Changing of iron(II) ions to iron(III) ions and vice versa

Changing of iron(II) ions to iron(III) ions and vice versa

1. Iron exhibits two oxidation numbers
   (a) +2 as iron(II) ion, Fe²⁺
   (b) +3 as iron(III) ion, Fe³⁺
2. An aqueous solution containing iron(II) ions, Fe²⁺ is pale green in colour, whereas that containing iron(III) ions, Fe³⁺ is yellow/yellowish-brown/ brown in colour.
3. Changing iron(II) ions to iron(III) ions is an oxidation and therefore requires an oxidising agent.
   
4. On the other hand, changing iron(III) ions to iron(II) ions is a reduction and therefore requires a reducing agent.
   

Table: Detecting the presence of iron(II) ions and iron(III) ions

The following are other oxidising agents that can replace bromine water in changing iron(II) ions to iron(III) ions.

Other reducing agents that can replace zinc powder in changing iron(III) ions to iron(II) ions are as follows.

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Changing of iron(II) ions to iron(III) ions and vice versa experiment

Aim: To investigate oxidation and reduction in the change of iron(II) ions to iron(III) ions and vice versa.
Materials: 0.5 mol dm^-3 freshly prepared iron(II) sulphate solution, 0.5 mol dm^-3 iron(III) sulphate solution, bromine water, zinc powder, 2.0 mol dm^-3 sodium hydroxide solution, filter paper.
Apparatus: Dropper, spatula, test tubes, test tube holder, Bunsen burner, filter funnel, test tube rack.
Procedure:
A. Changing of iron(II) ions to iron(III) ions

1. 2 cm³ of 0.5 mol dm^-3 iron(II) sulphate solution is poured into a test tube.
2. Using a dropper, bromine water is added to the solution drop by drop.
3. The test tube is warmed gently.
4. 2.0 mol dm^-3 sodium hydroxide solution is added slowly to the mixture until in excess.

B. Changing of iron(III) ions to iron(II) ions

1. 2 cm³ of 0.5 mol dm^-3 iron(III) sulphate solution is poured into a test tube.
2. Half a spatula of zinc powder is added to the solution.
3. The mixture is filtered.
4. 2.0 mol dm^-3 sodium hydroxide solution is added slowly to the filtrate until in excess.

Observations:

Discussion:
A. Changing of iron(II) ions to iron(III) ions

1. Bromine water oxidises iron(II) ions, Fe²⁺ to iron(III) ions, Fe³⁺. The presence of Fe³⁺ ions is confirmed by the formation of brown precipitate with sodium hydroxide solution.
2. Fe²⁺ ions lose their electrons and are oxidised to Fe³⁺ ions.
3. Bromine molecules, which give the bromine water its brown colour, gain the electrons and are reduced to colourless bromide ions, Br^–. This explains why the bromine water is decolourised.
4. In this reaction, bromine water acts as the oxidising agent, where as Fe²⁺ ions act as the reducing agent.
   

B. Changing of iron(III) ions to iron(II) ions

1. Zinc powder reduces iron(III) ions, Fe³⁺ to iron(II) ions, Fe²⁺. The presence of Fe²⁺ ions is confirmed by the formation of green precipitate with sodium hydroxide solution.
2. Zinc atoms lose their electrons and are oxidised to zinc ions, Zn²⁺. This explains why zinc powder dissolves in iron(III) sulphate solution.
3. Fe³⁺ ions accept these electrons and are reduced to Fe²⁺ ions.
4. In this reaction, Fe³⁺ ions act as the oxidising agent, whereas zinc acts as the reducing agent.
   

Conclusion:

1. Bromine water acts as an oxidising agent, changing iron(II) ions to iron(III) ions.
2. Zinc acts as a reducing agent, changing iron(III) ions to iron(II) ions.