When aqueous solutions of and are mixed

CHEMISTRY · Single correct · A Level · Chemistry · Reactions of ions in aqueous solution · Reactions of ions in aqueous solution

Problem

When aqueous solutions of Na2CO3\mathrm{Na_2CO_3} and HCl\mathrm{HCl} are mixed, the net ionic equation is 2H+(aq)+CO32−(aq)→CO2(g)+H2O(l)2\mathrm{H^+}(aq)+\mathrm{CO_3^{2-}}(aq)\rightarrow \mathrm{CO_2}(g)+\mathrm{H_2O}(l) Which of the following best explains why Na+\mathrm{Na^+} and Cl−\mathrm{Cl^-} are omitted from the net ionic equation? (a) They combine to form aqueous NaCl\mathrm{NaCl}, so the compound rather than the separate ions is shown in the equation. (b) Being a Group 1 cation and a halide anion, Na+\mathrm{Na^+} and Cl−\mathrm{Cl^-} are always left out of net ionic equations by convention. (c) They remain as aqueous ions that do not participate in the chemical change. (d) They precipitate together as NaCl(s)\mathrm{NaCl(s)}, which is then removed before the net ionic equation is written.

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