This free net ionic equations worksheet teaches Grade 11 students to predict precipitates with the solubility rules and write molecular, total ionic and net ionic equations.
Students classify compounds as soluble or insoluble, decide whether a precipitate forms, write all three equation types for three reactions, find spectator ions, reduce neutralizations to H+ + OH− → H2O, and identify an unknown ion. Every equation has been checked for both atom and charge balance.
- Grade 11 Chemistry
- 29 marks
- 40–50 minutes
- Answer key included
What's in This Net Ionic Equations Worksheet
| Part | Skill practised | Marks |
|---|
| A | Soluble or insoluble? (solubility rules) | 8 |
| B | Will a precipitate form? | 4 |
| C | Molecular, total ionic and net ionic equations | 9 |
| D | Spectator ions | 2 |
| E | Neutralization net ionic equations | 2 |
| F | Spot the mistake | 2 |
| G | Challenge: identifying and separating ions | 2 |
It supports the Ontario Grade 11 chemistry curriculum expectations in the Solutions and Solubility unit.
Solubility Rules
Every question on this net ionic equations worksheet starts with one decision: does this compound dissolve? These are the rules printed on the worksheet:
| Usually soluble (aq) | Exceptions (form a precipitate) |
|---|
| Group 1 (Li+, Na+, K+) and NH4+ compounds | none |
| Nitrates (NO3−) and acetates | none |
| Chlorides, bromides, iodides (Cl−, Br−, I−) | Ag+, Pb2+, Hg22+ |
| Sulfates (SO42−) | Ba2+, Pb2+, Ca2+, Sr2+ |
| Usually insoluble (s) | Exceptions (soluble) |
|---|
| Carbonates, phosphates, sulfides (CO32−, PO43−, S2−) | Group 1 and NH4+ |
| Hydroxides (OH−) | Group 1, NH4+, Ba2+ |
Compounds labelled (aq) are written as separate ions in ionic equations. Compounds labelled (s), (l) or (g) stay together. For a fuller chart, see the solubility chart on Wikipedia.
How to Write a Net Ionic Equation
Here's question 13 from the worksheet, mixing silver nitrate and sodium chloride, worked through all three stages:
Molecular: AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq)
Total ionic: Ag+(aq) + NO3−(aq) + Na+(aq) + Cl−(aq) → AgCl(s) + Na+(aq) + NO3−(aq)
Net ionic: Ag+(aq) + Cl−(aq) → AgCl(s)
- Write the balanced molecular equation with state symbols. Check the solubility rules to label each product.
- Split every (aq) ionic compound into its ions. Leave the solid AgCl together.
- Cancel spectator ions, here Na+ and NO3−, which appear unchanged on both sides.
- Check atoms and charge. The left side has charge (+1) + (−1) = 0, which matches the neutral solid.
Students need correct formulas before they can split them into ions. The naming ionic compounds worksheet and the types of chemical reactions worksheet are good warm-ups for this net ionic equations worksheet.
Net Ionic Equations Practice Questions
These match the net ionic equations worksheet PDF. Include state symbols in every equation.
Part A – Soluble or Insoluble?
- NaCl
- AgCl
- KNO3
- BaSO4
- CaCO3
- (NH4)3PO4
- PbI2
- Mg(OH)2
Part B – Will a Precipitate Form?
If yes, name the precipitate. If no, explain.
- AgNO3(aq) + NaCl(aq)
- KNO3(aq) + NaCl(aq)
- BaCl2(aq) + Na2SO4(aq)
- Pb(NO3)2(aq) + KI(aq)
Part C – Molecular, Total Ionic and Net Ionic Equations
- Aqueous silver nitrate and sodium chloride are mixed. Write the (a) balanced molecular, (b) total ionic and (c) net ionic equations.
- Aqueous barium chloride and sodium sulfate are mixed. Write the (a) balanced molecular, (b) total ionic and (c) net ionic equations.
- Aqueous lead(II) nitrate and potassium iodide are mixed. Write the (a) balanced molecular, (b) total ionic and (c) net ionic equations.
Part D – Spectator Ions
- In question 14, which ions are spectator ions?
- CaCl2(aq) + Na2CO3(aq) → CaCO3(s) + 2NaCl(aq)
Write the net ionic equation and name the spectator ions.
Part E – Neutralization
- HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)
Write the net ionic equation. - H2SO4(aq) + 2KOH(aq) → K2SO4(aq) + 2H2O(l)
Write the net ionic equation. Why is it the same as question 18?
Part F – Spot the Mistake
- For AgNO3 + NaCl, a student’s “net ionic equation” is Ag+(aq) + NO3−(aq) + Na+(aq) + Cl−(aq) → AgCl(s) + Na+(aq) + NO3−(aq). Explain the error and correct it.
- A student writes the precipitate AgCl(s) as Ag+(aq) + Cl−(aq) on the product side. Explain the error and correct it.
