Net Ionic Equation Examples: 47 Problems with Answers

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 sides) removed.

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

Read the full concept explanation →

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: Net Ionic Equation starts by comparing the reactant-product pattern, charges, states, and conserved atoms.

Common stuck point: Students often know a formula related to net ionic equation but skip the recognition step: Does the balanced equation match a recognizable pattern of reactants, products, ions, oxygen, or electron transfer? That leads to a correct-looking substitution attached to the wrong chemical model.

Sense of Study hint: Ask: Does the balanced equation match a recognizable pattern of reactants, products, ions, oxygen, or electron transfer?

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.

Answer

{Ag}^{+} (aq) + {Cl}^{-} (aq) \to AgCl(s)

First step

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)}

Full solution

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
Net ionic equation removes spectator ions ( $\text{Na}^+$ and $\text{NO}_3^-$ ) that appear unchanged on both sides: $\text{Ag}^+\text{(aq)} + \text{Cl}^-\text{(aq)} \rightarrow \text{AgCl(s)}$ .

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)}

Example 3

medium

Write the net ionic equation for

\text{Mg(s)} + 2\text{HCl(aq)} \rightarrow \text{MgCl}_2\text{(aq)} + \text{H}_2\text{(g)}

Example 4

medium

Write the net ionic for the reaction of

\text{NaHCO}_3\text{(aq)}

with

\text{HCl(aq)}

Example 5

hard

Determine the net ionic equation for

\text{AgNO}_3\text{(aq)} + \text{Na}_3\text{PO}_4\text{(aq)} \rightarrow \text{Ag}_3\text{PO}_4\text{(s)} + \text{NaNO}_3\text{(aq)}

Example 6

hard

Write the net ionic for

\text{Zn(s)} + \text{CuSO}_4\text{(aq)} \rightarrow \text{ZnSO}_4\text{(aq)} + \text{Cu(s)}

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.

Example 3

easy

What does a net ionic equation show?

Example 4

easy

What are spectator ions?

Example 5

easy

Which species are written as separate ions in an ionic equation?

Example 6

easy

Should a precipitate

(s)

be split into ions?

Example 7

easy

Ag^+ + Cl^- \rightarrow AgCl(s)

, is this already a net ionic equation?

Example 8

easy

Why must a net ionic equation balance charge as well as atoms?

Example 9

easy

NaCl(aq) + AgNO_3(aq)

, which ions are spectators when AgCl precipitates?

Example 10

easy

Are state symbols needed to write net ionic equations?

Example 11

medium

Write the net ionic equation for

AgNO_3(aq) + NaCl(aq) \rightarrow AgCl(s) + NaNO_3(aq)

Net ionic equation for AgNO₃(aq) + NaCl(aq)

Example 12

medium

Net ionic equation for

HCl(aq) + NaOH(aq) \rightarrow NaCl(aq) + H_2O(l)

Net ionic equation for HCl(aq) + NaOH(aq)

Example 13

medium

Net ionic for

BaCl_2(aq) + Na_2SO_4(aq) \rightarrow BaSO_4(s) + 2NaCl(aq)

Net ionic equation for BaCl₂(aq) + Na₂SO₄(aq)

Example 14

medium

Verify charge balance:

Ba^{2+} + SO_4^{2-} \rightarrow BaSO_4(s)

Example 15

medium

Should weak acid acetic acid

CH_3COOH

be split in a net ionic equation?

Example 16

medium

Net ionic for

Na_2CO_3(aq) + CaCl_2(aq) \rightarrow CaCO_3(s) + 2NaCl(aq)

Example 17

medium

Why are spectator ions left out of the net ionic equation?

Example 18

medium

2HCl + CaCO_3(s) \rightarrow CaCl_2 + H_2O + CO_2

, why is

CaCO_3

kept whole?

Example 19

medium

Net ionic for

Pb(NO_3)_2(aq) + 2KI(aq) \rightarrow PbI_2(s) + 2KNO_3(aq)

Net ionic equation for Pb(NO₃)₂(aq) + 2KI(aq)

Example 20

challenge

Write the balanced net ionic equation for

3CaCl_2(aq) + 2Na_3PO_4(aq) \rightarrow Ca_3(PO_4)_2(s) + 6NaCl(aq)

Net ionic equation for 3CaCl₂(aq) + 2Na₃PO₄(aq)

Example 21

challenge

Net ionic for

Zn(s) + 2HCl(aq) \rightarrow ZnCl_2(aq) + H_2(g)

Net ionic equation for Zn(s) + 2HCl(aq)

Example 22

challenge

Verify the net ionic

3Ca^{2+} + 2PO_4^{3-} \rightarrow Ca_3(PO_4)_2(s)

balances atoms and charge.

