Calcium hypoclorite

[mark]

I just found a big tub of this stuff, 68% pure. Its got a verry large oxidiser symbol on it. Any uses for it? I read about potasium chlorate from hypoclorite bleach, could I make chlorate from this stuff? Could I just uses it state off and mix it with a fuel and put it in cratemakers? Any ideas? My mouth watered when I saw that oxidiser sign on it.

[FadeToBlackened]

A search would have yielded your info but,...
Yes, you can make chlorate from it, but no, its not a great oxidizer. Convert it to chlorate or perchlorate

[mark]

How do I concert it to a chlorate? I did a search, and all I found was how to make it from bleach. Also, where can I find potasium chloride?

[tvs17]

Well, let's give you another hint. Bleach contains a solution of sodiumhypochlorite.

Edit: in my country you can find KCl in diet-salt. They contain several percentages, in my country up to 70% KCl. This can be separated from NaCl by fractional recrystallization, since KCl is less soluble than NaCl.



[This message has been edited by tvs17 (edited September 18, 2001).]

[CodeMason]

Fucking hell, I'm sick of hearing this same goddamn question over and over.

[mark]

Yes,I can tell by the verry unhapy smililey of yours. But all the posts I have read make it from a liquid, and I'm dealing with a solid. Does anyone have any instructions?

[Anthony]

"all the posts I have read make it from a liquid"

No. They make it from a solution. Recall what a solution is and apply the idea to your solid.

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"Shit happens. Get a fucking helmet"

[A-BOMB]

Read this here
http://huizen.dds.nl/~wfvisser/EN/chlorate_EN.html#thermal

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live by the bomb
die by the bomb

[tvs17]

<font face="Verdana, Arial" size="2">Originally posted by mark:
Yes,I can tell by the verry unhapy smililey of yours. But all the posts I have read make it from a liquid, and I'm dealing with a solid. Does anyone have any instructions?</font>

Arghhh..
Learn some chemistry man! It may safe your life!

[mark]

Thanks all, you've been varry help full. Ive decided not to try the experiment, as the idea of boiling chemicals does not sound apealing.I might try the electrolic method, though.

[skunkdude]

sorry to be a bitch ladies and gents, but i was wondering how much NaCl i should use for both proceedures (bleach and CaHCI) in A bombs link for making NaCl3 instead of KCl3.

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"Fighting for peace is like fucking for virginity"

[CodeMason]

Calcium hypochlorite is Ca(OCl)₂, since the calcium ion has a charge of +2, and it is hypochlorite, a salt of chloric(I) acid, HOCl. CaHCl would not exist, since there is no H₂Cl acid (hydrogen and chlorine both have valencies of 1), and if it did it would be called calcium hydrochloride or something similar. Chlorate is Cl<u>O</u>₃. Don't forget the O!
Sorry for being finicky, but you really shouldn't be playing with pyrotechnics if you don't even know the very basics like this.

[skunkdude]

Don't appolagise it was a stupid mistake to make, i'm just very tired. Also i'm only an A levle student, unlike most of you guys here who probably have phd's and the like. I'm trying to learn and it's constrictive criticisms like yours which really help. I find that the forum is kind of like a class, where i can learn, except that its more fun.
As much as i hate to admit it, i'm still a newb with much to learn.

p.s. i don't play with pyrotechnics, it is an art, not a toy.

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"Fighting for peace is like fucking for virginity"

[This message has been edited by skunkdude (edited September 27, 2001).]

[CodeMason]

It's alright, I was once a newb too. Chemistry is a breeze once you get the hang of it.

[The_Executioner]

Sorry if this sounds a bit stupid but I have searched many sites (including this one) and found no answer.
Why when making chlorates from calcium hypochlorite or bleach cant aluminium containers/pots be used? It says under equipment when using hypochlorites to make chlorates to use a “heat resistant glass or stainless steel container.” It doesn’t have aluminium container as a selection only stainless steel. Is it because hypochlorites are corrasive in water and may eat the metal away? But that wouldn’t explain that when I have boiled bleach in aluminium pots nothing went wrong.
Thank you very much for your help, The Executioner.

[Mumble]

If it worked for one hypochlorite, don't you think it will still work for the others?

What may have happened with the bleach, if it indeed does corrode Al, is that the white Al2O3/Al(OH)3 may just be unnoticable with the white chlorate. Many metals have colored oxides so it is easy to distinguish, transition metals expecially. Use aluminum containers if you wish, but I wouldn't recomend mother's cooking dishes. At least use a cheap one from goodwill. If it does corrode it's not that big of a deal. You can just filter the oxide out of a hot solution.

[lucas]

QUOTE: "hypochlorite, a salt of chloric(I) acid, HOCl"
CORRECTION: Hypoichlorites are salts of hypochlorous acid HOCl. Chloric acid is HO2Cl and forms chlorites. They are not common and chloric acid only exists in solution, it cant be isolated as a pure species.

