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Author: Subject: Problem in Chlorate
pioneer
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[*] posted on 18-10-2012 at 03:09
Problem in Chlorate


Hello everyone I'm new ..
I have a problem making Chlorate and I really need help I Lha see the problem
Well I will have a cell size of 2 liters amplifier 5 volts 20 amps anode and a cathode titanium put on every liter of water 350 grams of sodium chloride that worked 10 hours and nothing was created just nothing Remarks my tank made ​​of plastic if this problem can someone explain to me what the problem is and help me Please thank everyone


[Edited on 18-10-2012 by pioneer]
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hyfalcon
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[*] posted on 18-10-2012 at 03:23


Titanium by itself will not make Chlorate. You need Platinized titanium or MMO titanium or a PbO2 anode to be able to produce chlorate. Carbon will work also.
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plante1999
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[*] posted on 18-10-2012 at 03:36


Sodium chlorate won't precipitate in these condition. You would be better to use potassium chloride.



I never asked for this.
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[*] posted on 18-10-2012 at 03:46


So you're saying instead of putting sodium chloride to potassium chloride? And the cathode and anode is Titan mmo

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plante1999
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[*] posted on 18-10-2012 at 04:01


You said you used sodium chloride. You need to use potassium chloride, pyro.



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[*] posted on 18-10-2012 at 04:07


Okay so now I bought potassium chloride will it in a few hours I would say if something is created

And that's all my problem? Just put potassium chloride without sodium chloride?



[Edited on 18-10-2012 by pioneer]

[Edited on 18-10-2012 by pioneer]
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plante1999
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[*] posted on 18-10-2012 at 04:12


Yes that's the problem, of course you need to have current connected to the electrodes, It may precipitate in a few day (especially if there is no electricity), so wait.

[Edited on 18-10-2012 by plante1999]




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[*] posted on 18-10-2012 at 04:13


Thank you very much now I do it and a few hours will return an answer

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hissingnoise
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[*] posted on 18-10-2012 at 05:30


Quote:
You said you used sodium chloride. You need to use potassium chloride.

NaCl is the correct salt to use in chlorate synthesis!
The K salt, because of its relatively low solubility can precipitate large crystals of KClO3 on electrodes, with potential damage to fragile anode coatings!
The high solubility of NaClO3 means solution saturation seems to take ages but the solution, if filtered hot, will on cooling, precipitate fairly pure chlorate!

Metathesis then with KCl is a breeze . . .

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[*] posted on 18-10-2012 at 05:47


Heated three liters of water and added kcl and now I'm giving it to cool, and I see some salt water returned back to room temperature I put it in the tank and starts the process hope to work

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hyfalcon
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[*] posted on 18-10-2012 at 05:49


Quote: Originally posted by hissingnoise  
Quote:
You said you used sodium chloride. You need to use potassium chloride.
NaCl is the correct salt to use in chlorate synthesis!
The K salt, because of its relatively low solubility can precipitate large crystals of KClO3 on electrodes, with potential damage to fragile anode coatings!
The high solubility of NaClO3 means solution saturation seems to take ages but the solution, if filtered hot, will on cooling, precipitate fairly pure chlorate!

Metathesis then with KCl is a breeze . . .



If his end use is pyro related the left over sodium in your product can ruin your colors in stars. It's better to start with KCl and deal with the lower solubility than to have to go through several recrystallizations to achieve a clean product.



[Edited on 18-10-2012 by hyfalcon]
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[*] posted on 18-10-2012 at 06:03


I started the process and the water starts to get yellow color
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hissingnoise
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[*] posted on 18-10-2012 at 06:12


There should be but little Na contamination from the mother-liquors and this can be largely removed by repeated tossing of the product on absorbent paper!
If ultra-pure chlorate is what's required, then a very large excess of HCl added to the saturated solution of NaClO3 will precipitate essentially all of the NaCl present, leaving a fairly strong sol. of HClO3!

The acid should be handled with care ─ 'highly dangerous in contact with organic materials . . .

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[*] posted on 18-10-2012 at 06:14


Now my electrolysis works with saturated solution of kcl and water have become a bit Yellows it good? It starts to produce crystals or what?


Can anyone tell me if I'm on the right track for making chlorate cell 3 gallon 20 amp 5 V cathode and anode titanium mmo that runs half an hour and the solution turned yellow, some is good???


[Edited on 18-10-2012 by pioneer]
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[*] posted on 18-10-2012 at 06:44


Until now not even one grain why???

I make a solution of salt should I use tap water or distilled water?


[Edited on 18-10-2012 by pioneer]
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hyfalcon
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[*] posted on 18-10-2012 at 07:21


Run for 2 days and get back to us. It takes time.
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[*] posted on 18-10-2012 at 07:56


Well just now I did something last titanium cathode and anode My steel is good?
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hyfalcon
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[*] posted on 18-10-2012 at 09:14


Do not use steel. I would use carbon electrodes before attempting steel.
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[*] posted on 18-10-2012 at 09:37


I recommend against carbon electrodes. They disintegrate rapidlu, leaving your product dirty looking and contaminated with carbon.
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[*] posted on 18-10-2012 at 10:04


Quote:
If ultra-pure chlorate is what's required, then a very large excess of HCl added to the saturated solution of NaClO3 will precipitate essentially all of the NaCl present, leaving a fairly strong sol. of HClO3!

'My apologies, that's the procedure for perchloric acid.

Chloric acid is a bit too unstable for such metathesis . . .

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[*] posted on 18-10-2012 at 10:04


I have no coal so I use iron and titanium that can lead me to Chlorate?
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[*] posted on 18-10-2012 at 10:05


I have to figure out something I see a man 20 amperes 5 V 3-liter container that can produce Chlorate me please answer me yes or no if not then what to do?
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[*] posted on 18-10-2012 at 11:45


Not without the anode materials I've already posted above.
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[*] posted on 18-10-2012 at 13:55


It does not work There is nothing that's why I have mmo titanium and it does not work can someone give me step by step instructions including how to make saturated salt solution thanks
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[*] posted on 18-10-2012 at 13:58


I hate to sound like and echo in here, but try using the search button. There is quite a bit already covering this topic already posted. Better material then I can repeat here.

Here, go do some more reading:

http://www.oxidizing.110mb.com/chlorate/chlorate.html

[Edited on 18-10-2012 by hyfalcon]
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