a sample of iron ore (m=0,330g)consisting of a mixture of FeOand Fe2O3 was dissolved in dilute sulfuric acid and titrated with apotassium permanganate solution containing 0.0200g of KMnO4 perlitre, and required 20,3 mL for complete reaction. The secondsample of iron ore (m=0,370g)was dissolved in dilute sulfuric acidsolution and fe3+ is reduced to fe2+ then titrated with the samepotassium permanganate solution. 42,6mL was required for the secondtitration. Calculate the mass of each iron oxide in the originalsample.
im not sure about chemical reactions because Fe2o3 is not reactingwith KMno4
