A_Ch
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#1
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The question I need help with is
Q/ Calculate the concentration of an iron(II) sulphate solution, given that 20 cm3 of the solution reacts completely with 23.5 cm3 of 0.02 mol l-1 potassium permanganate solution, in the presence of acid. (Hint – you must decide which ion will be oxidised, which will be reduced, and write the redox equation before tackling the calculation).
I am not sure how to create the balanced equation? Also, I'm not sure what is being oxidised and reduced
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wombat746
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Some hints:

FeSO4 is oxidised to Fe2(SO4)3 and KMnO4 is reduced to Mn(2+).

Write out the respective oxidation and reduction equations, using electrons, protons and water molecules where necessary to balance. Then equate the two redox equations in terms of equal electrons, combine and cancel the electrons, water and protons to get the overall balanced equation.
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A_Ch
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Thanks, but I am still unsure about how you got that answer.
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chocochip_
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Write out the half equations for each, then you can decide what’s being oxidised and what’s being reduced you can do this by thinking about what’s going to be a stronger oxidising agent KmnO4 or FeSO4, if you’re OCR A a level student you can just remember what’s the stronger oxidising agent as they tend to use the example quite a lot
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chocochip_
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You can then find out which half equation goes which way, balance the electrons, H+, H20’s and then bing bam boom you got yourself a balance equation
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A_Ch
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Thanks, I think I've got it now.
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A_Ch
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I have just overthought this, wouldn't Fe be oxidised to Fe2+ and MnO4 be reduced to Mn2+?
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A_Ch
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#8
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Never mind, I've understood it now. Thanks for the help.
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