Asked by fadi
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!!
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!!
Answers
Answered by
DrBob222
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.
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.
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