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Net Ionic Equation Calculator

Convert molecular equations to net ionic forms. Features a solubility rule engine, spectator ion identifier, and step-by-step dissociation visualization.

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Category Physics & Science
Step 1: Molecular Equation
Step 2: Dissociation (Check Solubility)
Step 3: Cancel Spectators
Final: Net Ionic Equation
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About

Chemical reactions often occur in aqueous solutions where ionic compounds dissociate into their constituent ions. A molecular equation shows the complete formulas of reactants and products, but it fails to represent the actual microscopic species participating in the reaction. Accuracy in identifying the driving force of a reaction - usually the formation of a precipitate, gas, or weak electrolyte - is essential for predicting reaction outcomes in laboratory settings.

This tool automates the dissociation process using established solubility rules. It distinguishes between strong electrolytes, which exist as separate ions, and weak electrolytes or solids, which remain intact. The calculator isolates spectator ions (ions that do not change oxidation state or phase) and removes them to reveal the net ionic equation. This reduction is critical for simplifying complex stoichiometry and focusing on the species actually undergoing chemical change.

chemistry stoichiometry reactions precipitates solubility

Formulas

The transformation follows conservation of charge and mass. A general double displacement reaction is defined as:

AB(aq) + CD(aq) → AD(s) + CB(aq)

If AD is insoluble, it precipitates. The complete ionic equation splits aqueous species:

A+ + B- + C+ + D- → AD(s) + C+ + B-

Spectator ions (B- and C+) appear unchanged on both sides. Removing them yields the net ionic equation:

A+(aq) + D-(aq) → AD(s)

Reference Data

Ion TypeSolubility RuleExceptions (Insoluble/Precipitate)
NO3- (Nitrate)SolubleNone (Almost all nitrates are soluble)
Na+, K+, NH4+SolubleNone
Cl-, Br-, I-SolubleAg+, Pb2+, Hg22+
SO42- (Sulfate)SolubleBa2+, Pb2+, Ca2+, Sr2+
OH- (Hydroxide)InsolubleNa+, K+, Ca2+ (Slightly), Ba2+
S2-, CO32-, PO43-InsolubleNa+, K+, NH4+
CrO42- (Chromate)InsolubleNa+, K+, NH4+, Mg2+

Frequently Asked Questions

Spectator ions are necessary to maintain charge neutrality in the reactant solutions before mixing. While they do not participate in the formation of the precipitate or chemical change, the reaction cannot occur without a complete neutral salt as a starting material. They affect ionic strength but not the net reaction.
If both potential products of a double displacement reaction are soluble in water (marked as 'aq'), no reaction occurs. The result is simply a mixture of ions in the solution. In this case, there is no net ionic equation because all ions are spectators.
Most chloride salts are soluble, but there are notable exceptions. Silver chloride (AgCl), Lead(II) chloride (PbCl2), and Mercury(I) chloride (Hg2Cl2) are insoluble. Lead(II) chloride is marginally soluble in hot water but precipitates in cold water.