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

7.01

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

9.22

No worries! We‘ve got your back. Try BYJU‘S free classes today!

9.58

No worries! We‘ve got your back. Try BYJU‘S free classes today!

4.79

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is A 7.01
$B^{+} + A^{-} + H_{2} O \to B O H + H A$

pH of weak acid - weak base =

$p H = \frac{1}{2} p K_{w} + \frac{1}{2} p K_{a} - \frac{1}{2} p K_{b} = \frac{1}{2} (14 + 4.80 - 4.78) = 7.01$

Suggest Corrections

Similar questions

{p K}_{a}

{p K}_{b}

p H

A B

p K_{a}

H A

4

p K_{b}

Join BYJU'S Learning Program