Solutions Smith Ch.8 Test Bank

General, Organic and Biological Chemistry, 4e (Smith)

Chapter 8 Solutions

1) Which is not an example of a solution?

A) A dental filling

B) Chicken noodle soup

C) Gasoline

D) Tap water

2) Which of the following pairs of compounds forms a solution?

A) NaBr and CCl4

B) Methanol (CH3OH) and water

C) Octane (C8H18) and water

D) Nonanone (C9H18O) and water

3) Which substance is a nonelectrolyte?

A) NaCl

B) (NH4)2SO4

C) H2O2

D) KOH

4) Which substance is a colloid?

A) Mayonnaise

B) A dental filling

C) Mint chocolate chip ice cream

D) Gasoline

5) Which mixture has the largest particle size?

A) Solution

B) Suspension

C) Colloid

D) They all have the same particle size.

6) Nonpolar compounds are soluble in ________.

A) ionic compounds

B) electrolytes

C) polar solvents

D) nonpolar solvents

7) The attraction of an ion with a dipole in a molecule is called ________.

A) a dipole-dipole interaction

B) an ion–dipole interaction

C) hydrogen bonding

D) London dispersion forces

E) van der Waals forces

8) Which pair of compounds will form a solution?

A) Benzene (C6H6) and hexane (C6H14)

B) Na2SO4 and benzene (C6H6)

C) NaCl and hexane (C6H14)

D) H2O and CCl4

E) More than one of the combinations above will form solutions.

9) Which ionic compound is not soluble in water?

A) NaCl

B) AgCl

C) (NH4)2SO4

D) Ca(CH3CO2)2

10) Which ionic compound is soluble in water?

A) PbBr2

B) Fe(OH)3

C) BaSO4

D) Ca(NO3)2

E) More than one of the ionic compounds is soluble in water.

11) Henry's law states that the solubility of a gas in a liquid is proportional to the ________.

A) partial pressure of the gas above the liquid

B) temperature of the liquid

C) temperature of the gas above the liquid

D) molecular weight of the gas above the liquid

12) Which of the following would increase the solubility of solid NaCl in water ________.

A) decreasing the temperature of the solution

B) increasing the temperature of the solution

C) decreasing the pressure of the solution

D) increasing the pressure of the solution

13) Which of the following would increase the solubility of gaseous O2 in water?

A) Decreasing the temperature of the solution

B) Increasing the temperature of the solution

C) Decreasing the pressure of the solution

D) Increasing the pressure of the solution

E) Both A and D are correct

14) A solution is made by dissolving 3.88 g of NaCl in enough water to make 67.8 mL of solution. What is the concentration of sodium chloride in units of weight/volume percent?

A) 5.41% (w/v) NaCl

B) 94.3% (w/v) NaCl

C) 5.72% (w/v) NaCl

D) 0.0572% (w/v) NaCl

15) A solution is made by mixing 569 mL of water and 238 mL ethanol. What is the concentration of ethanol in units of volume/volume percent?

A) 41.8% (v/v) ethanol

B) 0.418% (v/v) ethanol

C) 29.5% (v/v) ethanol

D) 0.295% (v/v) ethanol

E) 70.5% (v/v) ethanol

16) A saline solution used in intravenous drips for patients who cannot take oral fluids contains 0.92% (w/v) NaCl in water. How many grams of NaCl are contained in 575 mL of this solution?

A) 53 g NaCl

B) 529 g NaCl

C) 5.3 g NaCl

D) 0.016 g NaCl

E) 1.6 g NaCl

17) A particular wine contains 11.2% (v/v) ethanol. What volume of ethanol is in a 750.-mL bottle of this wine?

A) 84.0 mL ethanol

B) 0.840 mL ethanol

C) 6.70 mL ethanol

D) 14.9 mL ethanol

18) A saline solution used in intravenous drips for patients who cannot take oral fluids contains 0.92% (w/v) NaCl in water. What volume of the saline solution must be administered to the patient in order to deliver 7.7 g of NaCl?

A) 8.4 mL of saline solution

B) 840 mL of saline solution

C) 7.1 mL of saline solution

D) 140 mL of saline solution

19) A sample of seawater contains 1.3 g of calcium ions in 3,100 kg of solution. What is the calcium ion concentration of this solution in units of ppm?

A) 4.2 × 10–4 ppm Ca2+ ions

B) 0.42 ppm Ca2+ ions

C) 420 ppm Ca2+ ions

D) 4.0 ppm Ca2+ ions

E) 4.0 × 103 ppm Ca2+ ions

20) Which solution contains the smallest number of moles of sucrose (C12H22O11, molar mass = 342.30 g/mol)?

