Direct answer first: A net ionic equation for a precipitation reaction shows only the ions that form the insoluble solid (the precipitate) when two soluble ionic compounds are mixed, with spectator ions canceled. It is obtained by writing the full ionic form of the complete reaction, removing ions that appear on both sides, and balancing charge. Key steps to determine the net ionic equation

• 1. Write the soluble reactants as their constituent ions in solution.
  

• 2. Write the precipitate as a solid (do not dissociate).
  

• 3. Cancel spectator ions (ions that appear on both sides in the same form).
  

• 4. Balance both mass and charge to obtain the net ionic equation.
  

Example template

• For a typical precipitation reaction AB(aq) + CD(aq) → AD(s) + CB(aq), the net ionic equation concentrates on the ions that form the insoluble product:
  • If A+ and D− form the solid AD(s), the net ionic equation focuses on A+(aq) + D−(aq) → AD(s).
• If all products are soluble, no net ionic equation for a precipitate exists.

Common pitfalls and tips

• Do not include spectator ions (e.g., common ions like Na+, NO3−, Cl− that stay in solution).
• Ensure both sides have the same total charge; adjust coefficients as needed to balance charge when removing spectators.
• If no precipitate forms (i.e., all possible products are soluble), then no net ionic equation for a precipitation reaction exists.

If you share the specific reaction you’re studying (the two soluble reagents and their ions), the exact net ionic equation can be written step by step.