Why does the colour of copper sulphate solution change when an iron nail is dipped in it?
When an iron nail is placed in a copper sulphate solution, iron displaces copper from copper sulphate solution forming iron sulphate, which is green in colour.
Therefore, the blue colour of copper sulphate solution fades and green colour appears.
Because Copper is produced at the Cathode (negative electrode) so the Copper ions in the solution are used up, causing the blue colour to fade.
It is because the zinc rod reacts with the solution. It forms zinc sulphate solution and the copper metal is deposited. The zinc sulphate solution is colourless and hence due to formation of this solution the blue starts fading.
The iron atoms are displacing the copper atoms from the copper sulphate solution, so the copper atoms are coming out of solution and accumulating along the iron nail, and the iron is combining with the sulfate ions to form the solution iron (II) sulfphate, which is a green color. This is a single displacement/replacement reaction with the chemical equation Fe(s) + CuSO4(aq) --> Cu(s) + FeSO4.
When an iron nail is dipped in the copper sulfate solution then iron displaces copper from the copper sulfate because iron is more reactive than copper.
This is a very complicated question and the answer would have to be figured out by experiment. Commiserations.
the copper sulfate reacts and changes colour
green colour
Most people think that Cupric sulfate or Copper(II) sulfate, is blue in colour. But actually it is not. Blue colour in Copper(II) sulfate is due to the presence of Water molecules in it. This form is called Copper(II) sulfate Pentahydrate[CuSO4.5H2O], which most people see. If it does not have any water molecules in it, the thing is in pure state and is White in colour. This form is Anhydrous Copper(II) sulfate[CuSO4]. This form is rarely seen, because it can absorb water itself from the nature and become blue in colour. So from this we know that very pure Copper(II) sulfate is not blue, But its Pentahydrate form is blue.
Zinc sulfate is colorless to white in appearance.
Its colour is nearly red and orange.
Colorless. The resulting solution is zinc sulfate, and Zn2+ ions are colorless.
When an iron nail is dipped in the copper sulfate solution then iron displaces copper from the copper sulfate because iron is more reactive than copper.
The chemical reaction is:CuSO4 + 2 AgNO3 = Cu(NO3)2 + Ag2SO4(s)Pure silver sulfate is white, copper(II) sulfate solution is blue.
During the electrolysis of Copper sulphate ,at the cathode ,copper and hydrogen both being positively charged migrate towards the cathode.While at the anode
Anhydrous copper sulfate solid is white. When it is added to water, it dissolves and the solution of aqueous copper sulfate becomes blue.
Copper sulfate solution starts of a blue colour. When Iron metal is added to the solution a REDOX reaction begins in which the copper is reduced (gains electrons) to become copper metal and the iron is oxidised (loses electrons) to become iron ions. When the iron ions go into solution, it will change to a green colour which is the colour of iron (II) sulfate. As a general principle, a more reactive metal will displace a less reactive metal from solution by the process described above.
blue
This is a very complicated question and the answer would have to be figured out by experiment. Commiserations.
the copper sulfate reacts and changes colour
Why does copper sulfate change its colour when water is added