A) 2,000 mL of a 5.0 × 10–5% (w/v) sucrose solution

B) 2,000 mL of a 5.0 ppm sucrose solution

C) 20 mL of a 5.0 M sucrose solution

D) All of the solutions contain the same number of moles of sucrose.

21) What is the molarity of a solution made by dissolving 3.09 moles of NaCl in 1.50 L of solution?

A) 4.64 M NaCl

B) 4.85 M NaCl

C) 2.06 M NaCl

D) 0.673 M NaCl

22) What is the molarity of a solution made by dissolving 36.29 g of NaCl in 2.30 L of solution?

A) 15.78 M NaCl

B) 0.0634 M NaCl

C) 0.270 M NaCl

D) 2.70 M NaCl

23) What is the molarity of a solution made by dissolving 4.88 g of KCl in 423 mL of solution?

A) 0.0115 M KCl

B) 11.5 M KCl

C) 1.55 × 10–4 M KCl

D) 0.155 M KCl

24) How many grams of glucose (C6H12O6) are contained in 555 mL of a 1.77 M glucose solution?

A) 0.982 g C6H12O6

B) 177 g C6H12O6

C) 0.555 g C6H12O6

D) 0.177 g C6H12O6

25) What is the maximum volume of a 0.788 M CaCl2 solution that can be prepared using 85.3 g CaCl2?

A) 1.00 L

B) 0.769 L

C) 0.975 L

D) 67.2 L

26) Which solution has the greatest mass of solute?

A) 2.00 L of a 0.75 M NaCl solution

B) 2.00 L of a 0.75 M CaCl2 solution

C) 2.00 L of a 0.75 M Ca(NO3)2 solution

D) 2.00 L of a 0.75 M Na2CO3 solution

E) All of the solutions have the same mass of solute.

27) Which compound will be the least soluble in water?

A)

B)

C)

D)

28) Which compound will be the most soluble in water?

A)

B)

C)

D)

29) What is the concentration of a solution formed by diluting 25.0 mL of a 3.2 M NaCl solution to 135.0 mL?

A) 17 M NaCl

B) 0.59 M NaCl

C) 0.50 M NaCl

D) 2.7 M NaCl

30) What is the concentration of a solution formed by adding 65.0 mL of water to 25.0 mL of a 3.2 M NaCl solution?

A) 0.89 M NaCl

B) 1.2 M NaCl

C) 2.3 M NaCl

D) 12 M NaCl

31) How many milliliters of a 5.25% (w/v) HCl solution must be used to prepare 250 mL of a 0.175% (w/v) HCl solution?

A) 8.3 mL HCl solution

B) 7,500 mL HCl solution

C) 230 mL HCl solution

D) 240 mL HCl solution

E) 8.6 mL HCl solution

32) Which solution has the highest boiling point?

A) A solution formed by dissolving 0.75 mol of KCl in 1.00 kg of water.

B) A solution formed by dissolving 0.75 mol of glucose (C6H12O6) in 1.00 kg of water.

C) A solution formed by dissolving 0.75 mol of Ca(NO3)2 in 1.00 kg of water.

D) A solution formed by dissolving 0.75 mol of Na3PO4 in 1.00 kg of water.

E) All of the solutions described have the same boiling point.

33) Which solution has the lowest boiling point?

A) A solution formed by dissolving 0.75 mol of KCl in 1.00 kg of water.

B) A solution formed by dissolving 0.75 mol of glucose (C6H12O6) in 1.00 kg of water.

C) A solution formed by dissolving 0.75 mol of Ca(NO3)2 in 1.00 kg of water.

D) A solution formed by dissolving 0.75 mol of Na3PO4 in 1.00 kg of water.

E) All of the solutions described have the same boiling point.

34) Which solution has the highest freezing point?

A) A solution formed by dissolving 0.75 mol of KCl in 1.00 kg of water.

B) A solution formed by dissolving 0.25 mol of KCl in 1.00 kg of water.

C) A solution formed by dissolving 0.75 mol of KCl in 4.00 kg of water.

D) A solution formed by dissolving 0.25 mol of KCl in 0.50 kg of water.

E) All of the solutions described have the same freezing point.

35) A hypotonic solution has ________ osmotic pressure than/as body fluids.

A) a higher

B) a lower

C) the same

36) If cells are placed in a hypertonic solution, ________.

