Try this microscale practical to explore the chemical changes in displacement, redox and precipitation reactions

In this visually engaging series of experiments, students observe and identify the chemical changes that take place in a range of reactions on a microscale. The practical features displacement, redox and precipitation reactions between various salts, including potassium manganate(VII), barium nitrate and ammonium vanadate(V).

The experiments should take approximately 20 minutes.

Equipment

Apparatus

  • Eye protection
  • Student worksheet
  • Clear plastic sheet (eg ohp sheet)
  • Magnifying glass

Chemicals

Note

Solutions should be contained in plastic pipettes. See the accompanying guidance on apparatus and techniques for microscale chemistry, which includes instructions for preparing a variety of solutions.

  • Barium nitrate, 0.2 mol dm–3
  • Sodium sulfate, 0.5 mol dm–3
  • Lead nitrate, 0.5 mol dm–3
  • Ammonia solution, 3 mol dm–3
  • Ammonium vanadate(V), 0.2 mol dm–3 (acidified with sulfuric acid)
  • Hydrochloric acid, 1 mol dm–3
  • Sodium hydroxide, 1 mol dm–3
  • Potassium manganate(VII), 0.01 mol dm–3
  • Silver nitrate, 0.1 mol dm–3
  • Copper(II) sulfate, 0.2 mol dm–3
  • Iron(II) sulfate, 0.2 mol dm–3
  • Iron(III) nitrate, 0.2 mol dm–3
  • Potassium thiocyanate, 0.2 mol dm–3
  • Zinc metal granules

Health, safety and technical notes

  • Read our standard health and safety guidance.
  • Wear eye protection throughout (splash-resistant goggles to BS EN166 3).
  • Silver nitrate, AgNO3(aq), 0.1 mol dm–3 is an eye irritant. Keep separate from organic waste containers.
  • Lead nitrate, Pb(NO3)2(aq), 0.5 mol dm–3 is a reproductive toxin, causes eye damage, causes damage to organs (especially the CNS) and is harmful to the aquatic environment. Avoid inhalation and skin contact.
  • Ammonia solution, NH3(aq), 3 mol dm–3 is CORROSIVE.
  • Ammonium vanadate(V), NH4VO3, 0.2 mol dm–3 (acidified with sulfuric acid) is a mutagen and extremely toxic if inhaled – but not by any other route.
  • Sodium hydroxide solution, NaOH(aq), 1 mol dm–3 is corrosive.
  • Copper(II) sulfate solution, CuSO4(aq), 0.2 mol dm–3 causes eye damage and is HAZARDOUS to the aquatic environment.
  • The following chemicals are all of low hazard:
    • Barium nitrate, Ba(NO3)2(aq), 0.2 mol dm–3
    • Sodium sulfate, Na2SO3(aq), 0.5 mol dm–3
    • Hydrochloric acid, HCl(aq), 1 mol dm–3
    • Iron(II) sulfate, FeSO4.7H2O(aq), 0.2 mol dm–3
    • Iron(III) nitrate, Fe(NO3)3.9H2O(aq), 0.2 mol dm–3
    • Potassium manganate(VII), 0.01 mol dm–3
    • Potassium thiocyanate, KSCN(aq), 0.2 mol dm–3
    • Zinc metal granules

Procedure

Cover the table on your worksheet with a clear plastic sheet, then follow steps 1–10 below.

  1. Put two drops of barium nitrate solution into box 1 (at the top of the middle column). Add two drops of sodium sulfate solution to the drops of barium nitrate solution.
  2. Put two drops of lead nitrate solution into box 2. Add two drops of potassium iodide solution to the drops of lead nitrate solution.
  3. Put two drops of iron(III) nitrate solution into box 3. Add one drop of potassium thiocyanate solution to the iron(III) nitrate solution.
  4. Put two drops of copper(II) sulfate solution into box 4. Add two drops of ammonia solution to the copper(II) sulfate solution.
  5. Put two drops of ammonium vanadate(V) solution into box 5. Add one drop of hydrochloric acid, then a small piece of zinc metal to the ammonium vanadate(V) solution.
  6. Put two drops of iron(II) sulfate solution into box 6. Add two drops of sodium hydroxide solution to the iron(II) sulfate solution.
  7. Put two drops of potassium manganate(VII) solution into box 7. Add two drops of iron(II) sulfate solution to the potassium manganate(VII) solution.
  8. Put two drops of barium nitrate solution into box 8. Add two drops of sodium hydroxide to the barium nitrate solution. Observe, and record any changes over the next ten minutes.
  9. Put one drop of silver nitrate solution into box 9. Add one drop of iron(II) sulfate to the silver nitrate solution. Observe closely using a magnifying glass.
  10. Put two drops of copper(II) sulfate solution into box 10. Add a small piece of zinc metal to the copper sulfate solution.

Teaching notes and expected observations

The following notes explain the expected observations for each step/reaction:

  1. A dense white precipitate of barium sulfate forms. Barium sulfate is used as a barium meal in medicine since it is opaque to X-rays. Because it is very insoluble it is non-toxic, unlike other, soluble, barium compounds.
  2. A bright yellow precipitate of lead nitrate forms. Lead nitrate is a very effective pigment but it is toxic.
  3. A deep red colour is produced due to iron(III) thiocyanate ions. This reaction is used to test for the presence of iron.
  4. A deep blue colour of tetra-amminocopper(II) forms. There may also be some light blue precipitate of copper(II) hydroxide.
  5. Bubbles (of hydrogen) are seen. The yellow colour of the ammonium vanadate gradually changes (as the vanadium is reduced) to blue owing to the formation of the vanadium(IV) ion (VO2+). The colour then changes to green due to the vanadium(III) ion (V3+) and finally to lilac due to the vanadium(II) ion (V2+). The changes in oxidation states of vanadium salts have been investigated for applications in battery technology.
  6. A greenish precipitate of iron(II) hydroxide forms. This gradually changes to the brown iron(III) hydroxide as the iron is oxidised.
  7. The deep purple colour of the potassium manganate(VII) gradually fades first to the brown manganese(IV) dioxide and then to the pale pink manganese(II) ion (Mn2+). Manganese(II) compounds in solution usually appear virtually colourless. However, a solid manganese(II) salt is pink.
  8. Barium hydroxide forms. This is soluble so nothing is seen at first. Barium hydroxide is alkaline and gradually absorbs carbon dioxide from the air to form the insoluble barium carbonate. The drop takes on a hazy appearance as a skin of barium carbonate forms on the surface.
  9. A glittering of metallic silver forms as the iron(III) reduces the silver nitrate. This is seen clearly using a magnifying glass.
  10. The surfaces of the pieces of zinc turn red-brown as copper metal deposits via a displacement reaction. The blue colour of the copper(II) sulfate solution fades.

Steps 9 and 10 in the procedure both involve the displacement of a valuable, but less reactive, metal using a less valuable, but more reactive, metal. This could be used as a topic for discussion.

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