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

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 $\%$)?

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

$1.0 \ mol$ of $HCl$ and $1.0 \ mol$ of $CH_3COONa$ are dissolved in water to make a $1 \ L$ solution. What is the concentration of $H^+$ in the solution? ($K_a$ for $CH_3COOH = 1.6 \times 10^{-5}$)

$0.02 \, M$ monobasic acid dissociates $2 \%$,hence,$pH$ of the solution is

The concentration of $[CN^{-}]$ in $0.1 \, M \, HCN$ solution is: $(K_a = 4 \times 10^{-10})$