Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: DQD on November 09, 2011, 06:30:06 AM
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I prepare Chrome Alum from K2Cr2O7, pure H2SO4 and Ethanol 95o
And the question is
What is the Ethanol's effect in process ?
Which substance can Inhibiti Hydrogen peroxide while storing ?
And its mechanism ?
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What you make is not a chrome alum. Chromic acid if anything.
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It's impossible, solution after reacting has dark green color
and I have let it for 1-2 week(s), it appear crystal ???
I do this experiment from my text book
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Hm, perhaps it makes sense - it guarantees correct Cr:K ratio. Interesting.
Think: why does the solution become green?
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i wonder
May ethanol cause ?
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Yes, it is because of the ethanol presence, but it is not ethanol that becomes green.
What is green in this solution? Initially the solution should be red/brown. What do you know about dichromate, especially in low pH?
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Green in this solution, I guess mixture of Cr2(SO4)3 and K2SO4 cause this color
not only Cr2(SO4)3, which has pink color
And in low pH, I dont be sure to know about dichromate :)
Plz explain this problem
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If memory serves me well Cr(III) in solutions is green as long as there are no chlorides.
I am not going to give you a direct answer. First paragraph of the wikipedia page on dichromate contains an important hint.
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Um
So in low pH, It means in acid solution the unstable blue peroxo complex Chromium(VI) oxide peroxide, CrO(O2)2, is formed
CrO(O2)2 is a substance which I have never learn it ::)
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Another hint: redox process.
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I think i dont have any anwser :D
btw, I hear my friend explain about it
due to the strong acid hydrolysis of dichromate, the ethanol presence is inhibiti this hydrolysis
According you, Does this thing right ?
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It is not about hydrolysis. It is about reducing Cr(VI) to Cr(III).
I already told you almost everything, start to follow hints and learn what a redox process is.