Question #b54aa

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Question #b54aa

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Answer 1 · 2017-05-02T15:53:41

A Bronsted-Lowry base.

Explanation:

An Arrhenius base is a species than ionises in water to produce $O H^{-}$ $OH^-$ ions. Since $C a C O_{3}$ $CaCO_3$ contains no $O H^{-}$ $OH^-$ at all, it does not fulfil the definition of an Arrhenius base.

On the other hand, a Bronsted-Lowry base is a species that can accept a proton or $H^{+}$ $H^+$ ion from a Bronsted-Lowry acid. The carbonate ion is able to take in protons to firstly form the bicarbonate ion and then form carbonic acid.

$C O_{3}^{2 -} + H^{+} \to H C O_{3}^{-}$ $CO_3 ^ (2-) + H^+ -> HCO_3 ^-$
$H C O_{3}^{- +} H^{+} \to H_{2} C O_{3}$ $HCO_3 ^- + H^+ -> H_2 CO_3$

Carbonic acid is in equilibrium with $C O_{2}$ $CO_2$ and $H_{2} O$ $H_2 O$ .

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