Net Ionic Equation Examples in Chemistry

Start with the recap, study the fully worked examples, then use the practice problems to check your understanding of Net Ionic Equation.

This page combines explanation, solved examples, and follow-up practice so you can move from recognition to confident problem-solving in Chemistry.

Concept Recap

A simplified chemical equation that shows only the ions and molecules directly involved in a chemical reaction, with all spectator ions (those unchanged on both.

Strip away the bystanders. Some ions just float around doing nothing — the net ionic equation shows only the ones that actually react.

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How to Use These Examples

  • Read the first worked example with the solution open so the structure is clear.
  • Try the practice problems before revealing each solution.
  • Use the related concepts and background knowledge badges if you feel stuck.

What to Focus On

Core idea: Spectator ions appear on both sides and cancel out. What remains is the essential chemistry of the reaction.

Common stuck point: Only split strong electrolytes (strong acids, strong bases, soluble salts) into ions. Keep weak electrolytes and precipitates as molecules.

Sense of Study hint: When writing a net ionic equation, follow three steps. First write the balanced molecular equation with correct formulas and states. Then write the complete ionic equation by splitting all strong electrolytes (soluble salts, strong acids, strong bases) into individual ions — keep precipitates, gases, water, and weak electrolytes as whole formulas. Finally, cancel all spectator ions that appear identically on both sides.

Worked Examples

Example 1

easy
Explain the difference between a molecular equation, a complete ionic equation, and a net ionic equation. Use the reaction of \text{NaCl(aq)} + \text{AgNO}_3\text{(aq)} as an example.

Solution

  1. 1
    Molecular equation shows all species as complete formulas: \text{NaCl(aq)} + \text{AgNO}_3\text{(aq)} \rightarrow \text{AgCl(s)} + \text{NaNO}_3\text{(aq)}.
  2. 2
    Complete ionic equation splits all aqueous ionic compounds into their ions: \text{Na}^+\text{(aq)} + \text{Cl}^-\text{(aq)} + \text{Ag}^+\text{(aq)} + \text{NO}_3^-\text{(aq)} \rightarrow \text{AgCl(s)} + \text{Na}^+\text{(aq)} + \text{NO}_3^-\text{(aq)}.
  3. 3
    Net ionic equation removes spectator ions (\text{Na}^+ and \text{NO}_3^-) that appear unchanged on both sides: \text{Ag}^+\text{(aq)} + \text{Cl}^-\text{(aq)} \rightarrow \text{AgCl(s)}.

Answer

\text{Ag}^+\text{(aq)} + \text{Cl}^-\text{(aq)} \rightarrow \text{AgCl(s)}
The net ionic equation shows only the species that actually participate in the chemical change. Spectator ions are present in solution but do not undergo any change — they merely 'watch' the reaction.

Example 2

medium
Write the net ionic equation for the reaction between \text{BaCl}_2\text{(aq)} and \text{Na}_2\text{SO}_4\text{(aq)}.

Practice Problems

Try these problems on your own first, then open the solution to compare your method.

Example 1

medium
Write the net ionic equation for the neutralization of hydrochloric acid with sodium hydroxide: \text{HCl(aq)} + \text{NaOH(aq)} \rightarrow \text{NaCl(aq)} + \text{H}_2\text{O(l)}.

Example 2

hard
Write the net ionic equation for the reaction: \text{K}_2\text{CO}_3\text{(aq)} + 2\text{HCl(aq)} \rightarrow 2\text{KCl(aq)} + \text{H}_2\text{O(l)} + \text{CO}_2\text{(g)}. Identify all spectator ions.
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Background Knowledge

These ideas may be useful before you work through the harder examples.

precipitation reactiondouble displacement