Final answer:
The balanced net ionic equation for the reaction of aqueous iron(III) nitrate and potassium phosphate forming iron(III) phosphate and potassium nitrate is: Fe³⁺(aq) + PO₄³⁺(aq) → FePO₄(s). This reaction adheres to the double replacement principle and the net ionic equation is balanced by mass and charge.
Step-by-step explanation:
To write the balanced net ionic equation for the reaction when aqueous solutions of iron(I) nitrate and potassium phosphate are mixed, we first need to recognize that iron(I) is unusually unstable and it is typically found in the +2 or +3 oxidation states as iron(II) or iron(III). Assuming it is a typo and referring to iron(III), which is Fe3+, we can proceed.
The initial step is identifying the products formed when these reactants are combined by following the double replacement reaction principle. Iron(III) phosphate and potassium nitrate are expected to form, with the iron(III) phosphate being insoluble in water and precipitating out of solution.
The molecular equation: Fe(NO3)3(aq) + K3PO4(aq) → FePO4(s) + 3 KNO3(aq)
To obtain the net ionic equation, we write the complete ionic equation and remove the spectator ions (potassium and nitrate ions).
The complete ionic equation: Fe3+(aq) + 3 NO3−(aq) + 3 K+(aq) + PO43−(aq) → FePO4(s) + 3 K+(aq) + 3 NO3−(aq)
The net ionic equation: Fe3+(aq) + PO43−(aq) → FePO4(s)
This equation is balanced by mass and charge, with each side of the equation having one iron (Fe), one phosphate (PO4), and a net charge of zero.