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 $\%$)

What is the percent dissociation of acetic acid in its $0.01 \ M$ solution if the dissociation constant of the acid is $1.34 \times 10^{-6}$ (in $\%$)?

$1.0 \ mol$ of $HCl$ and $1.0 \ mol$ of $CH_3COONa$ are dissolved in water to make a $1 \ L$ solution. What is the concentration of $H^+$ in the solution? ($K_a$ for $CH_3COOH = 1.6 \times 10^{-5}$)

At $27^{\circ} C$,the degree of dissociation of a weak acid $(HA)$ in its $0.5 \ M$ aqueous solution is $1 \%$. Its $K_{a}$ value is approximately:

$pH$ of $0.05 \ M$ aqueous solution of diethyl amine is $10$. The value of equilibrium constant $(K_b)$ is:

The ionization constant of $HF$ is $3.2 \times 10^{-4}$. Calculate the degree of dissociation of $HF$ in its $0.02 \ M$ solution. Calculate the concentration of all species present ($H_{3}O^{+}$,$F^{-}$ and $HF$) in the solution and its $pH$.