The $pK_{a}$ of a weak acid, HA, is 4.80. The $pK_{b}$ of a weak base, $BOH$ is 4.78. The pH of an aqueous solution of the corresponding salt, $BA$, will be

Question

Dr. Abubacker · Accepted Answer

(c)
For salt of weak acid and weak base
$pH = \frac{1}{2}\lbrack\log{K_{a} + \log{K_{w} - \log K_{b}}}brack$
$= \frac{1}{2}pK_{a} + \frac{1}{2}pK_{w} - \frac{1}{2}pK_{b}$
$= \frac{1}{2} 	imes 4.80 + 7 - \frac{1}{2} 	imes 4.78$
$= 7.01$

Q. The $pK_{a}$ of a weak acid, HA, is 4.80. The $pK_{b}$ of a weak base, $BOH$ is 4.78. The pH of an aqueous solution of the corresponding salt, $BA$, will be

Explanation

Reviewed by Dr. Abubacker

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