Explanation of Fe(ll) oxidation in acidic medium:

Fe(ll) can be oxidized to Fe(lll) in acidic medium by both KMnO4 and K2Cr2O7 solutions due to their strong oxidizing properties. The reaction involves the transfer of electrons from Fe(ll) to the oxidizing agent, leading to the formation of Fe(lll).

Volume of solutions:

- The volumes of 1M KMnO4 and 1M K2Cr2O7 solutions required for the oxidation of Fe(ll) will depend on the stoichiometry of the reaction and the molar ratios of the reactants.

- It is important to calculate the exact amount of each oxidizing agent needed based on the balanced chemical equation of the reaction and the concentration of the solutions.

Factors affecting Fe(ll) oxidation:

- The concentration of the oxidizing agent: Higher concentrations of KMnO4 or K2Cr2O7 will result in faster oxidation of Fe(ll) to Fe(lll) due to the increased availability of oxidizing species.

- pH of the medium: The reaction occurs in acidic medium to prevent the precipitation of Fe(lll) as hydroxide. The acidic conditions also help in stabilizing the oxidizing agent and promoting the oxidation reaction.

Overall reaction:

Fe(ll) + KMnO4 + H+ → Fe(lll) + Mn2+ + H2O

Fe(ll) + K2Cr2O7 + 14H+ → Fe(lll) + Cr3+ + 7H2O

In conclusion, the oxidation of Fe(ll) to Fe(lll) in acidic medium by KMnO4 and K2Cr2O7 solutions involves the transfer of electrons and the formation of Fe(lll) ions. The volume of solutions required will depend on the stoichiometry of the reaction and the concentrations of the oxidizing agents.

more by k2cr2o7 than KMNO4 it can be calculated by n factor