What would happen if you dipped an iron nail in blue copper sulphate solution?

Question

Homework..

Answer 1

The iron nail will become copper-plated because iron is more reactive than copper (it displaces it)
Fe(s) + CuSO4(aq) = FeSO4(aq) + Cu(s)

Answer 2

There would be a displacement reaction, with the iron replacing the copper.
In words: iron + copper sulphate = copper + iron sulphate
Under the conditions of the reaction, there would be very small amounts of iron(III) sulphate but the main product would be the iron(II) sulphate:
Fe(s) + Cu++(aq) ---> Cu(s) + Fe++(aq)

What you would see in practice is a brown deposit of copper gradually covering the nail and the blue colour of the copper sulphate solution gradually becoming paler. It would never become completely colourless, however, because the iron(II) sulphate itself has a very pale bluish-green colour.

Answer 3

Iron nail becomes coated with copper because in the activity series of metals iron is more reactive than copper. Fe + CuSO4 =FeSO4+ Cu. In addition blue colour of copper sulphate is replaced by green colour of iron sulphate. The reaction gives out heat.

Answer 4

The iron would oxidise to form Iron sulphate and the Copper ions would be reduced to form copper atoms. Copper sulphate is blue from copper ions and it would lose this colour as the copper ions are lost.

If I remember correctly from when I did this years ago you also end up with a blackish solid forming.

Answer 5

Iron will displace copper from copper salts. A brown furry deposit of copper forms on the surface of the nail and the blue colour fades as the copper salt gets weaker.

Answer 6

It would go copper coloured as a layer of copper would be deposited all over the submerged part. Because iron is higher (more positive) in the electro-chemical series.

Answer 7

you will get iron sulphate and copper Fe+CuSO4=FeSO4+Cu