Ionisation constant of HA (weak acid) and BOH (weak base) are 3.0×10−7 each at 298 K. The percentage extent of hydrolysis of BA at the dilution of 10 L is :

h1−h=KH=kwKakb=10−243×10−72=13h=0.25Hence, option A is correct.

Ionisation constant of HA (weak acid) and BOH (weak base) are 3.0×10−7 each at 298 K. The percentage extent of hydrolysis of BA at the dilution of 10 L is :

h1−h=KH=kwKakb=10−243×10−72=13h=0.25Hence, option A is correct.

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Ionisation constant of $H A$ (weak acid) and $B O H$ (weak base) are $3.0 \times 10^{- 7} each at 298 K$ . The percentage extent of hydrolysis of $B A$ at the dilution of $10 L$ is :

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$\frac{h}{1 - h} = \sqrt{KH} = \sqrt{\frac{kw}{K_{a} k_{b}}}$

$= \sqrt{\frac{10^{- 24}}{{(3 \times 10^{- 7})}^{2}}}$

$= \frac{1}{3}$

$h = 0.25$

Hence, option A is correct.

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Ionisation constant of HA (weak acid) and BOH (weak base) are 3.0×10−7 each at 298 K. The percentage extent of hydrolysis of BA at the dilution of 10 L is :

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Ionisation constant of $H A$ (weak acid) and $B O H$ (weak base) are $3.0 \times 10^{- 7} each at 298 K$ . The percentage extent of hydrolysis of $B A$ at the dilution of $10 L$ is :