mdahan
Harmless
Posts: 6
Registered: 5-6-2013
Member Is Offline
Mood: No Mood
|
|
Stannous Sulfate
Hey guys I was wondering if you can give me any information on the production of stannous sulfate with the most possible yield. I have looked at a few
way to produce this. Such copper sulfate solution and tin oxide, sulfuric acid and tin, and tin and HCl to stannous chloride, then add sodium
hydroxide and then filter precipatate and then dissolve in sulfuric acid. Any pointers would be nice as well as possible books to read (pages would
be nice ) and where i can find them because I cant find them here on science
madness. Sorry Im new to the forum.
|
|
|
NeutralIon
Harmless
Posts: 28
Registered: 19-6-2005
Member Is Offline
Mood: No Mood
|
|
Tin metal in a solution of CuSO4 -- use an excess of Sn to insure the reaction goes to completion, which is when the initial blue color of the
solution becomes clear.
Knowledge is Good
|
|
|
mdahan
Harmless
Posts: 6
Registered: 5-6-2013
Member Is Offline
Mood: No Mood
|
|
Thanks for the reply. I have done this reaction with tin flakes and still have impurities of copper sulfate within the system. And I wonder if I use
tin powder would that help the reaction go faster and more complete since there is more surface area compared to the flakes? and if get stannic would
adding fresh tin and heating up convert the stannic back to stannous? sorry for all the questions.
|
|
|
Finnnicus
Hazard to Others
Posts: 342
Registered: 22-3-2013
Member Is Offline
|
|
try heating the CuSO4/tin flake suspension, also, leave it for a long time.
|
|
|
WGTR
National Hazard
Posts: 971
Registered: 29-9-2013
Location: Online
Member Is Offline
Mood: Outline
|
|
An easy way is to use your tin metal as an anode, with a sulfuric acid solution as an electrolyte. The anode surface area must be very large
compared to the cathode surface area. You want the anode efficiency to be at least 100%. You should not see any oxygen bubbles forming on the
anode if the current density is low enough. In fact, you want the anode current density to be much lower than the point where gas starts forming.
The cathode need not be more than a small bit of wire touching the electrolyte. A lot of hydrogen will be released from this electrode. Once the
concentration of tin(II) sulfate is high enough in the bath, tin will start plating out on the cathode. Periodically the cathode can be stripped of
its tin, until a sizable collection of tin flakes is left on the bottom of the beaker. This excess tin will ensure that the tin in solution is kept
in the (+2) oxidation state.
The solution must be kept in a sealed container to keep it from being oxidized, with free tin metal in the bottom.
I've made impromptu tin plating baths this way, and have had good results when using pulse/pulse-reverse plating.
edit: oops. got the oxidation states of tin mixed up. 
[Edited on 7-10-2013 by WGTR]
|
|
|
jock88
National Hazard
Posts: 505
Registered: 13-12-2012
Member Is Offline
Mood: No Mood
|
|
http://pubs.acs.org/doi/abs/10.1021/ie50259a027
Try that
|
|
|
![[*]](images/xpblue/default_icon.gif){kind=icon}
