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When I stick some Copper (II) Sulfate * Pentahyrate into the blue flame of my butane torch, it turns green.
When I crush the tiny CuSO4 crystals up into a finer powder and mix them with a mixture of KClO3 and Sugar, then light that on fire, I get a very blue flame.
What is happening here? I thought that copper [+2] ions were suppose to color flames blue? How is it that the same substance is giving off two difference colors?
The only exaplanation I could fine for this is,
When I crush the tiny CuSO4 crystals up into a finer powder and mix them with a mixture of KClO3 and Sugar, then light that on fire, I get a very blue flame.
What is happening here? I thought that copper [+2] ions were suppose to color flames blue? How is it that the same substance is giving off two difference colors?
The only exaplanation I could fine for this is,
So if this is true, then that would explain it I suppose, assuming CuO produces a blue flame. Except, wouldn't the CuSO4 decompose just as easily in the butane torch flame? If I stick some of the power into the flame and leave it there, watching it, the color should change as it decomposes, but I just don't see that happening.Copper(II) sulfate decomposes before melting. The common pentahydrate form dehydrates, losing four water molecules at 110 °C and all five at 150 °C. At 650 °C copper(II) sulfate decomposes into copper(II) oxide (CuO), Sulfur dioxide (SO2) and oxygen (O2).