A sample of 1.55 g of iron ore is dissolved in a acid solution in which the iron is converted...


A sample of {eq}1.55\ g {/eq} of iron ore is dissolved in a acid solution in which the iron is converted into {eq}\rm Fe^{2+} {/eq}. The solution formed is then titrated with {eq}\rm KMnO_4 {/eq} which oxidises {eq}\rm Fe^{2+} {/eq} to {eq}\rm Fe^{3+} {/eq} while the {eq}\rm MnO_4^- {/eq} ions are reduced to {eq}\rm Mn^{2+} {/eq} ions. {eq}92.95\ mL {/eq} of {eq}\rm 0.020\ M\ KMnO_4 {/eq} is required for titration to reach the equivalent point.

a) Write the balanced equation for the titration.

b) Calculate the percentage of iron in the sample.

Redox Reaction:

In a redox reaction electrons are transferred from one species that loses electrons (oxidized) to another that gains electrons (reduced). Both processes represent a change in oxidation state of an element and can be written as a balanced half-reaction. The sum of these reactions produces the net redox reaction that is balanced in mass and charge.

Answer and Explanation: 1

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Question a)

This is a redox reaction between iron metal and the manganese in permanganate ion.

  • Iron is oxidized from zero in the metal to +2 in...

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Learn more about this topic:

Balancing Redox Reactions and Identifying Oxidizing and Reducing Agents


Chapter 10 / Lesson 13

Learn about oxidizing and reducing agents, how to find them, and how to identify them in redox reactions. Learn about the different types of redox reactions and how to identify a redox reaction.

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