Calculate the `pH` of `0.1` M ammonium acetate at `25^@C`. `K_a=K_b=1.8xx10^(-10)`

Explanation

To calculate the pH of a 0.1 M solution of ammonium acetate at 25°C, we can follow these steps:

### Step 1: Identify the components of ammonium acetate
Ammonium acetate (NH4C2H3O2) is a salt formed from the weak acid acetic acid (CH3COOH) and the weak base ammonium hydroxide (NH4OH). In solution, it dissociates into ammonium ions (NH4+) and acetate ions (C2H3O2-).

### Step 2: Determine the dissociation of ammonium ions
Ammonium ions (NH4+) can act as a weak acid and can dissociate in water:
\[ NH_4^+ \leftrightarrow NH_3 + H^+ \]
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