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.

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The concentration of ${CO}_{3}^{2 -}$ is $0.034 M$

The concentration of ${CO}_{3}^{2 -}$ is greater than that of ${HCO}_{3}^{-}$

The concentration of $H^{+}$ and ${HCO}_{3}^{-}$ are approximately equal

The concentration of $H^{+}$ is double that of ${CO}_{3}^{2 -}$

answer is C.

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Detailed Solution

For the carbonic acid of saturated $0.034 M$ solution,

$\begin{array}{l} [H_{2} {CO}_{3}] = 0.034 \\ = [{CO}_{3}^{2 -}] + [{HCO}_{3}^{-}] \end{array}$

$[{CO}_{3}^{2 -}] < [H {CO}_{3}^{-}]$ because $k_{1} >> k_{2}$

$[H^{+}] ≅ [{HCO}_{3}^{-}]$

Thus, the concentration of $H^{+}$ and ${HCO}_{3}^{-}$ are approximately equal.

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