The degree of dissociation of $0.1 \, M \, HCN$ solution is $0.01 \%$. Its ionisation constant would be

Derive the equation for the ionization constant $K_a$ of a weak acid $HX$.

The $pH$ of a $0.1 \ M$ solution of the acid $HQ$ is $3$. The value of the ionization constant,$K_a$ of the acid is:

The percentage of pyridine $(C_5H_5N)$ that forms pyridinium ion $(C_5H_5N^{+}H)$ in a $0.10 \ M$ aqueous pyridine solution ($K_b$ for $C_5H_5N = 1.7 \times 10^{-9}$) is (in $\%$)

At $25^{\circ} C$,the percentage of ionization of $x \ M$ acetic acid is $4.242$. What is the pH of the acetic acid solution?
$(\log 4.242=0.6275) ;(\log 0.04242=-1.372) \quad (K_a=1.8 \times 10^{-5})$

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