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Experiment Theory & Analysis

01 Oxidation & Reduction

This is a Redox titration where $KMnO_4$ acts as the oxidizing agent and Mohr's Salt ($Fe^{2+}$) acts as the reducing agent in acidic medium.

$$ MnO_4^- + 8H^+ + 5e^- \rightarrow Mn^{2+} + 4H_2O $$

02 Self-Indicator

$KMnO_4$ is a self-indicator. No external indicator is needed.

  • Start: Colorless ($Mn^{2+}$ formed instantly)
  • Endpoint: Permanent Pale Pink (Excess $MnO_4^-$)
  • Overshoot: Dark Purple

03 Stoichiometry

From the balanced equation, 1 mole of $KMnO_4$ reacts with 5 moles of Mohr's Salt.

$$ \frac{M_1 V_1}{n_1} = \frac{M_2 V_2}{n_2} $$

where $n_1=1$ ($KMnO_4$) and $n_2=5$ ($Fe^{2+}$).