Chapter 11 Test Bank Answers Solutions

Introduction to Chemistry, 5e (Bauer)

Chapter 11 Solutions

1) Which of the following substances is a strong electrolyte?

A) CH3OH

B) C6H14

C) C6H12O6

D) LiCl

E) SO2

2) Which of the following substances is a strong electrolyte?

A) CH3CH2OH

B) C6H6

C) KOH

D) SO2

E) PCl3

3) Which of the following substances is a strong electrolyte?

A) CH3CH2OH

B) C8H18

C) LiOH

D) CO2

E) PCl5

4) Which of the following substances is a nonelectrolyte?

A) KMnO4

B) CH3CH2OH

C) NaOH

D) K2SO4

E) Na2H

5) Which of the following substances is a nonelectrolyte?

A) Na2SO4

B) CH3OH

C) KOH

D) LiNO3

E) RbCl

6) Which of the following substances is a nonelectrolyte?

A) NaNO3

B) LiOH

C) C6H12O6

D) LiCN

E) CsCl

7) What ions, atoms, or molecules are present after CH3CH2OH(I) mixes with water?

A) CH3CH2OH(aq) and H2O(l)

B) CH3CH2O–(aq), H+(aq), and H2O(l)

C) CH3CH2O–(aq), and H3O+(aq)

D) 2C(aq), 6H(aq), and H2O2(l)

E) CH3+(aq), CH2O–(aq), H+(aq), and H2O(l)

8) What ions, atoms, or molecules (in addition to the water molecules) are present after Na2SO4(s) mixes with water?

A) Na2SO4(l)

B) Na2SO4(ag)

C) Na+(aq) + NaSO4–(aq)

D) Na2SO32+(aq) + O2–(aq)

E) 2Na+(aq) + SO42–(aq)

9) What ions, atoms, or molecules (in addition to the water molecules) are present after HNO3(l) mixes with water?

A) HNO3(l)

B) HNO3(aq)

C) H+(aq) + NO3–(aq)

D) H(aq) + NO3(aq)

E) H(aq) + N(aq) + 3O(aq)

10) Which of the diagrams in the figure best represents an aqueous solution of MgCl2?

A) I

B) II

C) III

D) either I or III

E) none of these is correct

11) Which of the diagrams in the figure best represents an aqueous solution of Na2SO4?

A) I

B) II

C) III

D) either I or III

E) none of these is correct

12) Which of the following equations describes what happens when HCl(g) dissolves in water?

A) HCl(g) → H+(aq) + Cl−(aq)

B) HCl(g) → H(aq) + Cl(aq)

C) 2HCl(g) → H2(aq) + Cl2(aq)

D) 2HCl(g) → H2(g) + Cl2(g)

E) HCl(g) + H2O(l) → H3OCl(l)

13) Which of the following equations describes what happens when CH3OH(l) dissolves in water?

A) CH3OH(l) → C(aq) + 4H(aq) + O(aq)

B) CH3OH(l) → C2−(aq) + 4H+(aq) + O2−(aq)

C) 2CH3OH(l) → 2C(aq) + 4H2(aq) + O2(aq)

D) CH3OH(l) → CH3OH(aq)

E) CH3OH(l) + H2O(l) → CH5O2H(l)

14) Which of the following statements regarding the rule "like dissolves like" is incorrect?

A) Since cooking oil is composed primarily of hydrocarbons, it is insoluble in water.

B) Iodine, I2, is very soluble in water.

C) Ethanol, CH3CH2OH, is water-soluble.

D) Cooking oil, a nonpolar substance, is soluble in hexane, C6H14.

E) Potassium nitrate, KNO3, is soluble in water.

15) Which of the following statements regarding the rule "like dissolves like" is incorrect?

A) Since cooking oil is composed primarily of hydrocarbons, it is soluble in water.

B) Oxygen, O2, is not very soluble in water.

C) Methanol, CH3OH, is water-soluble.

D) Cooking oil, a nonpolar substance, is soluble in heptane, C7H16.

E) Sodium nitrate, NaNO3, is soluble in water.

16) Which of the following statements regarding the rule "like dissolves like" is incorrect?

A) Since grease is nonpolar, it is not soluble in water.

B) Nitrogen, N2, is not very soluble in water.

