A weak base $MOH$ of $0.1\, N$ concentration shows a $pH$ value of $9$. What is the percentage degree of ionisation of the base ? ......$\%$
$0.01$
$0.001$
$0.1$
$0.02$
Ionic product of water at $310 \,K$ is $2.7 \times 10^{-14}$. What is the $\mathrm{pH}$ of neutral water at this temperature?
At $25\,^o C$, the dissociation constant of a base $BOH$ is $1.0 \times {10^{ - 12}}$. The concentration of Hydroxyl ions in $0.01\, M$ aqueous solution of the base would be
${K_a}$ of $C{H_3}COOH$ is $1.76 \times {10^{ - 5}}$ at $298$ $K$ temperature. Calculate dissociation constant of its conjugate base.
$p{K_a}$ of a weak acid is defined as
Which of the following base is weakest