Copper + Nitric Acid
Copper is a reddish-brown metal, widely used in plumbing and electrical wiring; it is perhaps most familiar to people in the United States in the form of the penny. (Although since 1983, pennies are actually made of zinc surrounded by a paper-thin copper foil to give them the traditional appearance of pennies.) Copper is oxidized by concentrated nitric acid, HNO3, to produce Cu2+ ions; the nitric acid is reduced to nitrogen dioxide, a poisonous brown gas with an irritating odor:
Cu(s) + 4HNO3(aq) ——> Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l)
When the copper is first oxidized, the solution is very concentrated, and the Cu2+ product is initially coordinated to nitrate ions from the nitric acid, giving the solution first a green, and then a greenish-brownish color. When the solution is diluted with water, water molecules displace the nitrate ions in the coordinate sites around the copper ions, causing the solution to change to a blue color.
In dilute nitric acid, the reaction produces nitric oxide, NO, instead:
3Cu(s) + 8HNO3(aq) ——> 3Cu(NO3)2(aq) + 2NO(g) + 4H2O(l)
In the following demonstration, a balled-up piece of thin copper wire is added to about 100 mL of concentrated nitric acid; once the copper is added the evolution of nitrogen dioxide occurs quickly. Once all of the copper has reacted, the solution is diluted with distilled water, changing the solution from a dark brown to a pale blue color.
This demonstration can be done with copper in the form of shot, pellets, thicker wire, or bars, but is a great deal slower than with copper wire.
Video Clip: REAL, 7.02 MB
A Historical Sidelight: Ira Remsen on Copper and Nitric Acid
Ira Remsen (1846-1927) founded the chemistry department at Johns Hopkins University, and founded one of the first centers for chemical research in the United States; saccharin was discovered in his research lab in 1879. Like many chemists, he had a vivid "learning experience," which led to a heightened interest in laboratory work:
While reading a textbook of chemistry I came upon the statement, "nitric acid acts upon copper." I was getting tired of reading such absurd stuff and I was determined to see what this meant. Copper was more or less familiar to me, for copper cents were then in use. I had seen a bottle marked nitric acid on a table in the doctor's office where I was then "doing time." I did not know its peculiarities, but the spirit of adventure was upon me. Having nitric acid and copper, I had only to learn what the words "act upon" meant. The statement "nitric acid acts upon copper" would be something more than mere words. All was still. In the interest of knowledge I was even willing to sacrifice one of the few copper cents then in my possession. I put one of them on the table, opened the bottle marked nitric acid, poured some of the liquid on the copper and prepared to make an observation. But what was this wonderful thing which I beheld? The cent was already changed and it was no small change either. A green-blue liquid foamed and fumed over the cent and over the table. The air in the neighborhood of the performance became colored dark red. A great colored cloud arose. This was disagreeable and suffocating. How should I stop this? I tried to get rid of the objectionable mess by picking it up and throwing it out of the window. I learned another fact. Nitric acid not only acts upon copper, but it acts upon fingers. The pain led to another unpremeditated experiment. I drew my fingers across my trousers and another fact was discovered. Nitric acid acts upon trousers. Taking everything into consideration, that was the most impressive experiment and relatively probably the most costly experiment I have ever performed. . . . It was a revelation to me. It resulted in a desire on my part to learn more about that remarkable kind of action. Plainly, the only way to learn about it was to see its results, to experiment, to work in a laboratory.
from F. H. Getman, "The Life of Ira Remsen"; Journal of Chemical Education: Easton, Pennsylvania, 1940; pp 9-10; quoted in Richard W. Ramette, "Exocharmic Reactions" in Bassam Z. Shakhashiri, Chemical Demonstrations: A Handbook for Teachers of Chemistry, Volume 1. Madison: The University of Wisconsin Press, 1983, p. xiv:
!!! Hazards !!!
Nitric acid is extremely corrosive. Handle with care.
The nitrogen dioxide produced in this reaction is poisonous. This reaction must be done in a fume hood!
Ira Remsen's Investigation of Nitric Acid: Lee R. Summerlin, Christie L. Borgford, and Julie B. Ealy, Chemical Demonstrations: A Sourcebook for Teachers, Volume 2, 2nd ed. Washington, D.C.: American Chemical Society, 1988, p. 4-5.
Preparation and Properties of Nitrogen(II) Oxide [a variation on the procedure illustrated above]: Bassam Z. Shakhashiri, Chemical Demonstrations: A Handbook for Teachers of Chemistry, Volume 2. Madison: The University of Wisconsin Press, 1985, p. 163-166.
"Coin-Operated Red, White, and Blue Demonstration": Fountain Effect with Nitric Acid and Copper [a variation on the procedure illustrated above]: Bassam Z. Shakhashiri, Chemical Demonstrations: A Handbook for Teachers of Chemistry, Volume 3. Madison: The University of Wisconsin Press, 1989, p. 83-91.
