On the basis of the standard electroe potential values stated for acid solution, predict whether, `Ti^(4+)` species may be used to oxidise `Fe^(II) " to " Fe^(III)`. Given.
`Ti^(4+) +_e^(-) to Ti^(3+),E^(ɵ)=+0.01 V,Fe^(3+)+e^(-) to Fe^(2+),E^(ɵ)=+0.77 V`

(i) On the basis of the standard electrode potential values stated for acid solutions, predict whether Ti^(4+) species may be used to oxidise Fe(II) to Fe(III) {:(Ti^(4+) + e^(-) to Ti^(3+), E^(@) = +0.01V), (Fe^(3+) + e^(-) to Fe^(2+), E^(@)= +0.77V):} (ii) Based on the data arrange Fe^(3+), Mn^(2+) " and " Cr^(2+) in the increasing order of stability of +2 oxidation state. (Give a brief reason) E_(Cr^(3+)//Cr^(2+))^(@) = -0.4V E_(Mn^(3+)//Mn^(2+))^(@) = +1.5V E_(Fe^(3+)//Fe^(2+))^(@) = +0.8V

On the basis of the standard electrode potential velues, state whether Ti^(4+) species can be used to oxidise Fe(II) to Fe(III). Ti^(4+)+e^(-) to Ti^(3+)," "E^(@)=+0.1 V Fe^(3+)+e^(-) to Fe^(2+)," "E^(@)=+0.77 V

On the basis of the following E^(@) values, the stongest oxidizing agent is [Fe(CN)_(6)]^(4-) rarr [Fe(CN)_(6)]^(3-)+e^(-), E^(@) = -0.35 V Fe^(2+) rarr Fe^(3+)+e^(-), E^(@) = -0.77 V

What is the standard reducing potential (E^(@)) for Fe^(3+)to Fe ? (Given that Fe^(2+)+2e^(-)rightarrowFe, E_(Fe^(2+)//Fe^(@)) =-0.47V Fe^(3+) + e^(-)to Fe^(2+) , E_(Fe^(3+)//Fe^(2+))^(@)= +0.77V