In a significant experiment performed many years ago, 5.6977...

In a significant experiment performed many years ago, 5.6977 g of cadmium iodide in 44.69 g of water raised the boiling point $0.181^{\circ} \mathrm{C}$. What does this suggest about the nature of a solution of $\mathrm{CdI}_{2}$ ?

Key Concepts

Electrolyte Dissociation

Electrolyte dissociation refers to the process where an ionic compound dissolves in a solvent and separates into its constituent ions. The significant boiling point elevation observed suggests that cadmium iodide dissociates into multiple ions when dissolved, thereby producing more solute particles than would be expected if it remained intact.

van't Hoff Factor

The van't Hoff factor is a measure of the number of particles a solute yields in solution due to dissociation. In the experiment, the extent of boiling point elevation can be used to estimate the van't Hoff factor, which indicates that cadmium iodide produces multiple particles, confirming its behavior as a strong electrolyte when dissolved in water.

Colligative Properties

Colligative properties are characteristics of solutions that depend only on the number of solute particles present, rather than their identity. In this context, the observed boiling point elevation is a colligative property indicating that the number of particles, not their nature, is what affects the boiling point.

Boiling Point Elevation

Boiling point elevation is the phenomenon where the boiling point of a solvent increases upon addition of a solute. This is due to the reduction in the solvent’s vapor pressure caused by the presence of solute particles, requiring a higher temperature to reach the boiling point.

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