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

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(B) The cell reaction is $Ti^{2+} + Co^{2+} \rightarrow Ti^{3+} + Co$. The standard cell potential is given by $E_{cell}^{o} = E_{cathode}^{o} - E_{an

Vedclass · Accepted Answer

$0.37$

Vedclass · Answer

(B) The cell reaction is $Ti^{2+} + Co^{2+} \rightarrow Ti^{3+} + Co$. The standard cell potential is given by $E_{cell}^{o} = E_{cathode}^{o} - E_{anode}^{o}$. Here,the cathode is the $Co^{2+}|Co$ electrode and the anode is the $Ti^{2+}|Ti^{3+}$ electrode. $E_{cell}^{o} = E_{Co^{2+}|Co}^{o} - E_{Ti^{3+}|Ti^{2+}}^{o}$. Substituting the given values: $0.09 \ V = -0.28 \ V - E_{Ti^{3+}|Ti^{2+}}^{o}$. $E_{Ti^{3+}|Ti^{2+}}^{o} = -0.28 \ V - 0.09 \ V = -0.37 \ V$. The standard oxidation potential is the negative of the standard reduction potential: $E_{ox}^{o} = -E_{red}^{o} = -(-0.37 \ V) = 0.37 \ V$.

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 oxidation potential of the $Ti^{2+}_{(aq)}|Ti^{3+}_{(aq)}$ electrode? ............. $V$

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