1. © 2015 Pearson Education, Inc. a.NaCl is a polar covalent molecule and a solvent dissolves solutes that have similar intermolecular forces as the solvent. b.NaCl is a neutral substance and is not attracted to nonpolar hexane. c.NaCl is ionic and ion-ion forces in the lattice are not broken by ion-nonpolar interactions. d.NaCl has large ions that are hard to separate and dissolve in any solvent. Why doesn’t NaCl dissolve in nonpolar solvents such as hexane, C 6 H 14 ?

2. © 2015 Pearson Education, Inc. a.NaCl is a polar covalent molecule and a solvent dissolves solutes that have similar intermolecular forces as the solvent. b.NaCl is a neutral substance and is not attracted to nonpolar hexane. c.NaCl is ionic and ion-ion forces in the lattice are not broken by ion-nonpolar interactions. d.NaCl has large ions that are hard to separate and dissolve in any solvent. Why doesn’t NaCl dissolve in nonpolar solvents such as hexane, C 6 H 14 ?

3. © 2015 Pearson Education, Inc. (a)(b) a.EndothermicEndothermic b.EndothermicExothermic c.ExothermicEndothermic d.ExothermicExothermic Label the following processes as exothermic or endothermic: (a)breaking solvent–solvent interactions to form separated particles (b)forming solvent–solute interactions from separated particles

4. © 2015 Pearson Education, Inc. (a)(b) a.EndothermicEndothermic b.EndothermicExothermic c.ExothermicEndothermic d.ExothermicExothermic Label the following processes as exothermic or endothermic: (a)breaking solvent–solvent interactions to form separated particles (b)forming solvent–solute interactions from separated particles

5. © 2015 Pearson Education, Inc. a.More solute dissolves. b.The additional solute does not dissolve and some of the original dissolved solute comes out of the solution. c.The additional solute does not dissolve and the solution remains saturated. d.The temperature of the solution changes and some of the added solute dissolves. What happens if a solute is added to a saturated solution?

6. © 2015 Pearson Education, Inc. a.More solute dissolves. b.The additional solute does not dissolve and some of the original dissolved solute comes out of the solution. c.The additional solute does not dissolve and the solution remains saturated. d.The temperature of the solution changes and some of the added solute dissolves. What happens if a solute is added to a saturated solution?

7. © 2015 Pearson Education, Inc.

8. a.Higher solubility b.Lower solubility c.About the same solubility Suppose the hydrogens on the OH groups in glucose (Figure on the last slide) if were replaced with methyl groups, CH 3. Would you expect the water solubility of the resulting molecule to be higher than, lower than, or about the same as glucose?

9. © 2015 Pearson Education, Inc. a.Higher solubility b.Lower solubility c.About the same solubility Suppose the hydrogens on the OH groups in glucose (Figure 13.10) were replaced with methyl groups, CH 3. Would you expect the water solubility of the resulting molecule to be higher than, lower than, or about the same as glucose?

10. © 2015 Pearson Education, Inc. a.Some water molecules break down into gases as water is heated. b.Dissolved gases are less soluble in solution as temperature increases. c.Water molecules begin to enter the gas phase to stimulate boiling. d.Boiling actually begins on a small scale at temperatures below the boiling point. Why do bubbles form on the inside wall of a cooking pot when water is heated on the stove, even though the water temperature is well below the boiling point of water?

11. © 2015 Pearson Education, Inc. a.Some water molecules break down into gases as water is heated. b.Dissolved gases are less soluble in solution as temperature increases. c.Water molecules begin to enter the gas phase to stimulate boiling. d.Boiling actually begins on a small scale at temperatures below the boiling point. Why do bubbles form on the inside wall of a cooking pot when water is heated on the stove, even though the water temperature is well below the boiling point of water?

12. © 2015 Pearson Education, Inc. a.2.3 ppm; 2.3 × 10 3 ppb b.23 ppm; 2.3 × 10 4 ppb c.230 ppm: 2.30 × 10 5 ppb d.2300 ppm; 2.300 × 10 6 ppb A solution of SO 2 in water contains 0.00023 g of SO 2 per liter of solution. What is the concentration of SO 2 in ppm? In ppb?

13. © 2015 Pearson Education, Inc. a.2.3 ppm; 2.3 × 10 3 ppb b.23 ppm; 2.3 × 10 4 ppb c.230 ppm: 2.30 × 10 5 ppb d.2300 ppm; 2.300 × 10 6 ppb A solution of SO 2 in water contains 0.00023 g of SO 2 per liter of solution. What is the concentration of SO 2 in ppm? In ppb?

14. © 2015 Pearson Education, Inc. a.Molality will be greater than its molarity. b.Molality will be nearly the same as its molarity. c.Molality will be smaller than its molarity. If an aqueous solution is very dilute, will its molality be greater than its molarity, nearly the same as its molarity, or smaller than its molarity?

15. © 2015 Pearson Education, Inc. a.Molality will be greater than its molarity. b.Molality will be nearly the same as its molarity. c.Molality will be smaller than its molarity. If an aqueous solution is very dilute, will its molality be greater than its molarity, nearly the same as its molarity, or smaller than its molarity?

