posted on Apr, 9 2010 @ 07:01 AM
reply to post by zzombie
Iodine is not solube in water. They report slight solubility due to the presence of 5 ppb average in waters (yet they mention ppm recordings too). 5
ppb is the low limit of detection for inductively coupled plasma spectroscopy that is universally used today to derive this number. Therefore, they
did not factor out the instrument resolution. It is not soluble in water.
The ions you're so fascinated by...triodide is what forms when an alkali based iodide is dissolved in water. So solubility of iodine in any aqueous
solution is the solubility of the iodide ion, not the iodine. Triodide (sp?) is the favored ionic state in an aqueous solution and there is nothing
in the water to drive a reaction to create hypoiodite. There is a hypochlorite species due to water treatment that should not interfere with the
stability of the trioidite.
I'm puzzled why they even mention the reaction the more that I looked at it. To state a potential reaction that is equilibrium is a statement of
nothing. The water is at a ph of 7 so no reaction can occur (i guess the fancy pants scientists like in "equilibrium"). Because it's drinking
water, pH should not be a factor. So, if you're comfortable, it's in equilibrium with hypoiodite and many other reaction products that it won't
form because it's in equilibrium. What's confusing is that (even at ambient temp/atmos press), you would need electrolysis to dissociate the water
molecule. I don't see any other way...just ask the hydrogen fuel cell guys about water...a tough nut to crack.
If they understood water at Lenntech, they wouldn't state that iodine does not occur in nature. Two paragraphs later, they state that iodine is
found naturally in rivers and streams. Actually, it's not iodine, it's an aqueous solution of triodide.
Okay I'm done now, let the insults begin...wait, let me get my coffee first...
[edit on 9-4-2010 by ibiubu]