0.1 M of HA is titrated with 0.1 M NaOH, calculate the pH at end point. Given `K_(a)(HA)=5xx10^(-5)` and `alpha lt lt 1`

Explanation

To calculate the pH at the endpoint of the titration of a weak acid (HA) with a strong base (NaOH), we can follow these steps:

### Step 1: Understanding the Reaction
At the endpoint of the titration, all the weak acid (HA) has reacted with the strong base (NaOH) to form the salt (A⁻) and water. The balanced reaction is:
\[ \text{HA} + \text{NaOH} \rightarrow \text{NaA} + \text{H}_2\text{O} \]

### Step 2: Determine the Concentration of the Salt
Given that both the acid and the base are 0.1 M and equal volumes are used, the concentration of the salt (NaA) formed at the endpoint will be:
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