What is the complete ionic equation for the following reaction? Aqueous iron(III) sulfate is added to aqueous sodium sulfide to produce solid iron(III) sulfide and aqueous sodium sulfate.

Ionize all compounds except iron(III) sulfide which is a ppt driving force.

To determine the complete ionic equation for the given reaction, we need to identify the ionic compounds involved and break them down into their respective ions. Here's how you can get the answer:

Step 1: Write the balanced chemical equation for the reaction.
Fe2(SO4)3(aq) + 3 Na2S(aq) → Fe2S3(s) + 3 Na2SO4(aq)

Step 2: Identify the ionic compounds.
In this reaction, the ionic compounds are iron(III) sulfate (Fe2(SO4)3) and sodium sulfide (Na2S).

Step 3: Write the dissociation equations.
The dissociation equation for iron(III) sulfate is:
Fe2(SO4)3 → 2 Fe^3+(aq) + 3 SO4^2-(aq)

The dissociation equation for sodium sulfide is:
2 Na2S → 4 Na+(aq) + S^2-(aq)

Step 4: Formulate the complete ionic equation.
Substitute the dissociated ions into the balanced chemical equation:
2 Fe^3+(aq) + 3 SO4^2-(aq) + 4 Na+(aq) + S^2-(aq) → Fe2S3(s) + 3 Na+(aq) + 3 SO4^2-(aq)

Step 5: Simplify the equation by removing the spectator ions.
The spectator ions are the ones that remain unchanged on both sides of the equation. In this case, the spectator ions are the sulfate ions (SO4^2-) on both sides.

Therefore, the complete ionic equation for the reaction is:
2 Fe^3+(aq) + S^2-(aq) + 4 Na+(aq) → Fe2S3(s) + 3 Na+(aq)