50AE Posted November 30, 2010 Posted November 30, 2010 I'm planning to make Ba(ClO3)2 for my greens for NYE by electrolysis, but there's a problem. Solubilities of BaCl2 and Ba(ClO3)2 are very close. If I recrystallize the product and wash it with water, many of the chlorate will be lost. So I have two ideas. 1. Adding a lead nitrate solution to the electrolyte. Insoluble lead chloride should precipitate out and there will be barium nitrate in the solution, which won't hurt the color and it's also slightly soluble, so it can be precipitated as well.What I'm not sure it's the solubility of lead chlorate. Is it soluble? Can't find information about it. Also it is stable, so traces of it won't pose safety problems? Pb(NO3)2 + BaCl2 -> PbCl2 + Ba(NO3)2 2. Evaporating the whole eletrolyte until the crystals form, and then pouring them in methanol. Barium chloride should dissolve in the methanol, but the chlorate should not, as far as I read.
bikemaster Posted November 30, 2010 Posted November 30, 2010 There is some tips on production of barium chlorate there : http://oxidizing.110mb.com/chlorate/barium.html
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