Hydroxylamine reduces iron (III) according to the equation: 2 NH2 OH+4 Fe^3+ →N2 O(g) ↑+H2 O+4 F

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Hydroxylamine reduces iron (III) according to the equation:...

Hydroxylamine reduces iron (III) according to the equation: $2 \mathrm{NH}_{2} \mathrm{OH}+4 \mathrm{Fe}^{3+} \rightarrow \mathrm{N}_{2} \mathrm{O}(\mathrm{g}) \uparrow+\mathrm{H}_{2} \mathrm{O}+4 \mathrm{Fe}^{2+}+4 \mathrm{H}^{+}$ Iron (II) thus produced is estimated by titration with a standard permanganate solution. The reaction is : $$ \mathrm{MnO}_{4}^{-}+5 \mathrm{Fe}^{2+}+8 \mathrm{H}^{+} \rightarrow \mathrm{Mn}^{2+}+5 \mathrm{Fe}^{3+}+4 \mathrm{H}_{2} \mathrm{O} $$ A $10 \mathrm{~mL}$. sample of hydroxylamine solution was diluted to 1 litre. $50 \mathrm{~mL}$. of this diluted solution was boiled with an excess of iron (III) solution. The resulting solution required $12 \mathrm{~mL}$. of $0.02 \mathrm{M} \mathrm{KMnO}_{4}$ solution for complete oxidation of iron (II). Calculate the weight of hydroxylamine in one litre of the original solution. $(\mathrm{H}=1, \mathrm{~N}=14, \mathrm{O}$ $=16, \mathrm{~K}=39, \mathrm{Mn}=55, \mathrm{Fe}=56)$ [1982 - 4 Marks]

Hydroxylamine reduces iron (III) according to the equation:
$2 \mathrm{NH}_{2} \mathrm{OH}+4 \mathrm{Fe}^{3+} \rightarrow \mathrm{N}_{2} \mathrm{O}(\mathrm{g}) \uparrow+\mathrm{H}_{2} \mathrm{O}+4 \mathrm{Fe}^{2+}+4 \mathrm{H}^{+}$
Iron (II) thus produced is estimated by titration with a standard permanganate solution. The reaction is :
$$
\mathrm{MnO}_{4}^{-}+5 \mathrm{Fe}^{2+}+8 \mathrm{H}^{+} \rightarrow \mathrm{Mn}^{2+}+5 \mathrm{Fe}^{3+}+4 \mathrm{H}_{2} \mathrm{O}
$$
A $10 \mathrm{~mL}$. sample of hydroxylamine solution was diluted to 1 litre. $50 \mathrm{~mL}$. of this diluted solution was boiled with an excess of iron (III) solution. The resulting solution required $12 \mathrm{~mL}$. of $0.02 \mathrm{M} \mathrm{KMnO}_{4}$ solution for complete oxidation of iron (II). Calculate the weight of hydroxylamine in one litre of the original solution. $(\mathrm{H}=1, \mathrm{~N}=14, \mathrm{O}$ $=16, \mathrm{~K}=39, \mathrm{Mn}=55, \mathrm{Fe}=56)$
[1982 - 4 Marks]

Key Concepts

Redox Titration

Redox titration is an analytical method that uses a redox reaction between an oxidizing agent and a reducing agent to determine the concentration of an unknown solution. It involves a titrant, often a strong oxidizer like permanganate, which reacts with the analyte until an endpoint is reached, allowing for quantification of the analyte through stoichiometric relationships.

Molar Mass Calculations

Molar mass calculations involve determining the mass of one mole of a given compound using the atomic masses of its constituent elements. This concept is important for converting between mass and moles in stoichiometric calculations, enabling the quantification of compounds in a solution.

Dilution and Concentration Calculations

These calculations are used to determine the concentrations of solutions after they have been diluted from a stock solution. They involve using the relationship between the initial and final volumes and concentrations, which is critical when preparing samples for analysis.

Redox Reactions

This concept involves the transfer of electrons between species. In redox reactions, one reactant is oxidized (loses electrons) while another is reduced (gains electrons). Understanding redox reactions is critical for balancing chemical equations, determining oxidation states, and analyzing reaction mechanisms in both qualitative and quantitative methods.

Stoichiometry

Stoichiometry deals with the quantitative relationships between reactants and products in a chemical reaction. It involves using balanced chemical equations to convert between amounts in moles, mass, and volume. This concept is essential for determining how much of one substance reacts with or produces another, particularly in titrimetric analyses and yield calculations.

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