Terminus_Est
Harmless
Posts: 9
Registered: 9-10-2012
Member Is Offline
Mood: No Mood
|
|
What exactly is produced when copper is added to a mixture of vinegar, H2O2, and NaCL table salt?
I know that copper acetate is produced when copper is added to a mixture of just vinegar and peroxide, but what about salt?
So today in a small 16 oz jar I made a really saturated solution of vinegar and salt and added pieces of copper wire to it and then poured some
hydrogen peroxide into the mix. Then I noticed a vigorous reaction in which the peroxide was consumed quicker than what I've normally observed with a
plain vinegar/H2O2 mix. The solution turned blue-green rather quickly also. But I want to know is that when NaCL is added, does it affect the end
product in any way or is it merely just catalyzing the reaction and decomposition of H2O2 without getting consumed?
[Edited on 8-7-2013 by Terminus_Est]
|
|
|
watson.fawkes
International Hazard
Posts: 2793
Registered: 16-8-2008
Member Is Offline
Mood: No Mood
|
|
The chlorine is forming a complex around the copper, helping to solvate it. There's lot of material on this board about this system, in part because
of the copper/chloride system as an etchant for printed circuit boards.
|
|
|
violet sin
International Hazard
Posts: 1480
Registered: 2-9-2012
Location: Daydreaming of uraninite...
Member Is Offline
Mood: Good
|
|
how to clean copper pots....
you will get copper in solution as much as the vinegar will allow, what it does from there is messy. equilibrium between the following should occur.
NaCl solubility 359 g/100ml
CuCl2 solubility 75.7 g/100 mL (25 °C
NaOAc sol 46.4 g/100 mL (20 °C)
Cu(OAc)2 sol 7.2 g/100 mL cold
20 g/100 mL (hot water) all sol data from wiki
NaCl being the most soluble of all, I would think the equilibrium would be favored by NaCl + Cu(OAc)2 predominantly. but you would still have notable
contamination of NaOAc + CuCl2 *I think*. equilibrium stuff was a WHILE ago for me so this is best I can do, and subject to error.
@ watson, does the equilibrium I speak of exist enough to be a prob? or am I dead wrong and the Cl- stays w/ Na+ only? like I stated it has been a
while
|
|
|
Terminus_Est
Harmless
Posts: 9
Registered: 9-10-2012
Member Is Offline
Mood: No Mood
|
|
@ violet
So both copper chloride and acetate are formed is that right? If so is there any way the copper chloride can be separated out of the whole mess?
|
|
|
sargent1015
Hazard to Others
Posts: 315
Registered: 30-4-2012
Location: WI
Member Is Offline
Mood: Relaxed
|
|
Lol, ok guys, making copper chloride is much easier than this.
1) Buy copper sulfate (Super cheap chemical!! 10 pounds of it!)
2) Precipitate with sodium carbonate (Baking soda that has been decomposed, also very cheap).
3) Isolate and rinse off sodium sulphate (filter)
4) React CuCO3 with storebought HCl
5) Boil off water and excess HCl (Outside, obviously)
Separating copper acetate and copper chloride will not happen. Why waste time, money, and resources for something so cheap and abundant?
|
|
|
Terminus_Est
Harmless
Posts: 9
Registered: 9-10-2012
Member Is Offline
Mood: No Mood
|
|
Yes I know that there are quicker and easier methods to making CuCl2 but right now I am more interested in exploring the science and using
what I already have available to me.
[Edited on 9-7-2013 by Terminus_Est]
|
|
|
![[*]](images/xpblue/default_icon.gif){kind=icon}
