Answer :
Answer:
[tex]2Ag^+(aq)+CO_3^{2-}(aq)\rightarrow Ag_2CO_3(s)[/tex]
Explanation:
Hello.
In this case, since the reaction is not given but a typical precipitation of silver from silver nitrate could be represented by its reaction with a soluble metallic sulfide or carbonate since silver carbonate and silver sulfide are insoluble, we can use for instance sodium carbonate to obtain:
[tex]2AgNO_3(aq)+Na_2CO_3(aq)\rightarrow Ag_2CO_3(s)+2NaNO_3(aq)[/tex]
Thus, since, silver nitrate, sodium carbonate and sodium nitrate are fully ionized by silver carbonate remains solid, the complete ionic equation is:
[tex]2Ag^+(aq)+2NO_3^-(aq)+2Na^+(aq)+CO_3^{2-}(aq)\rightarrow Ag_2CO_3(s)+2Na^+(aq)+2NO_3^-(aq)[/tex]
Then, since nitrate and sodium ions are the spectator ions since they are at both reactants and products, the net ionic equation turns out:
[tex]2Ag^+(aq)+CO_3^{2-}(aq)\rightarrow Ag_2CO_3(s)[/tex]
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