Identify the salt and its hydrolysis nature

Ammonium acetate is a salt of:

• weak acid: $\mathrm{CH_3COOH}$ with $K_a = 1.8 \times 10^{-5}$
• weak base: $\mathrm{NH_4OH}$ with $K_b = 1.8 \times 10^{-5}$

For a salt of a weak acid and a weak base, the pH is given by: $\mathrm{pH} = 7 + \frac{1}{2}\log\left(\frac{K_b}{K_a}\right)$

Substitute the given values

Since $K_a = 1.8 \times 10^{-5}, \qquad K_b = 1.8 \times 10^{-5}$ we have $\frac{K_b}{K_a} = \frac{1.8 \times 10^{-5}}{1.8 \times 10^{-5}} = 1$

Calculate the pH

$\mathrm{pH} = 7 + \frac{1}{2}\log(1)$

Since $\log(1)=0$, $\mathrm{pH} = 7$

Final answer

The pH of ammonium acetate solution is: $\boxed{7}$

Comparison with stored correct answer

Stored correct answer = $7$

My derived answer also is $7$, so they agree.