$A$ monobasic weak acid dissociates $2 \%$ in its $0.002 \ M$ solution. Calculate the dissociation constant of the weak acid.

Derive the expression for the ionization constant $(K_b)$ of a weak base.

Calculate the $pH$ of a solution containing $6.0 \ g$ of acetic acid $(CH_3COOH)$ in $250 \ mL$ of water. Given: $K_a = 1.8 \times 10^{-5}$ at $298 \ K$,and atomic masses are $C = 12, H = 1, O = 16$. (in $.57$)

The $pH$ of $0.004 \, M$ hydrazine solution is $9.7$. Calculate its ionization constant $K_{b}$ and $pK_{b}$.

Dissociation constant for a monobasic acid is $10^{-4}$. What is the $pH$ of the monobasic acid? (If $\%$ dissociation $= 2\,\%$)

An organic monobasic acid has a dissociation constant of $1.96 \times 10^{-8}$. What is its percentage dissociation in a $0.01 \text{ M}$ solution (in $\%$)?