1. Write the balanced molecular equation:
Fe(NO₃)₃(aq) + 3NH₃(aq) + 3H₂O(l) → Fe(OH)₃(s) + 3NH₄NO₃(aq)
2. Identify the soluble ionic compounds:
* Fe(NO₃)₃(aq): Iron(III) nitrate is soluble in water.
* NH₃(aq): Ammonia is soluble in water, but it's a weak base.
* NH₄NO₃(aq): Ammonium nitrate is soluble in water.
* Fe(OH)₃(s): Iron(III) hydroxide is insoluble in water.
3. Write the complete ionic equation:
Fe³⁺(aq) + 3NO₃⁻(aq) + 3NH₃(aq) + 3H₂O(l) → Fe(OH)₃(s) + 3NH₄⁺(aq) + 3NO₃⁻(aq)
4. Cancel out the spectator ions (ions that appear on both sides of the equation):
The nitrate ions (NO₃⁻) are spectator ions.
5. Write the net ionic equation:
Fe³⁺(aq) + 3NH₃(aq) + 3H₂O(l) → Fe(OH)₃(s) + 3NH₄⁺(aq)
Therefore, the net ionic equation for the reaction between iron(III) nitrate and ammonia is:
Fe³⁺(aq) + 3NH₃(aq) + 3H₂O(l) → Fe(OH)₃(s) + 3NH₄⁺(aq)
