Question

In: Chemistry

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?

Solutions

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


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