Copper Metal and Nitric Acid
Many of the less metals (copper is one example) that do not react with hydrochloric acid will react with concentrated nitric acid. They do not produce hydrogen gas (as is the case when reactive metals such as zinc or aluminum react with hydrochloric acid) but react to produce brown nitrogen dioxide gas. The nitrogen dioxide results from reduction of the nitrate ion. This is considered to be a reduction because in the nitrate ion nitrogen has an oxidation state of +5 but in nitrogen dioxide it has an oxidation state of +4; the oxidation state of the nitrogen is therefore decreased or "reduced." We can represent this process with the half-reaction shown below.
2H+ + NO3- = NO2 + H2O
In turn, the solid copper is oxidized to copper(II), which
dissolves in the solution. We can represent this process with the hald-reaaction
Cu(s) = Cu2+(aq) + 2e-
Most students of chemsitry are familiar with the blue color of the copper(II) ion. However, copper is only blue when water moelecules are coordinated to it. In concentrated nitric acid, the nitrate ions are coordinated to the copper(II) ion, imparting a green color to the solution as the reaction proceeds. Finally, in the last portion of the video, the solution turns blue as water is added and the nitric acid is diluted.
|Copper metal is added to
concentrated nitric acid
|Evolution of brown nitrogen
dioxide gas begins
|Evolution of gas continues||Water is added; acid is diluted and
reaction is quenched
Hazards: concentrated nitric acid is extremely
corrosive and is a strong oxidizer; it should be handed with care. This
nitrogen dioxide gas generated by this reaction is hazardous. This reaction
should be performed only in a fully functional fume hood.
Download the video here
(Windows AVI formation, Microsoft Video9 Compression)
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