Assertion (A): The pH of a buffer solution co | vedclass

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(B) Both $(A)$ and $(R)$ are true statements, but $(R)$ is not the correct explanation of $(A)$.The $pH$ of a buffer solution is given by the Henderso

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Both $(A)$ and $(R)$ are true and $(R)$ is not the correct explanation of $(A)$

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(B) Both $(A)$ and $(R)$ are true statements, but $(R)$ is not the correct explanation of $(A)$.The $pH$ of a buffer solution is given by the Henderson-Hasselbalch equation:$pH = pK_a + \log \frac{[	ext{salt}]}{[	ext{acid}]}$When the moles of salt and acid are equal, $[	ext{salt}] = [	ext{acid}]$, so:$pH = pK_a + \log(1) = pK_a = 4.8$.Thus, $(A)$ is true. The ionic product of water $(K_w)$ at $25^{\circ} C$ is indeed $10^{-14} \ mol^2 \ L^{-2}$, making $(R)$ a true statement, but it does not explain the $pH$ calculation of the buffer.

Assertion $(A)$: The $pH$ of a buffer solution containing equal moles of acetic acid and sodium acetate is $4.8$ ($pK_a$ of acetic acid is $4.8$).
Reason $(R)$: The ionic product of water at $25^{\circ} C$ is $10^{-14} \ mol^2 \ L^{-2}$. The correct answer is

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Assertion $(A)$: The $pH$ of a buffer solution containing equal moles of acetic acid and sodium acetate is $4.8$ ($pK_a$ of acetic acid is $4.8$).Reason $(R)$: The ionic product of water at $25^{\circ} C$ is $10^{-14} \ mol^2 \ L^{-2}$. The correct answer is