Chemistry, 29.06.2019 16:10, tingzontumbler9061

Asample of 1.55 g of iron ore is dissolved in an acid solution in which the iron is converted into
fe2+. the solution formed is then titrated with kmno4 which oxidises fe2+ to fe3+ while the mno4-
ions are reduced to mn2+ ions. 92.95 ml of 0.020 m kmno4 is required for the titration to reach
the equivalence point.
a) write the balanced equation for the titration.
b) calculate the percentage of iron in the sample.

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Asample of 1.55 g of iron ore is dissolved in an acid solution in which the iron is converted into