Crystal growing: acetates of copper and calcium

Left to right: Ca(CH3COO)2·H2O (calcium acetate monohydrate); CuCa(CH3COO)4·6H2O (copper calcium acetate hexahydrate); Cu(CH3COO)2·H2O (copper acetate monohydrate)

Blue crystal in the middle of the above picture is a new addition to my collection of crystals: copper calcium acetate hexahydrate, a compound with formula CuCa(CH3COO)4·6H2O. It is an example of double salts (wiki): salts, having two different anions or cations. For comparison, crystals of pure calcium and copper acetates are put at the sides.

Calcium acetate

Left crystal is calcium acetate (wiki): Ca(CH3COO 2·H2O. The crystals are colorless, their form resembles needles. The specimens on the photo were made accidentally a year or so ago. I've forgot a flask, containing mix of calcium acetate and acetic acid on the shelf. When I opened it, these transparent needles were on the bottom. This crystal have triclinic crystal system.

Copper acetate

Seemingly black (actually dark blue-green) crystals on the right are copper acetate monohydrate: Cu(CH3COO)2·H2O (wiki). I've grew them half year ago, slowly evaporating saturated solution of copper acetate. This crystal have monoclinic crystal system.

Copper-calcium acetate

And finally, in the middle is the new addition to my collection: double salt, copper-calcium acetate hexahydrate, CuCa(CH3COO)4·6H2O. It has prismatic form, with improper 8-gon at the base. This reflects its structure, which is different from the both pure acetates; it is tetragonal.

Alas, the photo can't reproduce the beautiful blue color of this crystal. It is blue with a light violet tint, different from the well known copper sulphate. The crystal was grown rather fast, by the method of cooling supersaturated solution. Because of the fast growth, it is not completely transparent, and bases of the prism have some visible defects. Nevertheless, it's beautiful.

Here are some more photos


Another picture of the same copper-calcium acetate crystal.

Copper-calcium acetate grows readily from the supersaturated solution and may be grown by cooling or by evaporation. The key point is to prepare solution that have 4x times more calcium then needed. Despite in the crystal there is 1 ion of Ca2+ per each ion of Cu2+, the solution must have around 4 ions of calcium per each ion of copper, or the usual copper acetate will form. I used the proportion: 7.2g of Ca(OAc)2 per 2g of Cu(OAc)2.

Preparing the chemicals

The chemicals to grow the above crystals can be prepared from widely available compounds: vinegar, chalk and copper sulphate.

The easiest one is calcium acetate Ca(CH3COO)2. I have obtained it by treating white chalk (almost pure calcium carbonate) with acetic acid. In this reaction, large amount of CO2 gas is released, so don't put all chalk at once, or the foam will spill from the flask. The equation of this reaction is:

CaCO3 + 2CH3COOH → Ca(CH3COO)2 + H2O + CO2

Copper II acetate Cu(CH3COO)2 is a bit harder to make. I've made it electrochemically, by dissolving copper anode in acetic acid. An easier way would be the following 2-step reaction, starting from copper (II) sulphate (CuSO4, "blue vitriol").

First, dissolve some CuSO4 in water and add baking soda (NaHCO3). Sodium carbonate or hydroxide are fine too. Again, CO2 gas will release (beware of foam), and green-blue sediment of the basic copper (II) carbonate will form:

2CuSO4 + 2NaHCO3 → CuCO3·Cu(OH)2 + Na2SO4 + CO2

Let the sediment to precipitate, remove excess of the liquid, then dissolve the sediment it in the acetic acid:

CuCO3·Cu(OH)2 + 4CH3COOH → 2Cu(CH3COO)2 + 2H2O + CO2
You will obtain blue solution of the copper (II) acetate. Again, carbon dioxide gas would form, so don't add a lot of acid at once.

Growing the copper-calcium acetate crystal

I've made the solution by dissolving dried acetates of copper and calcium in hot water, in proportion 7.2g of calcium acetate per 2g of copper acetate. Though, I believe that exact proportion is not very important here. If the solution was concentrated enough, then after cooling it, light blue crystals of double salt copper-calcium acetate will form spontaneously. If you instead see dark-blue crystals of copper acetate, the, calcium is probably not enough. If you don't have any crystals, then there is too much water, let it evaporate in the warm place.

The rest is as usual:

  • find some well-formed small seed crystal,
  • attach it to the thin thread (I used a thread from the fake Santa's beard, lol),
  • suspend the seed in the supersaturated solution,
  • let it grow.
When the crystal stops growing (from several hours to a day), make the solution supersaturated again. To do this, I heated it and dissolved additional salts, then cooled again. Of course, growing crystal must be removed before heating, or it dissolve too.

Alternatively, you may grow the crystal by slowly evaporating the solution. It takes more time, but should produce much more clear and well formed crystal. I am planning to do this soon.


Note that copper salts are mildly toxic. They won't harm you if you don't try to eat them, but put the chemicals and crystals away from little children and wash your hands (must-have habit for any home chemist). Concentrated acetic acid may be harmful too. Calcium salts are safe.


Michael said…
When I suspend a seed crystal from a thread, I am always unhappy with the thread embedded in the larger crystal. I should find some finer thread. But for copper acetate, I find if I lay the seed crystal on a piece of copper, it grows well. I use the end cap of copper plumbing.

When I let my copper acetate solution evaporate, I get some fine beautiful green-blue powder in addition to the dark-coloured solid that makes the crystal. I would love to get this lighter green-blue into a crystal, but it doesn't happen. I'm not sure if this lighter coloured powder is just a different hydrate of the copper acetate, or is it copper hydroxide or carbonate (although the colour looks deeper than that.)

The other weird effect I see in an evaporating dish of copper salts is that the solid creeps up and over the side of the container. It's odd and I can't explain why that happens. It looks like it's trying to escape, lol.