Convert molecular chemical equations into complete total ionic equations, cancel spectator ions, and derive simplified, charge-balanced net ionic equations with physical state designations using our free Net Ionic Equation Calculator.
Spectator Ions Cancelled • Mass & Charge Conserved
Insoluble Solid
Na⁺ & NO₃⁻
Ag⁺ + Cl⁻
Stoichiometric
Net Neutral
Halide Exception
A Net Ionic Equation is a simplified chemical equation that depicts exclusively the chemical species (dissolved cations, anions, insoluble precipitate lattices, liquid water molecules, or evolved gases) that actively participate in a chemical transformation within an aqueous solution:
When soluble strong electrolytes dissolve in water, the high dielectric constant of water (\(\epsilon_r \approx 78.4\) at \(25\text{ }^\circ\text{C}\)) breaks apart ionic crystalline lattices into freely solvated hydrated ions. While standard molecular equations portray all substances as intact neutral molecules, only a fraction of those ions undergo bond formation, phase changes, or proton transfers. Spectator ions exist identically on both reactant and product sides of the complete ionic equation; cancelling them isolates the true driving force of the reaction in the net ionic equation.
Prevents incorrectly splitting weak electrolytes (such as acetic acid \(\text{CH}_3\text{COOH}\)), insoluble salts (\(\text{BaSO}_4\)), and gases into separate ions.
Identifies non-participating bystander ions (such as \(\text{Na}^+, \text{NO}_3^-, \text{K}^+\)) and removes them cleanly while maintaining stoichiometric balance.
Guarantees that both atomic molar counts and net electrical charges on the reactant side equal the product side simultaneously.
Instantly displays the Balanced Molecular Equation, the Complete (Total) Dissociated Ionic Equation, and the final Simplified Net Ionic Equation side-by-side.
Highlights cancelled spectator ions with custom strikethrough badges, illustrating exactly which species remain chemically inert in the aqueous matrix.
Applies standard aqueous solubility guidelines to categorize products automatically as insoluble precipitates \((s)\), soluble electrolytes \((aq)\), pure liquids \((l)\), or gases \((g)\).
Copies clean, publication-ready chemical equations directly to your clipboard for use in lab reports, chemistry problem sets, and academic manuscripts.
| Ion Category | Generally Soluble \((aq)\) | Important Insoluble Exceptions \((s)\) |
|---|---|---|
| Group 1 & Ammonium | \(\text{Li}^+, \text{Na}^+, \text{K}^+, \text{Rb}^+, \text{Cs}^+, \text{NH}_4^+\) | None (Universally Soluble) |
| Nitrates & Acetates | \(\text{NO}_3^-, \text{C}_2\text{H}_3\text{O}_2^-\) / \(\text{CH}_3\text{COO}^-, \text{ClO}_4^-\) | None (Always Soluble) |
| Halides (Chlorides, Bromides, Iodides) | \(\text{Cl}^-, \text{Br}^-, \text{I}^-\) | \(\text{Ag}^+, \text{Pb}^{2+}, \text{Hg}_2^{2+}\) (e.g. \(\text{AgCl}, \text{PbI}_2\)) |
| Sulfates | \(\text{SO}_4^{2-}\) | \(\text{Ba}^{2+}, \text{Pb}^{2+}, \text{Ca}^{2+}, \text{Sr}^{2+}\) (e.g. \(\text{BaSO}_4\)) |
| Hydroxides & Carbonates | Insoluble except Group 1 & \(\text{NH}_4^+\) | \(\text{CaCO}_3, \text{Fe(OH)}_3, \text{Cu(OH)}_2, \text{BaCO}_3\) |
Pick a classic reaction preset (such as \(\text{AgCl}\), \(\text{BaSO}_4\), \(\text{PbI}_2\), Acid-Base Neutralization) or input custom chemical formulas.
Specify physical states for products: \((s)\) for solid precipitates, \((aq)\) for dissolved salts, \((l)\) for liquid water, and \((g)\) for gases.
Click "Derive Net Ionic Equation" to generate the complete total ionic equation, strip spectator ions, and format the net result.
Review the step-by-step KaTeX derivation, verify mass/charge conservation, and copy formatted equations directly into your lab notebook.
Problem: When aqueous lead(II) nitrate is combined with aqueous potassium iodide, bright yellow crystals of lead(II) iodide precipitate out of solution. Derive the molecular, complete ionic, and net ionic equations.
1. Balanced Molecular Equation:
2. Complete Ionic Equation:
3. Net Ionic Equation (Spectators \(2\text{K}^+\) and \(2\text{NO}_3^-\) Cancelled):
Problem: Aqueous acetic acid (\(\text{CH}_3\text{COOH}\)) reacts with sodium hydroxide (\(\text{NaOH}\)). Because acetic acid is a weak electrolyte (\(<5\%\) ionized), it does not dissociate fully in the net ionic equation.
1. Molecular: \(\text{CH}_3\text{COOH}(aq) + \text{NaOH}(aq) \longrightarrow \text{CH}_3\text{COONa}(aq) + \text{H}_2\text{O}(l)\)
2. Complete Ionic: \(\text{CH}_3\text{COOH}(aq) + \text{Na}^+(aq) + \text{OH}^-(aq) \longrightarrow \text{CH}_3\text{COO}^-(aq) + \text{Na}^+(aq) + \text{H}_2\text{O}(l)\)
3. Net Ionic (\(\text{Na}^+\) Cancelled):
Never dissociate weak acids (such as \(\text{HF}, \text{CH}_3\text{COOH}, \text{HCN}, \text{H}_2\text{CO}_3\)) into separated ions. Only the 6 strong acids (\(\text{HCl}, \text{HBr}, \text{HI}, \text{HNO}_3, \text{HClO}_4, \text{H}_2\text{SO}_4\)) fully dissociate.
Do not break internal covalent bonds within polyatomic groups. For instance, \(\text{SO}_4^{2-}\) dissociates as a single unit, never into separated sulfur and oxygen atoms.
Solid precipitates like \(\text{BaSO}_4(s)\) or \(\text{AgCl}(s)\) have negligible aqueous solubility. They must remain intact in solid crystalline form on the product side.
Always check that the sum of positive and negative charges on the reactant side exactly equals the net charge on the product side (e.g. \(+2 + 2(-1) = 0\)).
Environmental facilities treat electroplating wastewater containing toxic lead (\(\text{Pb}^{2+}\)) or cadmium (\(\text{Cd}^{2+}\)) by injecting sodium sulfide (\(\text{Na}_2\text{S}\)). The net ionic reaction \(\text{Pb}^{2+}(aq) + \text{S}^{2-}(aq) \to \text{PbS}(s)\) precipitates lead down to parts-per-billion limits.
Water treatment plants remove hard-water calcium ions (\(\text{Ca}^{2+}\)) by adding slaked lime (\(\text{Ca(OH)}_2\)). The net ionic reaction \(\text{Ca}^{2+}(aq) + \text{CO}_3^{2-}(aq) \to \text{CaCO}_3(s)\) precipitates scale-forming calcium carbonate out of drinking water grids.
Authoritative answers to common questions regarding net ionic equations, spectator ions, and solubility rules.
