Chemical Forums
Chemistry Forums for Students => Organic Chemistry Forum => Topic started by: junoso on July 25, 2007, 06:33:23 PM
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I'm trying to figure out how many grams is equal to 1N(normal) of ceric ammonium nitrate. The molecular weight is 548.26grams. Please *delete me* I've been stuck on this question for 2 days!
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With respect to what?
The issue with normalities is that you need a base reaction to say what you're (hypothetically) titrating against.
1 mole of CAN will formally dissociate to give 2 moles of ammonium ions, 1 mole of ceric ions and 6 moles of nitrate ions.
So if you're looking at wrt to anions, 1N would be 91.4g per litre, but if it's ammonium, 274g / l
S
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It depends on the method of titration. In redox titration
Ce4+ => Ce3+
and an equivalent is equal to mole
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Yes, this is a redox titration. I'm using this as a titrant and my sample contains ferric ammonium sulfate solution(10% in 15% H2SO4). I thought it would be 1N=1M correct?
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Do you mean (NH4)2Fe(SO4)2 ? (ferrous)
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No, ferric FeNH4(SO4)2 12H2O
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Then, how can you perform titration
Fe(III) cannot be easily oxidzed .
Most redox titration use oxidation Fe(II) to Fe(III)