how many ml of a 0.050 M kMno4 solution are required to oxidize 2.00 g of feso4 in a dilute...
Homework Answers
MnO4 - + 5 Fe2+ + 8 H+ = Mn2+ + 5Fe 3+ + 4H2O
For 1 mole of KMnO4 , moles of FeSO4 required =5
So, 2/56*5 = M*V
So, V = 1/(140*0.05) l = 1000/7 ml = 142.857 ml
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