Calculate the pH at the equivalence point when a solution of 0.1 M `CH_3COOH` is titrated with a solution of 0.1 M NaOH.
`K_a(CH_3COOH)= 1.8 xx 10^(-5)`

Explanation

To calculate the pH at the equivalence point when a solution of 0.1 M acetic acid (CH₃COOH) is titrated with a solution of 0.1 M NaOH, we need to follow these steps:

### Step 1: Understand the Reaction
At the equivalence point, all the acetic acid (CH₃COOH) has reacted with NaOH to form sodium acetate (CH₃COONa). The reaction can be represented as:
\[ \text{CH}_3\text{COOH} + \text{NaOH} \rightarrow \text{CH}_3\text{COONa} + \text{H}_2\text{O} \]

### Step 2: Determine the Concentration of the Conjugate Base
At the equivalence point, the concentration of the conjugate base (acetate ion, CH₃COO⁻) will be the same as the initial concentration of acetic acid, since they are in a 1:1 molar ratio. Therefore, the concentration of CH₃COO⁻ will also be 0.1 M.
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