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Salt of Weak Acid and Strong Base

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Question

Calculate the pH of an aqueous solution of $1 M$ ammonium formate, assuming complete dissociation.
$(p K_{a} = 3.8, p K_{b} = 4.8)$

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Solution

Ammonium formate is a salt of weak acid and weak base.
So $p H = 7 + \frac{1}{2} (p K_{a} - {p K}_{b})$
$p H = 7 + \frac{1}{2} (3.8 - 4.8)$
$p H = 6.5$

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