A 0.0140-g sample of an ionic compound with the formula Cr(NH3)5 Cl3 was dissolved in water to g

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A 0.0140-g sample of an ionic compound with the formula...

A $0.0140-\mathrm{g}$ sample of an ionic compound with the formula $\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{Cl}_{3}$ was dissolved in water to give $25.0 \mathrm{~mL}$ of solution at $25^{\circ} \mathrm{C}$. The osmotic pressure was determined to be $119 \mathrm{mmHg}$. How many ions are obtained from each formula unit when the compound is dissolved in water?

Key Concepts

Ionic Dissociation

Ionic dissociation is the process by which ionic compounds separate into their individual ions when dissolved in a solvent. This process can yield a greater number of particles than the original formula unit, and measuring colligative properties helps in understanding the extent of dissociation, particularly in compounds that form complex ions.

Osmotic Pressure

Osmotic pressure is a colligative property that results from the movement of a solvent across a semipermeable membrane, driven by a difference in solute concentration. Its measurement allows for the determination of the total number of solute particles in a solution, as it is directly proportional to the molarity of these particles.

van't Hoff Factor

The van't Hoff factor (i) quantifies the number of particles a solute produces when it dissolves. It is used in colligative property calculations, such as those involving osmotic pressure, to account for the degree of ionization or dissociation and thus the effective concentration of particles in solution.

Colligative Properties

Colligative properties are characteristics of a solution that depend solely on the number of solute particles present, not on their chemical identity. These properties include osmotic pressure, boiling point elevation, freezing point depression, and vapor pressure lowering, making them essential for analyzing solutions and determining molecular and ionic behavior.

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