At $298 \ K$,$0.1 \ M$ solution of acetic acid is $1.34 \ \%$ ionized. What is the dissociation constant of acetic acid?

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 $HOCl$.

What is the percentage dissociation of $0.1 \ M$ acetic acid (in $\%$)? $(K_a = 10^{-5})$

The $K_a$ of monobasic acid $A, B$ and $C$ are $10^{-6}, 10^{-8}$ and $10^{-10}$ respectively. The concentrations of $A, B$ and $C$ are respectively $0.1 \ M, 0.01 \ M$ and $0.001 \ M$. Which of the following is correct for $pOH$ of $A, B$ and $C$?

Sulphurous acid $(H_{2}SO_{3})$ has $Ka_{1} = 1.7 \times 10^{-2}$ and $Ka_{2} = 6.4 \times 10^{-8}$. The $pH$ of $0.588 \ M \ H_{2}SO_{3}$ is ..... . (Round off to the Nearest Integer)

$A$ weak monobasic acid is $2 \%$ dissociated in its $0.1 \ M$ solution. What is its dissociation constant?