What does the colour of copper sulphate solution change when an iron nail is dipped in it?

Question

Answer

*when an iron nail is placed in a copper sulphate solution solution, iron displaces copper from copper sulphate solution forming iron sulphate, which is light  green in colour. It is because iron is more reactive than copper.

Answer

When an iron nail is dipped in copper sulphate solution, displacement reaction take place in which iron displaces copper from copper sulphate to form iron sulphate, as a result the blue colour of the copper sulphate solution turns into green which represent the colour of iron sulphate solution.the reaction can be represented as-->Cuso4+Fe=FeSo4+Cu

Answer

Green due to formation of iron sulphate

Answer

The colour of Copper Sulphate solution is Blue colour, when an iron nail dipped in it.

Answer

The Color Change of Copper Sulphate Solution when an Iron Nail is Dipped in it

When an iron nail is dipped in a copper sulphate solution, a series of chemical reactions occur which result in a noticeable color change. This color change can be explained through the process of displacement reactions between the iron and copper ions present in the solution.

1. Initial State: Blue Colored Copper Sulphate Solution
The copper sulphate solution is initially blue in color. This is because copper ions (Cu2+) are present in the solution and they absorb light in the red region of the spectrum, giving the solution its blue color.

2. Reaction Between Iron and Copper Sulphate Solution
When an iron nail is placed in the copper sulphate solution, a displacement reaction occurs. The iron atoms lose electrons, forming iron(II) ions (Fe2+) in the solution. At the same time, the copper(II) ions (Cu2+) in the solution gain electrons, forming copper atoms. This displacement reaction can be represented by the following chemical equation:
Fe(s) + CuSO4(aq) → FeSO4(aq) + Cu(s)

3. Formation of Iron Sulphate Solution
As a result of the displacement reaction, iron(II) sulphate (FeSO4) is formed in the solution. This compound dissolves in water, forming iron(II) sulphate solution. The iron(II) ions give the solution a pale green color.

4. Formation of Copper Metal
Simultaneously, the copper ions in the solution gain electrons and are reduced to copper atoms. These copper atoms then deposit on the surface of the iron nail, forming a layer of copper metal. This is visible as a brownish-red coating on the iron nail.

5. Overall Color Change
As the iron nail is dipped in the copper sulphate solution, the initial blue color of the solution gradually fades. This is because the copper ions are being displaced by the iron atoms, resulting in the formation of iron(II) sulphate solution and the deposition of copper metal on the nail. The final color of the solution turns greenish, while the iron nail acquires a reddish-brown coating of copper.

Summary
The color change of the copper sulphate solution when an iron nail is dipped in it can be explained by the displacement reaction between the iron and copper ions. The initial blue color of the solution fades as copper ions are displaced by iron atoms, leading to the formation of iron(II) sulphate solution. Simultaneously, copper metal is deposited on the iron nail, resulting in a greenish color of the solution and a reddish-brown coating on the nail.

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