Calculate the pH at equivalence point when a solution of `0.10 M ` acetic acid is titrated with a solution of `0.10 ` M hydroxide
`(K_(a) " for acetic acid is " 1.9 xx10^(-5))`

Explanation

To calculate the pH at the equivalence point when titrating a solution of 0.10 M acetic acid with a solution of 0.10 M hydroxide, we can follow these steps:

### Step 1: Understand the Reaction
When acetic acid (a weak acid) is titrated with sodium hydroxide (a strong base), they react to form sodium acetate (a salt) and water. The reaction is as follows:
\[ \text{CH}_3\text{COOH} + \text{NaOH} \rightarrow \text{CH}_3\text{COONa} + \text{H}_2\text{O} \]

### Step 2: Determine the Concentration of the Salt at Equivalence Point
At the equivalence point, all the acetic acid will have reacted with the hydroxide. Since both the acetic acid and hydroxide are 0.10 M, and assuming equal volumes are mixed, the concentration of the resulting sodium acetate will be:
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