Quickly grow your own ‘stalagmite’ from a supersaturated solution of sodium ethanoate.
In this demonstration experiment a supersaturated solution of sodium ethanoate crystallises rapidly forming a ‘stalagmite’.
This is a demonstration used to show the rapid crystallisation of a supersaturated solution in a spectacular way and explore the energy change involved. It can also be used to stimulate interest in public presentations.
The teacher requires
Beaker (250 cm3)
Measuring cylinder (25 cm3)
Watch glass (large one, about 10 cm diameter)
Bunsen burner, tripod and gauze
Access to a top-pan balance (1 d.p. is sufficient)
Sodium ethanoate-3-water (sodium acetate-3-water), 125 g
Refer to Health & Safety and Technical notes section below for additional information.
Health & Safety and Technical notes
Wear eye protection.
Sodium ethanoate-3-water (sodium acetate-3-water), CH3COONa.3H2O - see CLEAPSS Hazcard.
1 A black background is probably better than a white one for this demonstration.
2 The ‘stalagmite’ can be re-heated and used again. Keep the solution clean and free from dust – this could cause it to crystallise prematurely.
Before the demonstration
a Weigh 125 g of the hydrated sodium ethanoate into the beaker and add 12.5 cm3 of water.
b Heat the beaker over a low flame and stir until a clear solution is obtained.
c Cover the beaker with a watch glass and allow to cool to room temperature to give a supersaturated solution.
d Remove the watch glass and place a few ‘seed’ crystals of sodium ethanoate on it.
e Pour the supersaturated solution slowly onto the sodium ethanoate cystals. The solution should crystallise immediately on contact with the crystals. It will form a growing ‘stalagmite’ of solid sodium ethanoate as more and more of the solution is poured onto it. The watch glass becomes warm as heat is released during the crystallisation process.
If re-heating is shown to the class, emphasise that the solid is dissolving (in its own water of crystallisation) and not melting. A supersaturated solution of sodium thiosulfate, obtained in a similar way, is also stable until a seed crystal is added.
Commercial ‘heat packs’ are available which use the principle of supersaturation. Here a mechanical disturbance, usually a spring loaded button inside the pack, induces crystallisation. The packs can be re-used by heating in boiling water to re-dissolve the crystals.
Health & Safety checked, 2016
This Practical Chemistry resource was developed by the Nuffield Foundation and the Royal Society of Chemistry.
© Nuffield Foundation and the Royal Society of Chemistry
Page last updated October 2015
This is a resource from the Practical Chemistry project, developed by the Nuffield Foundation and the Royal Society of Chemistry. This collection of over 200 practical activities demonstrates a wide range of chemical concepts and processes. Each activity contains comprehensive information for teachers and technicians, including full technical notes and step-by-step procedures. Practical Chemistry activities accompany Practical Physics and Practical Biology.