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

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9.22

9.58

4.79

7.01

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detailed solution

Correct option is D

For the salt formed from a weak acid and a weak base, the pH of the solution is given by $pH = \frac{1}{2} (p K_{w}^{\circ} + p K_{a}^{\circ} - p K_{b}^{\circ})$

Hence, at 25 ° C, we will have $pH = \frac{1}{2} (14 + 4.80 - 4.78) = 7.01$

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The pKa∘ of a weak acid, HA, is 4.80. The pKb∘, of a weak base, BOH, is 4.78. The pH of an aqueous solution of the corresponding salt, BA, will be