Net Ionic Equation Calculator
Convert a molecular equation to its complete ionic and net ionic forms. Identify which ions are spectators and which form products.
Enter as: Formula or Formula(aq)
Enter as: Formula or Formula(aq)
What is a net ionic equation?
A net ionic equation shows only the species that actually participate in the reaction, removing spectator ions. For example, NaCl(aq) + AgNO₃(aq) → AgCl(s) + NaNO₃(aq) becomes Ag⁺(aq) + Cl⁻(aq) → AgCl(s).
What are spectator ions?
Spectator ions are ions present in the solution that do not participate in the chemical reaction. They appear on both sides of a complete ionic equation and cancel out. Common examples include Na⁺, K⁺, NO₃⁻, and most alkali metal and nitrate ions.
How do I identify strong electrolytes?
Strong electrolytes completely dissociate in water: strong acids (HCl, HBr, HI, HNO₃, H₂SO₄, HClO₄), strong bases (NaOH, KOH, Ca(OH)₂, Ba(OH)₂), and soluble salts. Weak electrolytes partially dissociate (weak acids, weak bases, insoluble salts).
What makes a reaction go to completion?
Reactions go to completion when a precipitate forms, a gas evolves, or water is produced (neutralization). Look for: AgCl, BaSO₄, PbI₂ (insoluble), CO₂, SO₂ (gases), or H₂O (from strong acid-strong base).
Can all ionic compounds form net ionic equations?
Only ionic compounds that dissolve in water (aqueous) can be written as separate ions. Solids (s), liquids (l), and gases (g) are written as intact species. Insoluble compounds remain as complete formulas.
What is the difference between complete ionic and net ionic?
Complete ionic shows all dissociated ions: 2Ag⁺(aq) + 2NO₃⁻(aq) + 2Na⁺(aq) + 2Cl⁻(aq) → 2AgCl(s) + 2Na⁺(aq) + 2NO₃⁻(aq). Net ionic removes spectators: 2Ag⁺(aq) + 2Cl⁻(aq) → 2AgCl(s).