Dissociation constant of $0.01 \ M$ weak acid is $10^{-4}$. What is percent dissociation of acid (in $\%$)?

Calculate the value of the dissociation constant $(K_a)$ of a weak acid,which dissociates to $0.01 \%$ in its $0.1 \ M$ solution.

$K_{a}$ for butyric acid $(C_{3}H_{7}COOH)$ is $2 \times 10^{-5}$. The $pH$ of $0.2 \ M$ solution of butyric acid is $........... \times 10^{-1}$. (Nearest integer) [Given $\log 2 = 0.30$]

Calculate the $pH$ of a $0.08 \ M$ solution of hypochlorous acid,$HOCl$. The ionization constant of the acid is $2.5 \times 10^{-5}$. Determine the percent dissociation of $HOCl$.

The ionization constant of $0.1$ $M$ weak acid is $1.74 \times 10^{-5}$ at $298$ $K$ temperature. Calculate the $pH$ of its $0.1$ $M$ solution. (in $.88$)

$A$ monobasic weak acid dissociates to $1.2 \%$ in its $0.01 \ M$ solution at $298 \ K$. Calculate the dissociation constant of it.