Chemical Properties
Copper(II) sulfate pentahydrate decomposes before melting at 150 °C (302 °F), losing two water molecules at 63 °C (145 °F), followed by two more at 109 °C (228 °F) and the final water molecule at 200 °C (392 °F).
Dehydration proceeds by decomposition of the tetraaquacopper(2+) moiety, two opposing aqua groups are lost to give a diaquacopper(2+) moiety. The second dehydration step occurs with the final two aqua groups are lost. Complete dehydration occurs when the only unbound water molecule is lost.
At 650 °C (1,202 °F), copper(II) sulfate decomposes into copper(II) oxide (CuO) and sulfur trioxide (SO3).
Its blue color is due to water of hydration. When heated in an open flame the crystals are dehydrated and turn grayish-white.
Copper sulfate reacts with concentrated hydrochloric acid very strongly. In the reaction the blue solution of copper(II) turns green, due to the formation of tetrachlorocuprate(II):
- Cu2+ + 4 Cl– → CuCl2−
4
It also reacts with more reactive metals than copper (e.g. Mg, Fe, Zn, Al, Sn, Pb, etc.):
- CuSO4 + Zn → ZnSO4 + Cu
- CuSO4 + Fe → FeSO4 + Cu
- CuSO4 + Mg → MgSO4 + Cu
- CuSO4 + Sn → SnSO4 + Cu
- 3 CuSO4 + 2 Al → Al2(SO4)3 + 3 Cu
The copper formed is deposited on the surface of the other metal. The reaction stops when no free surface of the metal is present anymore.
Read more about this topic: Copper(II) Sulfate
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