Rehydrating Copper (II) Sulfate

Rehydrating Copper (II) Sulfate

Someone gave me an idea and I want to do it:

Screenshot (80)

See what he said? Let’s follow him.

The last time we used test tubes and destroyed all of them! So I’m going to use a beaker.


I put the copper sulfate in it and going to burn it.


It’s white now. I’ll drop water on it.


It worked!


I’m guessing that it works like this: I took the water molucles out by evaporating the water, now I have this white dust without water in there, and when I added the water, it turned back to blue (it’s like adding the water molucles back to it). This is why I love chemistry. It’s so awesome!

8 Replies to “Rehydrating Copper (II) Sulfate”

  1. I know about the water molecules. It loses two water molecules when heating at 63 °C, two more at about 105 °C and the final water molecule at 200 °C. Thanks for the idea. The experiment was very fun.

  2. Well done on your experiment and thank you for the mention 🙂
    If you google copper sulphate you’ll find that it normally has about 5 water molecules attached to it and is blue. Heating it removes the water and it turns white. It’s still copper sulphate, but is anhydrous – no water. – But you figured that out by yourself. 🙂

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