At $298\,K$ a $0.1 \,M $ $C{H_3}COOH$ solution is $ 1.34\%$ ionized. The ionization constant ${K_a}$ for acetic acid will be
$1.82 \times {10^{ - 5}}$
$18.2 \times {10^{ - 5}}$
$0.182 \times {10^{ - 5}}$
None of these
At $298$ $K$ temperature, the ${K_b}$ of ${\left( {C{H_3}} \right)_2}NH$ is $5.4 \times {10^{ - 4}}$ $0.25$ $M$ solution.
The $pH$ value of decinormal solution of $N{H_4}OH$ which is $20\%$ ionised, is
$0.01\, M \,HA(aq.)$ is $2\%$ ionized, $[OH^-]$ of solution is :-
Derive the equation of ionization constant $({K_b})$ of weak base.
For a weak acid $HA$ with dissociation constant ${10^{ - 9}},\,\,pOH$ of its $0.1 \,M$ solution is