fusso
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KI+HNO3->KIO3 fail?
Trying to make some iodate by adding excess HNO3 to 0.5g KI (assume byproduct is NO2) and I2 is formed but didn't disappear to form HIO3 even after a
few days. Why?
[Edited on 190704 by fusso]
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Sulaiman
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HNO3 is an oxidising acid, the result that you got is the expected one
https://chemiday.com/en/reaction/3-1-0-6575
CAUTION : Hobby Chemist, not Professional or even Amateur
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Ubya
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https://www.sciencedirect.com/science/article/pii/0022190275...
It works but you need azeotropic nitric acid, maybe your acid was not strong enough?
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fusso
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@Sulaiman I do expect HNO3 to oxidise I- to I2, but I also expect HNO3 to oxidise I2 up to HIO3 too![:(](./images/smilies/sad.gif)
@Ubya Do you have the rest of the paper?
[Edited on 190704 by fusso]
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Boffis
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@fusso, wouldn't it be better to liberate the free iodine first and then oxidise it with nitric acid? It would certainly be more economical on the
nitric acid. Also check out Brauer's book in the SM library.
Are you aware of the chlorate oxidation process for producing iodates/iodic acid? This route is covered in great detail in the Inorganic Preparations
series of books which can be downloaded from the internet.
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Ubya
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@fusso
https://zero.sci-hub.se/1597/fb68cdbc1bce08575418686b47aff11...
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Boffis
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Mmmmm Ubya, that's an interesting paper but turning the data in it into a useful prep. is going to require a pretty good chemist. Brauer contains a
workable method with both nitric acid and nitric acid+H2O2.
The main issue I see with these methods is the low molar efficiency based on nitric acid. While nitric acid is cheap it is getting increasing
difficult to obtain for the amateur. Mind you so is 30% H2O2.
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Ubya
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Quote: Originally posted by Boffis ![](images/xpblue/lastpost.gif) | Mmmmm Ubya, that's an interesting paper but turning the data in it into a useful prep. is going to require a pretty good chemist. Brauer contains a
workable method with both nitric acid and nitric acid+H2O2.
The main issue I see with these methods is the low molar efficiency based on nitric acid. While nitric acid is cheap it is getting increasing
difficult to obtain for the amateur. Mind you so is 30% H2O2. |
i know, it's not a preparative paper, more a study on kinetics, but at least demonstrates that it is possible to use nitric acid, it just needs to be
concentrated enough, that was my point
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fusso
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@Boffis unfortunately I don't have any chlorates
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clearly_not_atara
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"The oxidation of iodine to iodate by hydrogen peroxide", Guy Schmitz, Physical Chemistry Chemical Physics, 2001.
Now that's a journal name!
Attachment: schmitz2001.pdf (117kB) This file has been downloaded 311 times
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Tsjerk
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Haha, and they even have an impact factor of almost 4!
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