Standard electrode potentials are given as under :
`Ti^(4+)+e^(-)toTi^(3+)E^(@)=+0.01V`
`Fe^(3+)+e^(-)toFe^(2+)E^(@)=+0.77V`
Tell whether `Ti^(4+)` ion may be used to oxidies `F^(II)` to `Fe^(III)` .

Explanation

The given reaction is :
`Fe^(2+)+Ti^(4+)toFe^(3+)+Ti^(3+)`
The electrochemical cell based upon above redox reaction is :
`underset("Anode")Fe^(2+)|Fe^(3+)||underset("Cathode")Ti^(4+)|Ti^(3+)`
`E_("cell")^(@)=E_("cathode")^(@)-E_("anode")^(@)`
`=0.01-0.77`
`=-0.76V`
Since `E^(@)` cell is negative, `:.Ti^(4+)` cannot be used to oxidise `Fe^(2+)` to `Fe^(3+)`.