What percentage of iron is present in the ore, if a 1.120 g sample requires 25.00 ml of 0.050 M KMnO4 to fully oxidize all of the dissolved Fe2+?
8H+ + 5Fe2+ + MnO4- à 5Fe3+ + Mn2+ + 4H2O
A. 5 * (1000 / 25.00) * 0.050 * 55.85 * (1 / 1.120) * 100 %
B. 5 * (1000 / 25.00) * 0.050 * 55.85 * 1.120 * 100 %
C. 5 * (0.050 / 1000) * 25.00 * 55.85 * 1.120 * 100 %
D. 5 * (25.00 / 1000) * 0.050 * 55.85 * (1 / 1.120) * 100 %
E. 5 * (25.00 / 1000) * 0.050 * 55.85 * 1.120 * 100 %
Answer is D.
I don't even understand what they are asking.
Please, explain me. anybody?
Thank you~~~
8H+ + 5Fe2+ + MnO4- à 5Fe3+ + Mn2+ + 4H2O
A. 5 * (1000 / 25.00) * 0.050 * 55.85 * (1 / 1.120) * 100 %
B. 5 * (1000 / 25.00) * 0.050 * 55.85 * 1.120 * 100 %
C. 5 * (0.050 / 1000) * 25.00 * 55.85 * 1.120 * 100 %
D. 5 * (25.00 / 1000) * 0.050 * 55.85 * (1 / 1.120) * 100 %
E. 5 * (25.00 / 1000) * 0.050 * 55.85 * 1.120 * 100 %
Answer is D.
I don't even understand what they are asking.
Please, explain me. anybody?
Thank you~~~