A solution is prepared by dissolving 0.67 mol of MgCl2 in 0.50 kg of water. (a) How many moles

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A solution is prepared by dissolving 0.67 mol of MgCl2 in...

A solution is prepared by dissolving 0.67 mol of $\mathrm{MgCl}_{2}$ in $0.50 \mathrm{~kg}$ of water.
(a) How many moles of ions are present in solution?
(b) What is the change in the boiling point of the aqueous solution?

Key Concepts

Molality

Molality is a concentration unit defined as the moles of solute per kilogram of solvent. It is widely used in colligative property calculations because it remains unaffected by changes in temperature and pressure, making it a reliable measure for determining how solution concentration affects properties like boiling point.

van't Hoff Factor

The van't Hoff factor is a numerical value that represents the effective number of particles into which a solute dissociates in solution. It is essential for accurately calculating colligative effects like boiling point elevation, since these depend on the total number of dissolved particles, and not simply the concentration of the compound added.

Colligative Properties

Colligative properties are characteristics of solutions that depend primarily on the number of solute particles, rather than their identity. Boiling point elevation is one of these properties, whereby the addition of solute particles (ions in the case of electrolytes) increases the boiling point of the solvent relative to its pure state.

Electrolyte Dissociation

This concept describes the process by which an ionic compound breaks apart into its constituent ions when dissolved in a solvent such as water. Understanding the degree and stoichiometry of dissociation is crucial for determining the total number of ions present in a solution, which directly affects various properties of the solution.

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