The osmotic pressure of 0.010 M solutions of CaCl2 and urea at 25^∘ C are 0.605 atm and 0.245 at

step 1 Okay, so we want the Vanhoff factor for a solution of calcium chloride. So let's first write dow

The osmotic pressure of 0.010 M solutions of CaCl2 and urea...

The osmotic pressure of $0.010 M$ solutions of $\mathrm{CaCl}_{2}$ and urea at $25^{\circ} \mathrm{C}$ are 0.605 atm and 0.245 atm, respectively. Calculate the van't Hoff factor for the $\mathrm{CaCl}_{2}$ solution.

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Key Concepts

Colligative Properties

Colligative properties are physical properties of solutions that depend on the number of solute particles rather than their identity. These properties, which include osmotic pressure, boiling point elevation, and freezing point depression, are used to study solute behavior and interactions in a solvent.

Molarity

Molarity is a unit of concentration defined as the number of moles of solute per liter of solution. It is fundamental in calculating various solution properties including osmotic pressure, as it provides a direct measure of solute particle concentration.

Osmotic Pressure

Osmotic pressure is a colligative property that represents the pressure required to prevent the flow of a solvent through a semipermeable membrane into a solution. It depends on the concentration of solute particles and is used to infer properties like the effective number of dissociated particles in a solution.

Van't Hoff Factor

The van't Hoff factor is a measure of the number of particles into which a solute dissociates in solution, relative to the number of formula units initially added. It is instrumental in predicting colligative properties because it adjusts the idealized count of solute particles based on actual dissociation or association in the solution.

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