Write the net ionic equation for the precipitation of iron(II) sulfide from aqueous solution:
To write the net ionic equation for the precipitation of iron(II) sulfide from aqueous solution, we need to first write the balanced chemical equation for the reaction. The reactants in this case are iron(II) ions (Fe^2+) and sulfide ions (S^2-), which combine to form solid iron(II) sulfide (FeS).
The balanced chemical equation is as follows:
Fe^2+ (aq) + S^2- (aq) → FeS (s)
Now, let's break down the equation into its ionic components:
Fe^2+ (aq) + S^2- (aq) → FeS (s)
In this equation, Fe^2+ (aq) and S^2- (aq) are the ions that are present in aqueous solution, while FeS (s) represents the solid iron(II) sulfide that precipitates out.
Finally, we can write the net ionic equation by removing the spectator ions, which are ions that do not take part in the overall reaction. In this case, the spectator ions are Fe^2+ and S^2-.
The net ionic equation for the precipitation of iron(II) sulfide from aqueous solution is:
Fe^2+ (aq) + S^2- (aq) → FeS (s)
To write the net ionic equation for the precipitation of iron(II) sulfide (FeS) from aqueous solution, we need to first write the balanced chemical equation and then determine the species that exist in the solution in their ionic forms.
1. Write the balanced chemical equation:
Fe2+ (aq) + S2- (aq) → FeS (s)
2. Identify the species in the equation:
In the given equation, we have Fe2+ and S2- ions. These are the ionic forms of iron(II) and sulfide, respectively.
3. Determine the spectator ions:
The spectator ions are the ions that remain unchanged throughout the reaction. In this case, the spectator ion is Fe2+.
4. Write the net ionic equation:
The net ionic equation is obtained by removing the spectator ions from the balanced equation. In this case, we remove Fe2+ from both sides of the equation:
S2- (aq) → FeS (s)
Thus, the net ionic equation for the precipitation of iron(II) sulfide is S2- (aq) → FeS (s).