1. © 2014 Pearson Education, Inc. Chemistry: A Molecular Approach, 3rd Edition Nivaldo J. Tro Follow all questions (example, practice, and more practice problems from book ) from chapter 10 and then follow following problems for Chapter 11 and 12. Example 11.1 Dipole–Dipole Forces Which of these molecules have dipole–dipole forces? a.CO 2 b. CH 2 CI 2 c. CH 4\ For Practice 11.1 Which molecules have dipole–dipole forces? a.CI 4 b. CH 3 Cl c. HCI Example 11.2 Hydrogen Bonding One of these compounds is a liquid at room temperature. Which one and why? For Practice 11.2 Which has the higher boiling point, HF or HCl? Why? Example 11.5 Methanol has a normal boiling point of 64.6 ° C and a heat of vaporization ( Δ Hvap) of 35.2 kJ/mol. What is the vapor pressure of methanol at 12.0 °C? For Practice 11.5 Propane has a normal boiling point of –42.0 ° C and a heat of vaporization ( Δ H vap ) of 19.04 kJ/mol. What is the vapor pressure of propane at 25.0 ° C?

2. © 2014 Pearson Education, Inc. Chemistry: A Molecular Approach, 3rd Edition Nivaldo J. Tro Example 12.2Henry’s Law What pressure of carbon dioxide is required to keep the carbon dioxide concentration in a bottle of club soda at 0.12 M at 25 °C ? For Practice 12.2 Determine the solubility of oxygen in water at 25 °C exposed to air at 1.0 atm. Assume a partial pressure for oxygen of 0.21 atm. For Practice 12.3 What mass of sucrose (C 12 H 22 O 11 ), in g, is contained in 355 mL (12 ounces) of a soft drink that is 11.5% sucrose by mass? (Assume a density of 1.04 g/mL.) For More Practice 12.3 A water sample is found to contain the pollutant chlorobenzene with a concentration of 15 ppb (by mass). What volume of this water contains 5.00 × 10 2 mg of chlorobenzene? (Assume a density of 1.00 g/mL.) Example 12.4 A solution is prepared by dissolving 17.2 g of ethylene glycol (C 2 H 6 O 2 ) in 0.500 kg of water. The final volume of the solution is 515 mL. For this solution, calculate the concentration in each unit. a. molarity b. molality c. percent by mass d. mole fraction e. mole percent Example 12.6 Calculate the vapor pressure at 25 °C of a solution containing 99.5 g sucrose (C 12 H 22 O 11 ) and 300.0 mL water. The vapor pressure of pure water at 25 °C is 23.8 torr. Assume the density of water to be 1.00 g/mL. For Practice 12.6 Calculate the vapor pressure at 25 °C of a solution containing 55.3 g ethylene glycol (HOCH 2 CH 2 CH 2 OH) and 285.2 g water. The vapor pressure of pure water at 25 °C is 23.8 torr.

3. © 2014 Pearson Education, Inc. Chemistry: A Molecular Approach, 3rd Edition Nivaldo J. Tro Example 12.8 Calculate the freezing point of a 1.7 m aqueous ethylene glycol solution For Practice 12.8 Calculate the freezing point of a 2.6 m aqueous sucrose solution. Example 12.9 What mass of ethylene glycol (C 2 H 6 O 2 ), in grams, must be added to 1.0 kg of water to produce a solution that boils at 105.0 °C? For Practice 12.9 Calculate the boiling point of a 3.60 m aqueous sucrose solution. Example 12.10 The osmotic pressure of a solution containing 5.87 mg of an unknown protein per 10.0 mL of solution is 2.45 torr at 25 °C. Find the molar mass of the unknown protein. For Practice 12.10 Calculate the osmotic pressure (in atm) of a solution containing 1.50 g ethylene glycol (C 2 H 6 O 2 ) in 50.0 mL of solution at 25 °C. Example 12.11 The freezing point of an aqueous 0.050 m CaCl 2 solution is −0.27 °C. What is the van’t Hoff factor (i) for CaCl 2 at this concentration? How does it compare to the expected value of i? For Practice 12.11 Calculate the freezing point of an aqueous 0.10 m FeCl 3 solution using a van’t Hoff factor of 3.2.