dann2 - 28-7-2007 at 12:52
Hello,
Can SnCl4:5H20 be converted easily to Anhydrous SnCl4?
TIA,
Dann2
garage chemist - 28-7-2007 at 12:55
Cant you just make anhydrous SnCl4? Not that it would be difficult, someone made it in a simple distillation setup with Sn granules in the pot and a
tube for leading in chlorine. The SnCl4 distilled off as it formed.
dann2 - 28-7-2007 at 13:09
Hello,
I was going to try that and then I found a source of SnCl4:5H20. I want SnCl4:5H20 and I would like anydrous SnCl4 too.
The SnCl4:5H2O is about 38 euro for 500 grams.
If I make the Anhydrous SnCl4 will I be able to convert that to SnCl4:5H2O?
It is a bit of a chicken and egg siutation.
Dann2
Xenoid - 28-7-2007 at 15:43
SnCl4 is prepared by the action of chlorine on molten metallic tin. It is a colourless fuming liquid, which boils at 114.1oC, and fumes strongly in
moist air. The action of a little moisture converts it into the solid pentahydrate SnCl4.5H2O, known as oxymuriate of tin, which is used as a mordant.
With an excess of water, basic chlorides and ultimately stannic acid are formed:
SnCl4 + H2O <-> Sn(OH)Cl3 + HCl
Sn(OH)Cl3 + 3H2O <-> Sn(OH)4 + 3HCl
That from my Mellor's!
Xenoid
Eclectic - 28-7-2007 at 16:24
You can't easily get anhydrous SnCl4 from SnCl4.(H2O)5. You can't easily and safely get SnCl4.(H2O)5 from anhydrous SnCl4.
If you don't trust the chemistry, or yourself to be able to do the inorganic prep. work, just buy it.
Otherwize, you know already how to make hydrated SnCl4, just evaporate, crystallize, and filter if you want to get some dry material.
A medium glass frit works well to gravity filter saturated SnCl4.(H2O)5 solutions.
[Edited on 7-28-2007 by Eclectic]
dann2 - 28-7-2007 at 18:03
Thanks Electic,
Perhaps I will go that way. I'm doing alot of toing and froeing at the moment.
Dann2