IV B The first solution with 02 M MnO 4 aq turned a light clear orange The

Iv b the first solution with 02 m mno 4 aq turned a

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IV. B. The first solution with .02 M MnO4-(aq) turned a light, clear orange. The second solution with 1 M SCN-(aq) turned a light, blood red. After these tests, it is apparent that both forms of the iron ion (Fe3+and Fe2+) are in the ore sample. The sample that turned light red after the SCN-addition indicated the presence of Fe2+. The sample that was the light orange showed the presence of Fe3+.C. After the Cr2O7-(aq) was added to one dilution, the solution turned a blue-green. The diluted solution with SCN-turned clear. The Cr2O7- showed that there was Fe2+after the Sn2+treatment. Since the book illustrates that the product is Sn4+, it is known that this a redox reaction. The equation being: 2Fe2+(aq) + Sn2+(aq) → 2Fe2+(aq) + Sn4+(aq)D. The solid ore sample would need to be added to an acidic mixture in order for there to be an acidic environment where the redox reaction can occur. The ore sample would needto be heated so that the iron can dissolve. After this step, the MnO4-can titrate the mixtureto get a quantitative measurement of the iron.
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