F. Albert Cotton and Geoffrey Wilkinson, Advanced Inorganic Chemistry, 5th ed. New York: John Wiley & Sons, 1988, p. 769-771.
John Emsley, The Elements, 3rd ed. Oxford, Clarendon Press, 1998, p. 120-121.
David L. Heiserman, Exploring Chemical Elements and their Compounds. New York: TAB Books, 1992, p. 118-121.
Martha Windholz (ed.), The Merck Index, 10th ed. Rahway: Merck & Co., Inc., 1983.
When zinc is added to copper (II) sulfate, a single displacement reaction will take place, creating a solid, copper, and zinc sulfate.
When zinc is added to hydrochloric acid, hydrogen gas will be released a solid, zinc chloride, will be formed.
- Hydrochloric acid
- Copper (II) sulfate
- Test tubes (4)
- Graduated cylinder
- Watch glasses
- Pour 2ml of copper (II) sulfate in a test tube. Record the physical properties of the solution.
- Record the physical properties of zinc.
- Add the zinc to the solution.
- Observe and record the reaction.
- After 30 minutes, record the new colour of the solution and the physical properties of zinc.
- Pour 2 ml of hydrochloric acid into the test tube. Record the physical properties of the solution.
- After recording the physical properties of zinc, add it to the solution.
- Observe and record the reaction.
- What indicated that a chemical reaction took place when zinc and copper (II) sulfate were combined?
- Observations such as zinc turning black soon after being placed in water indicated that a chemical reaction had taken place.
- What indicated that a chemical reaction took place when zinc and hydrochloric acid were combined?
- When zinc and hydrochloric acid were combined, zinc turned black and hydrogen bubbles were released. This indicated that a chemical reaction had taken place.
- Name the reactants in Part A:
- copper (I) sulfate + zinc
- Name the products in Part A:
- zinc sulfate + copper
- Name the reactants in Part B:
- hydrochloric acid + zinc
- Name the products in Part B:
- hydrogen + zinc chloride
- What new elements were formed in Part A? In Part B?
- Part A – copper
Part B – hydrogen
- What new compounds were formed in Part A? In Part B?
- Part A – zinc sulfate
Part B – zinc chloride
- Complete and balance the chemical equations below that represent the chemical reactions, which took place:
- What is a single replacement reaction?
- A single displacement reaction occurs when an element reacts with a compound in a chemical reaction. During the reaction, the element replaces the anion or the cation in the compound.
- Complete and balance the following single replacement reactions:
- Write the names of the reactants and products for the equations listed in question number 12:
|A.||iron||copper (I) sulfate||iron (II) sulfate||copper|
|B.||copper||silver nitrate||copper (I) nitrate||silver|
|C.||zinc||silver nitrate||zinc nitrate||silver|
|D.||copper||mercury (II) chloride||copper (II) chloride||mercury|
|E.||potassium||sodium chloride||potassium chloride||sodium|
|F.||water||calcium||calcium hydroxide||hydrogen gas|
|G.||magnesium bromide||chlorine gas||magnesium chloride||bromine gas|
|H.||iron (III) oxide||aluminum||aluminum oxide||iron|
|I.||sulfuric acid||aluminum||aluminum sulfate||hydrogen gas|
|J.||potassium iodide||chlorine gas||potassium chloride||iodine gas|
In order for a single displacement reaction to occur, an element and a compound need to be present. When the element and the compound are mixed, the element replaces the anion or the cation in the compound. During the experiment, when zinc was added to copper (II) sulfate, zinc reacted with copper (II) sulfate to create zinc sulfate and copper. In this reaction, the element, zinc, replaced copper in the compound copper sulfate, thus creating zinc sulfate. Similarly, when hydrochloric acid reacted with zinc, zinc replaced hydrogen, creating zinc chloride and hydrogen gas.
|Copper (II) sulfate||Blue||Liquid|
Fig 1. Physical properties of the reactants
|Zinc sulfate||Light blue||Liquid|
Fig 2. Physical properties of the reactants
When zinc was added to copper (II) sulfate, it reacted to create a solution, zinc sulfate, and a solid, copper. When zinc was added to hydrochloric acid, hydrogen gas and zinc sulfate were produced, therefore the hypothesis was supported.
Sources of error:
During the experiment, several factors could have possibly affected the results of the observations. One of these factors includes the contamination of the test tubes. After washing the test tubes, water or other acids could have been left behind, affecting the results of the upcoming experiments. Another factor that would have affected the results would have been the inaccurate measurement of the solution. Even if the solution differed by few drops, it could have affected the results.
Clancy, Christina et al. McGraw-Hill Ryerson Chemistry 11. Toronto: McGraw-Hill Ryerson, 2011. Print