azpcpXX
Harmless
Posts: 5
Registered: 8-8-2015
Member Is Offline
Mood: No Mood
|
|
Dissolving unreactive metals in diluted sulfuric acid
My chemistry teacher said that copper and another unreactive metal can be dissolved in diluted sulfuric acid. She says that if you pass oxygen
thrŠ¾ugh diluted sulfuric acid it will become very reactive and can react with copper without heating. I looked for more information about that but i
wasnt able to find anything. Do anyone knows more?
|
|
|
gsd
National Hazard
Posts: 847
Registered: 18-8-2005
Member Is Offline
Mood: No Mood
|
|
I don't know about reaction happening without heating, but it will certainly happen.
In fact even dilute acetic acid reacts with copper in presence of air but it needs reflux temperature. (about 100 Deg C)
gsd
|
|
|
azpcpXX
Harmless
Posts: 5
Registered: 8-8-2015
Member Is Offline
Mood: No Mood
|
|
Do you now about the reaction mechanism, how does oxygen interacts with the hydrogen ions?
|
|
|
gsd
National Hazard
Posts: 847
Registered: 18-8-2005
Member Is Offline
Mood: No Mood
|
|
I guess oxygen converts surface layer of copper into cupric oxide which then reacts with acid to form the salt. The salt gets leached into the
solution exposing fresh surface for further oxidation and so on.
gsd
[Edited on 4-3-2016 by gsd]
|
|
|
woelen
Super Administrator
Posts: 8014
Registered: 20-8-2005
Location: Netherlands
Member Is Offline
Mood: interested
|
|
This indeed works, but the reaction is slow.
As a test, put some copper piece or wire in a thin layer (a few mm) of dilute sulphuric acid in a petri dish and set aside. Do not cover the dish.
Slowly, over the course of days, the copper will dissolve and you get a blue solution. It may be necessary to add water every other day or so, because
of evaporation.
|
|
|
Fulmen
International Hazard
Posts: 1716
Registered: 24-9-2005
Member Is Offline
Mood: Bored
|
|
Another reaction route is Cu0 + Cu2+ = 2Cu+, oxygen can in turn oxidize the Cu+ back to Cu2+.
This reaction is used to leach copper with ammonia and ammonium carbonate to form cupric ammonium carbonate. It's initially very slow, but as the
copper concentration increases it speeds up.
We're not banging rocks together here. We know how to put a man back together.
|
|
|
woelen
Super Administrator
Posts: 8014
Registered: 20-8-2005
Location: Netherlands
Member Is Offline
Mood: interested
|
|
This route only works in the presence of suitable coordinating agents for Cu(+). The ion Cu(+) cannot exist in water without suitable coordinating
agents. It works well in the presence of chloride ions and in the presence of ammonia. Both easily form complexes with Cu(+).
Copper etching with CuCl2 and HCl is based on this reaction. Cu(2+) and chloride ion oxidize copper(0) to copper(I), which dissolves as CuCl2(-).
Oxygen from the air oxidizes the copper(I) to copper(II), and in this process, acid is used as well, hence the need for HCl. The concentration of
copper(II) increases in this situation. Acid needs to be replenished every now and then.
|
|
|
ave369
Eastern European Lady of Mad Science
Posts: 596
Registered: 8-7-2015
Location: No Location
Member Is Offline
Mood: No Mood
|
|
Not only oxygen can do this. Any oxidizer mixed with a non-oxidizing acid lets it react with unreactive metals. Usually, hydrogen peroxide is used,
mixed with either dilute sulfuric or hydrochloric acid.
Smells like ammonia....
|
|
|
![[*]](images/xpblue/default_icon.gif){kind=icon}
