Question #65be7

2$A {g}^{+}$(aq) + $C {O}_{3}^{-} 2$(aq) -> $A {g}_{2} C {O}_{3}$(s)

Explanation:

The steps involved are:
* Write the skeleton equation

$A g N {O}_{3}$(aq) + $N {a}_{2} C {O}_{3}$(aq) -> $A {g}_{2} C {O}_{3}$(s) + $N a N {O}_{3}$(aq)
note: you know the silver carbonate is the precipitate(s) because nitrate compounds are always water soluble

*Write the (aq) compounds show show the ions have been pulled apart by the dissolving properties of water

$A {g}^{+}$(aq) + $N {O}_{3}^{-}$(aq) + $N {a}^{+}$(aq) + $C {O}_{3}^{-} 2$(aq) ->
$A {g}_{2} C {O}_{3}$(s) + $N {a}^{+}$(aq) + $N {O}_{3}^{-}$(aq)

*Identify spectator ions which exist in the dissolved state as both reactants and products and cross them out then re-write the remaining ions and precipitated compound.
($N {a}^{+}$(aq) and $N {O}_{3}^{-}$(aq) are the spectator ions)

$A {g}^{+}$(aq) + $C {O}_{3}^{-} 2$(aq) -> $A {g}_{2} C {O}_{3}$(s)

Now balance number of ions and charges to find the final answer shown at the top.

Here is a video which gives another example of how to write a net ionic equation for a precipitation reaction.

Hope this helps!