Okie dokez. The goal is to isolate phosphorous acid (H3PO3), after titrating a 400g/l* aq. Solution of potassium phosphites.
The end products formed in the aqueous solution after addition of Hcl will simply bee Kcl, Hcl, and most importantly H3PO3, the desired end product..
Rcently it has been learned that one method to lose much of the Kcl is to extract H3PO3 from the solution using excess Hcl. Hence, leaving the Kcl precipitation behind since it is practically insoluble in concentrated Hcl...
Alcohol I figure would just enhance this effect, that's all. (because kcl isn't very soluble in OH at all either. But HsPO3 is soluble in both OH and h2o)
Separation of the end product and water and alcohol is no problem, as it will just bee evapped after leaving behind the Kcl precipitation.
What do you think Bandil the bandicoot? Charge forward with it boldly on horseback, or, fuggit and wallow away in the castle?
Don't worry about the second question, you gave me enough information, and it would take a lot of really boring background information. Ill have to hack it, should bee A-OK.