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 the carbonic acid.
The concentration of $CO_3^{2-}$ is $0.034\, M.$
The concentration of $CO_3^{2-}$ is greater than that of $HCO_3^-.$
The concentrations of $H^+$ and $HCO_3^-$ are approximately equal.
The concentration of $H^+$ is double that of $CO_3^{2-}.$
A weak base $MOH$ of $0.1\, N$ concentration shows a $pH$ value of $9$. What is the percentage degree of ionisation of the base ? ......$\%$
A $0.1\,N $ solution of an acid at room temperature has a degree of ionisation $ 0.1$ . The concentration of $O{H^ - }$ would be
A solution of weak acid $HA$ containing $0.01$ moles of acid per litre of solutions has $pH = 4$. The percentage degree of ionisation of the acid and the ionisation constant of acid are respectively.
Find $pH$ of $5 \times 10^{-3}\, M$ $H_2CO_3$ solution having $10\%$ dissociation
$25$ $mL$ $0.1$ $M$ $HCl$ solution is diluted till $500$ $mL$. Calculate $pH$ of dilute solution.