16. © 2015 Pearson Education, Inc. a.NaCl is highly polar whereas C 6 H 12 O 6 is weakly polar and this causes the difference. b.NaCl has a smaller molar mass than that of C 6 H 12 O 6 and this causes the difference. c.NaCl is polar whereas C 6 H 12 O 6 is nonpolar and this causes the difference. d.The total solute concentration of NaCl is twice that of C 6 H 12 O 6 because NaCl forms Na + and Cl – ions and this causes the difference. Adding 1 mol of NaCl to 1 kg of water lowers the vapor pressure of water more than adding 1 mol of C 6 H 12 O 6. Explain.

17. © 2015 Pearson Education, Inc. a.NaCl is highly polar whereas C 6 H 12 O 6 is weakly polar and this causes the difference. b.NaCl has a smaller molar mass than that of C 6 H 12 O 6 and this causes the difference. c.NaCl is polar whereas C 6 H 12 O 6 is nonpolar and this causes the difference. d.The total solute concentration of NaCl is twice that of C 6 H 12 O 6 because NaCl forms Na + and Cl – ions and this causes the difference. Adding 1 mol of NaCl to 1 kg of water lowers the vapor pressure of water more than adding 1 mol of C 6 H 12 O 6. Explain.

18. © 2015 Pearson Education, Inc. a.Yes b.No c.Depends on whether the solute is a strong or weak electrolyte d.Depends on if the solute is a nonpolar, nonelectrolyte A solute dissolved in water causes the boiling point to increase by 0.51 ° C. Does this necessarily mean that the concentration of the solute is 1.0 m (Table 13.3)?

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20. a.Yes b.No c.Depends on whether the solute is a strong or weak electrolyte d.Depends on if the solute is a nonpolar, nonelectrolyte A solute dissolved in water causes the boiling point to increase by 0.51 ° C. Does this necessarily mean that the concentration of the solute is 1.0 m (Table 13.3)?

21. © 2015 Pearson Education, Inc. a.The 0.20 m KCl solution is hypotonic with the 0.50 m KCl solution. b.The 0.50 m KCl solution is hypotonic with the 0.20 m KCl solution. c.Neither is hypotonic to each other. d.They are isotonic solutions. Of two KBr solutions, one 0.50 m and the other 0.20 m, which is hypotonic with respect to the other?

22. © 2015 Pearson Education, Inc. a.The 0.20 m KCl solution is hypotonic with the 0.50 m KCl solution. b.The 0.50 m KCl solution is hypotonic with the 0.20 m KCl solution. c.Neither is hypotonic to each other. d.They are isotonic solutions. Of two KBr solutions, one 0.50 m and the other 0.20 m, which is hypotonic with respect to the other?

23. © 2015 Pearson Education, Inc. a.The osmotic pressure of a 0.10 M solution of NaCl is greater than that of a 0.10 M solution of KBr. b.The osmotic pressure of a 0.10 M solution of NaCl is equal to that of a 0.10 M solution of KBr. c.The osmotic pressure of a 0.10 M solution of NaCl is less than than that of a 0.10 M solution of KBr. Is the osmotic pressure of a 0.10 M solution of NaCl greater than, less than, or equal to that of a 0.10 M solution of KBr?

24. © 2015 Pearson Education, Inc. a.The osmotic pressure of a 0.10 M solution of NaCl is greater than that of a 0.10 M solution of KBr. b.The osmotic pressure of a 0.10 M solution of NaCl is equal to that of a 0.10 M solution of KBr. c.The osmotic pressure of a 0.10 M solution of NaCl is less than than that of a 0.10 M solution of KBr. Is the osmotic pressure of a 0.10 M solution of NaCl greater than, less than, or equal to that of a 0.10 M solution of KBr?

25. © 2015 Pearson Education, Inc. a.Yes, proteins have hydrophilic groups on the exterior. b.No, the hydrophilic groups would be repelled by the hydrophobicity of the lipids. Some proteins reside in the hydrophobic lipid bilayer of the cell membrane. Would hydrophilic groups of these proteins still be facing the lipid “solvent”?

26. © 2015 Pearson Education, Inc. a.Yes, proteins have hydrophilic groups on the exterior. b.No, the hydrophilic groups would be repelled by the hydrophobicity of the lipids. Some proteins reside in the hydrophobic lipid bilayer of the cell membrane. Would hydrophilic groups of these proteins still be facing the lipid “solvent”?

27. © 2015 Pearson Education, Inc. a.Ion-dipole forces b.Dipole-dipole forces c.Dispersion forces d.Hydrogen bonding Why don’t oil drops stabilized by sodium stearate coagulate to form larger oil drops?

28. © 2015 Pearson Education, Inc. a.Ion-dipole forces b.Dipole-dipole forces c.Dispersion forces d.Hydrogen bonding Why don’t oil drops stabilized by sodium stearate coagulate to form larger oil drops?