The $pH$ of a $1.0 \ M$ monobasic acid $HX$ is $2$. The van't Hoff factor for the aqueous solution of the acid will be ........

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

$A$ weak monobasic acid is $20 \%$ dissociated in its $0.01 \ M$ solution. What is the dissociation constant of the weak acid?

The dissociation constant of an acid $HA$ is $1 \times 10^{-5}$. The $pH$ of $0.1 \ M$ solution of the acid will be

$1.0 \ mol$ 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 $CH_3COOH = 1.6 \times 10^{-5}$)