A 100 mL, 0.1 M solution of ammonium acetat | vedclass

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(C) Ammonium acetate $(CH_3COONH_4)$ is a salt formed from a weak acid $(CH_3COOH)$ and a weak base $(NH_4OH)$.For a salt of a weak acid and a weak ba

Vedclass · Accepted Answer

$7$

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(C) Ammonium acetate $(CH_3COONH_4)$ is a salt formed from a weak acid $(CH_3COOH)$ and a weak base $(NH_4OH)$.For a salt of a weak acid and a weak base, the pH of the solution is given by the formula:$pH = 7 + \frac{1}{2} pK_a - \frac{1}{2} pK_b$Since the pH of such a salt solution is independent of the concentration (dilution), the pH remains constant upon dilution.Given that $pK_a \approx pK_b$, the equation simplifies to:$pH = 7 + \frac{1}{2} (pK_a - pK_b) = 7 + 0 = 7$Therefore, the pH of the resulting solution is $7$.

$A$ $100 \ mL$, $0.1 \ M$ solution of ammonium acetate is diluted by adding $100 \ mL$ of water. The pH of the resulting solution will be ($pK_{a}$ of acetic acid is nearly equal to $pK_{b}$ of $NH_{4}OH$)

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