Does copper metal disolve in hot HCl?

Answer 1

yes. sure
I think all metal, except gold and platinum, disolve in hot HCl

Answer 2

There is no reaction between copper and hot concentrated HCl alone. This is primarily due to the positive electrode potential of copper. HCl is not an oxidising acid, either.

However, if a mixture of copper metal, copper(II) chloride and concentrated HCl is heated, a reverse disproportionation reaction occurs, and on dilution copper(I) chloride, CuCl, is seen as a white precipitate.

Answer 3

Lancenigo di Villorba (TV), Italy

YES, IT DOES!

GENERALITIES
In the electrochemical series you can see that copper is a chemical species more noble than hydrogen.
The fast statement that you retrieve might be the following :
"I need oxiding acids for dissolve metalic copper".
In effect, aqueous nitric acid's solutions do it.
Hydrochloric acid is not an oxidizing reactive, so you may think it is not influent.
In electrochemical series you retrieve another information, that is concentrated hydrochloric acid's aqueous solutions modify electrochemical potential of copper.
You forgive the following electrodic half-reaction :
Cu++(aq) + 2e ---> Cu(s)
and you begin considerate the other one :
CuCl(s) + e ---> Cu(s) + Cl-(aq)
Nonetheless hydrogen ions become not a chemical specie more noble than copper's compounds, you may see some copper's corrosion phenomena.

ANOTHER WAY
What it happens? If you permit a good aeration of a strong HCl's solution, the air's oxygen execute copper's oxidation, so you obtain copper's compounds (e.g. CuCl in whitish flakes).
You need day and days for this process....several weeks will permit you see a pale greenish coloration of the liquid, thus part of CuCl become copper soluble compounds (e.g. HCuCl2 as dichloro-cupric(I) acid, CuCl2 as copper(II) chloride).

CONCLUSION
Preceeding answers suggested you a mixture of copper(II) chloride in concentrated hydrochloric acid's aqueous solution. This is a fast lab's way to obtain copper's corrosion phenomenon.
I suggest you a "cheaper" method, in effect requesting not some chemical stuffs (e.g. where you can buy CuCl2?). My feature need good aeration of concentrated aqueous solution...it is NOT FAST.

I hope this helps you.

Answer 4

I perform a niffty demonstration for my students using copper pennies (dated prior to 1972) and nitric acid. The reaction is quite impressive, with a lot of bubbling, reddish gasses being produce, quite exothermic . . . and the copper pennies dissolve. I imagine that HCl would work, but haven't tried it myself. The HCl would have to be concentrated.

CHEMISTRY TEACHER

Answer 5

So, it really does not 'dissolve'. It 'reacts', forming new substances.

Get an "A".