1. Properties of Solutions
March 13, 2018
Learning TargetI can apply intermolecular forces to the properties of solutions

2. DO NOW (4 MIN)
Learning Target: I can apply intermolecular forces to the properties of solutions and understand my current standing using the AP exam rubric
Do Now: (on your DO Now Sheet)
Rank the following in terms of increasing vapor pressure when added to H2O?
NaCl C6H12O6 MgCl2 FeCl3 Al2(SO4)3 MgS
March 13, 2018
Learning TargetI can apply intermolecular forces to the properties of solutions

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4. Question leader
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5. 180 g/mole b. 360 g/mole c. 720 g/mole d. 1800 g/mole
What is the molecular weight of adrenaline if 0.64 grams of adrenaline dissolved in 36.0 g of CCl4 raises the boiling point by 0.49 degrees Celsius?
Answer: a
180 g/mole b g/mole
c g/mole d g/mole

6. 180 g/mole b. 360 g/mole c. 720 g/mole d. 1800 g/mole
What is the molecular weight of adrenaline if 0.64 grams of adrenaline dissolved in 36.0 g of CCl4 raises the boiling point by 0.49 degrees Celsius?
Answer: a
180 g/mole b g/mole
c g/mole d g/mole

7. Which substance below is not a colloid?
butter
smoke
whipped cream
d. salt water
Answer: d

8. Which substance below is not a colloid?
butter
smoke
whipped cream
d. salt water
Answer: d

9. Tyndall Raoult Hall d. Meissner
Light scattering by colloidally dispersed particles is an example of the _______ effect.
Tyndall
Raoult
Hall
d. Meissner
Answer: a

10. Tyndall Raoult Hall d. Meissner
Light scattering by colloidally dispersed particles is an example of the _______ effect.
Tyndall
Raoult
Hall
d. Meissner
Answer: a

11. What is the molality of a solution of phosphoric acid, H3PO4, that contains 24.5 g of phosphoric acid (molar mass 98.0 g) in 100. g of H2O?
A) m
(B) 2.50 m
(C) 4.00 m
(D) 25.0 m
(E) 40.0 m
Answer: a

12. What is the molality of a solution of phosphoric acid, H3PO4, that contains 24.5 g of phosphoric acid (molar mass 98.0 g) in 100. g of H2O?
A) m
(B) 2.50 m
(C) 4.00 m
(D) 25.0 m
(E) 40.0 m
Answer: a

13. Why doesn’t NaCl dissolve in nonpolar solvents such as hexane, C6H14?
NaCl is a polar covalent molecule and a solvent dissolves solutes that have similar intermolecular forces as the solvent.
NaCl is a neutral substance and is not attracted to nonpolar hexane.
NaCl is ionic and ion-ion forces in the lattice are not broken by ion-nonpolar interactions.
NaCl has large ions that are hard to separate and dissolve in any solvent.
Answer: c

14. Why doesn’t NaCl dissolve in nonpolar solvents such as hexane, C6H14?
NaCl is a polar covalent molecule and a solvent dissolves solutes that have similar intermolecular forces as the solvent.
NaCl is a neutral substance and is not attracted to nonpolar hexane.
NaCl is ionic and ion-ion forces in the lattice are not broken by ion-nonpolar interactions.
NaCl has large ions that are hard to separate and dissolve in any solvent.
Answer: c

15. 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
(a) (b)
Endothermic Endothermic
Endothermic Exothermic
Exothermic Endothermic
Exothermic Exothermic
Answer: b

16. 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
(a) (b)
Endothermic Endothermic
Endothermic Exothermic
Exothermic Endothermic
Exothermic Exothermic
Answer: b

17. What happens if a solute is added to a saturated solution?
More solute dissolves.
The additional solute does not dissolve and some of the original dissolved solute comes out of the solution.
The additional solute does not dissolve and the solution remains saturated.
The temperature of the solution changes and some of the added solute dissolves.
Answer: c

18. What happens if a solute is added to a saturated solution?
More solute dissolves.
The additional solute does not dissolve and some of the original dissolved solute comes out of the solution.
The additional solute does not dissolve and the solution remains saturated.
The temperature of the solution changes and some of the added solute dissolves.
Answer: c

19. Suppose the hydrogens on the OH groups in glucose (Figure 13
Suppose the hydrogens on the OH groups in glucose (Figure 13.10) were replaced with methyl groups, CH3. Would you expect the water solubility of the resulting molecule to be higher than, lower than, or about the same as glucose?
Higher solubility
Lower solubility
About the same solubility
Answer: b

21. Suppose the hydrogens on the OH groups in glucose (Figure 13
Suppose the hydrogens on the OH groups in glucose (Figure 13.10) were replaced with methyl groups, CH3. Would you expect the water solubility of the resulting molecule to be higher than, lower than, or about the same as glucose?
Higher solubility
Lower solubility
About the same solubility
Answer: b

22. 2 minute brain break
Discuss: Would you rather eat chicken pot pie with a buffalo or fly a kite with a hippo?

