Consider these half-reactions: $$ \begin{array}{lr} \hline \text { Half-Reaction } & \boldsymbol{E}^{\circ}(\mathrm{V}) \\ \hline \mathrm{Ce}^{4+}(\mathrm{aq})+\mathrm{e}^{-} \longrightarrow \mathrm{Ce}^{3+}(\mathrm{aq}) & 1.72 \\ \mathrm{Ag}^{+}(\mathrm{aq})+\mathrm{e}^{-} \longrightarrow \mathrm{Ag}(\mathrm{s}) & 0.80 \\ \mathrm{Hg}_{2}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-} \longrightarrow 2 \mathrm{Hg}(\ell) & 0.80 \\ \mathrm{Sn}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-} \longrightarrow \mathrm{Sn}(\mathrm{s}) & -0.14 \\ \mathrm{Ni}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-} \longrightarrow \mathrm{Ni}(\mathrm{s}) & -0.25 \\ \mathrm{Al}^{3+}(\mathrm{aq})+3 \mathrm{e}^{-} \longrightarrow \mathrm{Al}(\mathrm{s}) & -1.68 \\ \hline \end{array} $$ (a) Which is the weakest oxidizing agent? (b) Which is the strongest oxidizing agent? (c) Which is the strongest reducing agent? (d) Which is the weakest reducing agent? (e) Will Sn(s) reduce $\mathrm{Ag}^{+}$ (aq) to $\mathrm{Ag}(\mathrm{s})$ ? (f) Will $\mathrm{Hg}(\ell)$ reduce $\mathrm{Sn}^{2+}(\mathrm{aq})$ to $\mathrm{Sn}(\mathrm{s}) ?$ (g) Name the ions that can be reduced by $\operatorname{Sn}(\mathrm{s})$. (h) Which metals can be oxidized by $\mathrm{Ag}^{+}(\mathrm{aq})$ ?
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In this case, it is $\mathrm{Al}^{3+}(\mathrm{aq})$ with a standard reduction potential of $-1.68 \, \mathrm{V}$. Show more…
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Consider these half-reactions: $$ \begin{array}{lr} \hline \text { Half-reaction } & E^{\circ}(\mathrm{V}) \\ \hline \mathrm{Ce}^{4+}(\mathrm{aq})+\mathrm{e}^{-} \longrightarrow \mathrm{Ce}^{3+}(\mathrm{aq}) & 1.72 \\ \mathrm{Ag}^{+}(\mathrm{aq})+\mathrm{e}^{-} \longrightarrow \mathrm{Ag}(\mathrm{s}) & 0.80 \\ \mathrm{Hg}_{2}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-} \longrightarrow 2 \mathrm{Hg}(\ell) & 0.80 \\ \mathrm{Sn}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-} \longrightarrow \mathrm{Sn}(\mathrm{s}) & -0.14 \\ \mathrm{Ni}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-} \longrightarrow \mathrm{Ni}(\mathrm{s}) & -0.25 \\ \mathrm{Al}^{3+}(\mathrm{aq})+3 \mathrm{e}^{-} \longrightarrow \mathrm{Al}(\mathrm{s}) & -1.68 \\ \hline \end{array} $$ (a) Which is the weakest oxidizing agent? (b) Which is the strongest oxidizing agent? (c) Which is the strongest reducing agent? (d) Which is the weakest reducing agent? (e) Will $\mathrm{Sn}(\mathrm{s})$ reduce $\mathrm{Ag}^{+}(\mathrm{aq})$ to $\mathrm{Ag}(\mathrm{s}) ?$ (f) Will $\mathrm{Hg}(\ell)$ reduce $\mathrm{Sn}^{2+}(\mathrm{aq})$ to $\mathrm{Sn}(\mathrm{s}) ?$ (g) Name the ions that can be reduced by $\operatorname{Sn}(\mathrm{s})$. (h) Which metals can be oxidized by $\mathrm{Ag}^{+}(\mathrm{aq}) ?$
Consider these half-reactions: $$ \begin{array}{lr} \hline \text { Half-Reaction } & E^{\circ}(\mathrm{V}) \\ \hline \mathrm{Ce}^{4+}(\mathrm{aq})+\mathrm{e}^{-} \longrightarrow \mathrm{Ce}^{3+}(\mathrm{aq}) & 1.61 \\ \mathrm{Ag}^{+}(\mathrm{aq})+\mathrm{e}^{-} \longrightarrow \mathrm{Ag}(\mathrm{s}) & 0.80 \\ \mathrm{Hg}_{2}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-} \longrightarrow 2 \mathrm{Hg}(\ell) & 0.79 \\ \mathrm{Sn}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-} \longrightarrow \mathrm{Sn}(\mathrm{s}) & -0.14 \\ \mathrm{Ni}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-} \longrightarrow \mathrm{Ni}(\mathrm{s}) & -0.25 \\ \mathrm{Al}^{3+}(\mathrm{aq})+3 \mathrm{e}^{-} \longrightarrow \mathrm{Al}(\mathrm{s}) & -1.66 \\ \hline \end{array} $$ (a) Which is the weakest oxidizing agent? (b) Which is the strongest oxidizing agent? (c) Which is the strongest reducing agent? (d) Which is the weakest reducing agent? (e) Will Sn(s) reduce $\mathrm{Ag}^{+}$ (aq) to $\mathrm{Ag}(\mathrm{s})$ ? (f) Will $\mathrm{Hg}(\ell)$ reduce $\mathrm{Sn}^{2+}(\mathrm{aq})$ to $\mathrm{Sn}(\mathrm{s})$ ? (g) Name the ions that can be reduced by $\operatorname{Sn}(s)$. (h) Which metals can be oxidized by $\mathrm{Ag}^{+}(\mathrm{aq})$ ?
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