C) Methanol, CH3OH, is not very water-soluble.

D) Butane, C4H10, is soluble in cooking oil, a nonpolar substance.

E) Calcium nitrate, Ca(NO3), is soluble in water.

17) Which of the following should be most soluble in water?

A) fat (a nonpolar triglyceride molecule)

B) C6H6(l)

C) CH3NH2(l)

D) I2(s)

E) O2(g)

18) Which of the following should be most soluble in water?

A) Vitamin C (a very good hydrogen bonder)

B) Vitamin A (a mostly nonpolar molecule)

C) C6H6(l)

D) I2(s)

E) O2(g)

19) Which of the following should be most soluble in hexane, C6H14?

A) NaCl

B) NaNO3

C) H2O

D) CH3OH

E) Br2

20) Which of the following should be most soluble in benzene, C6H6?

A) H2O

B) CH3OH

C) I2

D) NaCl

E) NaNO3

21) Which of the following should be most soluble in ethanol, CH3CH2OH?

A) CH3NH2

B) CCl4

C) I2

D) C6H6

E) CO2

22) Sodium chloride, NaCl, dissolves in water because

A) there are attractive forces between ions and water molecules.

B) there are no attractive forces between ions and water molecules.

C) the entropy of the solution is greater than the entropy of pure NaCl and pure H2O.

D) the entropy of the solution is less than the entropy of pure NaCl and pure H2O.

E) Both "there are attractive forces between ions and water molecules" and "the entropy of the solution is greater than the entropy of pure NaCl and pure H2O" are correct.

23) Which of the following occurs when an ionic compound dissolves in water to form a solution?

A) Ionic bonds break.

B) Hydrogen bonds are disrupted.

C) H2O – Ion attractive forces form.

D) Entropy increases.

E) All of these

24) Many cold packs contain ammonium nitrate and water. The dissolving of ammonium nitrate is endothermic. Which of the following best describes the energy and entropy changes that occur for the NH4NO3 system when ammonium nitrate and water are mixed to make a solution?

A) There is a net energy increase and an entropy increase.

B) There is a net energy increase and an entropy decrease.

C) There is a net energy decrease and an entropy decrease.

D) There is no a net change in energy or entropy.

25) Which of the following statements regarding the solution process is incorrect?

A) In a sodium chloride solution, the ions interact with the water molecules through ion-dipole forces.

B) Hydration is the process whereby water molecules surround solute particles.

C) A hydrated cation is surrounded by the partially positive end of the water molecules.

D) When an ionic compound dissolves, the ionic bonds break.

E) Some of the hydrogen bonds among the water molecules must break.

26) Which of the following statements regarding the solution process is incorrect?

A) When a solution is formed from an ionic compound, the anions and cations are evenly distributed throughout the solution.

B) When a polar covalent compound dissolves in water, dipole-dipole interactions take place between the water molecules and the solute molecules.

C) A nonpolar compound such as hexane, C6H14, forms London dispersion forces with a nonpolar solute, such as I2 during the solution process.

D) The solution process is always exothermic.

E) When an ionic solute dissolves, the entropy of the solution is usually greater than the original entropy of the crystalline form of the ionic substance.

27) When potassium nitrate is dissolved in water, the resulting solution feels cool to the touch. This means that

A) the strength of attraction between the solute particles is greater than that of the attraction between the solute and solvent.

B) the strength of attraction between the solute and solvent particles is greater than that of the attraction between the solute particles.

C) the strength of attraction between the solute particles is equal to that of the attraction between the solute and solvent.

D) hydrogen bonds must be broken, which is an exothermic process.

E) there is a decrease in entropy for the solution.

28) Which of the following statements regarding solubility is incorrect?

A) A polar compound dissolves an ionic compound due to ion-dipole interactions.

B) A nonpolar solvent will not interact strongly enough with ions to dissolve an ionic compound.

C) Nonpolar liquids will dissolve in one another because the intermolecular forces in the pure liquids are weak, and there is an increase in entropy.

D) Most ionic solids are more soluble in water at higher temperatures than at lower temperatures.

E) Most gases are more soluble in water at higher temperatures than at lower temperatures.

29) Which of the following statements regarding the solubility of oxygen in water is incorrect?

A) Water in contact with air contains a small amount of dissolved oxygen.

