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Topic: Redox Titration  (Read 1710 times)

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Offline ChuckleBuckle

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Redox Titration
« on: April 21, 2015, 09:00:57 PM »
For my school practical, we were told to prepare a standard iron (ii) ammonium sulphate solution and then titrate it when potassium permanganate.
The procedure goes like this:
-Weigh 4g of hydrated iron (ii) ammonium sulphate.
-Dissolve it in water and place into a volumetric flask
-Add 5mL of 12M sulphuric acid
 -Shake the mixture and add distilled water until the calibration mark

-Pipette 25mL of the iron (ii) ammonium sulphate solution into a conical flask.
 -Add 10mL of 2M sulphuric acid into the concical flask -Titrate with potassium permanganate

What i want to know is why do you add two different concentrations of sulphuric acid and do they both have different purposes?

Offline Borek

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Re: Redox Titration
« Reply #1 on: April 22, 2015, 02:40:39 AM »
The first one is there just to stabilize the solution (prevent precipitation of iron hydroxides), the second one is a necessary reagent for the permanganate reaction (try to write balanced reaction equation).
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Offline ChuckleBuckle

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Re: Redox Titration
« Reply #2 on: April 22, 2015, 02:54:07 AM »
The first one is there just to stabilize the solution (prevent precipitation of iron hydroxides), the second one is a necessary reagent for the permanganate reaction (try to write balanced reaction equation).

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