At 10:01 13/06/2002 +0000, AGROFEKTA wrote: >Message: 7 > Date: Thu, 13 Jun 2002 09:56:44 -0000 > From: "agroefekta" <[EMAIL PROTECTED]> >Subject: How to make calcium chloride? > >I have read some time before that CaCl2 can be used to "dry" alcohols >as well as esters. >I am not good in chemistry, but believe that reaction of CaO and HCl >can produce CaCl 2. >Im my country there are many manufacturers of Cao, so I could make it >quite easy. > >One more question. Can this salt be recovered after it has been used >for dehidration? >===================================================
Hi, Yes you can use solid calcium chloride to dry organic liquids. But why you like to hurt your self with a very dangerous and almost explosive reaction of CaO with HCL? This reaction would be so exothermic ( giving of heat) that you find it hard to keep the chems in a container ( if it's plastic it will even melt!) So please " don't do this at home !!! "... never ever! BTW the HCL is actuel a gas dissolved in water, not good for eyes and lungs! There is even no reason to, because CaO might be cheap and HCL ( which is a industrial waste product or by-product) and also cheap; the Calciumcloride you want to make is also easily available, is also a industrial by-product cq waste product and also, or even cheaper than your HCL. It normal commercial use ( of CaCL 2 ) is melt salt for de-icing roads ( table salt go's to -9ĄC, CaCL2 go's to -21ĄC ). So here in Europe it cost less than 0.50 euro or ¤ per Kilo depending on the quantity you will buy. Normally sold in PE sacs of 5 and 50 Kg. Solvay is the best known firm of producing it ( world famous Belgian company ;-) but any brand will do. http://www.solvaycaso.com/safety_environment/0,5508,3324-_EN,00.html You can find it in refills for those dehumidifiers for cellars and so, like this one: http://be.bison.net/servlet/AdvisorServlet20?cmd=show&id=283&ident1=28&ident2=0 You would have an other problem by producing it your self, You need CaCl2 ( anhydride ) the reaction you describes will give you Ca CL2.2H2O, that is, every CaCL2 molecule has 2 molecules of water to it. So you have to cook the crystal mass to get that water out. Now about recuperating used CaCL2, if the crystals ( or pellets) are nearly saturated with water, it is possible to put them in an oven on +- 110ĄC for a wile until the bounded water is evaporated, but is it economically interesting? I don't know it out of my head, but that Cacl2 is not the best "dryer" for "every" organic fluid, what I mean is that it possibly dissolves a bit in some fluids and not in others, I'm afraid it might dissolve in your alcohols because alcohol and water are both 'polaire' solvents. So that have to be checked first ( if dissolved CaCL2 in the alcohol, might hinder its further use in your process.) Maybe I'll find an answer to that for you tomorrow. So Long Bruno Meersman ( Belgian chemist ) ----------------------------------------------------- Reply's to [EMAIL PROTECTED] ------------------------ Yahoo! Groups Sponsor ---------------------~--> Will You Find True Love? Will You Meet the One? Free Love Reading by phone! http://us.click.yahoo.com/Deo18C/zDLEAA/Ey.GAA/FGYolB/TM ---------------------------------------------------------------------~-> Biofuel at Journey to Forever: http://journeytoforever.org/biofuel.html Biofuels list archives: http://archive.nnytech.net/ Please do NOT send "unsubscribe" messages to the list address. To unsubscribe, send an email to: [EMAIL PROTECTED] Your use of Yahoo! Groups is subject to http://docs.yahoo.com/info/terms/
