Use the standard reduction potentials below to determine which of the following metals can be oxidized by 1.0 M
HCl: Al,Zn,Sn,Cu.
$\begin{array}{l}
\mathrm{Al}^{3+}(a q)+3 e-\rightarrow \mathrm{Al}(s) & \bar{E}_{1 e d}^{0}=-1.68 \mathrm{~V}\
\mathrm{Zn}^{2+}(a g)+2 e^{-} \rightarrow \mathrm{Zn}(s) & E_{\circ \mathrm{z}}=-0.762 \mathrm{~V}\
\mathrm{Sn}^{2+}(a q)+2 e-\underline{\mathrm{Sn}}(s) & E_{o \mathrm{z}}^{0}=-0.141 \mathrm{~V}\
\mathrm{Cu}^{2+}(a q)+2 e^{-} \rightarrow \mathrm{Cu}(s) &E_{\mathrm{red}=+0.339 \mathrm{~V}}^{\rho}
\end{array}$

Question

Use the standard reduction potentials below to determine which of the following metals can be oxidized by 1.0 M 
HCl: Al,Zn,Sn,Cu. 
$\begin{array}{l}
\mathrm{Al}^{3+}(a q)+3 e-\rightarrow \mathrm{Al}(s) & \bar{E}_{1 e d}^{0}=-1.68 \mathrm{~V}\
\mathrm{Zn}^{2+}(a g)+2 e^{-} \rightarrow \mathrm{Zn}(s) & E_{\circ \mathrm{z}}=-0.762 \mathrm{~V}\
\mathrm{Sn}^{2+}(a q)+2 e-\underline{\mathrm{Sn}}(s) & E_{o \mathrm{z}}^{0}=-0.141 \mathrm{~V}\
\mathrm{Cu}^{2+}(a q)+2 e^{-} \rightarrow \mathrm{Cu}(s) &E_{\mathrm{red}=+0.339 \mathrm{~V}}^{\rho}
\end{array}$

Quizplus · Accepted Answer

The standard reduction potential for $H^+ \rightarrow H_2$ is $0 \,V$. Metals with a more negative reduction potential compared to $H^+$ can be oxidized by $HCl$. Al, Zn, and Sn have more negative potentials than $0 \,V$, so they can be oxidized by $HCl$, while Cu cannot because its potential is positive.

Use the Standard Reduction Potentials Below to Determine Which of the Following