32. Which one of the following is not a part of osmosis? a. osmotic pressure c. overall flow of solvent b. semipermeable membrane d. overall flow of solute. 33. The addition of sodium chloride to water will cause the boiling point of solution to increase above that of pure water. What is happening on the molecular level to cause this to happen? a. The ions at the surface are blocking water molecules from leaving until they attain a higher kinetic energy. b. The ions are forming precipitates with water that fall to the bottom of the container. c. The water is ionized by the ions and the new set of ions form an ionic compound that is nonvolatile.

32. Which one of the following is not a part of osmosis? a. osmotic pressure c. overall flow of solvent b. semipermeable membrane d. overall flow of solute. 33. The addition of sodium chloride to water will cause the boiling point of solution to increase above that of pure water. What is happening on the molecular level to cause this to happen? a. The ions at the surface are blocking water molecules from leaving until they attain a higher kinetic energy. b. The ions are forming precipitates with water that fall to the bottom of the container. c. The water is ionized by the ions and the new set of ions form an ionic compound that is nonvolatile.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter10: Properties Of Solutions

Section: Chapter Questions

Problem 5ALQ: You have read that adding a solute to a solvent can both increase the boiling point and decrease the...

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You have read that adding a solute to a solvent can both increase the boiling point and decrease the freezing point. A friend of yours explains it to you like this: The solute and solvent can be like salt in water. The salt gets in the way of freezing in that it blocks the water molecules from joining together. The salt acts like a strong bond holding the water molecules together so that it is harder to boil. What do you say to your friend?
Refer to Figure 13.10 ( Sec. 13-4b) to determine whether these situations would result in an unsaturated, saturated, or supersaturated solution. 120. g RbCl is added to 100. g H2O at 50 °C. 30. g KCl is dissolved in 100. g H2O at 70 °C. 20. g NaCl is dissolved in 50. g H2O at 60 °C. Figure 13.10 Solubility of ionic compounds versus temperature.
Water at 25 C has a density of 0.997 g/cm3. Calculate the molality and molarity of pure water at this temperature.
Consider three test tubes. Tube A has pure water. Tube B has an aqueous 1.0 m solution of ethanol, C2H5OH. Tube C has an aqueous 1.0 m solution of NaCl. Which of the following statements are true? (Assume that for these solutions 1.0m=1.0M.) (a) The vapor pressure of the solvent over tube A is greater than the solvent pressure over tube B. (b) The freezing point of the solution in tube B is higher than the freezing point of the solution in tube A. (c) The freezing point of the solution in tube B is higher than the freezing point of the solution in tube C. (d) The boiling point of the solution in tube B is higher than the boiling point of the solution in tube C. (e) The osmotic pressure of the solution in tube B is greater than the osmotic pressure of the solution in tube C.