The dissociation constant of acetic acid is $10^{-6}$ and the dissociation constant of formic acid is $10^{-5}$. What is the value of $pK_a(\text{acetic acid}) - pK_a(\text{formic acid})$?

The first and second ionization constants of $H_2X$ are $2.5 \times 10^{-8}$ and $1.0 \times 10^{-13}$ respectively. The concentration of $X^{2-}$ in $0.1 \ M$ $H_2X$ solution is . . . . . . $\times 10^{-15} \ M$. The value of $Y$ is:

The $pH$ of a $0.1 \ M$ solution of the acid $HA$ is $3$. The value of the ionization constant,$K_a$ of this acid is

If the degree of dissociation is $1.30\%$,what is the $K_a$ for $0.1 \ M \ CH_3COOH$?

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

For a weak acid $HA$ with dissociation constant $10^{-9}$,the $pOH$ of its $0.1 \ M$ solution is: