FeSO4 + KMnO4 + H^+ ==> Fe2(SO4)3 + K2SO4 + MnSO4 + H2O.
Fe is oxidized from +2(each atom) to +3 while Mn is reduced from +7 to +2. I assume you can balance from here.
Use the coefficients in the balanced equation to convert mole Fe to moles KMnO4. Post your work if you get stuck.
A 0.2mol/L solution of KMnO4 has been added to 10 ml of 0.5mol/L acidified FeSO4.
write the balance equation of the reacttion then calculate the volume of the oxidizing solution that should be added to oxidize all the Fe^2+ ions.
please help and thank you!!
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