Don't use hypochlorite solutions on aluminium. Hypochlorite salts are strong and very unstable oxidisers. They will react with reactive metals when they are exposed to them. Foreign metalic and other ions in mixture with the chlorate salts you seek will make them less stable and can act as catalysts for decomposition in certain mixtures.

Before the "Idefence incident" I posted in this thread about ammonium salts of oxychlorine acids. I also made reference to trichloroisocyanuric acid, CAS [87-90-1], the other chlorinator for pools. This compound, reacts with water to release chlorine and cyanuric acid. It is an unstable compound with potential react with oxidisers, acids,water and reducing agents to form a number of toxic compounds including carbon monoxide hydrogen chloride and nitrogen oxides. It can cause fire with fuels. It is a cyclic compound, the main six membered ring is of alternating Carbon and Nitrogen with carbonyl on the carbons and chlorine on the nitrogens. (Iso)cyanuric acid, CAS [108-80-5], has hydrogen bonded to oxygen bonded to the carbons and alternating double bonds between the carbons and nitrogens.

All ammonium oxychlorine salts are more unstable than the analogs with metalic cations. Ammonium chlorate is a prime example. Before the loss of the old material and posts, ammonium nitrate / hypochlorite salt mixtures were mentioned. I believe this to be a substance of potentially high sensitivity for an ammonium nitrate mixture. If water or other solvents are able to facilitate exchange of ions between ammonium nitrate and, eg, calcium hypochlorite, the particularly unstable ammonium hypochlorite will render the mixture unsafe for storage, and possibly spontaneously combustible with fuels. NM / AN / K chlorate is a mixture of note. It is used as a "reactive target". The sensitivity is facilitated by the formation of ammonium chlorate in the mixture. This is advantageous on occasion but dangerous if not anticipated. I therefore warn and inform others that calcium hypochlorite and other hypochlorite salts are sensitisers for ammonium nitrate. For example sulphur will spontaneously ignite in contact with hydrated calcium hypochlorite. This can be put to use if desired, in the form of a primative delayed smoke grenade. A barrier in the device seperating the two substances is removed before use and the device shaen to mix the substances. Time of delay is commonly around 20 seconds in such devices used by yours truly. The limited amount of oxygen in hypochlorite, ClO- means it is not partilularly usefull as an oxidiser on it's own. Chloride Cl- ions are the usual product of reactions of hypochlorite.

On a not so happy side note hypochlorite will react with secondary carbonyls to form chloroform. Than means the hypochlorite/hypochlorous acid in YOUR drinking water, used to kill bacteria reacts with organic material in natural fresh water to form chloroform in your drinking water. Thats a fact. The same reaction mechanism canbe used to create chloroform from hypochlorite solution and acetone. Is such a case the hypochlorite should be used in solution and addition of acetoneshould be very slow to avoid boiling of the chloroform as the reaction is quite exothermic.
3 mole ClO- : 1 mole acetone.

[cyclonite4]

QUOTE: "hypochlorite, a salt of chloric(I) acid, HOCl"
CORRECTION: Hypoichlorites are salts of hypochlorous acid HOCl. Chloric acid is HO2Cl and forms chlorites. They are not common and chloric acid only exists in solution, it cant be isolated as a pure species.

umm... lucas, hypochlorous acid IS chloric(I) acid. The "I" refers to the oxidation state of the chlorine in the acid. For example, perchloric acid is the same as chloric(VII) acid. It helps when your correcting someone to actually prove what you say.

[tmp]

Using a glass cooking pot(Pyrex or Kimax), put the Ca(OCl)2 in water
and boil for about 30 minutes. The thermal decomposition will result
in Ca(ClO3)2 and CaCl2. Wouter's page discusses the thermal
decomposition of hypochlorites to chlorates and chlorides. Chill the
pot down to freezing. Most of the CaCl2 can be filtered out. The
more the solution is boiled down, the more CaCl2 will precipitate out.

My CRC manual, 52nd Edition, 1971-1972 lists the following solubility
data(in grams per 100 ml water):

CaCl2, 74.5 @ 20 C, 159 @ 100 C

The data for Ca(OCl)2 and Ca(ClO3)2 are listed as soluble, but no
amounts listed.

[FUTI]

Just a simple question...is that pure Ca(OCl)2 or Ca(OCl)2*CaCl2? It makes thing little trickier you know...

[cyclonite4]

Just a simple question...is that pure Ca(OCl)2 or Ca(OCl)2*CaCl2? It makes thing little trickier you know...

The 'granulated pool chlorine' bought from pool/hardware stores is fairly pure Ca(OCl)2.4H2O, when doing stoich. with it you have to make sure you account for the water of hydration, otherwise it will fuck up like my friends attempt at KClO3 from Ca(OCl)2.4H2O (He thought it was Ca(OCl)2 ), and as a result he ended up with an impure sample which proved almost useless, thanks to excess KCl.