The $pH$ of $0.001 \ M$ acetic acid is $.......$

Ionisation constant of $CH_3COOH$ is $1.7 \times 10^{-5}$ and concentration of $H^{+}$ ions is $3.4 \times 10^{-4} \ M$. Find the initial concentration of $CH_3COOH$ molecules.

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

Acetic acid dissociates to $1.20 \%$ in its $0.01 \ M$ solution. What is the value of its dissociation constant?

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 $\%$)

If a $0.1 \ N$ solution of $CH_3COOH$ is $1.3\%$ ionized,what will be the $pH$ of the solution? (Given: $\log 1.3 = 0.11$)