Property 5: The reaction of metals with solutions of other metal salts
There is a particular pattern in which metals will react with solutions of other metal salts.
The more reactive metal will displace the less reactive metal from their compounds. For instance, if metal A is more reactive than metal B, then the reaction will be as follows:
Metal A + Salt solution of Metal B → Salt Solution of A + Metal B
This is also called a Displacement reaction. Let us consider a simple experiment to verify this. Things needed:
- Two test tubes
- Iron sulphate solution
- Copper sulphate solution
- Iron nail
- Copper wire
Procedure:
- Take two test tubes. Fill one with the solution of iron sulphate, and another with the solution of copper sulphate.
- Put the copper wire in a solution of iron sulphate, and the iron nail in a solution of copper sulphate for about half an hour and observe
- Let it stay for a few more hours and observe.
Initial setup Observations and Conclusions:
- Post half an hour: A reaction has taken place only in the test tube in which the iron nail is placed. The nail is coated with a pinkish brown deposit which is copper. This is not rust, it happens because iron displaces copper from the copper sulphate solutions.
- Post few hours: A large amount of copper will be displaced from the copper sulphate solution and iron takes the place to form iron sulphate solution which is green in color.
𝑭𝒆(𝒔) + 𝑪𝒖𝑺𝑶𝟒(𝒂𝒒) → 𝑭𝒆𝑺𝑶𝟒(𝒂𝒒) + 𝑪𝒖(𝒔)
The second test tube will display no reaction. And that’s because iron is more reactive
than copper. Copper will not displace the iron here.
𝑪𝒖(𝒔) + 𝑭𝒆𝑺𝑶𝟒(𝒂𝒒) → 𝑵𝒐 𝒓𝒆𝒂𝒄𝒕𝒊𝒐𝒏
This is how the reactivity order will look like:
Summary
The Reaction of Metals with Solutions of Other Metal Salts | The more reactive metal will displace the less reactive one from their compounds
Metal A + Salt solution of Metal B → Salt Solution of A + Metal B |
Also Check:
Chemical Properties of Metals – Property 1