Calculate the pH of a 1.0 M aqueous solution of ammonium formate, assuming complete dissociation of — Ionic Equilibrium Chemistry Question
Question
Calculate the pH of a 1.0 M aqueous solution of ammonium formate, assuming complete dissociation of the salt. ($pK_a$ of formic acid = 3.8 & $pK_b$ of ammonia = 4.8).
Answer: B
💡 Solution & Explanation
Ammonium formate is a salt of a weak acid and a weak base (WA-WB). Its pH is given by $pH = 7 + \frac{1}{2}(pK_a - pK_b) = 7 + \frac{1}{2}(3.8 - 4.8) = 7 - 0.5 = 6.5$.
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