I‘m fine on letter A, but not sure how to do B or C!!!!!(3) A sample of iron ore weighing 2.00 g was dissolved in acid to produce Fe2+ ions. The solution was then titrated with27.45 mL of 0.100 M KMnO4 solution. In acidic solution, Fe2+ reacts with MnO4- to produce Fe3+ and Mn2+.(a) Write the balanced chemical equation for this reaction.(b) Determine the mass of pure iron in the sample of iron ore.(c) Determine the percent iron in the sample of iron ore.This is a review question for our chemistry test tomorrow. I would like to know how to work b and c. The answers are below, but I‘m not sure what work to show to get to the .767 and 38.4 percent. Thanks!!!ANSWERS(3) (a) 5Fe3+ + MnO4- + 8H+ → 5Fe2+ + Mn2+ + 4H2O(b) 0.767 g Fe(c) 38.4%