B) When water is heated, the first tiny bubbles that you see escaping from the warm water contain N2 and O2.

C) In warm weather, fish must come to the surface more often than in cool weather to get oxygen, since there is less dissolved oxygen in the water than in cooler weather.

D) If a sealed container has both oxygen and water, changing the pressure of the oxygen above the water will have no effect on the solubility of the oxygen in the water.

E) An increase in temperature causes an increase in the kinetic energy of the molecules in a solution, allowing dissolved oxygen molecules to escape the solution more readily.

30) Which of the following increases the solubility of a gas in solution?

A) increasing gas pressure and increasing temperature

B) increasing gas pressure and decreasing temperature

C) decreasing gas pressure and increasing temperature

D) decreasing gas pressure and decreasing temperature

E) adding more water

31) If the solubility of a solid substance is 18.2 g/100 g water, which of the following best describes what eventually forms after 10.0 grams of the substance is mixed with 50.0 grams of water?

A) a saturated solution with some undissolved solid

B) an unsaturated solution with some undissolved solid

C) a saturated solution with no undissolved solid

D) an unsaturated solution with no undissolved solid

E) a supersaturated solution

32) If the solubility of sodium chloride at 25ºC is 36.0 g/100 g water, which of the following best describes what eventually forms after 15.0 grams of sodium chloride is mixed with 50.0 grams of water at 25ºC?

A) a saturated solution with some undissolved solid

B) an unsaturated solution with some undissolved solid

C) a saturated solution with no undissolved solid

D) an unsaturated solution with no undissolved solid

E) a supersaturated solution

33) Given that the solubility of potassium chlorate in water is 10.0 g/100 g water at 30°C, what mass of potassium chlorate is dissolved in 250 grams of a saturated solution at 30°C?

A) any mass greater than 25.0 g

B) any mass less than 10.0 g

C) any mass less than 25.0 g

D) 25.0 g

E) 10.0 g

34) The solubility of potassium chloride is 34.2 g/100.0 g of water at 20ºC. Which of the following best describes a solution prepared by adding 58.3 g of potassium chloride to 150.0 g of water at this temperature?

A) 34.2 g of KCl will dissolve and 24.1 g will remain undissolved.

B) 51.3 g of KCl will dissolve and 7.0 g will remain undissolved.

C) 24.1 g of KCl will dissolve and 34.2 g will remain undissolved.

D) 58.3 g of KCl will dissolve and the solution will be unsaturated.

E) 107 g of KCl will dissolve and the solution will be saturated.

35) What is the percent-by-mass concentration of KCl in a solution that is prepared by adding 13.0 g of KCl to 85.0 g of water?

A) 15.3%

B) 17.2%

C) 13.3%

D) 72.0%

E) 65.4%

36) What is the percent-by-mass concentration of KOH in a solution that is prepared by adding 18.0 g of KOH to 95.0 g of water?

A) 18.9%

B) 15.9%

C) 31.5%

D) 5.28%

E) 77.0%

37) What is the percent-by-mass concentration of NaCl in a solution that is prepared by adding 14.0 g of NaCl to 75.0 g of water?

A) 61.0%

B) 15.7%

C) 18.7%

D) 24.0%

E) 5.36%

38) What mass of sodium nitrate is dissolved in 455 g of a solution that is 15.0% by mass NaNO3?

A) 68.3 g

B) 30.3 g

C) 4.40 × 102 g

D) 3.03 × 103 g

E) 15.0 g

39) What mass of sodium hydroxide is dissolved in 295 g of a solution that is 12.0% by mass NaOH?

A) 3540 g

B) 35.4 g

C) 4.07 g

D) 40.7 g

E) 12.0 g

40) What mass of sodium chloride is dissolved in 365 g of a solution that is 14.0% by mass NaCl?

A) 5110 g

B) 26.1 g

C) 351 g

D) 51.1 g

E) 14.0 g

41) What is the percent-by-mass concentration of antifreeze (ethylene glycol, C2H6O2) in an aqueous solution that contains 420.0 g of ethylene glycol in 1.00 L of solution? The density of the solution is 1.05 g/mL.

