In the following reaction $[C u (H_{2} O)_{4}]^{2 +} (a q) + H C O_{3}^{-} (a q) ⇌ [C u (H_{2} O)_{4} O H^{-}]^{+} (a q) + H_{2} C O_{3} (a q)$
species behaving as a bronsted- lowry acid are:

[C u (H_{2} O)_{4}]^{2 +}, H C O_{3}^{-}

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H C O_{3}^{-}, [C u (H_{2} O)_{4} O H^{-}]^{+}

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[C u (H_{2} O)_{4}]^{2 +}, H_{2} C O_{3}

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[H C O_{3}^{-}, H_{2} C O_{3}

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Solution

The correct option is C $[C u (H_{2} O)_{4}]^{2 +}, H_{2} C O_{3}$
According to Bronsted- lowry acid concept acids are ions or molecules which have tendency to donate protons.
$[C u (H_{2} O)_{4}]^{2 +}$ will donate a proton to $H C O_{3}^{-}$
so, $H C O_{3}^{-}$ (base) changes to $H_{2} C O_{3}$ (acid)
hence both $[C u (H_{2} O)_{4}]^{2 +}$ and $H_{2} C O_{3}$ behaving as a bronsted- lowry acid.

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[C u (H_{2} O)_{4}]^{2 +} (a q) + H C O_{3}^{-} (a q) ⇌ [C u (H_{2} O)_{4} O H^{-}]^{+} (a q) + H_{2} C O_{3} (a q)

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Identify Bronsted acids in the reaction : $H_{2} C O_{3} + H P O_{4}^{2 -} ⇌ H_{2} P O_{4}^{-} + H C O_{3}^{-}$

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