Calculate the boiling point elevation of 0.100 kg of water...

Calculate the boiling point elevation of $0.100 \mathrm{kg}$ of water containing $0.010 \mathrm{mol}$ of $\mathrm{NaCl}, 0.020$ mol of $$\mathrm{Na}_{2} \mathrm{SO}_{4}$$ and 0.030 mol of $\mathrm{MgCl}_{2}$, assuming complete dissociation of these electrolytes and ideal solution behavior.

Key Concepts

Colligative Properties

Colligative properties are characteristics of solutions that depend on the number of solute particles rather than their specific identity. In the case of boiling point elevation, the addition of a non-volatile solute increases the boiling point of the solvent by reducing its vapor pressure, and this elevation is directly proportional to the concentration of solute particles in the solution.

Boiling Point Elevation Formula

The boiling point elevation can be calculated using the formula ?T = i × Kb × m, where ?T is the change in boiling point, i is the van’t Hoff factor representing the number of particles produced per solute unit, Kb is the ebullioscopic constant specific to the solvent, and m is the molality of the solution. This formula applies under the assumption of ideal solution behavior.

Molality

Molality is a measure of solute concentration defined as the number of moles of solute per kilogram of solvent. It is independent of temperature and is used instead of molarity in colligative property calculations because it provides a more consistent measure when dealing with temperature changes.

van’t Hoff Factor (i)

The van’t Hoff factor (i) quantifies the effect of solute dissociation in solution by indicating the number of particles formed per formula unit. For electrolytes that dissociate completely into ions, this factor is greater than one, and it directly influences the magnitude of the boiling point elevation as calculated by the colligative property equation.

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