`0.1M NaOH` is titrated with `0.1M HA` till the end point. `K_(a)` of HA is `5.6xx10^(-6)` and degree of hydrolysis is less compared to 1. Calculate pH of the resulting solution at the end point ?

Explanation

To calculate the pH of the resulting solution at the end point when titrating 0.1 M NaOH with 0.1 M HA, we can follow these steps:

### Step 1: Understand the Reaction
When NaOH (a strong base) reacts with HA (a weak acid), the reaction can be represented as:
\[ \text{NaOH} + \text{HA} \rightarrow \text{NaA} + \text{H}_2\text{O} \]

At the end point of the titration, all the HA will have reacted with NaOH to form the salt NaA.

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