Standard electrode potential data are used for understanding the stability of an oxidant in a redox titration . Some half reactions and their standard potentials are given below: MnO_4^(-) (aq) +8H^(+)(aq)+5e^(-)rarrMn^(2+)(aq)+4H_2O(l) ""E^@=1.51V Cr_2O_7^(2-) (aq)+14H^(+)(aq)+6e^(-) rarr 2Cr^(3+)(aq)+7H_2O(l) ""E^@=1.38V Fe^(3+)(aq)+e^(-) rarr Fe^(2+)(aq) ""E^@=0.77V Cl_2(g)+2e^(-) rarr2Cl^(-) (aq)""E^@=1.40V Identify the only incorrect statement regarding the quantitative estirnation of aqueous Fe(NO_3)_2.

Standard electrode potential data are used for understanding the stabi

1.	Standard electrode potential data are used for understanding the stability of an oxidant in a redox titration . Some half reactions and their standard potentials are given below: MnO_4^(-) (aq) +8H^(+)(aq)+5e^(-)rarrMn^(2+)(aq)+4H_2O(l) ""E^@=1.51V Cr_2O_7^(2-) (aq)+14H^(+)(aq)+6e^(-) rarr 2Cr^(3+)(aq)+7H_2O(l) ""E^@=1.38V Fe^(3+)(aq)+e^(-) rarr Fe^(2+)(aq) ""E^@=0.77V Cl_2(g)+2e^(-) rarr2Cl^(-) (aq)""E^@=1.40V Identify the only incorrect statement regarding the quantitative estirnation of aqueous Fe(NO_3)_2.
Answer» `MnO_4^(-)` can be used inaqueous HCL `Cr_2O_7^(2-)` can be used in aqueous HCl `MnO_4^(-)` can be used inaqueous `H_2SO_4` `Cr_2O_7^(2-)` can be used in aqueous `H_2SO_4` SOLUTION :`MnO_4^(-)` will positive , the reaction is spontaneous . `2KMnO_4+16H^(+)+16Cl^(-)rarr 2Mn^(2+)+8H_2O+5Cl_2` The corresponding CELL is `Pt\|Cl_2(g)\|Cl^(-)(aq)\|\|MnO_(4)^(-)(aq), Mn^(2+),H^(+)\|Pt` `E_("cell")^@=E^@` (cathode) `-E^@` (anode) = 1.51 - 1.40 = 0.11 V Since , `E_("cell")^@` is +ve , the above reaction is feasible . Therefore , `MnO_4^(-)` will oxidise both `Fe^(2+) and Cl^(-)` IONS in aqueous medium . THUS, quantitative estimation of `Fe(NO_3)_2` is not suitable.