Convert a molecular equation to its complete ionic and net ionic equation, with spectator ions, the precipitate, and states from solubility rules.
Tap a reaction to solve it.
Enter a balanced equation with -> between sides. Add states like (aq), (s), (l), (g) to override the predicted ones.
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A net ionic equation strips a chemical reaction down to the ions and compounds that actually change — leaving out the spectator ions that float through unchanged. This calculator takes a balanced molecular equation, uses solubility rules to decide which compounds dissolve into ions, writes the complete ionic equation, cancels the spectator ions, and gives you the net ionic equation, the spectator ions, and any precipitate. It also shows why each compound got its state, so it teaches the method instead of just handing over an answer.
There are three ways to write an aqueous reaction. The molecular equation shows whole compounds (AgNO₃ + NaCl → AgCl + NaNO₃). The complete ionic equation splits every soluble strong electrolyte into its ions. The net ionic equation removes the spectator ions — those that appear unchanged on both sides — to show only the species that react (Ag⁺ + Cl⁻ → AgCl). Writing one requires knowing which compounds are aqueous (and dissociate) versus solid, liquid, or gas, which is where solubility rules come in.
The Method
Convert molecular equations to net ionic equations and check your answers.
See the rules applied to real compounds to predict precipitates.
Identify the precipitate and the net ionic equation for double-displacement reactions.
Get the classic H⁺ + OH⁻ → H₂O net ionic equation and its variations.
Quickly find which ions don't participate in a reaction.
Practice the three equation forms for general chemistry tests.
Get the molecular, complete ionic, and net ionic equations from one input.
See exactly which ions are spectators and which product is the precipitate.
Each compound's state is annotated with the rule that determined it — not just guessed for you.
If you already know the states, type (aq), (s), (l), or (g) and the calculator uses them.
A built-in solubility-rules reference and labeled steps make it a study aid, not just a solver.
Start with the balanced molecular equation and assign states. Split every aqueous strong electrolyte (soluble salts, strong acids, strong bases) into ions to get the complete ionic equation. Then cancel the spectator ions — those identical on both sides. What remains is the net ionic equation. For example, AgNO₃ + NaCl → AgCl + NaNO₃ becomes Ag⁺ + Cl⁻ → AgCl.
A spectator ion appears unchanged on both sides of the complete ionic equation — it doesn't take part in the reaction. For instance, in AgNO₃ + NaCl, the Na⁺ and NO₃⁻ ions are spectators because they stay dissolved before and after. They're cancelled to form the net ionic equation.
The complete (or total) ionic equation shows every dissolved strong electrolyte broken into its ions, including spectators. The net ionic equation removes the spectator ions, leaving only the species that actually react. The net ionic equation is the essence of the reaction.
Use solubility rules. Nitrates and Group 1 salts are always soluble (aqueous), while most carbonates, phosphates, and hydroxides are insoluble (solids). Halides are soluble except with silver, lead, and mercury. This calculator applies these rules and shows which one decided each state.
It's Ag⁺(aq) + Cl⁻(aq) → AgCl(s). Silver chloride is insoluble, so it precipitates, while the sodium and nitrate ions are spectators that stay in solution and cancel out.
If every ion is a spectator — meaning no precipitate, gas, or water forms — there is no net reaction. This happens when you mix two soluble salts that simply exchange partners without forming an insoluble product, such as NaCl + KNO₃.