The standard potential of a Co^{2+} | Co elec | vedclass

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(B) The cell reaction is: $Ti^{2+}(aq.) + Co^{2+}(aq.) \rightarrow Ti^{3+}(aq.) + Co(s)$.$E_{cell}^o = E_{cathode}^o - E_{anode}^o$.Here,the cathode i

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$0.37$

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(B) The cell reaction is: $Ti^{2+}(aq.) + Co^{2+}(aq.) \rightarrow Ti^{3+}(aq.) + Co(s)$.$E_{cell}^o = E_{cathode}^o - E_{anode}^o$.Here,the cathode is the $Co^{2+}|Co$ electrode and the anode is the $Ti^{3+}|Ti^{2+}$ electrode.$E_{cell}^o = E_{Co^{2+}|Co}^o - E_{Ti^{3+}|Ti^{2+}}^o$.Given $E_{cell}^o = 0.09 \ V$ and $E_{Co^{2+}|Co}^o = -0.28 \ V$.$0.09 = -0.28 - E_{Ti^{3+}|Ti^{2+}}^o$.$E_{Ti^{3+}|Ti^{2+}}^o = -0.28 - 0.09 = -0.37 \ V$.The electrode potential for the oxidation half-reaction $Ti^{2+} \rightarrow Ti^{3+} + e^-$ is the negative of the reduction potential $E_{Ti^{3+}|Ti^{2+}}^o$.Therefore,$E_{Ti^{2+}|Ti^{3+}}^o = -(-0.37 \ V) = 0.37 \ V$.

$V^{2+}_{(aq)} + 2e^{-} \rightarrow V_{(s)}$	$E^0 = -1.19 \ V$
$Fe^{3+}_{(aq)} + 3e^{-} \rightarrow Fe_{(s)}$	$E^0 = -0.04 \ V$
$Ag^{+}_{(aq)} + e^{-} \rightarrow Ag_{(s)}$	$E^0 = 0.80 \ V$
$Au^{3+}_{(aq)} + 3e^{-} \rightarrow Au_{(s)}$	$E^0 = 1.40 \ V$

The standard potential of a $Co^{2+} | Co$ electrode is $-0.28 \ V$ and the standard potential of the cell $Pt | Ti^{2+}(aq.), Ti^{3+}(aq.) || Co^{2+}(aq.) | Co_{(s)}$ is $0.09 \ V$. What is the standard potential of the $Ti^{2+}(aq.) | Ti^{3+}(aq.)$ electrode (in $V$)?

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