question_answer

On the basis of the standard electrode potential values stated for acid solution, predict whether,\[T{{i}^{4+}}\] species may be used to oxidise \[F{{e}^{II}}\] to \[F{{e}^{III}}\]. Given \[T{{i}^{4+}}+{{e}^{-}}\,\xrightarrow{{}}\,T{{i}^{3+}};\]\[{{E}^{\odot -}}=+0.01\,V;\]\[F{{e}^{3+}}\,+{{e}^{-}}\,\xrightarrow{{}}\,F{{e}^{2+}};\,\]\[{{E}^{\odot -}}=+0.77\,V\].

Answer:

                  The \[{{E}^{\odot -}}\] (standard reduction potential) values show that \[F{{e}^{II}}\] ions can be oxidised to \[F{{e}^{III}}\] ions by accepting electrons from \[T{{i}^{3+}}\] ion. However, the reverse reaction i.e., oxidation of\[F{{e}^{11}}\] to \[F{{e}^{III}}\] is not possible.