Any takes on this? I'm having a hard time taking it step by step and what equations to use to solve this questions... =(
What percentage of iron is present in the ore, if a 1.120 g sample requires 25mL of 0.050M KMnO4 to fully oxidize all of the dissolved Fe2+?
8H+ + 5Fe2+ + MnO4- ---> 5Fe3+ + Mn2+ + 4H2O
What percentage of iron is present in the ore, if a 1.120 g sample requires 25mL of 0.050M KMnO4 to fully oxidize all of the dissolved Fe2+?
8H+ + 5Fe2+ + MnO4- ---> 5Fe3+ + Mn2+ + 4H2O