Net Ionic Equation Calculator
Mixing sodium chloride and silver nitrate produces a white precipitate of silver chloride, AgCl. This net ionic equation calculator shows the molecular, total ionic, and net ionic equations for common double displacement reactions. Select two aqueous ionic compounds, and the tool identifies any precipitate, the spectator ions, and the net ionic equation, the one that shows only the ions directly involved in forming the solid.
Quick answer
The molecular equation shows the full formulas of all reactants and products.
Net Ionic Equation
Ag+(aq) + Cl-(aq) → AgCl(s)
Molecular Equation
NaCl(aq) + AgNO3(aq) → AgCl(s) + NaNO3(aq)
Total Ionic Equation
Na+(aq) + Cl-(aq) + Ag+(aq) + NO3-(aq) → AgCl(s) + Na+(aq) + NO3-(aq)
Spectator Ions
Na+, NO3-
Precipitate
AgCl (silver chloride)
What this tells you
- •The molecular equation shows the full formulas of all reactants and products.
- •The total ionic equation splits every aqueous ionic compound into its individual ions.
- •The net ionic equation cancels spectator ions that appear unchanged on both sides.
- •Spectator ions remain dissolved in solution and do not participate in the reaction.
- •A precipitate forms when two ions combine to make an insoluble solid.
- •This tool covers five common reaction pairs taught in high school and introductory college chemistry.
How to Use
- 1Select the two aqueous reactant compounds from the dropdowns.
- 2The calculator immediately shows all four equation forms.
- 3Spectator ions are listed separately so you can see what cancels out.
How It Works
Formula
net ionic = total ionic - spectator ionsStart with the molecular equation showing complete compound formulas. Split all aqueous compounds into their individual ions to get the total ionic equation. Then cancel any ion that appears in the same form on both the reactant and product sides. What remains is the net ionic equation, which shows only the ions that combine to form the solid precipitate. For NaCl and AgNO3, Na+ and NO3- appear unchanged on both sides and are spectator ions, leaving Ag+(aq) + Cl-(aq) → AgCl(s).
Calculation note: values are processed in the order shown above, using the current input units.
Worked Examples
NaCl + AgNO3
A white precipitate of silver chloride forms. Sodium and nitrate are spectator ions.
Common Precipitates
| Reaction | Precipitate | Color |
|---|---|---|
| NaCl + AgNO3 | AgCl | White |
| BaCl2 + Na2SO4 | BaSO4 | White |
| Pb(NO3)2 + KI | PbI2 | Bright yellow |
| CuSO4 + NaOH | Cu(OH)2 | Blue |
| CaCl2 + Na2CO3 | CaCO3 | White |
Common mistakes
- Forgetting to balance charges. The net ionic equation must be balanced for both mass and charge.
- Including spectator ions in the net ionic equation. Only ions that change their state belong in the net ionic equation.
- Writing a precipitate that is actually soluble. Not all double displacement reactions produce a solid.
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