The $pK_{a}$ of acetic acid and $pK_{b}$ of ammonium hydroxide are $4.76$ and $4.75$ respectively. Calculate the $pH$ of ammonium acetate solution.
(7.005) The $pH$ of a salt of a weak acid and a weak base is given by the formula:
$pH = 7 + \frac{1}{2} [pK_{a} - pK_{b}]$
Given:
$pK_{a} = 4.76$
$pK_{b} = 4.75$
Substituting the values:
$pH = 7 + \frac{1}{2} [4.76 - 4.75]$
$pH = 7 + \frac{1}{2} [0.01]$
$pH = 7 + 0.005 = 7.005$
$pH = 7 + \frac{1}{2} [pK_{a} - pK_{b}]$
Given:
$pK_{a} = 4.76$
$pK_{b} = 4.75$
Substituting the values:
$pH = 7 + \frac{1}{2} [4.76 - 4.75]$
$pH = 7 + \frac{1}{2} [0.01]$
$pH = 7 + 0.005 = 7.005$
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