Using Vieta's formulas, k = 3 + 4 = 7.

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

Using Raoult's law, the vapor pressure of the solution = (moles of solvent / total moles) * P0 = (10 / 11) * P0 = 0.909 P0.

Vapor pressure lowering = (moles of solute / total moles) * P0 = (1 / (1 + 3)) * P0 = 0.25 P0, so vapor pressure = P0 - 0.25 P0 = 0.75 P0.

Using Raoult's law, P_solution = X_solvent * P°_solvent = (9/10) * 100 mmHg = 90 mmHg.

Using Raoult's law, P_solution = X_solvent * P°_solvent. X_solvent = 3/(1+3) = 0.75, so P_solution = 0.75 * 100 mmHg = 75 mmHg.

Using Raoult's law, the vapor pressure of the solution = (moles of solvent / total moles) * P0 = (3 / (3 + 1)) * P0 = 0.75 P0.

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.

Using the formula M = moles/volume, Volume = moles/M = 0.5 moles / 1 M = 0.5 L.

Volume = moles of solute / molarity = 4 moles / 2 M = 2 L.

Volume percent = (volume of solute / total volume) x 100 = (30 mL / 150 mL) x 100 = 20%.

Volume percent = (volume of solute / total volume) × 100 = (30 mL / (30 mL + 70 mL)) × 100 = 30%.

Negative deviation from Raoult's Law occurs when strong solute-solvent interactions lower the vapor pressure more than expected.

Raoult's Law applies most accurately to ideal solutions, where interactions between different molecules are similar to those in pure substances.

Raoult's Law applies primarily to ideal solutions, where the interactions between different molecules are similar to those in pure substances.

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.

MgCl2 dissociates into 3 ions (1 Mg²⁺ and 2 Cl⁻), leading to the highest boiling point elevation due to the greatest number of particles.

Raoult's Law is primarily affected by the nature of the solute, temperature, and mole fraction of the solvent, but not by the pressure of the system.

The volume of solvent does not directly affect the solubility of a gas; pressure and temperature do.

Raoult's Law states that the vapor pressure is affected by the nature of the solute, temperature, and mole fraction of the solvent, but not by the pressure of the system.