Chemistry - Ionic Equilibrium Question with Solution | TestHub

$\mathrm{p}{\mathrm{K}}_{\mathrm{b}}=10.83,$
$\text{log}{\text{K}}_{\text{b}}=-10.83-(11-0.17)$
On taking antilog
${\mathrm{K}}_{\mathrm{b}}=1.479\times 10^{-11}$
${\mathrm{K}}_{\mathrm{a}}.{\mathrm{K}}_{\mathrm{b}}={\mathrm{K}}_{\mathrm{w}}$
or${\mathrm{K}}_{\mathrm{a}}\times 1.479\times 10^{-11}=1.0\times 10^{-14}$
${\mathrm{K}}_{\mathrm{a}}=6.76\times 10^{-4}$