The presence of solute particles reduces the number of solvent molecules at the surface, leading to a lower vapor pressure.

Boiling point elevation is directly proportional to the molality of the solution.

NaCl dissociates into two ions (Na+ and Cl-), so the van 't Hoff factor (i) is 2.

The van 't Hoff factor (i) is equal to the number of particles the solute dissociates into. For a strong electrolyte that dissociates into 3 ions, i = 3.

The van 't Hoff factor (i) for glucose is 1, as it does not dissociate in solution.

For a non-electrolyte solute, the van 't Hoff factor (i) is 1, as it does not dissociate into ions.

Vapor pressure = P°_solvent * (n_solvent / (n_solvent + n_solute)) = 23.76 * (55.5 / (55.5 + 0.1)) = 22.88 mmHg

The vapor pressure of a solution containing a non-volatile solute is lower than that of the pure solvent due to the presence of solute particles.

All of these colligative properties can be used to determine the molar mass of a solute.

Electrolytes dissociate into ions, affecting all colligative properties by increasing the number of solute particles.

All of these colligative properties can be used to determine the molar mass of a solute by applying the appropriate formulas.

All of the listed colligative properties can be used to determine the molar mass of a solute.

Vapor pressure lowering is a colligative property that depends on the number of solute particles in a solution.

All of the listed colligative properties can be used to determine the molar mass of a solute.

Freezing point depression can be used to determine the molar mass of a solute by measuring the decrease in freezing point.

CaCl2 dissociates into 3 ions (Ca2+ and 2 Cl-), resulting in the highest freezing point depression.

The 0.1 M NaCl and KCl solutions will have lower vapor pressures than pure water due to the presence of solute particles.

0.1 M MgCl2 will have the highest boiling point due to the highest van 't Hoff factor (i = 3).

Colligative properties depend on the number of solute particles in a solution, not their identity.

Colligative properties depend on the number of solute particles, not their identity.

0.1 M K2SO4 will exhibit the greatest freezing point depression due to its van 't Hoff factor of 3.

CaCl2 dissociates into three ions (Ca2+ and 2 Cl-), leading to the greatest vapor pressure lowering among the options.

The 0.1 M NaCl solution will exhibit the lowest vapor pressure due to the presence of more solute particles (2 ions per formula unit).

0.1 m MgCl2 produces 3 particles (Mg2+ and 2 Cl-), leading to the lowest freezing point among the options.