O.K. principle is straight forward.
When you expose tin to the Cl2 gas you get SnCl4,
and when you react it with HCl (aq) you get SnCl2.
But it really isn't that simple.
I strongly suspect that you can just gas the hell out of
metal block or wire to get SnCl4 at the room temperature and pressure,and even if you got it,anhydrous form is dangerous chemical weapon.
(I know you can make SnCl4 x 5H20 or "tin butter" out of it by adding water,but how dangerous pure form really is?!)
Do you need to make ß-tin by cooling it and then gass it or what?!
SnCl2 may be weaker catalyst, but sound much easier to make.
Do you simply add metallic tin to the HCl(what concentration
and does it need to be in excess) or what!?
Thanksentropy51 - 3-1-2010 at 14:47
Quote:
Does anybody know how to make SnCl2 and SnCl4 !?
The prep for one (maybe both) is in some of the preparatory inorganic lab manuals in the forum library. There are also threads here that you can
search for. mfilip62 - 3-1-2010 at 15:17
