Potassium Hydroxide Separation

Potassium Hydroxide Separation Rate Topic:

#21 5 March 2012 - 02:13 PM Suxamethonium

Baryon

The point of it is that more can dissolve once the sulfate or carbonate precipitates- thats why it is included as a solid and 'washed' with water. That is also why I proposed my initial procedure to try- its the same principle without the ash (using readily available suflate instead)- I still think its worth a try but its up to you. Kudos if you can be arsed to get the clippings and burn them.

Edit- sentence structure.

This post has been edited by Suxamethonium: 5 March 2012 - 02:14 PM

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#22 5 March 2012 - 07:09 PM John Cuthber

Chemistry Expert

elementcollector1, on 1 March 2012 - 04:19 AM, said:

Still, 0.173 is rather small. What about electrolysis? Or is there a more soluble hydroxide that converts to an insoluble carbonate?

http://en.wikipedia....arium_hydroxide
does better but it's rather toxic and much more difficult to get hold of.

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#23 5 March 2012 - 10:46 PM elementcollector1

Baryon

John Cuthber, on 5 March 2012 - 07:09 PM, said:

http://en.wikipedia....arium_hydroxide
does better but it's rather toxic and much more difficult to get hold of.

Luckily for me, I have a baryte rose I can convert if necessary, but not a lot.
So, I think electrolysis is still the best route here (no possible contaminants except for K₂CO₃). So, what is the best setup for this? I have a 12V plug-in adapter for electricity (does that convert amps as well?) Should I use carbon electrodes (taken from zinc-carbon batteries, I also have titanium if necessary)? What kind of apparatus should I use? I've heard that I should use two beakers with a saltwater-soaked tissue between them, and a saturated solution of KCl in each. Is there a better way to maintain electron flow between the two half-cells (gold wire)?
Sorry for the barrage of questions, I've tried electrolysis of KCl before with not-so-good results (9V battery source).

EDIT: Trying this with a 6V cell (made of 4 of those fat Duracell's), gold anode, graphite cathode (14k gold corroded), and an aqueous solution of NaCl. Will measure pH when the thing stops bubbling.

This post has been edited by elementcollector1: 5 March 2012 - 11:38 PM