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6. A student studying the iron content in a mineral ore was given 3.9 g of the ore. The student dissolved all the ore in sulfuric acid solution to convert all the iron to iron (II) which was then titrated with 0.15 M potassium permanganate solution. In the titration, iron (II) was oxidized to iron (III). The titration required 19.5 mL of the permanganate solution to reach the end point. Use the information provided to answer the questions that follow. [Fe=55.85; 0-16.00] a. Write down the oxidation and reduction ion-electron half-cell reactions involved in the titration. [4 marks] b. Deduce the balanced chemical equation for the titration reaction. [2 marks] STUDENT ID:... SIGNATURE.. c. What is the percentage of iron in the iron ore sample? [5 marks] d. If the iron was present in the sample as FeOs, what would be the percentage by mass of Fe-O, in the sample? [3 marks] 6:49 PM