Is the dissolution of a solid metal in an acidic solution an example of a #"redox reaction?"#

Question

Henry Antrim · Accepted Answer

#Zn(s) + 2HCl(aq) rarr ZnCl_2(aq) + H_2(g)uarr#

The metal is oxidized, and the hydrogen ion is reduced.

#Zn(s) rarr Zn^(2+) + 2e^-#; #"oxidation (i)"# #H^(+) + e^(-) rarr 1/2H_2(g)#; #"reduction (ii)"# We add these equations together such that electrons do not appear in the equation: #(i) +2xx(ii):# #Zn(s) +2H^(+) rarr Zn^(2+) + H_2(g)uarr# We would repeat this for iron metal and sulfuric acid, except that sulfuric acid is a non-oxidizing acid under normal circumstances, and the question SHOULD have been asked with respect to hydrochloric acid or nitric acid. Iron filings will react with #HCl# in precisely the same stoichiometry as zinc: #Fe(s) + 2HCl(aq) rarr FeCl_2(aq) + H_2(g)uarr#

Wyatt Atkins · Answer

undefined Yes, the dissolution of a solid metal in an acidic solution is an example of a redox reaction. In this process, the metal atoms lose electrons (oxidation) to form metal cations, while the hydrogen ions from the acid gain electrons (reduction) to form hydrogen gas. Therefore, both oxidation and reduction occur simultaneously, making it a redox reaction.