Equation balancer and net ionic equations
Balance any equation, then get the full ionic and net ionic equations with states and spectator ions.
Use + between substances and -> between the sides. Formulas are case-sensitive (Co is cobalt, CO is carbon monoxide). States are optional: add (s), (l), (g) or (aq) after a formula to set them yourself. Write ion charges after a ^, like Fe^3+ or SO4^2-.
BIE, FIE and NIE
The balanced equation (BIE) writes every substance as a complete formula with the smallest whole-number coefficients. The full ionic equation (FIE), also called the total or complete ionic equation, splits every dissolved strong electrolyte into its ions. The net ionic equation (NIE) then removes the spectator ions, the ions that appear unchanged on both sides, leaving only the species that actually react.
What gets split into ions
Only strong electrolytes in solution are split: soluble ionic compounds (aq), strong acids (HCl, HBr, HI, HNO₃, H₂SO₄, HClO₄, HClO₃) and strong bases (group 1 hydroxides, Ca(OH)₂, Sr(OH)₂, Ba(OH)₂). Solids, liquids, gases, water, weak acids such as HC₂H₃O₂ and HF, weak bases such as NH₃, and molecular compounds stay written as whole formulas.
Solubility rules used
Group 1 and ammonium compounds, nitrates, acetates, chlorates and perchlorates are soluble. Chlorides, bromides and iodides are soluble except with Ag⁺, Pb²⁺ and Hg₂²⁺. Sulfates are soluble except with Ca²⁺, Sr²⁺, Ba²⁺, Pb²⁺ and Ag⁺. Hydroxides, carbonates, phosphates, sulfides and oxides are insoluble except with group 1 and NH₄⁺ (plus a few group 2 exceptions). If your course uses slightly different rules, type the state yourself, like Ca(OH)2(s).
When there is no NIE
If every ion is a spectator, no precipitate, gas or water forms and there is no net reaction. Mixing NaCl and KNO₃ solutions is the classic example.