23. What did you just say?

24. 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?
Some water molecules break down into gases as water is heated.
Dissolved gases are less soluble in solution as temperature increases.
Water molecules begin to enter the gas phase to stimulate boiling.
Boiling actually begins on a small scale at temperatures below the boiling point.
Answer: b

25. 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?
Some water molecules break down into gases as water is heated.
Dissolved gases are less soluble in solution as temperature increases.
Water molecules begin to enter the gas phase to stimulate boiling.
Boiling actually begins on a small scale at temperatures below the boiling point.
Answer: b

26. A solution of SO2 in water contains 0
A solution of SO2 in water contains g of SO2 per liter of solution. What is the concentration of SO2 in ppm? In ppb?
2.3 ppm; 2.3 × 103 ppb
23 ppm; 2.3 × 104 ppb
230 ppm: 2.30 × 105 ppb
2300 ppm; × 106 ppb
Answer: c

27. A solution of SO2 in water contains 0
A solution of SO2 in water contains g of SO2 per liter of solution. What is the concentration of SO2 in ppm? In ppb?
2.3 ppm; 2.3 × 103 ppb
23 ppm; 2.3 × 104 ppb
230 ppm: 2.30 × 105 ppb
2300 ppm; × 106 ppb
Answer: c

28. 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?
Molality will be greater than its molarity.
Molality will be nearly the same as its molarity.
Molality will be smaller than its molarity.
Answer: b

29. 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?
Molality will be greater than its molarity.
Molality will be nearly the same as its molarity.
Molality will be smaller than its molarity.
Answer: b

30. Adding 1 mol of NaCl to 1 kg of water lowers the vapor pressure of water more than adding 1 mol of C6H12O6. Explain.
NaCl is highly polar whereas C6H12O6 is weakly polar and this causes the difference.
NaCl has a smaller molar mass than that of C6H12O6 and this causes the difference.
NaCl is polar whereas C6H12O6 is nonpolar and this causes the difference.
The total solute concentration of NaCl is twice that of C6H12O6 because NaCl forms Na+ and Cl– ions and this causes the difference.
Answer: d

31. Adding 1 mol of NaCl to 1 kg of water lowers the vapor pressure of water more than adding 1 mol of C6H12O6. Explain.
NaCl is highly polar whereas C6H12O6 is weakly polar and this causes the difference.
NaCl has a smaller molar mass than that of C6H12O6 and this causes the difference.
NaCl is polar whereas C6H12O6 is nonpolar and this causes the difference.
The total solute concentration of NaCl is twice that of C6H12O6 because NaCl forms Na+ and Cl– ions and this causes the difference.
Answer: d

32. A solute dissolved in water causes the boiling point to increase by 0
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)?
Yes No
Depends on whether the solute is a strong or weak electrolyte
Depends on if the solute is a nonpolar, nonelectrolyte
Answer: c

34. A solute dissolved in water causes the boiling point to increase by 0
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)?
Yes No
Depends on whether the solute is a strong or weak electrolyte
Depends on if the solute is a nonpolar, nonelectrolyte
Answer: c

35. Of two KBr solutions, one 0. 50 m and the other 0
Of two KBr solutions, one 0.50 m and the other m, which is hypotonic with respect to
the other?
The 0.20 m KCl solution is hypotonic with the m KCl solution.
The 0.50 m KCl solution is hypotonic with the m KCl solution.
Neither is hypotonic to each other.
They are isotonic solutions.
Answer: a

36. Of two KBr solutions, one 0. 50 m and the other 0
Of two KBr solutions, one 0.50 m and the other m, which is hypotonic with respect to
the other?
The 0.20 m KCl solution is hypotonic with the m KCl solution.
The 0.50 m KCl solution is hypotonic with the m KCl solution.
Neither is hypotonic to each other.
They are isotonic solutions.
Answer: a

37. Is the osmotic pressure of a 0
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?
The osmotic pressure of a 0.10 M solution of NaCl is greater than that of a 0.10 M solution of KBr.
The osmotic pressure of a 0.10 M solution of NaCl is equal to that of a 0.10 M solution of KBr.
The osmotic pressure of a 0.10 M solution of NaCl is less than than that of a 0.10 M solution of KBr.
Answer: b

38. Is the osmotic pressure of a 0
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?
The osmotic pressure of a 0.10 M solution of NaCl is greater than that of a 0.10 M solution of KBr.
The osmotic pressure of a 0.10 M solution of NaCl is equal to that of a 0.10 M solution of KBr.
The osmotic pressure of a 0.10 M solution of NaCl is less than than that of a 0.10 M solution of KBr.
Answer: b

39. Some proteins reside in the hydrophobic lipid bilayer of the cell membrane. Would hydrophilic groups of these proteins still be facing the lipid “solvent”?
Yes, proteins have hydrophilic groups on the exterior.
No, the hydrophilic groups would be repelled by the hydrophobicity of the lipids.
Answer: b

40. Some proteins reside in the hydrophobic lipid bilayer of the cell membrane. Would hydrophilic groups of these proteins still be facing the lipid “solvent”?
Yes, proteins have hydrophilic groups on the exterior.
No, the hydrophilic groups would be repelled by the hydrophobicity of the lipids.
Answer: b

41. Why don’t oil drops stabilized by sodium stearate coagulate to form larger oil drops?
Ion-dipole forces
Dipole-dipole forces
Dispersion forces
Hydrogen bonding
Answer: c

42. Why don’t oil drops stabilized by sodium stearate coagulate to form larger oil drops?
Ion-dipole forces
Dipole-dipole forces
Dispersion forces
Hydrogen bonding
Answer: c

43. Nice Job. Now grab a packet and try your hand at a new set of problems
Nice Job!!!! Now grab a packet and try your hand at a new set of problems. Consider skipping the notes packet and trying the problems at the back.
Answer: a

44. Use the rubric on the back of your exam to calculate your score Since we did not answer FR 6 or FR 7, you can figure out your score if you were to receive 4’s on it, or a value from 0-4 of your choice. What did you get?
Answer: a

45. Use the remainder of the period to look over your answers and compare with your peers. If you have specific questions, please ask. Return your exams, please.
Answer: a

46. Exit Ticket (4 min) Answer on a separate sheet of paper:
March 13, 2018
Exit Ticket (4 min)
Answer on a separate sheet of paper:
Calculate the partial pressure of 2 moles of H2 (g) in a container with 6 moles of Cl2 (g) with a total pressure of 16 atm.
Learning Target: I can apply intermolecular forces to the properties of solutions