At 25,^oC,the dissociation constant for aceti | vedclass

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(D) Ammonium acetate $(CH_3COONH_4)$ is a salt of a weak acid (acetic acid) and a weak base (ammonium hydroxide). For a salt of a weak acid and a weak

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Neutral

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(D) Ammonium acetate $(CH_3COONH_4)$ is a salt of a weak acid (acetic acid) and a weak base (ammonium hydroxide). For a salt of a weak acid and a weak base,the $pH$ of the aqueous solution is given by the formula: $pH = 7 + \frac{1}{2}(pK_a - pK_b)$. Given that $K_a = 1.8 	imes 10^{-5}$ and $K_b = 1.8 	imes 10^{-5}$,we have $pK_a = pK_b$. Substituting these values into the formula: $pH = 7 + \frac{1}{2}(pK_a - pK_a) = 7 + 0 = 7$. Since the $pH$ is $7$,the solution is neutral.

At $25\,^oC$,the dissociation constant for acetic acid is $K_a = 1.8 \times 10^{-5}$ and for $NH_4OH$ is $K_b = 1.8 \times 10^{-5}$. Determine the nature of an aqueous solution of ammonium acetate.

Similar Questions

Assertion $(A)$: The aqueous solution of $CH_3COONa$ is alkaline in nature.
Reason $(R)$: Acetate ion undergoes anionic hydrolysis.
The correct answer is

For a weak acid $HX$ with $K_a = 1 \times 10^{-5}$,the reaction with $NaOH$ gives $NaX$. What is the percentage of hydrolysis $(\% \, h)$ for a $0.1 \, M$ aqueous solution of $NaX$?

In which of the following salts,only cationic hydrolysis is involved?

$A$ $100 \ mL$, $0.1 \ M$ 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 $NH_{4}OH$)

Which of the following salts does not undergo hydrolysis in water?

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