Let's improve in Chemistry
A 3 . 0 0 g sample containing F e X 3 O X 4 , F e X 2 O X 3 and an inert impure substance, is treated with excess of K I solution in presence of dilute H X 2 S O X 4 . The entire ion is converted into F e X 2 + along with liberation of Iodine. The resulting solution is diluted to 1 0 0 mL . A 2 0 mL of the dilute solution requires 1 1 . 0 mL of 0 . 5 M N a X 2 S X 2 O X 3 to reduce iodine present. A 5 0 mL of dilute solution, after complete extraction of Iodine requires 1 2 . 8 0 mL of 0 . 2 5 M K M n O X 4 solution in dilute H X 2 S O X 4 medium for oxidation of F e X 2 + . Calculate the percentage of F e X 2 O X 3 in the mixture.
The answer is 49.33.
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Consider Fe3O4 to be. A coordinated mixture of FeO and Fe2O3 (In 1:1 ratio) Next use Law of chemical equivalences to form 2 relations in x(amount of Fe3O4) and y(amount of Fe2O3) Using the 2 given info regarding iodometry and permanganate titrations To find x and y separately That finishes the problem