Answer:
[tex]\rm Cu^{2+}\,(aq) + {CO_3}^{2-}\, (aq) \to CuCO_3 \, (s)[/tex].
Explanation:
Start by balancing the chemical equation. (In this question, the equation was already balanced.)
[tex]\rm Cu(NO_3)_2\, (aq) + Na_2 CO_3\, (aq) \to CuCO_3\, (s) + 2\, NaNO_3\, (aq)[/tex].
Go through all the chemicals in the equation. If the chemical is one of the followings, rewrite it as the ions it contains:
In this case, all four chemicals are salts. However, only the three of them are soluble: [tex]\rm (aq)[/tex]: [tex]\rm Cu(NO_3)_2[/tex], [tex]\rm Na_2 CO_3[/tex], and [tex]\rm NaNO_3[/tex].
After rewriting, the chemical equation becomes an ionic equation. However, this equation is not a "net" ionic equation due to all the duplicates.
[tex]\begin{aligned}&\rm Cu^{2+}\, (aq) + 2\, \rm {NO_3}^{-}\, (aq) + 2\, \rm Na^{+}\, (aq)+ \rm {NO_3}^{-}\, (aq) \cr & \to\rm CuCO_3\, (s) + 2\, Na^{+}\, (aq) + 2\, \rm {NO_3}^{-}\, (aq)\end{aligned}[/tex].
To obtain the net ionic equation, simply eliminate the duplicates.
[tex]\begin{aligned}&\rm Cu^{2+}\, (aq) + \rm {CO_3}^{2-}\, (aq)\to\rm CuCO_3\, (s)\end{aligned}[/tex].
