The pH of an aqueous solution of 1.0 M ammonium formate assuming complete dissociation is (p of form — Ionic Equilibrium Chemistry Question
Question
The pH of an aqueous solution of 1.0 M ammonium formate assuming complete dissociation is (p$K_a$ of formic acid = 3.8 and p$K_b$ of ammonia = 4.8)
Answer: C
💡 Solution & Explanation
Ammonium formate is a salt of a weak acid and a weak base. The pH of its aqueous solution is given by the formula $\text{pH} = 7 + \frac{1}{2}(pK_a - pK_b)$. Substituting the given values: $\text{pH} = 7 + \frac{1}{2}(3.8 - 4.8) = 7 + \frac{1}{2}(-1.0) = 7 - 0.5 = 6.5$.
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