(A) The standard reduction potential of $Fe^{3+}/Fe^{2+}$ is $+0.77 \ V$. In a mixture of $H_{2}SO_{4}$ and $H_{3}PO_{4}$, $Fe^{3+}$ ions react with p

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formation of the species $[FeHPO_{4}]^{+}$

(A) The standard reduction potential of $Fe^{3+}/Fe^{2+}$ is $+0.77 \ V$. In a mixture of $H_{2}SO_{4}$ and $H_{3}PO_{4}$, $Fe^{3+}$ ions react with phosphate ions to form a stable complex, $[FeHPO_{4}]^{+}$. According to the Nernst equation, $E = E^{\circ} - (0.059/n) \log(1/[Fe^{3+}])$. As the concentration of free $Fe^{3+}$ ions decreases due to complex formation, the reduction potential decreases from $+0.77 \ V$ to $+0.61 \ V$.

Class 12 Chemistry Electrochemistry Electrode potential and ECell

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The formal potential of $Fe^{3+}/Fe^{2+}$ in a sulphuric acid and phosphoric acid mixture $(E^{\circ}=+0.61 \ V)$ is much lower than the standard potential $(E^{\circ}=+0.77 \ V)$. This is due to

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A
formation of the species $[FeHPO_{4}]^{+}$
B
lowering of potential upon complexation
C
formation of the species $[FeSO_{4}]^{+}$
D
high acidity of the medium

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Electrode potential and ECell

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The standard electrode potential $(E^{\circ}_{M^{3+}/M^{2+}})$ for $V$,$Cr$,$Mn$,and $Co$ are $-0.26 \ V$,$-0.41 \ V$,$+1.57 \ V$,and $+1.97 \ V$,respectively. The metal ions which can liberate $H_2$ from a dilute acid are

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For $Mg^{2+} + 2e^{-} \rightarrow Mg_{(s)}$,$E^{0} = -2.37 \, V$ and for $Cu^{2+} + 2e^{-} \rightarrow Cu_{(s)}$,$E^{0} = +0.33 \, V$. The $emf$ of the cell $(E^{0}_{Cell})$ is .......... $V$.

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The $EMF$ of a cell in terms of the reduction potential of its left and right electrodes is:

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The $E^{\ominus}$ for $Cl_{2}/Cl^{-}$ is $+1.36 \ V,$ for $I_{2}/I^{-}$ is $+0.53 \ V,$ for $Ag^{+}/Ag$ is $+0.79 \ V,$ $Na^{+}/Na$ is $-2.71 \ V$ and for $Li^{+}/Li$ is $-3.04 \ V.$ Arrange the following ionic species in decreasing order of reducing strength: $I^{-}, Ag, Cl^{-}, Li, Na$

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Discuss the method to determine the cell potential of any cell when a standard hydrogen electrode is considered as the anode,with a suitable example.

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The formal potential of $Fe^{3+}/Fe^{2+}$ in a sulphuric acid and phosphoric acid mixture $(E^{\circ}=+0.61 \ V)$ is much lower than the standard potential $(E^{\circ}=+0.77 \ V)$. This is due to

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The standard electrode potential $(E^{\circ}_{M^{3+}/M^{2+}})$ for $V$,$Cr$,$Mn$,and $Co$ are $-0.26 \ V$,$-0.41 \ V$,$+1.57 \ V$,and $+1.97 \ V$,respectively. The metal ions which can liberate $H_2$ from a dilute acid are

For $Mg^{2+} + 2e^{-} \rightarrow Mg_{(s)}$,$E^{0} = -2.37 \, V$ and for $Cu^{2+} + 2e^{-} \rightarrow Cu_{(s)}$,$E^{0} = +0.33 \, V$. The $emf$ of the cell $(E^{0}_{Cell})$ is .......... $V$.

The $EMF$ of a cell in terms of the reduction potential of its left and right electrodes is:

The $E^{\ominus}$ for $Cl_{2}/Cl^{-}$ is $+1.36 \ V,$ for $I_{2}/I^{-}$ is $+0.53 \ V,$ for $Ag^{+}/Ag$ is $+0.79 \ V,$ $Na^{+}/Na$ is $-2.71 \ V$ and for $Li^{+}/Li$ is $-3.04 \ V.$ Arrange the following ionic species in decreasing order of reducing strength: $I^{-}, Ag, Cl^{-}, Li, Na$

Discuss the method to determine the cell potential of any cell when a standard hydrogen electrode is considered as the anode,with a suitable example.

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