Question

What changes do you observe in the iron nails and colour of copper sulphate solution, if iron nails are dipped in CuSO4 solution for 15 minutes ?

Answer 1

When Iron nail (Ferrum) is dipped in Copper sulphate (CuSO4) there takes reaction between them and coppersulphate change its color from blue to light green. This shows Iron is more reactive than Copper, it can replace Copper from CuSO4. CuSO4 is in blue Color and FeSO4 is in light green color.

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Answer 2

Answer:

The copper sulfate solution coloring varies from blue to pale green.

Explanation:

When an iron nail exists immersed in the solution of copper sulfate then iron substitutes copper from the solution of copper Sulphate because iron exists more reactive than copper. Therefore copper sulfate solution coloring varies from blue to pale green.

Reaction

CuSO4 (aq) + Fe (s) → FeSO4 (aq) + Cu (s)

In this reaction following two functions take place:

Cu²⁺ + 2e = Cu⁰ (re­duc­tion process, Cu²⁺ is the ox­i­dizing agent)

Fe⁰ – 2e = Fe²⁺ (ox­i­da­tion process, Fe⁰ is the re­duc­ing agent)

The reaction can be a double displacement response as well as a redox reaction (oxidation and reduction both bring place simultaneously).

When an iron nail is dipped in copper sulfate solution, a brown layer of copper is formed on the surface of iron and the color of the copper sulfate solution varies from blue to pale green. The reaction indicates that iron exists more reactive than copper because it replaces copper from the copper sulfate solution. The iron passes into the solution as Fe (II) creating the ferrous sulfate solution.

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