A) 2.50%

B) 42.1%

C) 40.0%

D) 44.1%

E) 60.0%

42) What is the percent-by-mass concentration of hydrogen peroxide, H2O2, in an aqueous solution that contains 30.0 g of hydrogen peroxide in 1.00 L of solution? The density of the solution is 1.00 g/mL.

A) 30.0%

B) 3.00%

C) 33.3%

D) 31.0%

E) 70.0%

43) What is the percent-by-mass concentration of citric acid, C6H8O7, in an aqueous solution that contains 263.2 g of citric acid in 1.00 L of solution? The density of the solution is 1.10 g/mL.

A) 73.7%

B) 26.3%

C) 23.9%

D) 3.80%

E) 29.0%

44) A solution of ethanol, C2H5OH, is prepared by dissolving 25.0 mL of ethanol in enough water to give a total volume of 250.0 mL. What is the percent-by-volume concentration of ethanol?

A) 10.0%

B) 9.09%

C) 90.0%

D) 1.00%

E) 225%

45) A solution of acetic acid, CH3CO2H, is prepared by dissolving 30.0 mL of acetic acid in enough water to give a total volume of 150.0 mL. What is the percent-by-volume concentration of acetic acid?

A) 16.7%

B) 15.0%

C) 30.0%

D) 20.0%

E) 25.0%

46) A solution of acetic acid, CH3CO2H, is prepared by dissolving 40.0 mL of acetic acid in enough water to give a total volume of 250.0 mL. What is the percent-by-volume concentration of acetic acid?

A) 19.0%

B) 16.0%

C) 25.0%

D) 40.0%

E) 13.8%

47) How many moles of NaOH are contained in 100.0 mL of 3.00 M NaOH?

A) 0.300 moles

B) 300.0 moles

C) 33.3 moles

D) 0.00300 moles

E) 0.333 moles

48) How many moles of NaCl are contained in 50.0 mL of 2.50 M NaCl?

A) 2.50 moles

B) 0.050 moles

C) 5.00 moles

D) 2.45 moles

E) 0.125 moles

49) How many moles of HCl are contained in 75.0 mL of 2.00 M HCl?

A) 2.00 moles

B) 1.50 ×102 moles

C) 0.150 moles

D) 37.5 moles

E) 26.7 moles

50) What volume of 2.00 M HCl contains 0.50 mol HCl?

A) 1.0 L

B) 0.25 L

C) 2.5 L

D) 0.50 L

E) 1.5 L

51) What volume of 6.00 M NaOH contains 2.50 mol NaOH?

A) 2.50 L

B) 6.00 L

C) 2.40 L

D) 0.417 L

E) 15.0 L

52) What volume of 3.00 M NaOH contains 1.75 mol NaOH?

A) 1.75 L

B) 3.00 L

C) 4.75 L

D) 0.583 L

E) 1.71 L

53) A solution contains 15.5 g of NaOH dissolved in sufficient water to give a total mass of 125.0 g. What is the molality of the solution?

A) 3.54 m

B) 0.124 m

C) 0.00310 m

D) 3.10 m

E) 124 m

54) A solution contains 25.5 g of NaCl dissolved in sufficient water to give a total mass of 325.0 g. What is the molality of the solution?

A) 0.146 m

B) 0.785 m

C) 1.34 m

D) 1.46 m

E) 134 m

55) A solution contains 22.0 g of HCl dissolved in sufficient water to give a total mass of 125.0 g. What is the molality of the solution?

A) 0.250 m

B) 5.86 m

C) 2.75 m

D) 4.83 m

E) 0.176 m

56) What is the molal concentration of ions in a 2.40 m solution of Al(NO3)3?

A) 2.40 m

B) 7.20 m

C) 9.60 m

D) 0.800 m

E) 31.2 m

57) What is the molal concentration of ions in a 1.60 m solution of Fe(NO3)3?

A) 1.60 m

B) 3.20 m

C) 4.80 m

D) 6.40 m

E) 20.8 m

58) A 150.0 g sample of ocean water contains 3.5 mg of mercury. How many parts per million of mercury are in the sample?

A) 15 ppm

B) 23 ppm

C) 2.4 × 102 ppm

D) 2.3 × 104 ppm

E) 43 ppm

59) A 200.0 g sample of river water contains 6.4 mg of lead. How many parts per million of lead are in the sample?

