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InterviewSolution
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Standard electrode potential data are useful for understanding the suitability of an oxidant in a redox titration. Some half cell reaction and their standard potentials are given below `MnO_(4)^(-)(aq)+8H^(+)(aq)+5e^(-)toMn^(2+)(aq)+4H_(2)O(l)" "E^(@)=1.51V` `Cr_(2)O_(7)^(2-)(aq)+14H^(+)(aq)+6e^(-)to2Cr^(3+)(aq)+7H_(2)O(l)" "E^(@)=1.38V` `Fe^(3+)(aq)+e^(-)toFe^(2+)(aq)" "E^(@)=0.77V` `Cl_(2)(g)+2e^(-)to2Cl^(-)(aq)" "E^(@)=1.40V` Identify the only incorrect statement regarding the quantitative estimation of aqueous `Fe(NO_(3))_(2)`A. `MnO_(4)^(-)` can be used in aqueous HClB. `Cr_(2)O_(7)^(2-)` can be used in aqueous HClC. `MnO_(4)^(-)` can be used in aqueous `H_(2)SO_(4)`D. `Cr_(2)O_(7)^(2-)` can be used in aqueous `H_(2)SO_(4)` |
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Answer» Correct Answer - A `MnO_(4)^(-)` will oxidize `Cl^-` ion according to the equation, `2MnO_(4)^(-)+16H^(+)+10Cl^(-)to2Mn^(2+)+8H_(2)O+5Cl_(2)uarr` The cell corresponding to this reaction is as follows: `Pt,Cl_(2)("1 atm")|Cl^(-)||MnO_(4)^(-), Mn^(2+),H^(+)|Pt,` `E_(cell)^(o)=1.51-1.40=0.11V` `E_(cell)^(o)` bring +ve, `DeltaG^(o)` will be -ve and hence the above reaction is feasible. `MnO_(4)^(-)` will not only oxidize `Fe^(2+)` ion but also `Cl^(-)` ion simultaneously. |
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