What volume of 0.0100 M KMnO4 solution is required to oxidize 42.5 mL of 0.0190 M...

What volume of 0.0100 M KMnO₄ solution is required to oxidize 42.5 mL of 0.0190 M FeSO₄ in sulfuric acid solution?

Expert Solution

Number of moles of FeSO₄ is , n = molarity x volume in L

= 0.0190 M x 0.0425 L

= 8.075 x 10 ^-4 moles

The reaction between KMnO4 & FeSO4 in acidic medium is

2 KMnO₄ + 10 FeSO₄ + 8 H₂SO₄ K₂SO₄ + 2MnSO₄ + 5 Fe₂(SO₄)₃ + 8 H₂O

According to the balanced equation ,

10 moles of FeSO₄ reacts with 2 moles of KMnO₄

8.075 x 10 ^-4 moles of FeSO₄ reacts with Z moles of KMnO₄

Volume of KMnO₄ is

queen_honey_blossom answered 6 months ago

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