The K_{a} for CH_{3}COOH is 1.8 times 10^{-5} | vedclass

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(B) Ammonium acetate $(CH_{3}COONH_{4})$ is a salt of a weak acid $(CH_{3}COOH)$ and a weak base $(NH_{4}OH)$.The formula for the $pH$ of a salt of a

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$7$

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(B) Ammonium acetate $(CH_{3}COONH_{4})$ is a salt of a weak acid $(CH_{3}COOH)$ and a weak base $(NH_{4}OH)$.The formula for the $pH$ of a salt of a weak acid and a weak base is given by: $pH = \frac{1}{2} (pK_{w} + pK_{a} - pK_{b})$.Given that $K_{a} = 1.8 	imes 10^{-5}$ and $K_{b} = 1.8 	imes 10^{-5}$,we have $pK_{a} = pK_{b}$.Substituting this into the formula: $pH = \frac{1}{2} (pK_{w} + pK_{a} - pK_{a}) = \frac{pK_{w}}{2}$.Since $pK_{w} = 14$ at $25^{\circ}C$,$pH = \frac{14}{2} = 7$.

The $K_{a}$ for $CH_{3}COOH$ is $1.8 \times 10^{-5}$ and $K_{b}$ for $NH_{4}OH$ is $1.8 \times 10^{-5}$. The $pH$ of ammonium acetate solution will be

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