An organic monobasic acid has a dissociation constant of $2.25 \times 10^{-6}$. What is the percent dissociation in its $0.01 \ M$ solution (in $\%$)?

The dissociation constant of a weak monobasic acid is $2.7 \times 10^{-5}$. If the degree of dissociation of the acid is $3 \times 10^{-2}$,what is the concentration of the acid (in $M$)?

The $pH$ of a $0.1 \ M$ solution of acetic acid will be (degree of dissociation of acetic acid is $0.0132$).

In aqueous solution,the ionization constants for carbonic acid are $K_1 = 4.2 \times 10^{-7}$ and $K_2 = 4.8 \times 10^{-11}$. Select the correct statement for a saturated $0.034 \ M$ solution of carbonic acid.

$A$ weak monobasic acid dissociates to $0.001 \%$ in its $0.01 \ M$ solution. What is its dissociation constant?

For a $0.1 \ M$ solution of a weak acid $HA$ $(K_a = 1.4 \times 10^{-5})$ in $2 \ L$ of solution,calculate the percentage of dissociation and the $pH$ of the solution.