A) 6.5 ppm

B) 21 ppm

C) 3.2 × 102 ppm

D) 32 ppm

E) 54 ppm

60) A 200.0 g sample of rainwater contains 4.8 mg of sulfuric acid. How many parts per million of sulfuric acid are in the sample?

A) 42 ppm

B) 21 ppm

C) 2.4 × 102 ppm

D) 4.8 ppm

E) 24 ppm

61) The EPA has determined that the maximum safe level of lead ion in drinking water is 15 ppb. If a sample of tap water has a lead ion concentration of 0.0065 ppm, what is the concentration of the lead ion in ppb, and is the water safe to drink? Assume the density of the solution is 1.00 g/mL.

A) 65 ppb, not safe

B) 6.5 ppb, safe

C) 650 ppb, not safe

D) 0.65 ppb, safe

E) 6.5 × 10–6 ppm, safe

62) The EPA has determined that the maximum safe level of lead ion in drinking water is 15 ppb. If a sample of tap water has a lead ion concentration of 0.016 ppm, what is the concentration of the lead ion in ppb, and is the water safe to drink? Assume the density of the solution is 1.00 g/mL.

A) 160 ppb, not safe

B) 16 ppb, not safe

C) 1600 ppb, not safe

D) 0.16 ppb, safe

E) 1.6 × 10–6 ppm, safe

63) Silver nitrate, AgNO3, can be used to test for the presence of chloride ions in solution, because it readily forms a precipitate of AgCl. What volume of 2.0 M AgNO3 will be required to react with 50.0 mL of a 0.10 M HCl solution? AgNO3(aq) + HCl(aq) → AgCl(s) + HNO3(aq)

A) 0.25 mL

B) 25 mL

C) 5.0 × 101 mL

D) 2.5 × 102 mL

E) 2.5 mL

64) Silver nitrate, AgNO3, can be used to test for the presence of chloride ions in solution, because it readily forms a precipitate of AgCl. What volume of 1.5 M AgNO3 will be required to react with 30.0 mL of a 0.45 M HCl solution AgNO3(aq) + HCl(aq) → AgCl(s) + HNO3(aq)?

A) 45 mL

B) 9.0 mL

C) 9.0 L

D) 1.0 L

E) 1.1 × 102 mL

65) How many moles of potassium iodide, KI, are required to precipitate all of the lead(II) ion from 50.0 mL of a 1.2 M Pb(NO3)2 solution? (First, write a balanced equation for the reaction.)

A) 0.12 mole

B) 0.060 mole

C) 0.24 mole

D) 0.030 mole

E) 0.048 mole

66) How many moles of potassium iodide, KI, are required to precipitate all of the lead (II) ion from 25.0 mL of a 1.6 M Pb(NO3)2 solution? (First, write a balanced equation for the reaction.)

A) 0.040 mole

B) 0.080 mole

C) 0.020 mole

D) 64 mol

E) 0.64 mol

67) What volume of 0.1243 M KOH is required to neutralize 25.00 mL of 0.1540 M H2SO4? (First, write a balanced equation for the reaction.)

A) 10.09 mL

B) 30.97 mL

C) 61.95 mL

D) 20.18 mL

E) 40.36 mL

68) What volume of 0.1452 M KOH is required to neutralize 25.00 mL of 0.1020 M H2SO4? (First, write a balanced equation for the reaction.)

A) 17.79 mL

B) 17.56 mL

C) 8.781 mL

D) 35.12 mL

E) 71.18 mL

69) When a 25.00 mL sample of H2SO4 is titrated with 0.2453 M NaOH, 32.47 mL of NaOH solution is required to neutralize the H2SO4. What is the molarity of the H2SO4?

A) 0.3186 M

B) 0.1889 M

C) 0.3777 M

D) 3.309 M

E) 0.1593 M

70) When a 25.00 mL sample of H2SO4 is titrated with 0.3423 M NaOH, 26.67 mL of NaOH solution is required to neutralize the H2SO4. What is the molarity of the H2SO4?

A) 0.3652 M

B) 0.3209 M

C) 0.1604 M

D) 0.1826 M

E) 0.1988 M

71) When a 25.00 mL sample of NaOH is titrated with 0.4523 M H2SO4, 36.69 mL of H2SO4 solution is required to neutralize the NaOH. What is the molarity of the NaOH?

