What does FeSO4.7H2O + KMnO4 =what?
by 
Darth 5349U11
ANSWERS: 1
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The equation should be 10FeSO4 + 2KMnO4 + 8H2SO4 -> 5Fe2(SO4)3 + K2SO4 + 2MnSO4 + 8H2O You need the number of moles of FeSO4xnH2O, which is equal to the number of moles of FeSO4. You need to determine the volume of KMnO4 needed to react with the solution (the equivalence point is reached when the purple colour won't disappear anymore, as there are no Fe2+ ions left to oxidize). Now you can calculate the number of moles of KMnO4 and then using the equation you can find out the amount of FeSO4 in the solution. As you have diluted the original solution you have to do some additional calculations to determine the amount of Fe2+ ions you started with. The main formula to use is concentration (mol/dm3) = number of moles (mol) / volume (dm3) Sorry if this was a bit confusing, I hope this helps a bit. H2SO4 is needed because acidic environment is needed for the reaction to take place. FeSO4 shouldn't produce anything when H2SO4 is added. Is the original FeSO4*nH2O in solid state or an aqueous solution?
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