The pH of an aqueous solution of 1.0 M ammonium formate assuming complete dissociation is (p Ka.

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The pH of an aqueous solution of 1.0 M ammonium formate...

The $\mathrm{pH}$ of an aqueous solution of $1.0 \mathrm{M}$ ammonium formate assuming complete dissociation is $\left(\mathrm{p} K_{\mathrm{a}}\right.$ of formic acid $=3.8$ and $\mathrm{p} K_{\mathrm{b}}$ of ammonia $=4.8$ )
(a) $7.0$
(b) $7.5$
(c) $6.5$
(d) $4.3$

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Key Concepts

Salt Hydrolysis

Salt hydrolysis describes the process by which salts formed from a weak acid and a weak base react with water to produce acidic or basic solutions. When a salt like ammonium formate dissolves, its cation and anion undergo hydrolysis, meaning the ammonium ion (a weak acid) donates a proton while the formate ion (a weak base) accepts a proton, affecting the overall pH of the solution.

Conjugate Acid?Base Pairs

This concept refers to the relationship between an acid and its corresponding base formed when the acid donates a proton, and vice versa. In a solution containing ammonium formate, ammonium is the conjugate acid of ammonia and formate is the conjugate base of formic acid. Their interactions with water determine the degree of proton transfer, which directly influences the pH of the solution.

pKa and pKb Relationships in pH Calculations

Understanding pKa and pKb values is essential for predicting the behavior of weak acids and bases in solution. These values represent the strengths of the acid and its conjugate base, respectively. In a salt solution of a weak acid and weak base, the pH can be estimated using relationships such as pH = 7 + ½(pKa - pKb), which balances the contributions of both the acidic and basic components and provides insight into the resultant solution pH.

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