A) 0.3319 M

B) 0.6638 M

C) 1.328 M

D) 0.6164 M

E) 0.1988 M

72) When a 25.00 mL sample of NaOH is titrated with 0.2523 M H2SO4, 26.69 mL of H2SO4 solution is required to neutralize the NaOH. What is the molarity of the NaOH?

A) 0.1347 M

B) 0.4726 M

C) 0.5387 M

D) 0.2694 M

E) 0.2363 M

73) Consider two aqueous glucose solutions of different concentrations, separated by a semi-permeable membrane. Which of the following best describes the process of osmosis at the molecular level?

A) The smaller water molecules move in a net direction from the more dilute side to the more concentrated side.

B) The smaller water molecules move in a net direction from the more concentrated side to the more dilute side.

C) The larger glucose particles move in a net direction from the more dilute side to the more concentrated side.

D) The larger glucose particles move in a net direction from the more concentrated side to the more dilute side.

E) Osmosis will not occur.

74) What will happen to a blood cell that is placed in pure water?

A) The cell will shrink because there will be a net flow of water to the outside of the cell.

B) The cell will shrink because there will be a net flow of electrolytes to the outside of the cell.

C) The cell will expand because there will be a net flow of water to the inside of the cell.

D) The cell will expand because there will be a net flow of electrolytes to the inside of the cell.

E) Nothing will happen because the cell is impermeable.

75) What will happen to a blood cell that is placed in an aqueous solution that has a high salt concentration relative to the blood cell concentration?

A) The cell will shrink because there will be a net flow of water to the outside of the cell.

B) The cell will shrink because there will be a net flow of electrolytes to the outside of the cell.

C) The cell will expand because there will be a net flow of water to the inside of the cell.

D) The cell will expand because there will be a net flow of electrolytes to the inside of the cell.

E) Nothing will happen because the cell is impermeable.

76) Calculate the freezing point of a 2.0 m solution of sucrose in water. Sucrose is a nonelectrolyte. The normal freezing point of pure water is 0.00ºC. Kf (water) = –1.86ºC/m.

A) –1.86ºC

B) –3.72ºC

C) –2.00ºC

D) 3.72ºC

E) 1.86ºC

77) Calculate the boiling point of a 4.0 m solution of sucrose in water. Sucrose is a nonelectrolyte. The normal boiling point of pure water is 100.0ºC. Kb (water) = 0.52ºC/m.

A) 2.1ºC

B) 97.9ºC

C) 96.0ºC

D) 94.0ºC

E) 102.1ºC

78) Calculate the freezing point of a 2.0 m solution of NaCl in water. Remember that NaCl is an electrolyte. The normal freezing point of pure water is 0.00ºC. Kf (water) = –1.86ºC/m.

A) –2.08ºC

B) –3.72ºC

C) –7.44ºC

D) 7.44ºC

E) 3.74ºC

79) Calculate the boiling point of a 4.0 m solution of KI in water. Remember that KI is an electrolyte. The normal boiling point of pure water is 100.0ºC. Kb (water) = 0.52ºC/m.

A) 101.0 ºC

B) 104.2ºC

C) 96.0ºC

D) 102.1ºC

E) 4.16ºC

80) Calculate the freezing point of a 1.0 m solution of Ca(NO3)2 in water. Remember that Mg(NO3)2 is an electrolyte. The normal freezing point of pure water is 0.00ºC. Kf (water) = –1.86ºC/m.

A) 1.56 ºC

B) 5.58ºC

C) 1.86ºC

D) –5.58ºC

E) –1.86ºC

81) Which of the following aqueous solutions should have the lowest freezing point?

A) 1.0 m C12H22O11

B) 1.0 m NaNO3

C) 1.0 m NaCl

D) 1.0 m MgCl2

E) All should have the same freezing point

82) Which of the following aqueous solutions should have the highest boiling point?

A) 1.0 m MgCl2

B) 1.0 m NaNO3

C) 1.0 m NaCl

D) 1.0 m C12H22O11

E) All should have the same boiling point

83) Which of the following properties of water increases as the concentration of particles dissolved in the water increases?

A) vapor pressure

B) boiling point

C) freezing point

D) melting point

E) none of these

84) What happens to the vapor pressure, boiling point, and freezing point of a liquid when a solute is dissolved in the liquid to form a solution?

