the solution obtained by mixing equal volumes of two buffers (X and Y) with pH 4.0 and 6.0 respectively, we can follow these steps:

### Step 1: Determine the concentrations of salt (A⁻) in each buffer.

1. **Buffer X (pH = 4.0)**:
- The formula for pH in a buffer solution is given by:
\[
\text{pH} = -\log K_a + \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right)
...