Question

What happens when you dip Iron nail in copper sulphate solution? Also mention the change of colour in it...​

Answer 1

Explanation:

When an iron nail immersed in the solution of copper sulphate than iron displaces copper from the solution of copper sulphate because iron is more reactive than copper. Therefore copper sulphate solution colour changes from blue to pale green.

Reaction

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

In this reaction following two processes 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 double displacement reaction as well as redox reaction (oxidation and reduction both takes place simultaneously).

Explanation

When an iron nail is dipped in copper sulphate solution, a brown coating of copper is formed in the surface of iron and the colour of copper sulphate solution changes from blue to pale green. The reaction shows that iron is more reactive than copper because it displaces copper from the copper sulphate solution. The iron passes into the solution as Fe (II) forming the ferrous sulphate solution

Answer 2

When a grey colour of an iron nail is immersed in blue solution of copper sulphate and the mixture is allowed to left for more than 12 hrs. then we observed that arround the iron nail brown solid of copper is deposit and the colour of solution changes to light green due to the formation of iron sulphate .

Reactionn is : Fe(s) + CuSO4(aq) → FeSO4(aq) + Cu(s)

The above reaction is an example of Displacement reaction

${ \huge\rm \pink {H}\rm \blue {A} \rm \purple {N}\ \rm \green{J} \rm\red {U}\ \rm \orange {H} \rm{U} \rm \gray{I}}$