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Esplosivo
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Being a hypochlorite I suppose that on heating >70 deg C it would disproportionate in the same way sodium hypochlorite does. The passage of
chlorine through hot, conc. calcium hydroxide was at one time the method of production of chlorates, the calcium chlorate produced being reacted with
KCl and the KClO3 crystallized.
Edit: I don't suppose this had anything to do with the thread except to show that calcium hypochlorite cannot be decomposed by heat, although I
do think that water is required for a disproprotionation to occur.
May I suggest bubbling carbon dioxide through a conc. solution of calcium hypochlorite in an isolated site. This would produce carbonic acid which
would probably react with the hypochlorite to give chlorine (you're in the desert, so the small quantity given off over a long time should not be
a problem) and calcium carbonate, which is surely not a problem to dispose of. Somebody correct me if I am wrong.
[Edited on 22-4-2005 by Esplosivo]
Theory guides, experiment decides.
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sparkgap
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Esplosivo, nice suggestion, but methinks he'd have to apply pressure of some sort so that an appreciable concentration of carbonic acid is
present. Besides, normal daytime desert temperatures tend to disfavor dissolution of gases into water, but maybe a cooling system of some sort can
rectify this, or they can run it in the nighttime, when the temperature is more agreeable.
What is the Henry's law constant for CO<sub>2</sub> anyway?
sparky (^_^)
"What's UTFSE? I keep hearing about it, but I can't be arsed to search for the answer..."
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Esplosivo
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I am no university chem student (in fact I am more of the biochem/medicine guy - lets see next year), but according to my poorish knowledge of
Henry's law constant (which I did not do at school), the inverse of this constant multiplied by the partial pressure of the gas above the
solution should give the molar solubility. Now assuming that carbon dioxide gas is at one atmosphere above the solution (Henry's constant being
29.76 atm/(mol/dm3) at 25 deg C) the molar solubiltiy should be about 0.034moles/dm3.
More would dissolve as more of the CO2 reacts with the hypochlorite, since the dissolved conc. of CO2 decreases. I suppose a cooling jacket would be
necessary to increase solubility.
IIRC, this fact about carbonic acid decomposing is why the solid calcium hypochlorite smells of chlorine, but I might be mistaken.
[Edited on 22-4-2005 by Esplosivo]
Theory guides, experiment decides.
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neutrino
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Actually, the bisulfite would form sodium chloride and <b>calcium</b> sulfate, which would precipitate. Don’t try filtering it out,
though, as CaSO<sub>4</sub> forms a gelatinous mass that is almost impossible to filter out in this form.
A wild idea (it probably won’t work, though) goes as follows: add sodium sulfate to your calcium hypochlorite solution. Spread out the resulting
gelatinous mass in the sun. The sodium hypochlorite will decompose while drying, leaving sodium chloride and chlorate. I’m not sure how hazardous
those are, though.
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MadHatter
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Ca(OCl)2
Sarge, if you're in a desert, I would try baking it in the sun. I don't know how long it
would take but eventually it will decompose into chlorine and calcium oxide. Of
course, I also don't know what environmental regulations you're bound by either.
In a way I envy you. Personally, if I had to dispose of 800 LBS, I'd dissolve it in water,
boil it for 30 minutes, throw away the chloride, and keep the chlorate that's left.
Yes, the hypochlorite, boiled in water will thermally decompose into the chlorate and
chloride. Check Wouter's page about that one.
From opening of NCIS New Orleans - It goes a BOOM ! BOOM ! BOOM ! MUHAHAHAHAHAHAHA !
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sparkgap
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A little ponderance for our intrepid HazMat manager:
Should you end up converting your hypochlorite to chlorate, you may not want to dispose of this in or near an area with a plant population, since
chlorate is a nice total herbicide.
sparky (^_^)
"What's UTFSE? I keep hearing about it, but I can't be arsed to search for the answer..."
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frogfot
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Is there a way to decompose aqueous hypochlorite without changing the pH in solution?
I'm trying to estimate OH- concentration in chlorate cell electrolyte by titration with phenolphtalein as indicator.. but the indicator discolors
too fast.. Oh, and heating it event for 0,5 hours doesn't help..
How would for example H2O2 or sodium formeate react with hypochlorite..?
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verode
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try with urea CO(NH2)2 + water
or Na2SO3
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Sgt HAZMAT
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We are thinking of a unique solution. Keep those ideas flowing!!!
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vulture
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You're in the army right? Can your kitchen unit donate about 100lbs of sugar to you? 
Mix the stuff, then call the EOD, tell them you have some unstable old rocket fuel and they'll probably end up blowing it right there in your
desert.
You have alot of fun and get an easy disposal 
One shouldn't accept or resort to the mutilation of science to appease the mentally impaired.
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neutrino
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Urea can react with hypochlorites to form explosive NCl<sub>3</sub>.
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praseodym
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Or you can bubble chlorine gas through a solution of ammonium nitrate to get NCl3. NCl3 is exciting as it is very reactive and explosive but storage
could be a problem as it is easily decomposed into ammonia and chlorine due to its high unstability (especially when it is pure).
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neutrino
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We're trying to <b>avoid</b> anythig dangerous here. Several dozen liters of ultra-sensitive high explosive isn't something you
want to have to deal with.
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sparkgap
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praseodym, he's going for a way to safely dispose of hypochlorite... jeez... FCOL, he's a freakin' HazMat Manager!!! He'd be in deep shit for trying that stunt of yours...
vulture was taking the damn piss...
sparky (~_~)
"What's UTFSE? I keep hearing about it, but I can't be arsed to search for the answer..."
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