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Help with potassium chlorate


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#61 Arthur

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Posted 17 October 2020 - 03:55 AM

The product as tested by the two listed youtubers works, It comes cheaply from China. Whether anyone here want's to be limited to a one amp cell who knows. Whether the Chinese electrode pair would survive 24/7/365 use who knows!

 

One of the arts of household bleach is using it weakly enough to kill bio without it destroying lots of other things (dyes, fabrics etc. )



#62 AnthonyGibson

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Posted 17 October 2020 - 07:52 AM

As mentioned before, this is done by treating the raw brine with sodium carbonate and sodium hydroxide, which causes the calcium, magnesium and even some iron ions to drop out of solution as flocculant precipitates. This means the contaminating minerals bind together and form heavier particles which eventually drop to the bottom of the container.

 

The resulting, purified brine is then poured (decanted) off the precipitated minerals and collected in separate containers for further treatment before being used for our electro-chemical cell. The precipitated sediment can be further vacuum filtered to remove the last remaining brine, which can be added to the rest of our purified brine and the left over precipitates disposed of. The filtration is done using SLOW grade filter paper (with very small, microscopic pores) because the precipitated minerals are a very fine dust when dry. Due to the extremely small pores of the filter paper, the filtering process usually proceeds slowly.

 

One final step I've used is to test the pH of the purified brine. Typically, after treating with alkali reagents, the pH is high. By treating the purified brine with very small amounts of hydrochloric acid drop-wise, the pH can be lowered to roughly neutral (pH 7.0), or slightly lower, which is ideal for our chlorate cells.

 

WSM, what sort of quantities were you using of the sodium carbonate and sodium hydroxide, say per 1kg of sodium chloride?
 



#63 WSM

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Posted 22 October 2020 - 12:04 PM

WSM, what sort of quantities were you using of the sodium carbonate and sodium hydroxide, say per 1kg of sodium chloride?


Per 4 gallons of sodium chloride solution (350g NaCl/liter H2O, if I remember correctly), I used about 350 ml of 1M sodium carbonate solution.

Sodium carbonate solution in water is more alkaline than expected because some sodium hydroxide is also formed as the carbonate is dissolved.

When I added the 1M Na2CO3 solution to the brine, it instantly turned milky white. After sitting for a day, the fine precipitates of calcium carbonate and magnesium hydroxide, had dropped to the bottom of the 5 gallon HDPE bucket I used for a reaction vessel.

After decanting the clear brine into another new bucket, I vacuum filtered the rest of the slurry through a fine laboratory filter in a Buckner funnel, to separate the fine solids from the residual brine.

The clear, purified brine tested alkaline, so I added HCl dropwise till the brine was neutral to slightly acid, and pure enough to run in my sodium chlorate cell.

I fully expect a similar process will work in a potassium chloride brine.

WSM B)

Edited by WSM, 22 October 2020 - 12:09 PM.





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