Part G – Challenge
- An unknown solution forms a white precipitate with Na2SO4(aq) but not with NaCl(aq). Which cation is most likely present: Ag+, Pb2+ or Ba2+? Explain.
- A solution contains both Ag+ and Ba2+. Describe how to separate them using precipitation.
Net Ionic Equations Worksheet Answer Key
Open each part to check your work on the net ionic equations worksheet. The printable key is at the end of the PDF.
Part A answers (Q1–8)
- NaCl: Soluble
- AgCl: Insoluble
- KNO3: Soluble
- BaSO4: Insoluble
- CaCO3: Insoluble
- (NH4)3PO4: Soluble
- PbI2: Insoluble
- Mg(OH)2: Insoluble
Part B answers (Q9–12)
- Yes: AgCl(s)
- No: every possible product (KCl, NaNO3) is soluble
- Yes: BaSO4(s)
- Yes: PbI2(s)
Part C answers (Q13–15)
- (a) AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq)
(b) Ag+(aq) + NO3−(aq) + Na+(aq) + Cl−(aq) → AgCl(s) + Na+(aq) + NO3−(aq)
(c) Ag+(aq) + Cl−(aq) → AgCl(s) (spectators: Na+, NO3−) - (a) BaCl2(aq) + Na2SO4(aq) → BaSO4(s) + 2NaCl(aq)
(b) Ba2+(aq) + 2Cl−(aq) + 2Na+(aq) + SO42−(aq) → BaSO4(s) + 2Na+(aq) + 2Cl−(aq)
(c) Ba2+(aq) + SO42−(aq) → BaSO4(s) (spectators: Na+, Cl−) - (a) Pb(NO3)2(aq) + 2KI(aq) → PbI2(s) + 2KNO3(aq)
(b) Pb2+(aq) + 2NO3−(aq) + 2K+(aq) + 2I−(aq) → PbI2(s) + 2K+(aq) + 2NO3−(aq)
(c) Pb2+(aq) + 2I−(aq) → PbI2(s) (spectators: K+, NO3−)
Part D answers (Q16–17)
- Na+ and Cl−
- Ca2+(aq) + CO32−(aq) → CaCO3(s); spectators: Na+, Cl−
Part E answers (Q18–19)
- H+(aq) + OH−(aq) → H2O(l)
- H+(aq) + OH−(aq) → H2O(l) (after dividing by 2). Every strong acid–strong base neutralization reduces to H+ + OH− → H2O; the other ions are spectators.
Part F answers (Q20–21)
- That is the total ionic equation. Cancel the spectator ions (Na+, NO3−): Ag+(aq) + Cl−(aq) → AgCl(s)
- Solids, liquids and gases are never split into ions. Only soluble (aq) ionic compounds are written as ions.
Part G answers (Q22–23)
- Ba2+: BaSO4 is insoluble but BaCl2 is soluble. Ag+ and Pb2+ would also have precipitated with Cl−.
- Add Cl− first: only AgCl(s) forms, so filter it off. Then add SO42− to the filtrate to precipitate BaSO4(s).
5 Common Net Ionic Equation Mistakes
Part F of the net ionic equations worksheet targets the first two.
- Stopping at the total ionic equation. If spectator ions are still there, it isn't the net ionic equation.
- Splitting solids into ions. Precipitates, water and gases are always written whole.
- Splitting polyatomic ions apart. SO42− stays as one ion; it is not S and O.
- Losing the coefficients. Pb(NO3)2 gives one Pb2+ and two NO3− ions.
- Forgetting state symbols. The (s) on the precipitate is the whole point of the equation.
How to Use This Net Ionic Equations Worksheet in Class
- Before a precipitation lab: Parts A and B, so students predict which mixtures will go cloudy.
- After the lab: Parts C and D using the reactions they observed.
- Review: Parts E–G. The ion identification question is a good lead-in to qualitative analysis.
After the net ionic equations worksheet, check understanding with the solutions and solubility quiz.
Frequently Asked Questions
Is this net ionic equations worksheet free?
Yes. The worksheet and its answer key are free to download and print as a PDF, with no account needed.
How do you write a net ionic equation?
Write the balanced molecular equation with states, split every soluble (aq) ionic compound into its ions, cancel the ions that appear unchanged on both sides, and check that atoms and charge balance.
What are spectator ions?
Ions that are present in the solution but don't take part in the reaction. They appear unchanged on both sides of the total ionic equation and are cancelled out.
How do you know if a precipitate will form?
Use the solubility rules to check each possible product. If one product is insoluble, it forms a precipitate (s). If every product is soluble, there is no reaction.
Why is the net ionic equation for every strong acid and strong base the same?
Because the metal and non-metal ions are always spectators, every strong acid–strong base reaction reduces to H+(aq) + OH−(aq) → H2O(l).
More Free Grade 11 Chemistry Resources
Ready to practise? Download the free net ionic equations worksheet PDF (use the Download button above), print it double-sided, and keep the answer key pages for marking.