If the degree of ionisation is $0.01$ for a decimolar solution of a weak acid $HA$,then the $pKa$ of the acid is:

Find the $pOH$ value of $10^{-3} \ M \ NH_4OH$. Given $K_b = 10^{-5}$.

$0.02 \, M$ monobasic acid dissociates $2 \%$,hence,$pH$ of the solution is

The $K_a$ of monobasic acid $A, B$ and $C$ are $10^{-6}, 10^{-8}$ and $10^{-10}$ respectively. The concentrations of $A, B$ and $C$ are respectively $0.1 \ M, 0.01 \ M$ and $0.001 \ M$. Which of the following is correct for $pOH$ of $A, B$ and $C$?

What is the $pH$ of a $2 \times 10^{-3} \ M$ solution of a monoacidic weak base if it ionizes to the extent of $5 \%$?

$A$ weak monoacidic base dissociates to $1.5 \%$ in $0.001 \ M$ solution at $298 \ K$. Calculate the dissociation constant of the weak base.