Question

Write two observations which you will make when an iron nail is kept in aqueous solution of copper sulphate ? Write the chemical equation for this rection

Answer 1

1) The initial blue colour of copper sulphate solution is changed to light green colour of iron sulphate.

2) The initial silver colour of iron nail is changed to reddish-brown colour due to coating of copper metal on the nail.

Hope this will help you....

Answer 2

Answer:

1) The iron sulphate solution's pale green colour replaces the copper sulphate solution's original blue hue.

2) The copper metal coating on an iron nail causes the nail's original silver colour to turn reddish-brown.

Explanation:

• Iron is more reactive as compared to copper. This means that iron will replace copper in its salt if it is mixed with copper salt solution. The reaction that takes place will be: -

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

• As iron is a more potent reducer than copper, it converts the Cu²⁺ ion in CuSO4 to metallic copper before being oxidised to the ion Fe²⁺.

• The blue colour of the solution fades away, and a greenish hue emerges as a result of the increase in the concentration of Fe²⁺ions in solution and reduction in the concentration of Cu²⁺ ions in solution.

• As a result, when iron is immersed in the copper sulphate solution, its colour changes and silver colour of iron nail is changed to reddish brown colour.