The $pH$ of $0.05 \ M$ acetic acid is $(K_a = 2 \times 10^{-5})$.

What is the value of $pH$ of a $NaOH$ solution that dissociates $2 \%$ in its $0.01 \ M$ solution?

$pH$ value of a solution,whose hydronium ion concentration is $6.2 \times 10^{-9} \ mol/L$,is

The $pH$ of $0.1 \ M$ acetic acid is $3$. The dissociation constant of the acid will be:

Nicotinic acid $(K_a = 10^{-5})$ is represented by the formula $HNiC$. Calculate the percentage of dissociation in a solution containing $0.1 \ mol$ of nicotinic acid in $2 \ L$ of solution.

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