How do we represent the reaction of hydrochloric acid with stoichiometric calcium carbonate? Do we need to consider oxidation states?

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How do we represent the reaction of hydrochloric acid with stoichiometric calcium carbonate? Do we need to consider oxidation states?

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Answer 1 · 2017-05-27T14:19:37

This is an acid-base reaction, in which no redox transfer occurs........

Explanation:

We can write out the stoichiometric equation:

$C a C O_{3} (s) + 2 H C l (a q) \to C a C l_{2} (a q) + C O_{2} (g) + H_{2} O (l)$ $CaCO_3(s) + 2HCl(aq) rarr CaCl_2(aq) + CO_2(g) +H_2O(l)$

And the net ionic equation:

$C O_{3}^{2 -} + 2 H_{3} O^{+} \to C O_{2} (g) ↑ ⏐ ⏐ + 3 H_{2} O (l)$ $CO_3^(2-) + 2H_3O^(+) rarr CO_2(g)uarr +3H_2O(l)$

And we can include oxidation numbers on reactants and products:

$+ I V C O_{3}^{2 -} + 2 H_{3} O^{+} \to + I V C O_{2} (g) ↑ ⏐ ⏐ ⏐ + 3 H_{2} O (l)$ $stackrel(+IV)CO_3^(2-) + 2H_3O^(+) rarr stackrel(+IV)CO_2(g)uarr +3H_2O(l)$

Are these equations balanced with respect to mass and charge? They need to be if we purport to represent chemical reality!

The oxidation numbers of hydrogen and carbon remain at $- I I O$ $stackrel(-II)O$ and $+ I H$ $stackrel(+I)H$ respectively.

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How do we represent the reaction of hydrochloric acid with stoichiometric calcium carbonate? Do we need to consider oxidation states?

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Explanation:

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