Colligative Properties Online Quiz

In osmosis, a semipermeable membrane permits the free passage of solvent molecules, such as water, while restricting the movement of solute particles dissolved in the solution. This allows the solvent to move down its concentration gradient.

Adding a non-volatile solute lowers the vapor pressure of the solvent because the solute particles occupy space at the surface, reducing the rate of evaporation.

When solute particles associate (clump together), the total number of particles in the solution decreases, resulting in a van't Hoff factor (i) of less than 1.

The van't Hoff equation for osmotic pressure is pi*V = nRT, where pi represents osmotic pressure (often denoted as p).

The ebullioscopic constant (Kb) is a property of the solvent, as it represents the boiling point elevation per unit molality of the solution.

In an ideal solution, the enthalpy change and volume change upon mixing are both zero. Therefore, stating that volume change is not equal to zero describes a non-ideal solution.

Colligative properties depend on the number of solute particles. Osmotic pressure, boiling point elevation, and freezing point depression are colligative; freezing point itself is a physical property, not a colligative property.

Molarity is defined as the number of moles of solute per liter of solution.

Osmotic pressure arises in systems where a semipermeable membrane separates a solution from a pure solvent, maintaining equilibrium between the two phases.