Reactions in solution bench – precipitation, acid–base, redox and net ionic equations
ChemistryReactions & RedoxAges 16–17
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Sign in to playMix any two of fifteen ionic solutions, predict the outcome with the solubility rules, then see what happens: a coloured precipitate, a gas, a temperature rise or a colour change. Each mixture shows the full, full ionic and net ionic equations, the spectator ions, the ion product Q compared with Ksp, and the reaction type: precipitation, gas-forming, acid–base (proton transfer) or redox (electron transfer, with oxidation numbers). Filter, wash, dry and weigh a precipitate to find the percentage yield, and record every mixture in a results table.
Lesson: Reactions of ions in solution: solubility rules, precipitation, net ionic equations and types of reaction
What it shows
When two ionic solutions are mixed, the ions can meet new partners. If a new combination is insoluble, it comes out as a precipitate; the solubility rules predict this, and comparing the ion product Q with the solubility product Ksp decides it for slightly soluble salts. Ions that stay unchanged in solution are spectator ions and are left out of the net ionic equation. Other mixtures transfer protons (acid–base reactions such as neutralisation, or an acid with a carbonate giving carbon dioxide) or electrons (redox reactions, where oxidation numbers change).
How to use
Choose solution A for the tube and solution B to pour in, and set the Volume and Concentration sliders. Use the solubility rules to decide, then press the Prediction buttons and Pour in B and shake. Read the observation, the equations and the spectator ions, and check your prediction. When a precipitate forms, press Filter, wash, dry, weigh to find the yield, then press Record.
Parameters you can change
- Solution A (in the tube) AgNO₃ – silver nitrate, Pb(NO₃)₂ – lead(II) nitrate, BaCl₂ – barium chloride, CaCl₂ – calcium chloride, CuSO₄ – copper(II) sulfate, FeSO₄ – iron(II) sulfate, FeCl₃ – iron(III) chloride, NaCl – sodium chloride, KI – potassium iodide, Na₂SO₄ – sodium sulfate, Na₂CO₃ – sodium carbonate, NaOH – sodium hydroxide, HCl – hydrochloric acid, H₂SO₄ – dilute sulfuric acid, NH₄Cl – ammonium chloride
- Solution B (poured in) AgNO₃ – silver nitrate, Pb(NO₃)₂ – lead(II) nitrate, BaCl₂ – barium chloride, CaCl₂ – calcium chloride, CuSO₄ – copper(II) sulfate, FeSO₄ – iron(II) sulfate, FeCl₃ – iron(III) chloride, NaCl – sodium chloride, KI – potassium iodide, Na₂SO₄ – sodium sulfate, Na₂CO₃ – sodium carbonate, NaOH – sodium hydroxide, HCl – hydrochloric acid, H₂SO₄ – dilute sulfuric acid, NH₄Cl – ammonium chloride
- Concentration of each solution 0.01–1 mol/L
- Volume of solution A 1–20 mL
- Volume of solution B 1–20 mL
- Show the ions model
Questions to explore
- Why is there no net ionic equation when sodium chloride is mixed with copper(II) sulfate?
- Why does calcium sulfate precipitate at 0.10 mol/L but not at 0.01 mol/L?
- In the reaction between iron(III) chloride and potassium iodide, which ion is the oxidising agent?
