vampirexevipex
Hazard to Self
Posts: 62
Registered: 22-2-2012
Location: Puerto Rico
Member Is Offline
Mood: Happy 
|
|
Sepparation Of copper chloride, brine and sodium acetate?
Well today i was working with copper ll chloride dihydrate and accidentally i mixed it with a mixture of sodium acetate with some super saturaded
sodium chloride (brine), and i was wondering... how do i get the copper chloride back? the solution is green btw.
|
|
|
kristofvagyok
National Hazard
Posts: 659
Registered: 6-4-2012
Location: Europe
Member Is Offline
Mood: No Mood
|
|
Quote: Originally posted by vampirexevipex  | | Well today i was working with copper ll chloride dihydrate and accidentally i mixed it with a mixture of sodium acetate with some super saturaded
sodium chloride (brine), and i was wondering... how do i get the copper chloride back? the solution is green btw. |
Mix it with some sodium hydroxide or carbonate and the copper will participate out of the solution. From the copper hydroxide/carbonatre it is easy to
make copper chloride with some hydrochloric acid, but trying to get the copper chloride out from that solution is really hard.
Or maybe try to reduce it to copper(I) chloride what is almost insoluble in solutions and filter it out, than oxidize it back to copper(II).
I have a blog where I post my pictures from my work: http://labphoto.tumblr.com/
-Pictures from chemistry, check it out(:
"You can’t become a chemist and expect to live forever." |
|
|
ManBearSwine
Harmless
Posts: 18
Registered: 27-1-2012
Location: Southern California
Member Is Offline
Mood: No Mood
|
|
Copper(I) Chloride will dissolve in the brine solution due to the formation of a complex ion. Also, unless you have a vacuum filtration apparatus, you
are going to have a hell of a time removing the brine solution from gelatinous precipitate of copper hydroxide or carbonate. I can't think of a
realistic way to directly separate the copper chloride, but you could add a strip of aluminum metal which would react quickly in the brine solution to
reduce the copper to its metallic form. You could then either heat the copper powder to convert it to oxide and dissolve the oxide in hydrochloric
acid, or react the metal with a mixture of hydrogen peroxide and hydrochloric acid (in an ice bath). Depending on the amount in question, it may not
even be worth it.
|
|
|
bbartlog
International Hazard
Posts: 1139
Registered: 27-8-2009
Location: Unmoored in time
Member Is Offline
Mood: No Mood
|
|
Depending on how good a separation you need (and also the amounts of your salts) you could try adding some isopropyl alcohol and see whether it forms
two separate layers. The sodium compounds are scarcely soluble in the alcohol, whereas CuCl2 is moderately soluble, so some of it would be extracted
into the alcohol. Of course only *some* CuCl2 would pass over so you would need to repeat this multiple times; also getting IPA to form a separate
layer from aqueous solution is not always easy. Possibly you'd be best off just starting over.
The less you bet, the more you lose when you win.
|
|
|
![[*]](images/xpblue/default_icon.gif){kind=icon}
