I'm completely lost as to how this should be approached. Can anyone please explain the basic principle behind this??
A2 Chemistry - Using redox titrations to calculate oxidation states Watch
- Thread Starter
- 06-04-2016 18:11
- 06-04-2016 22:55
Offline14ReputationRep:Community AssistantStudy Helper
- Community Assistant
- Study Helper
- 06-04-2016 22:58
If you know the change in oxidation state of one reactant you know the number of electrons transferred.
You then use the moles ratio to determine the number of moles of electrons either arriving in the other half equation or being removed from the other half equation.
This can then show you the oxidation state of the productof the other half equation.
Imagine that you are reacting iron(II) with manganate(VII) and you want to know what the oxidation state of the product of the manganate(VII) reduction is.
The titration tells you that 1 mole of manganate(VII) reacts with 5 mols of iron(II)
You already know that iron(II) is oxidised to iron(III) - in other words one mol of electrons per mol of iron(II).
So 5 mol of iron(II) releases 5 mol electrons.
This reduces 1 mol of manganate(VII)
Hence the manganese oxidation state must decrease by 5, i.e. the product is manganese(II)