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Net Ionic Equation Calculator

Blake Boege
Written by Blake Boege · Founder, Calculator Answers

A net ionic equation calculator is a chemistry tool that derives net reactions from molecular equations. By splitting soluble strong electrolytes in the aqueous phase into individual ions (total ionic equation), it identifies identical spectator ions on both sides and cancels them, yielding the simplified net ionic equation.

Convert standard molecular chemical equations into total ionic and net ionic equations. Enter your reactants and products, select their phases, and watch the spectator ions cancel out.

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Quick Answer

Convert molecular chemical equations into total ionic and net ionic equations by identifying and removing spectator ions.

Load Preset Reaction

Reactants

CoeffFormulaPhase

Products

CoeffFormulaPhase

Ionic Equations Breakdown

1. Molecular Equation
AgNO3(aq)+NaCl(aq)→AgCl(s)+NaNO3(aq)
2. Total Ionic Equation
Ag+(aq)+NO3-(aq)+Na+(aq)+Cl-(aq)→AgCl+Na+(aq)+NO3-(aq)
3. Spectator Ions Identified
NO3-(aq)Na+(aq)
4. Net Ionic Equation (Final)
Ag+(aq)+Cl-(aq)→AgCl
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Examples

Silver Nitrate + Sodium Chloride reaction

AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq) · Net Ionic: Ag+(aq) + Cl-(aq) → AgCl(s)

Hydrochloric Acid + Sodium Hydroxide neutralization

HCl(aq) + NaOH(aq) → H2O(l) + NaCl(aq) · Net Ionic: H+(aq) + OH-(aq) → H2O(l)

Barium Chloride + Sodium Sulfate reaction

BaCl2(aq) + Na2SO4(aq) → BaSO4(s) + 2 NaCl(aq) · Net Ionic: Ba2+(aq) + SO42-(aq) → BaSO4(s)

How it works

Writing a net ionic equation follows these analytical chemistry steps:

  1. Write the Balanced Molecular Equation: The standard chemical reaction showing full chemical formulas and phases (aq, s, l, g).
  2. Write the Total Ionic Equation: Dissociate all soluble strong electrolytes in the aqueous phase into their respective cations and anions. Non-electrolytes, solids, liquids, and gases do not dissociate.
  3. Identify Spectator Ions: Find ions that appear identically on both sides of the arrow with matching coefficients.
  4. Cancel and Simplify: Subtract the spectator ions from both sides. Divide all remaining coefficients by their greatest common divisor (GCD) if possible.

Understanding Solubility Rules & Strong Electrolytes

To write correct net ionic equations, it is critical to determine solubility. For instance, in a reaction between silver nitrate and sodium chloride, silver chloride precipitates because halides (Cl⁻, Br⁻, I⁻) are insoluble when paired with Silver (Ag⁺). Sodium nitrate remains aqueous because all sodium (Na⁺) and nitrate (NO₃⁻) salts are highly soluble. The spectator ions Na⁺ and NO₃⁻ cancel out, showing that the physical change taking place is simply silver and chloride ions bonding to form solid silver chloride.

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Frequently asked questions

A net ionic equation is a simplified chemical equation that shows only the chemical species (ions and molecules) directly involved in the reaction. It excludes spectator ions, which are ions that remain unchanged on both sides of the equation.

Spectator ions are ions that exist in the same state and concentration on both the reactant and product sides of a chemical equation. Because they do not participate in the actual chemical reaction, they are canceled out when writing the net ionic equation.

A total ionic equation shows all soluble strong electrolytes dissociated into their individual ions, while insoluble compounds and weak electrolytes stay as molecules. A net ionic equation takes this total ionic equation and removes the spectator ions, leaving only the reacting species.

Strong electrolytes are substances that completely dissociate into ions when dissolved in water. These include strong acids (like HCl, HNO3, H2SO4), strong bases (like NaOH, KOH, Ba(OH)2), and soluble salts (like NaCl, KNO3). Weak electrolytes (like acetic acid) only partially dissociate and are not split in ionic equations.