$0.2 \ M$ solution of formic acid is ionized $3.2 \%$. Its ionization constant is:

If the degree of ionisation is $0.01$ for a decimolar solution of a weak acid $HA$,then the $pKa$ of the acid 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 $NH_4OH = 35 \ g \ mol^{-1}$)

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

At $T$ $(K)$,if the ionisation constant of ammonia in solution is $2.5 \times 10^{-5}$,the $pH$ of $0.01 \ M$ ammonia solution and the ionisation constant of its conjugate acid respectively at that temperature are $(\log 2 = 0.30)$

The percentage dissociation of a decinormal solution of a weak acid $HA$ is: $(K_a = 4.9 \times 10^{-8})$