A) water diffuses out of the cells and the cells shrink in a process called hemolysis

B) water diffuses out of the cells and the cells shrink in a process called crenation

C) water diffuses into the cells and the cells swell and eventually burst in a process called hemolysis

D) water diffuses into the cells and the cells swell and eventually burst in a process called crenation

37) If cells are placed in an isotonic solution, ________.

A) water diffuses out of the cells and the cells shrink in a process called hemolysis

B) water diffuses out of the cells and the cells shrink in a process called crenation

C) water diffuses into the cells and the cells swell and eventually burst in a process called hemolysis

D) water diffuses into and out of the cell to an equal extent

38) Red Blood Cells are placed into a solution, and the cells begin to swell in a process called hemolysis. How should the solution be classified?

A) Isotonic

B) Hypertonic

C) Hypotonic

D) None of the choices are correct.

39) What is the molarity of a 25.0% (v/v) aqueous isopropyl alcohol solution? The density of isopropyl alcohol (C3H8O, molar mass 60.09 g/mol) is 0.786 g/mL.

A) 0.529 M

B) 1.18 M

C) 0.327 M

D) 3.27 M

40) What is the molarity of a 11.5% (w/v) glucose (C6H12O6, molar mass 180.16 g/mol) solution?

A) 0.0638 M

B) 0.638 M

C) 1.15 M

D) 1.76 M

41) The maximum level of lead allowed in drinking water is 15 mg/kg. What is this concentration in units of parts per million?

A) 15 ppm

B) 1.5 × 10–2 ppm

C) 1.5 × 104 ppm

D) 3.1 ppm

42) A flask contains two compartments (A and B) with equal volumes of solution separated by a semipermeable membrane. Which diagram represents the final level of the liquids if A is initially a 10% (w/v) glucose solution and B is initially a 20% (w/v) glucose solution?

A)

B)

C)

43) Which of the following statements best describes the solubility of a substance?

A) The ability of the substance to dissolve in water

B) The ability of the substance to dissociate into ions when dissolved in water

C) The maximum amount of a substance that can dissolve in a specific amount of solvent

D) The mass of solvent necessary to completely dissolve 100 g of the substance

44) Which of the following statements concerning a solution is NOT true?

A) A solution is a heterogeneous mixture of two or more pure substances.

B) A solution is composed of a solvent and one or more solutes; the solute(s) dissolve in the solvent.

C) A solution has its components uniformly distributed.

D) A solution is likely to form when the solute(s) and the solvent have similar polarities.

45) Which of the following statements concerning solution concentration is NOT true?

A) An unsaturated solution contains less than the maximum amount of solute that can be dissolved in the solvent.

B) A saturated solution contains more than 100 g of dissolved solute.

C) A solution can be made less concentrated by adding additional solvent.

D) The number of moles of solute present in exactly one liter of solution is referred to as the solution's molarity.

46) Which of the following describes an unsaturated solution?

A) A solution that has less than the maximum number of grams of solute dissolved

B) A solution that has the maximum number of grams of solute dissolved

C) A solution that has more that the maximum number of grams of solute dissolved

D) None of the choices are correct.

47) An unknown amount of water is added to 75 mL of a 3.5 M aqueous glucose solution. What can be said about the concentration of the resulting solution?

A) The concentration of the resultant glucose solution will be less than 3.5 M.

B) The concentration of the resultant glucose solution will be greater than 3.5 M.

C) The concentration of the resultant glucose solution will remain the same because the amount of glucose has not changed.

D) It is impossible to say anything about the concentration of the resultant glucose solution because the amount of added water has not been provided.

48) What interactions are responsible for holding dissolved Cl– ions in an aqueous solution?

A) Ion-ion attractions between K+ and Cl– ions

B) Ion-dipole attractions between Cl– ions and the hydrogen atoms of water

C) Ion-dipole attractions between Cl– ions and the oxygen atom of water

D) Hydrogen bonding between the Cl– ions and water

49) Magnesium hydroxide can be made by the reaction shown below. If a chemist requires 0.725 moles of NaOH for this reaction, what volume of a 1.50 M NaOH solution is needed to provide this amount?

MgCl2(aq) + 2 NaOH(aq) → Mg(OH)2(s) + 2 NaCl(aq)

A) 0.483 L of a 1.50 M NaOH solution

B) 0.967 L of a 1.50 M NaOH solution

C) 1.09 L of a 1.50 M NaOH solution

D) 967 mL of a 1.50 M NaOH solution

50) Any mixture of two or more components is a solution.

51) Water solubility for neutral molecules occurs only for small polar molecules or those with many O or N atoms that can hydrogen bond to water.