A) Vapor pressure increases, boiling point decreases, and freezing point decreases.

B) Vapor pressure decreases, boiling point decreases, and freezing point decreases.

C) Vapor pressure decreases, boiling point increases, and freezing point decreases.

D) Vapor pressure increases, boiling point decreases, and freezing point increases.

E) Vapor pressure increases, boiling point increases, and freezing point increases.

85) What happens to the osmotic pressure, boiling point, and freezing point of a solution when the concentration of the solute is decreased?

A) Osmotic pressure increases, boiling point increases, and freezing point increases.

B) Osmotic pressure decreases, boiling point increases, and freezing point decreases.

C) Osmotic pressure decreases, boiling point decreases, and freezing point decreases.

D) Osmotic pressure decreases, boiling point decreases, and freezing point increases.

E) Osmotic pressure increases, boiling point decreases, and freezing point increases.

86) Rank the following solutions in order of increasing boiling point:

2.5 m fructose, C6H12O6

2.0 m NaCl

1.5 m methanol, CH3OH

2.2 m Al(NO3)3

A) C6H12O6 < Al(NO3)3 < NaCl < CH3OH

B) CH3OH < Al(NO3)3 < NaCl < C6H12O6

C) Al(NO3)3 < NaCl < C6H12O6 < CH3OH

D) CH3OH < C6H12O6 < NaCl < Al(NO3)3

E) CH3OH < C6H12O6 < Al(NO3)3 < NaCl

87) Rank the following solutions in order of increasing boiling point:

3.5 m fructose, C6H12O6

1.0 m NaCl

2.5 m methanol, CH3OH

2.2 m Al(NO3)3

A) C6H12O6 < Al(NO3)3 < NaCl < CH3OH

B) CH3OH < Al(NO3)3 < NaCl < C6H12O6

C) Al(NO3)3 < NaCl < C6H12O6 < CH3OH

D) NaCl < CH3OH < C6H12O6 < Al(NO3)3

E) CH3OH < C6H12O6 < Al(NO3)3 < NaCl

88) Rank the following solutions in order of increasing boiling point:

1.5 m fructose, C6H12O6

2.2 m NaCl

2.0 m methanol, CH3OH

1.0 m Al(NO3)3

A) C6H12O6 < CH3OH < Al(NO3)3 < NaCl

B) CH3OH < Al(NO3)3 < NaCl < C6H12O6

C) Al(NO3)3 < NaCl < C6H12O6 < CH3OH

D) C6H12O6 < CH3OH < NaCl < Al(NO3)3

E) NaCl < C6H12O6 < CH3OH < Al(NO3)3

89) The images represent a solution of NaCl, a solution of glucose, and a more dilute solution of glucose. Rank the aqueous solutions in order of highest to lowest freezing point.

A) I > II > III

B) II > I > III

C) II > III > I

D) III > II > I

E) III > I > II

90) The images represent a solution of NaNO3, a more concentrated solution of NaNO3, and an MgCl2 solution. Rank the aqueous solutions in order of highest to lowest freezing point.

A) I > II > III

B) II > I > III

C) III > II > I

D) I > III > II

E) III > I > II

91) Which of the following is not a colligative property of a solution?

A) osmotic pressure

B) vapor pressure

C) density

D) boiling point

E) freezing point

92) Determine the molal concentration of solute particles in a 3.0 m CH3OH solution.

A) 6.0 m

B) 3.0 m

C) 18 m

D) 12 m

E) 1.0 m

93) Determine the molal concentration of solute particles in a 3.0 m Ca(NO3)2 solution.

A) 6.0 m

B) 3.0 m

C) 18 m

D) 9.0 m

E) 27 m

94) Determine the molal concentration of solute particles in a 3.0 m C2H5OH solution.

