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mun
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Hello all, this is my first time here.

I would like to know what crystals are produced when you place Fe in a solution of CuSO4. I would also like more info on the crystals.

Thanks in advance
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MadNatSci
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(Original post by mun)
Hello all, this is my first time here.

I would like to know what crystals are produced when you place Fe in a solution of CuSO4. I would also like more info on the crystals.

Thanks in advance

This should (if I can remember the reactivity series right) be a simple displacement reaction. The Fe is more reactive than Cu so it knocks it out and you get FeSO4 instead. What info do you need on the crystals?

Also this link might help (go to GCSE, then chemistry, then 'metals and the reactivity series'.)
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Jonatan
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(Original post by mun)
Hello all, this is my first time here.

I would like to know what crystals are produced when you place Fe in a solution of CuSO4. I would also like more info on the crystals.

Thanks in advance
It depends on the relative amounts of the substances. If you have a great excess of SO4-- ions you will get a crystal consisting of a mixture of CuSO4 and FeSO4, if the concentration of the SO4-- ions is small, however, I think you will get FeSO4 since Iron has a greater electrode potential than copper. Also, if you have very little iron you will also get a mixture of FeSO4 and CuSO4.

Remember, however, that both CuSO4 and FeSO4 dissolves readily in water. Therefore you need to first dissolve the substances in the solution, and then either decrease the concentration of water (allowing it to evaporate) or decrease the soluability of the water (dissolving the substances in a hot solution which you afterwards allow to cool is one possibility). Nevertheless, large crystals with few imperfections are obtained when they are grown slowly over time. As an example, a CuSO4 solution containing a large amount of CuSO4 could be left to evaporate with a CuSO4 crystal at the bottom. As the water evaportaes CuSO4 will bind to teh crystal increasing its size.
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JFN
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Also note that it is quite ambiguous to call it Fe. Make sure to refer to its oxidation state (2+ or 3+).
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matouwah
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(Original post by JFN)
Also note that it is quite ambiguous to call it Fe. Make sure to refer to its oxidation state (2+ or 3+).
isn't the 3+ alot more stable....
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mun
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oops.. my mistake...

the Fe should be Fe2+
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Jonatan
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(Original post by matouwah)
isn't the 3+ alot more stable....
Well, the ions do not occure as pure subtances but in combination with other ions. Thus you do not see Fe3+ , but typically some oxide or salt.
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mun
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ok.. I think I might rephrase the question

I put Fe (an Iron Nail) into a solution of CuSO4 (Copper Sulfate) and the solution is blue because of the Cu2+ ions. As time gradually passes, 'pure' Cu forms on the Fe (Iron Nail), in addition to the build-up of Cu, green crystals form on the nail just above the CuSO4 solution. I would like info on the crystals..

tQ
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