plante1999
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Question about iodate IO3-
I have two question:
Wath is the esiest way to make KIO3 from KI and HIO3 from I2?
I know that Cl2 in H2O + I2 make HIO3 but it will make large amount of HCl....
Thanks!!!
I never asked for this.
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hkparker
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I did a video on making potassium iodate from iodine, and I was told the process would work as well with KI but I cannot confirm through
experimentation, If that helps.
http://www.youtube.com/watch?v=RJBmNYKyb7s
As for making HIO3, you might be able to crystallize it from KIO3 and HCl, but I am not sure. Wikipedia claims it is a soluble solid so thats what
gave me the idea, not sure on its solubility curve.
My YouTube Channel
"Nothing is too wonderful to be true if it be consistent with the laws of nature." -Michael Faraday
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plante1999
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I already saw the video but I dont have nitrate (nitric acid)..... As an oxidiser I have NaClO, Ca(ClO)2 , NaClO3, 3%H2O2 and if I want I can
synthesise KClO3.
[Edited on 27-9-2011 by plante1999]
I never asked for this.
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AndersHoveland
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KI can be oxidized to KIO3 by using NaOCl bleach.
Iodine can be oxidized to iodic acid by using concentrated nitric acid.
Reaction of iodine with ozone
Iodine, I2 is not reactive towards with oxygen, O2, or nitrogen, N2. However, iodine does react with ozone, O3, the second allotrope of oxygen, to
form the unstable yellow I4O9, the nature of which is perhaps I(IO3)3.
Equilibrium of iodine with water
Iodine, I2, reacts with water to produce hypoiodite, OI-. The position of the equilibrium depends very much upon the pH of the solution.
I2(l) + H2O(l) <==> OI-(aq) + 2H+(aq) + I-(aq)
Reaction of iodine with the halogens
Iodine, I2, reacts with fluorine, F2, at room temperature to form the pentafluoride iodine(V) fluoride. At 250°C the same reaction affords the
heptafluoride iodine(VII) fluoride. With careful control of the reaction conditions, (-45°C, suspension in CFCl3), it is posible to isolate the
trifluoride iodine(III) fluoride.
I2(s) + 5F2(g) → 2IF5(l) [colourless]
I2(g) + 7F2(g) → 2IF7(g) [colourless]
I2(s) + 3F2(g) → 2IF3(s) [yellow]
Iodine, I2, reacts with bromine, Br2, form the very unstable, low melting solid, interhalogen species iodine(I) bromide.
I2(s) + Br2(l) → 2IBr(s)
Iodine reacts with chlorine at -80°C with excess liquid chlorine to form "iodine trichloride", iodine (III) chloride, actually I2Cl6. Iodine reacts
with chlorine in the presence of water to form iodic acid.
I2(s) + 3Cl2(l) + I2Cl6(s) [yellow]
I2(s) + 6H2O(l) + 5Cl2(g) → 2HIO3(s) + 10HCl(g)
Reaction of iodine with oxidizing acids
Iodine reacts with hot concentrated nitric acid to form iodic acid. The iodic acid crystallizes out on cooling
3I2(s) + 10HNO3(aq) → 6HIO3(s) + 10NO(g) + 2H2O(l)
Reaction of iodine with bases
Iodine, I2, reacts with hot aqueous alkali to produce iodate, IO3-. Only one sixth of the total iodine is converted in this reaction.
3I2(g) + 6OH-(aq) → IO3-(aq) + 5I-(aq) + 3H2O
[Edited on 27-9-2011 by AndersHoveland]
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plante1999
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Are you sure that NaClO + KI make Iodate and not Periodate? If it dont make periodate it will be an interessing way
I ave read that Because I2 is more stable with oxygen bond that chlorine Chlorate + iodate will make iodate + chloride.
KI + KClO3 -) KCl + KIO3
For Iodic acid I think I will do something like this (to test if it work).
Ca(ClO3)2 + H2SO4 + I2 -) Cl2 + CaSO4 + HIO3
HIO3 could be extracted with water.
[Edited on 27-9-2011 by plante1999]
I never asked for this.
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woelen
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Electrolysis of a solution of KI is a perfect way of makong iodate. Use graphite or platinum electrodes. I have a page on my website about this
process for making bromate from bromide, but it works equally well for making iodate.
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plante1999
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Quote: Originally posted by woelen  | | Electrolysis of a solution of KI is a perfect way of makong iodate. Use graphite or platinum electrodes. I have a page on my website about this
process for making bromate from bromide, but it works equally well for making iodate. |
Thanks!!!
I never asked for this.
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