My idea is that, since the solution should be 1moldm-3 with respect to both ions why not use 0.5 moldm-3 of both iron (II)sulphate and iron (III)sulphate?
I have doubt and I am weak in this topic.
And why use iron chloride instead of iron sulphate? ( according to mark scheme )
My idea is that, since the solution should be 1moldm-3 with respect to both ions why not use 0.5 moldm-3 of both iron (II)sulphate and iron (III)sulphate?
I have doubt and I am weak in this topic.
And why use iron chloride instead of iron sulphate? ( according to mark scheme )
Help me!
Your first two links are to the same image.
In order to produce the standard emf for the Fe2+/3+ half-cell, you need both ions to be the same conc as each other. So you can use 0.5 mol dm-3 (as you suggest).
Since I can't see the Q, I can't comment about the Cl- vs SO42- part. My guess is that you're given data for the Cl2/Cl- half-cell and the emf of that half-cell will interfere. I know that Cl2 can oxidise Fe2+ to Fe3+ (or Cl- can reduce 3+ back to 2+).
In order to produce the standard emf for the Fe2+/3+ half-cell, you need both ions to be the same conc as each other. So you can use 0.5 mol dm-3 (as you suggest).
Since I can't see the Q, I can't comment about the Cl- vs SO42- part. My guess is that you're given data for the Cl2/Cl- half-cell and the emf of that half-cell will interfere. I know that Cl2 can oxidise Fe2+ to Fe3+ (or Cl- can reduce 3+ back to 2+).Sorry
In order to produce the standard emf for the Fe2+/3+ half-cell, you need both ions to be the same conc as each other. So you can use 0.5 mol dm-3 (as you suggest).
Since I can't see the Q, I can't comment about the Cl- vs SO42- part. My guess is that you're given data for the Cl2/Cl- half-cell and the emf of that half-cell will interfere. I know that Cl2 can oxidise Fe2+ to Fe3+ (or Cl- can reduce 3+ back to 2+).
The examiner's report says '' A majority thought (incorrectly) that mixing equal volumes of two 0.50 mol dm-3 solutions would produce a 1.0 mol dm-3 solution "
"1mol dm-3 solution of iron(III) sulphate contains 2 moles Fe(III)."
But 1moldm-3 of FeSO4 contains 1mol of Fe(II). So if we use 2 moldm-3 of FeSO4 ( according to 1st line in mar scheme), then mol of Fe(II) = Fe (III) 😊
Therefore the mixture contains equal moles of each ion. Thats why the mark scheme states ' the mixture should be equimolar with respect to each ion ' Thanks !