Copper Sulphate and Iron Activity Class 10

Copper Sulphate and Iron Activity Class 10 : Activity 1.9 Ncert Science class 10

Copper Sulphate and Iron Activity Class 10

Activity 1.9 Ncert Science class 10

Write an activity to show that iron displaces copper from copper sulphate. (OR) Write an activity about how you conduct an experiment to show that more reactive metals replace less reactive metals from their compounds. (OR) Why is an iron nail kept in a solution brownish? Explain the activity.
 Brief Procedure:

Activity 1.9 asks us to dip iron nails in a copper sulphate solution and check the colour of the solution.

  1. Take two iron nails and clean them by rubbing with sand paper.
  2. Take two test tubes and mark them as A and B.
  3. Take about 10 ml of copper sulphate solution in each test tube.
  4. Dip one iron nail in copper sulphate solution of test tube A.
  5. Keep the test tube with iron nail undisturbed for 20 minutes.
  6. Keep the other iron nail and test tube aside.
  7. Compare the colours of the solutions in the test tubes.
  8. Now take out the iron nail from copper sulphate solution.
  9. Keep the iron nail and test tubes A and B side by side.
  10. Compare with the other iron nail that has been kept aside.
  11. We will observe that the iron nail dipped in copper sulphate solution becomes brownish.
  12. Blue colour of copper sulphate solution in test tube ‘A’ fades.
  13. Iron is more reactive than copper, so it displaces copper from copper sulphate.
  14. This is one of the examples for displacement reaction.
  15. Equation : Fe(s)+ CuSO4(aq) → FeSO4(aq) + Cu(s)

Copper Sulphate and Iron Activity Class 10

Observation: 

Colour of copper solution fades and nail becomes brown.

Explanation: 

Copper Sulphate and Iron Activity Class 10

Iron in nail displaces copper from the copper sulphate solution. As a result, solution fades in colour.

This displacement reaction results in the formation of elemental copper. Elemental copper deposits on the nail and impart a brown colour to the nail.

CuSO4(aq) + Fe(s) ——-> FeSO4(aq) + Cu(s)

Note: The faded blue appearance later change to green colour because ferrous sulphate is green.

Read also: Abnormal Molar Masses

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