The $pH $ of a $0.01\,M$ solution of acetic acid having degree of dissociation $12.5\%$ is
$5.623$
$2.903$
$3.723$
$4.509$
The ${K_b}$ of ammonia is $1.8 \times {10^{ - 5}}$ at $298$ $K$ temperature. Calculate the $pH$ of $0.1$ $M$ solution.
If degree of ionisation is $0.01$ of decimolar solution of weak acid $HA$ then $pKa$ of acid is
Heat of neutralisation of weak acid and strong base is less than the heat of neutralisation of strong acid and strong base due to
The hydrogen ion concentration of $0.1\,N$ solution of $C{H_3}COOH,$ which is $30\%$ dissociated, is
Concentration $C{N^ - }$ in $0.1\,M\,HCN$ is $[{K_a} = 4 \times {10^{ - 10}}]$