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Ferrous ion reaction

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How do I calculate the moles of iron (ore sample) and how do I calculate the mass percent of iron in the ore from this problem;

Ferrous ion reacts with permanganate ion Mno4 in acidic solution to produce the ferric ion Fe3. A 6.893 gram sample of ore was mechanically crushed and then treated with HCl which oxidized all the iron in the ore to the ferrous ion, next, the acid solution containing all the ferrous ions was titrated with.100M of KMno4 solution. The end point was reached when 13.889 ml of potassium permanganate solution was used.

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Solution Preview

The titration tells us the number of moles of iron present in the sample. Once the endpoint is reaced the number of moles ...

Solution Summary

This solution deals with the titration of iron ore in a sample. It finally concludes with the percent mass of the reaction.

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See Also This Related BrainMass Solution

Redox Reaction: Ferrous Ion and Permanganate Ion

The ferrous ion, Fe2+(aq), reacts with the permanganate ion, MnO4- (aq), in an acidic solution to produce the ferric ion, Fe3+(aq). A 6.893 g sample of ore was mechanically crushed and tehn treated with concentrated hydrochloric acid, which oxidized all of the iron in the ore to the ferrous ion, Fe2+(aq). Next the acid solution containing all of the ferrous ions was titrated with .100 M KMnO4 solution. The end point was reached when 13.899mL of the KMnO4 solution was used.

a. Write the oxidation half reaction
b. Write the reduction half reaction
c. Write the balanced final redox reaction
d. Identify the oxidizing agent, the reducing agent, the species being oxidized, and the species being reduced
e. Calculate the number of moles of iron in the sample or ore
f. Calculate the mass percent of the iron in the ore

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