Which of the following is NOT a colligative property?

Which beaker shows a greater decrease in liquid level after being left side by side on a lab bench for 1 week, a beaker with 100.0 mL of pure water or a beaker with 100.0 mL of seawater, and why?

A solution contains 4.08 g of chloroform (CHCl3) and 9.29 g of acetone (CH3COCH3). The vapor pressures at 35 °C of pure chloroform and pure acetone are 295 torr and 332 torr, respectively. Assuming ideal behavior, calculate the vapor pressures of each of the components and the total vapor pressure above the solution. The experimentally measured total vapor pressure of the solution at 35 °C is 312 torr. Is the solution ideal? If not, what can you say about the relative strength of chloroform–acetone interactions compared to the acetone–acetone and chloroform–chloroform interactions?

A solution of methanol and water has a mole fraction of water of 0.312 and a total vapor pressure of 211 torr at 39.9 °C. The vapor pressures of pure methanol and pure water at this temperature are 256 torr and 55.3 torr, respectively. Is the solution ideal? If not, what can be inferred about the relative strengths of the solute–solvent interactions compared to the solute–solute and solvent–solvent interactions?

Which of the following best explains why colligative properties are affected differently when a volatile solute is used compared to a nonvolatile solute?

Which of the following aqueous solutions has the highest boiling point?

Which of the following properties affects a colligative property?

Which of the following is considered a colligative property?

Which of the following statements correctly defines colligative properties?