A) 6.0 m

B) 3.0 m

C) 18 m

D) 9.0 m

E) 27 m

95) Rank the following solutions in order of increasing osmotic pressure: 1.0 m C2H5OH, 1.0 m Ca(NO3)2, 2.0 m NaCl, 3.0 m C6H12O6

A) C2H5OH = Ca(NO3)2 < NaCl < C6H12O6

B) C6H12O6 < NaCl < C2H5OH = Ca(NO3)2

C) C2H5OH < Ca(NO3)2 < NaCl < C6H12O6

D) C2H5OH < Ca(NO3)2 = NaCl < C6H12O6

E) C2H5OH < Ca(NO3)2 = C6H12O6 < NaCl

96) Rank the following solutions in order of increasing osmotic pressure: 2.0 m CH3OH, 1.0 m Ba(NO3)2, 3.0 m KCl, 3.0 m C6H12O6

A) Ba(NO3)2 < CH3OH < KCl = C6H12O6

B) C6H12O6 = KCl < CH3OH < Ba(NO3)2

C) CH3OH < Ba(NO3)2 = C6H12O6 < KCl

D) CH3OH < Ba(NO3)2 < C6H12O6 < KCl

E) KCl < CH3OH < Ba(NO3)2 < C6H12O6

97) Rank the following solutions in order of increasing osmotic pressure: 1.0 m CH3OH, 1.0 m Ba(NO3)2, 2.0 m KCl, 4.0 m C6H12O6

A) Ba(NO3)2 < CH3OH < KCl = C6H12O6

B) C6H12O6 = KCl < CH3OH < Ba(NO3)2

C) CH3OH < Ba(NO3)2 = C6H12O6 < KCl

D) CH3OH < Ba(NO3)2 < C6H12O6 = KCl

E) KCl < CH3OH < Ba(NO3)2 < C6H12O6

98) Vinegar is a mixture of about 5 g of acetic acid in every 95 g of water. Therefore, the acetic acid is the solvent, and the water is the solute.

99) Sterling silver is an alloy consisting of silver mixed with a small amount of copper. Therefore, the silver is the solvent and the copper is the solute.

100) The solute in the solution shown in the figure is a nonelectrolyte.

101) The solute in the solution shown in the figure is a nonelectrolyte.

102) Gases are more soluble in water at higher temperature.

103) Gases are more soluble in water at higher pressure.

104) Solids are generally more soluble in water at higher temperature.

105) The solubility of sodium chloride is 35 g/100 g of water at 20ºC. The solution that would be formed when 46 g of sodium chloride is added to 100.0 g of water at this temperature would consist of 35 g of sodium chloride dissolved in the water, and 11 g of sodium chloride remaining undissolved.

106) Percent-by-volume concentrations are often used for solutions with a liquid dissolved in a liquid.

107) The units of molality are moles of solute per kilogram of solution.

108) Colligative properties depend on the concentration of the particles in a solution, rather than on their identity.

109) Compared to a pure solvent, a solution of the same liquid has a lower boiling point.

110) The molality of a solution does not change with temperature, whereas the molarity does vary with temperature.

111) Calculate the molality of a solution prepared by dissolving 12.5 g of KNO3 in enough water to make 98.0 g of solution.

112) What volume (in milliliters) of 0.2500 M NaOH is required to neutralize 25.00 mL of 0.2000 M HCl?

113) What volume (in milliliters) of 0.2500 M NaOH is required to neutralize 10.00 mL of 0.4000 M H2SO4?

114) What volume (in milliliters) of 0.2500 M NaOH is required to neutralize 50.00 mL of 0.1000 M H3PO4?

115) The solubility of NaCl at 30ºC is 36.3 g/100 g of water. What mass (in grams) of NaCl is dissolved in a saturated solution that contains 300.0 grams of water?

116) A solution is prepared by dissolving 100.0 g of cesium chloride (CsCl) in 100.0 g of water. The density of the solution is 1.58 g/cm3. Calculate the mass percent of the cesium chloride in the solution.

117) A solution is prepared by dissolving 100.0 g of cesium chloride (CsCl) in 100.0 g of water. The density of the solution is 1.58 g/cm3. Calculate the molarity of the cesium chloride.

118) A solution is prepared by dissolving 100.0 g of cesium chloride (CsCl) in 100.0 g of water. The density of the solution is 1.58 g/cm3. Calculate the molality of the cesium chloride solution.

119) When solutions of silver nitrate, AgNO3, and calcium iodide, CaI2, are mixed, a yellow precipitate of silver iodide is formed. Calculate the mass (in grams) of silver iodide formed if 50.00 mL of 1.00 M AgNO3 is combined with 30.00 mL of 1.25 M CaI2.