A solution is prepared by dissolving 27.0 g urea, (NH2)2 CO, in 150.0 g water. Calculate the b

step 1 Let's first convert the 27 grams of urea into moles by using the molar mass of 60 grams per mole

A solution is prepared by dissolving 27.0 g urea, (NH2)2...

A solution is prepared by dissolving $27.0 \mathrm{~g}$ urea, $\left(\mathrm{NH}_{2}\right)_{2} \mathrm{CO}$, in $150.0 \mathrm{~g}$ water. Calculate the boiling point of the solution. Urea is a nonelectrolyte.

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Key Concepts

Colligative Properties

Colligative properties depend solely on the number of solute particles in a solution rather than their identity. These properties include boiling point elevation, freezing point depression, vapor pressure lowering, and osmotic pressure, and they are useful in determining various solution characteristics.

Boiling Point Elevation

Boiling point elevation is a colligative property that causes the boiling point of a solvent to increase when a nonvolatile solute is added. This effect is quantitatively described by the formula ?Tb = i · Kb · m, where ?Tb is the increase in boiling point, Kb is the ebullioscopic constant of the solvent, m is the solute molality, and i is the van’t Hoff factor.

Molality

Molality is a concentration unit defined as the number of moles of solute per kilogram of solvent. It is particularly useful in colligative property calculations because it remains unaffected by temperature changes, ensuring that the concentration measure remains consistent during thermal processes.

Nonelectrolyte

A nonelectrolyte is a substance that, when dissolved in a solvent, does not dissociate into ions. In colligative property calculations, nonelectrolytes are treated with a van’t Hoff factor (i) of 1, meaning they contribute a single particle per formula unit in solution.

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