Which equation best represents the net ionic equation for the reaction that occurs when aqueous solutions of potassium phosphate and iron(II) nitrate are mixed? Question 8 options: 3Fe2+(aq) + 2PO43–(aq) → Fe3(PO4)2(s) 2K+(aq) + Fe(NO3)2(aq) → 2KNO3(aq) + Fe2+(aq) 3Fe2+(aq) + 2PO43–(aq) → Fe3(PO4)2(aq) 2K3PO4(aq) + 3Fe2+(aq) → Fe3(PO4)2(s) + (K+)6(aq) 2K3PO4(aq) + 3Fe(NO3)2(aq) → Fe3(PO4)2(s) + 6KNO3(aq)

2PO₄³⁻ + 3Fe²⁺ → Fe₃(PO₄)₂(s)

Explanation:

In a net ionic equation you list only the ions that are participating in the reaction.

When potassium phosphate, K₃PO₄, reacts with iron (II) nitrate, Fe(NO₃)₂ producing iron (II) phosphate, Fe₃(PO₄)₂ that is an insoluble salt. The reaction is:

2K₃PO₄ + 3 Fe(NO₃)₂ → Fe₃(PO₄)₂(s) + 6NO₃⁻ + 6K⁺

The ionic equation is:

6K⁺ + 2PO₄³⁻ + 3Fe²⁺ + 6NO₃⁻→ Fe₃(PO₄)₂(s) + 6NO₃⁻ + 6K⁺

Subtracting the K⁺ and NO₃⁻ ions that are not participating in the reaction, the net ionic equation is:

a