Displacement reactions involving solutions of salts
3 marks · EasyThe table shows the results of placing samples of metals in solutions of metal nitrates:
| Metal added | Metal nitrate solution | Observation |
|---|---|---|
| Aluminium | Silver nitrate | Grey crystals form |
| Copper | Zinc nitrate | No change |
| Iron | Copper(II) nitrate | Reddish-brown deposit |
| Magnesium | Lead(II) nitrate | Grey solid forms |
Write the ionic equation for the reaction when aluminium is added to silver nitrate solution.
Which metal does not react in its experiment? Explain why based on the data.
Work this out on paper, then compare with the answer and worked solution below. With a free account you can submit written answers for marking.
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(a) Al(s) + 3Ag^{+}(aq) \to Al^{3+}(aq) + 3Ag(s)
(b) Copper does not react in zinc nitrate because there is 'no change.' Copper is less reactive than zinc and cannot displace zinc from solution.
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Marking points
A1 (a) · 1 mark · Correct ionic equation for Al + AgNO3 (with correct charges and balancing).
B1 (b) · 1 mark · Identifies copper as the non-reacting metal.
B2 (b) · 1 mark · Gives correct reason: copper is less reactive than zinc/cannot displace zinc.
Worked solution
a) The ionic equation for aluminium and silver nitrate:
b) Copper does not react in zinc nitrate because it is not reactive enough to displace zinc ions from solution.