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

The $pH$ of an aqueous solution of $H_2CO_3$ is $3.3$. If ${K_{a_1}} = {10^{-3}}$ and ${K_{a_2}} = {10^{-13}}$,then the concentration of $[HCO_3^-]$ is:

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.

What is the $pH$ of $10^{-1} \, M$ formic acid?

The $pK_a$ of a weak acid is $5.85$. The concentrations of the acid and its conjugate base are equal at a $pH$ of (in $.85$)

The $pH$ of $0.01 \ M$ solution of acetic acid is $5.0$. What are the values of $[H^{+}]$ and $K_a$ respectively?