The $pH$ of a monoacidic base is $10$. Calculate its percentage dissociation in $0.01 \ M$ solution at $298 \ K$. (in $\%$)

The $pH$ of two equimolar weak acids are $3.0$ and $5.0$ respectively. Their relative strength is

In aqueous solution,the ionization constants for carbonic acid are $K_1 = 4.2 \times 10^{-7}$ and $K_2 = 4.8 \times 10^{-11}$. Select the correct statement for a saturated $0.034 \ M$ solution of carbonic acid.

Calculate the $[H^{+}]$ ion concentration in a $1.00 \ M$ $HCN$ solution $(K_a = 4 \times 10^{-10})$.

The dissociation constants of monobasic acids $A$,$B$,$C$ and $D$ are $6 \times 10^{-4}$,$5 \times 10^{-5}$,$3.6 \times 10^{-6}$ and $7 \times 10^{-10}$ respectively. The $pH$ values of their $0.1 \ M$ aqueous solutions are in the order

The dissociation constant of a weak monobasic acid is $3.2 \times 10^{-4}$. Calculate the degree of dissociation in its $0.04 \ M$ solution.