52) In solution formation, solvation always releases more energy than that required to separate particles, so the overall process is always exothermic.

53) Methanol (CH3OH) is soluble in water.

54) Heptane (C7H16) is soluble in water.

55) For most ionic and molecular solids, solubility generally increases as temperature increases.

56) The solubility of gases increases with increasing temperature.

57) The greater the number of dissolved particles in a solution, the lower the solution's osmotic pressure.

58) The solubility of helium gas in water is greater at 25 °C than at 50 °C.

59) The ionic compound (NH4)2SO4 is soluble in water.

60) The ionic compound CaCO3 is soluble in water.

61) Ethylene glycol is more soluble in water than propane.  

62) Pure water has an osmotic pressure of 1 atm.

63) Since living cells are surrounded by biological solutions separated by a semipermeable membrane, the osmotic pressure must be higher in the cell than outside the cell membrane.

64) A nonvolatile solute makes it harder for solvent molecules to form a crystalline solid, thus decreasing its melting point.

65) If the attractive forces between the ions and water are stronger than the attraction between the ions in the crystal, an ionic compound dissolves in water.

66) Dialysis is a process that involves the selective passage of water, protein molecules, and ions across a semipermeable membrane.

67) Only solids dissolve in water to form solutions.

68) The solubility of KI in water at 20 °C is 140 g KI/100 g H2O. If 160 g of KI is mixed with 150 g of water, all of the KI will dissolve and the solution that results will be unsaturated.

69) The boiling point of a solution that contains 0.64 mol of Mg(NO3)2 in 1.00 kg of water is 100.98 °C.

70) The presence of a solute reduces the vapor pressure of the solvent above the solution, raising its boiling point.

71) A 6.10 M NaCl solution is made by adding 356 g of NaCl to a flask that contains 1.00 L of water.

72) The concentration unit of weight/volume percent concentration, (w/v)%, is the number of grams of solute dissolved in 100 mL of solution.

73) Nonpolar compounds are soluble in nonpolar solvents and insoluble in polar solvents.

74) Vitamin D is tested for its solubility in water and benzene (C6H6), and is found to be insoluble in water and soluble in benzene. These solubility results indicate that Vitamin D is most likely a nonpolar compound.

75) A solution containing the maximum number of grams of solute that can dissolve in the solvent is said to be supersaturated.

76) Liquid solutions are always transparent and colorless.

77) Sodium chloride is soluble in nonpolar solvents such as octane (C8H18).

78) The solubility of Ba(NO3)2 in water is lower at 25 °C than at 50 °C.

79) Compared to the pure solvent, the freezing point depression caused by adding 0.05 mol of sucrose to 1.0 L of water is greater than the boiling point elevation of the same solution.

80) A solution can be made less concentrated by adding additional solvent.

81) An aqueous solution with the label 0.25 M sucrose contains 0.25 grams of sucrose in every 1 L of solution.

82) When calculating the concentration of a solution in units of parts per million, the "parts" must be expressed in units of grams.

83) Dilution is the addition of solute to decrease the concentration of solvent.

84) Colligative properties are properties of a solution that depend on the concentration of the solute particles but not their identity.

85) All nonvolatile solutes are ionic compounds that do not readily escape into the vapor phase, and thus they have a negligible vapor pressure at a given temperature.

86) A liquid solution that contains a nonvolatile solute has a higher boiling point than the solvent alone.

87) Osmosis is the passage of water and small molecules across a semipermeable membrane from a solution of high solute concentration to a solution of lower solute concentration.

88) When two substances form a solution, the substance present in the lesser amount is called the ________, and the substance present in the larger amount is the ________.

89) A solution with water as the solvent is called a(n) ________ solution.

90) The process of solvent molecules surrounding solute particles is called ________.

91) Solubility is often summed up in three words: "________".

92) The melting point of a solution prepared from 2.00 moles of NaCl in 1.00kg of water is ______ºC.

93) ________ is the passage of water and small molecules across a semipermeable membrane from a solution of low solute concentration to a solution of higher solute concentration.

94) Two solutions with the same osmotic pressure are said to be ________.

95) Each day, the stomach produces 2.0 L of gastric juice that contains 0.10 M HCl. This corresponds to ________ grams of HCl each week.

96) In order for a solution to conduct electricity it must contain ________.

97) Ringer's solution is an aqueous solution of NaCl, KCl, and CaCl2 that is used for treating burns and wounds. The solvent in this solution is ________.

98) Dilution involves adding additional ________ to a solution in order to decrease the concentration of the ________.