Why does copper not replace hydrogen from acids?
(N/A) The ability of a metal to replace hydrogen from acids depends on its standard electrode potential $(E^{\circ})$.
Metals with a negative standard reduction potential can reduce $H^+$ ions to $H_2$ gas.
Copper $(Cu)$ has a positive standard electrode potential $(E^{\circ}_{Cu^{2+}/Cu} = +0.34 \ V)$.
Because its reduction potential is higher than that of hydrogen $(E^{\circ}_{H^+/H_2} = 0.00 \ V)$,copper cannot act as a reducing agent to displace hydrogen from acids.
Metals with a negative standard reduction potential can reduce $H^+$ ions to $H_2$ gas.
Copper $(Cu)$ has a positive standard electrode potential $(E^{\circ}_{Cu^{2+}/Cu} = +0.34 \ V)$.
Because its reduction potential is higher than that of hydrogen $(E^{\circ}_{H^+/H_2} = 0.00 \ V)$,copper cannot act as a reducing agent to displace hydrogen from acids.
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