(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

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(B) The cell reaction is $Ti^{2+} + Co^{2+} \rightarrow Ti^{3+} + Co$. The standard cell potential is given by $E_{cell}^{o} = E_{cathode}^{o} - E_{anode}^{o}$. 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: $E_{ox}^{o} = -E_{red}^{o} = -(-0.37 \ V) = 0.37 \ V$.

Class 12 Chemistry Electrochemistry Electrode potential and ECell

Medium

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? ............. $V$

A
$-0.37$
B
$0.37$
C
$-0.19$
D
$0.19$

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Class 12

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Electrochemistry

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Electrode potential and ECell

Given below are the half-cell reactions: $Mn^{2+} + 2e^- \rightarrow Mn$ $(E^0 = -1.18 \text{ V})$; $Mn^{3+} + e^- \rightarrow Mn^{2+}$ $(E^0 = +1.51 \text{ V})$. The $E^0_{cell}$ for $3Mn^{2+} \rightarrow Mn + 2Mn^{3+}$ will be . . . . . .

DifficultKCET 2026

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For the cell $Zn_{(s)} | Zn^{2+}_{(aq)} || M^{x+}_{(aq)} | M_{(s)}$,different half cells and their standard electrode potentials are given below:
$M^{x+}_{(aq)} / M_{(s)}$ $Au^{3+}_{(aq)} / Au_{(s)}$ $Ag^{+}_{(aq)} / Ag_{(s)}$ $Fe^{3+}_{(aq)} / Fe^{2+}_{(aq)}$ $Fe^{2+}_{(aq)} / Fe_{(s)}$
$E^o M^{x+} / M (V)$ $1.40$ $0.80$ $0.77$ $-0.44$

If $E^o Zn^{2+}/Zn = -0.76 \ V$,which cathode will give a maximum value of $E^o_{cell}$ per electron transferred?

DifficultJEE MAIN 2019

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If the $E^{0}$ values for $Mg^{+2} | Mg$,$Zn^{+2} | Zn$,and $Fe^{+2} | Fe$ are $-2.37 \ V$,$-0.76 \ V$,and $-0.44 \ V$ respectively,which statement is correct?

Medium

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Aluminium displaces hydrogen from acids but copper does not. $A$ galvanic cell prepared by combining $Cu/Cu^{2+}$ and $Al/Al^{3+}$ has an e.m.f. of $2.0 \ V$ at $298 \ K$. If the potential of copper electrode is $+0.34 \ V$,that of aluminium is .......... $V$

Medium

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Addition of powdered lead and iron to a solution which is $1.0 \, M$ in both $Pb^{2+}$ and $Fe^{2+}$ would result in [$E^{\circ}_{Fe^{2+}/Fe} = -0.44 \, V$ and $E^{\circ}_{Pb^{2+}/Pb} = -0.13 \, V$]

Medium

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$M^{x+}_{(aq)} / M_{(s)}$	$Au^{3+}_{(aq)} / Au_{(s)}$	$Ag^{+}_{(aq)} / Ag_{(s)}$	$Fe^{3+}_{(aq)} / Fe^{2+}_{(aq)}$	$Fe^{2+}_{(aq)} / Fe_{(s)}$
$E^o M^{x+} / M (V)$	$1.40$	$0.80$	$0.77$	$-0.44$

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? ............. $V$

Similar Questions

Given below are the half-cell reactions: $Mn^{2+} + 2e^- \rightarrow Mn$ $(E^0 = -1.18 \text{ V})$; $Mn^{3+} + e^- \rightarrow Mn^{2+}$ $(E^0 = +1.51 \text{ V})$. The $E^0_{cell}$ for $3Mn^{2+} \rightarrow Mn + 2Mn^{3+}$ will be . . . . . .

If the $E^{0}$ values for $Mg^{+2} | Mg$,$Zn^{+2} | Zn$,and $Fe^{+2} | Fe$ are $-2.37 \ V$,$-0.76 \ V$,and $-0.44 \ V$ respectively,which statement is correct?

Aluminium displaces hydrogen from acids but copper does not. $A$ galvanic cell prepared by combining $Cu/Cu^{2+}$ and $Al/Al^{3+}$ has an e.m.f. of $2.0 \ V$ at $298 \ K$. If the potential of copper electrode is $+0.34 \ V$,that of aluminium is .......... $V$

Addition of powdered lead and iron to a solution which is $1.0 \, M$ in both $Pb^{2+}$ and $Fe^{2+}$ would result in [$E^{\circ}_{Fe^{2+}/Fe} = -0.44 \, V$ and $E^{\circ}_{Pb^{2+}/Pb} = -0.13 \, V$]

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