Question

Why can a solid copper penny be dissolved in nitric acid, but not in hydrochloric acid? Modern pennies are made from zinc metal plated with copper. What happens to a modern penny when it is placed inside a bath of hydrochloric acid after the penny is scratched, exposing some of the zinc?

Answer 1

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Answer 2

Answer:

• Contrary to concentrated hydrochloric acid, which is not a strong oxidising agent and does not react with copper, concentrated nitric acid has the ability to oxidise copper to soluble copper(II) ions.
• In addition to a heated, concentrated solution of blue copper(II) nitrate, the reaction results in reddish-brown nitrogen dioxide gas.
• Cu(NO3)2(s) crystals start to form as the solution cools and the water evaporates.

$Cu(s) + 4HNO_3(aq) - > Cu(NO_3)_2(aq) + 2NO_2(g) + 2H_2O(l)$

• 1982-era pennies were either constructed of bronze or a zinc core with a copper plating.
• Hydrochloric acid and zinc react quickly, with the zinc replacing the hydrogen atoms to produce aqueous zinc chloride and hydrogen gas.
• On the other hand, under normal circumstances copper will not take the place of the hydrogen.
• This is represented by a metal reactivity series, such as the one below.
• The metals in the series are ordered according to decreasing levels of reactivity.
• The metals mentioned below a specific metal can be used in their place.
• Sodium, for instance, may take the place of all metals below it, including lithium, barium, and so forth.
• The metals below sodium, meanwhile, were unable to release sodium. Sodium can only be replaced by potassium.

$Zn (s) + 2 HCl (aq) - > ZnCl_2 (aq) + H_2 (g)$

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