0.01 M KMnO solution was added to 20.0 mL of 0.05 M Mohr's salt solution through a burette. The initial reading of 50 mL burette is zero. The volume of KMnO solution left in the burette after the end

Question

0.01 M KMnO solution was added to 20.0 mL of 0.05 M Mohr's salt solution through a burette. The initial reading of 50 mL burette is zero. The volume of KMnO solution left in the burette after the end point is ____ ml. (nearest integer) 4 4

Prashant Kotian · Accepted Answer

Correct answer: 30. **Step 1: Write the balanced redox equation** In acidic medium, MnO₄⁻ oxidizes Fe²⁺: MnO₄⁻ + 5Fe²⁺ + 8H⁺ → Mn²⁺ + 5Fe³⁺ + 4H₂O Mole ratio: 1 MnO₄⁻ : 5 Fe²⁺ **Step 2: Calculate moles of Mohr's salt (Fe²⁺)** Moles of Fe²⁺ = 0.05 M × 0.020 L = 0.001 mol **Step 3: Calculate moles of KMnO₄ required** Using the mole ratio: Moles of MnO₄⁻ = 0.001 mol Fe²⁺ × (1 mol MnO₄⁻/5 mol Fe²⁺) = 0.0002 mol **Step 4: Calculate volume of KMnO₄ solution used** Volume = moles/molarity = 0.0002 mol / 0.01 M = 0.02 L = 20 mL **Step 5: Calculate remaining volume in burette** Initial volume in burette = 50 mL Volume used = 20 mL Final reading = 50 - 20 = 30 mL Therefore, the answer is 30.

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