$pH$ of $0.1 \ M$ $NH_3$ aqueous solution is $(K_b = 1.8 \times 10^{-5})$

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

The degree of dissociation of acetic acid $(0.1 \ mol \ L^{-1})$ in water ($K_a$ of acetic acid is $10^{-5}$) is

What is the $pH$ of a solution containing $7 \ g$ of $NH_4OH$ per $500 \ mL$? (Given: $K_b$ of $NH_4OH = 1.8 \times 10^{-5}$,Molar mass of $NH_4OH = 35 \ g \ mol^{-1}$)

For an aqueous solution of $H_2CO_3$,the ionization constants are $K_1 = 4.2 \times 10^{-7}$ and $K_2 = 4.8 \times 10^{-11}$. Which statement is correct for a $0.034 \ M$ saturated solution of carbonic acid?

$A$ weak monobasic acid is $3.0 \%$ dissociated in its $0.04 \ M$ solution. What is the dissociation constant of the acid?