Example 23

easy

Write the net ionic equation for

\text{AgNO}_3\text{(aq)} + \text{KCl(aq)} \rightarrow \text{AgCl(s)} + \text{KNO}_3\text{(aq)}

Example 24

easy

\text{Na}_2\text{SO}_4 + \text{BaCl}_2 \rightarrow \text{BaSO}_4 + 2\text{NaCl}

, identify the spectator ions.

Example 25

easy

Write the net ionic equation for

2\text{NaOH(aq)} + \text{H}_2\text{SO}_4\text{(aq)} \rightarrow \text{Na}_2\text{SO}_4\text{(aq)} + 2\text{H}_2\text{O(l)}

Example 26

easy

\text{H}_2\text{O(l)}

a strong electrolyte to be split into ions?

Example 27

medium

Write the net ionic equation for

\text{Pb(NO}_3)_2\text{(aq)} + 2\text{NaCl(aq)} \rightarrow \text{PbCl}_2\text{(s)} + 2\text{NaNO}_3\text{(aq)}

Example 28

medium

Write the net ionic equation for

\text{NH}_3\text{(aq)} + \text{HCl(aq)} \rightarrow \text{NH}_4\text{Cl(aq)}

Example 29

medium

Write the net ionic equation for

\text{CaCO}_3\text{(s)} + 2\text{HCl(aq)} \rightarrow \text{CaCl}_2\text{(aq)} + \text{H}_2\text{O(l)} + \text{CO}_2\text{(g)}

Example 30

medium

Write the net ionic equation for

\text{CuSO}_4\text{(aq)} + \text{Fe(s)} \rightarrow \text{FeSO}_4\text{(aq)} + \text{Cu(s)}

Example 31

medium

Net ionic for

\text{HF(aq)} + \text{NaOH(aq)} \rightarrow \text{NaF(aq)} + \text{H}_2\text{O(l)}

Example 32

medium

Net ionic for

\text{FeCl}_3\text{(aq)} + 3\text{NaOH(aq)} \rightarrow \text{Fe(OH)}_3\text{(s)} + 3\text{NaCl(aq)}

Example 33

medium

Net ionic for

\text{Cu(NO}_3)_2\text{(aq)} + 2\text{NaOH(aq)} \rightarrow \text{Cu(OH)}_2\text{(s)} + 2\text{NaNO}_3\text{(aq)}

Example 34

medium

Net ionic for

\text{NH}_4\text{Cl(aq)} + \text{NaOH(aq)} \rightarrow \text{NaCl(aq)} + \text{NH}_3\text{(g)} + \text{H}_2\text{O(l)}

(warm).

Example 35

hard

Write the net ionic for

2\text{Al(s)} + 6\text{HCl(aq)} \rightarrow 2\text{AlCl}_3\text{(aq)} + 3\text{H}_2\text{(g)}

Example 36

hard

Net ionic for

2\text{HNO}_3\text{(aq)} + \text{Ba(OH)}_2\text{(aq)} \rightarrow \text{Ba(NO}_3)_2\text{(aq)} + 2\text{H}_2\text{O(l)}

Example 37

hard

Does mixing

\text{NaNO}_3\text{(aq)}

and

\text{KCl(aq)}

produce a net ionic reaction?

Example 38

hard

Net ionic for

\text{Sr(NO}_3)_2\text{(aq)} + \text{K}_2\text{SO}_4\text{(aq)} \rightarrow \text{SrSO}_4\text{(s)} + 2\text{KNO}_3\text{(aq)}

Example 39

hard

Net ionic for

\text{CH}_3\text{COOH(aq)} + \text{NaOH(aq)} \rightarrow \text{CH}_3\text{COONa(aq)} + \text{H}_2\text{O(l)}

Example 40

hard

Verify both atom and charge balance for

\text{Ba}^{2+}\text{(aq)} + 2\text{OH}^-\text{(aq)} + 2\text{H}^+\text{(aq)} + \text{SO}_4^{2-}\text{(aq)} \rightarrow \text{BaSO}_4\text{(s)} + 2\text{H}_2\text{O(l)}

Example 41

challenge

For the reaction

5\text{Fe}^{2+}\text{(aq)} + \text{MnO}_4^-\text{(aq)} + 8\text{H}^+\text{(aq)} \rightarrow 5\text{Fe}^{3+}\text{(aq)} + \text{Mn}^{2+}\text{(aq)} + 4\text{H}_2\text{O(l)}

, verify atom and charge balance.

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Related Concepts

Precipitation Reaction Double Displacement

Background Knowledge

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

precipitation reactiondouble displacement