The dissociation constant of a weak acid HA i | vedclass

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Question

(A) For a conjugate acid-base pair,the relationship between the dissociation constant of the acid $(K_a)$ and the dissociation constant of its conjuga

Vedclass · Accepted Answer

$5.5 	imes 10^{-11}$

Vedclass · Answer

(A) For a conjugate acid-base pair,the relationship between the dissociation constant of the acid $(K_a)$ and the dissociation constant of its conjugate base $(K_b)$ is given by the equation: $K_a 	imes K_b = K_w$. Given $K_a = 1.8 	imes 10^{-4}$ and $K_w = 1.0 	imes 10^{-14}$ at $298 \ K$. Substituting the values: $K_b = \frac{K_w}{K_a} = \frac{1.0 	imes 10^{-14}}{1.8 	imes 10^{-4}}$. $K_b = 0.555 	imes 10^{-10} = 5.55 	imes 10^{-11}$.

List-$I$ (Acid)	List-$II$ $(K_a)$
$A$. Phenol	$I$. $1 \times 10^{-13}$
$B$. Benzoic acid	$II$. $3.0 \times 10^{-8}$
$C$. $HClO$	$III$. $1.0 \times 10^{-10}$
$D$. $CH_3COOH$	$IV$. $6.5 \times 10^{-5}$
	$V$. $1.75 \times 10^{-5}$

The dissociation constant of a weak acid $HA$ is $1.8 \times 10^{-4}$. Calculate the dissociation constant of its conjugate base $A^{-}$.

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