Answer is: the precipitate is Fe₂S₃ (iron(III) sulfide) and the spectator ions are Na⁺ and Cl⁻.
Balanced chemical reaction: 2FeCl₃(aq) + 3Na₂S(aq) → Fe₂S₃(s) + 6NaCl(aq).
Ionic reaction:
2Fe³⁺(aq) + 6Cl⁻(aq) + 6Na⁺(aq) + 3S²⁻(aq) → Fe₂S₃(s) + 6Na⁺(aq) + 6Cl⁻(aq).
Net ionic reaction: 2Fe³⁺(aq) + 3S²⁻(aq) → Fe₂S₃(s).
A spectator ion is an ion that exists as a reactant and a product in a chemical equation.
Taking into account the definition of net ionic equation, a precipitate of Fe₂S₃ is formed when aqueous solutions of Na₂S and FeCl₃ are mixed.
The net ionic equation is a chemical equation for a reaction that lists only the species that participate in the reaction.
In other words, an ionic equation is a chemical equation where electrolytes in aqueous solution are written as dissociated ions.
A spectator ion is an ion that appears both as a reactant and as a product in an ionic equation.
Spectator ions can be either cations (positively charged ions) or anions (negatively charged ions).
When writing a net ionic equation, spectator ions found in the original equation are ignored. Thus, the total ionic reaction is different from the net chemical reaction.
The balanced equation will be:
2 FeCl₃ (aq) + 3 Na₂S (aq) → Fe₂S₃ (s) + 6 NaCl(aq)
where (aq) means aqueous and (s) solid.
Taking into account that:
The total ionic equation in separated aqueous solution will be:
2 Fe³⁺(aq) + 6 Cl⁻(aq) + 6 Na⁺(aq) + 3 S²⁻(aq) → Fe₂S₃(s) + 6 Na⁺(aq) + 6 Cl⁻(aq)
In this case, Na⁺ and Cl⁻ are the spectator ions because they appear unchanged in both the product and the reagent. So these ions cancel out by writing the net ionic equation and you get:
2 Fe³⁺(aq) + 3 S²⁻(aq) → Fe₂S₃(s)
Since Fe₂S₃ is an insoluble salt, it will precipitate.
Finally, a precipitate of Fe₂S₃ is formed when aqueous solutions of Na₂S and FeCl₃ are mixed.
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