What happens to MnO₄⁻ ions?
MnO₄⁻ is reduced to Mn²⁺.
What happens to Fe²⁺ ions?
Fe²⁺ is oxidised to Fe³⁺.
Which substance acts as the oxidising agent?
KMnO₄ / Acidified Potassium manganate(VII) solution
Which substance acts as the reducing agent?
FeSO₄ / Iron(II) sulphate
State the half-equation for reduction of MnO₄⁻ to Mn²⁺ in acidic medium.
MnO₄⁻ + 8H⁺ + 5e⁻ → Mn²⁺ + 4H₂O
This reaction occurs in a U-tube cell. State the direction of electron flow.
From Fe²⁺ (anode) to MnO₄⁻ (cathode).
State the half-equation for oxidation of Fe²⁺ to Fe³⁺.
Fe²⁺ → Fe³⁺ + e
Why is potassium manganate(VII) solution used in this experiment?
It is a strong oxidising agent
State the change in oxidation number of Fe in this reaction.
Fe: +2 to +3
Why must KMnO₄ be in acidic condition to act as an oxidising agent?
MnO₄⁻ only reduces in acidic medium.
In this reaction, which substance loses electrons?
Iron(II)