A 1.0 g sample of Fe2 O3 solid of 55.2 % purity is...

A $1.0 \mathrm{~g}$ sample of $\mathrm{Fe}_{2} \mathrm{O}_{3}$ solid of $55.2 \%$ purity is dissolved in acid and reduced by heating the solution with zinc dust. The resultant solution is cooled and made upto $100.0 \mathrm{~mL}$. An aliquot of $25.0 \mathrm{~mL}$ of this solution requires $17.0 \mathrm{~mL}$ of $0.0167 \mathrm{M}$ solution of an oxidant for titration. Calculate the number of electrons taken up by the oxidant in the reaction of the above titration. [1991 - 4 Marks]

Key Concepts

Electron Equivalents and n-factor

The n-factor in a redox reaction represents the number of electrons lost or gained per molecule (or formula unit) during the reaction. Understanding electron equivalents is fundamental in converting moles of reactants into equivalents, which allows for the correct interpretation of titration data and calculation of the reaction extent.

Redox Titration

Redox titration is an analytical method that involves a reaction based on the transfer of electrons between the titrant and analyte. It relies on balancing oxidation and reduction half-reactions, which enables the quantification of substances by determining the number of electrons exchanged during the reaction.

Molarity and Mole Calculations

Molarity is the number of moles of solute per liter of solution, and it is essential for converting between volumes of solutions and moles of reactive species in titration experiments. These calculations provide the basis for determining the quantities of chemicals that react in a given process.

Percent Purity

Percent purity refers to the proportion of a sample that is made up of the desired chemical substance, expressed as a percentage. It is crucial in analytical calculations to determine the actual amount of the active component present in the sample before any further quantitative analysis is performed.

Dilution and Aliquot Techniques

Dilution involves reducing the concentration of a solution by adding solvent, while an aliquot is a measured sub-volume of a larger solution. Both techniques are important for controlling reaction conditions and ensuring accurate titration measurements, allowing the determination of the analyte’s concentration in a manageable fraction of the total solution.

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