Rehydrating Copper (II) Sulfate

Rehydrating Copper (II) Sulfate

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

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. Yes, now I remember you saying – just shows I should not comment when I am tired! 😀
    But glad that you are having fun anyway. 🙂

  2. 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.

  3. Robyn Haynes – Australia – Robyn enthusiastically pursues a green and writerly life on the north coast of New South Wales, Australia, where her background as a doctor of social anthropology equips her with an interesting slant on the human condition. She spends much time indulging a passion for her garden where she ponders life and attempts to stave off existential angst. In her more reflective moments she makes wry observations on courtyard gardening and its parallels with life.
    Robyn Haynes says:

    Great experimentation Dan.

  4. 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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