Freezing Point of Solvent Quiz Online Practice Test

1. Which of the following gases has the smallest Henry's law constant?

2. If 10 ml of 0.1M NaCl solution is divided into 1000 equal drops, what is the concentration of NaCl in one drop?

3. A car coolant mixture consists of a 0.5 molal solution of ethylene glycol in water. Given that the freezing point depression constant of water is 1.86°C/m, the freezing point of the mixture will be:

4. Which statement accurately describes a 0.020M solution of H₂SO₃?

5. In a 500g sample of toothpaste containing 0.2g of fluoride, what is the fluoride concentration in parts per million (ppm)?

6. At a specific temperature, the vapor pressure of pure water is 25 mm Hg, and the vapor pressure of a very dilute aqueous urea solution is 24.5 mm Hg. What is the molality of the solution?

7. Among the following 0.10m aqueous solutions, which one will have the lowest freezing point?

8. How much urea should be dissolved in 500 cc of water (K = 1.86 °C/mol) to lower the freezing point by 0.186 °C?

9. What is the molecular formula of a non-electrolyte with an empirical formula of CH2O, if a 6g solution of this compound exerts the same osmotic pressure as a 0.05M glucose solution at the same temperature?

10. Given that the molar mass of sodium hydroxide obtained from the measurement of the osmotic pressure of its aqueous solution at 27°C is 25 g/mol, what is the percentage ionization in this solution?

11. Which substance has the highest freezing point?

12. What effect does a solute have when dissolved in water?

13. The freezing point of a solution prepared from 1.25g of a non-electrolyte solute in 20g of water is 271 K. Given that the molal depression constant is 1.86 K/mole, the molar mass of the solute will be:

14. An aqueous solution of a non-electrolyte has a boiling point of 100.52°C. Determine the freezing point of this solution.

15. Determine the freezing point of a 1% lead nitrate solution in water:

16. How does adding sugar to water affect its boiling and freezing points?

17. When freezing point depression occurs in a solution, which of the following pairs are in equilibrium?

18. Which of these molal aqueous solutions exhibits the highest freezing point?

19. A substance weighing 0.440 g, when dissolved in 22.2 g of benzene, results in a freezing point depression of 0.567°C. Given that the cryoscopic constant (Kf) of benzene is 5.12°C·mol/kg, calculate the molecular mass of the substance.

20. For a solution with a concentration of 0.1 M, which substance will cause the greatest decrease in the freezing point?