When hydrochloric acid is added to a sample of copper why does it look pink at first then form a pale blue solution ?

  • $\begingroup$ Well copper is pink... $\endgroup$ – Mithoron Sep 8 '15 at 22:55
  • $\begingroup$ The copper was not pure but contaminated with another substance. Likely your sweaty oily hands. $\endgroup$ – user5434678 Oct 11 '15 at 16:53

If pure hydrochloric acid is added to a sample of pure copper, there is essentially no reaction; the solution should not turn blue.

At a guess, you're seeing the copper turn pink because it has a significant oxide layer that is reacting with the acid, forming copper (II) chloride and leaving bare the pinkish metal. The solution could be pale blue or pale green, and the time delay of the color would be a result of the amount of time required for the reaction to occur. Note that if this is the case, you would not expect to see any bubbling on the copper, as copper (II) oxide will react with hydrochloric acid to form copper (II) chloride and water.

As Ivan Neretin pointed out in comments, large pieces of copper will react with hydrochloric acid over a period of several hours to days in the presence of air. Permeakra added that a fine copper powder will react in minutes with a solution of hydrochloric acid in the presence of air. In both cases it is the addition of oxygen that causes the copper to react, and in both cases the solution will be a greenish yellow color due to the excess of hydrochloric acid required.

As an example, a student of mine recently asked about this with regard to a penny. We cut open a modern US penny (95% zinc, 5% copper by mass) to expose the zinc core, and placed it in 200mL of 6M HCl. The oxidation layer on the penny was gone almost immediatley after it entered the HCl solution. The zinc reacted quickly and by the next day the penny had been converted into a hollow copper shell. The shell sat in the remaining HCl solution (still 5.7M) over the weekend with no visible reaction but the solution slowly turned green and the copper dissolved completely by the following Friday.

If your solution is turning pink, then I'm not entirely sure what's going on.

| improve this answer | |
  • $\begingroup$ In fact, copper would slowly dissolve in acid in the presence of air, even if initially there were no oxide layer at all. $\endgroup$ – Ivan Neretin Sep 9 '15 at 6:11
  • $\begingroup$ @IvanNeretin Indeed, but this takes a loooong time before the reaction is noticeable, at least with the acid concentrations I've used for this (several days.) Though kay_student doesn't specify a timeline, I assumed it was faster than that. I thought about mentioning the oxidizing acid aspect of HCl and air, but decided against it for simplicity's sake. $\endgroup$ – Jason Patterson Sep 10 '15 at 0:50
  • $\begingroup$ @JasonPatterson This depends on the copper sample. Fine powder in excess of acid dissolves within minutes. $\endgroup$ – permeakra Oct 11 '15 at 17:11
  • $\begingroup$ @permeakra Good point. Edited to include additional information from previous comments. $\endgroup$ – Jason Patterson Oct 11 '15 at 17:13

Your Answer

By clicking “Post Your Answer”, you agree to our terms of service, privacy policy and cookie policy

Not the answer you're looking for? Browse other questions tagged or ask your own question.