General, Organic And Biological Chemistry 2nd Edition By Laura D. Frost- Test Bank A+

Description

Which assumption is not part of the kinetic-molecular theory of gases?
	A)	A gas consists of particles that move randomly and rapidly.
	B)	The size of gas particles is small compared to the space between the particles.
	C)	Because the space between gas particles is large, gas particles exert no attractive forces on each other.
	D)	The kinetic energy of gas particles does not change with increasing temperature.
	E)	When gas particles collide with each other, they rebound and travel in new directions.
	Ans: D Difficulty: Easy

2.	A patient’s systolic pressure is measured as 128 mm Hg. What is this pressure in units of atm?
	A) 128 atm B) 1.28 atm C) 0.168 atm D) 9.73 x 104 atm
	Ans: C Difficulty: Easy

3.	An aerosol can has a pressure of 1.86 atm. What is this pressure expressed in units of mm Hg?
	A) 1.86 mm Hg B) 1410 mm Hg C) 1860 mm Hg D) 0.00245 mm Hg
	Ans: B Difficulty: Easy

4.	A scuba diver typically begins a dive with a compressed air tank at 2,350 psi. What is this pressure expressed in units of mm Hg?
	A)	160. mm Hg	C)	3.09 mm Hg
	B)	1.79 × 106 mm Hg	D)	1.21 × 105 mm Hg
	Ans: D Difficulty: Medium

5.	A scuba diver typically begins a dive with a compressed air tank at 2,350 psi. What is this pressure expressed in units of atmospheres?
	A) 160. atm B) 2.35 atm C) 3.45 × 104 atm D) 3.09 atm
	Ans: A Difficulty: Easy

6.	A scuba diver typically begins a dive with a compressed air tank at 2,350 psi. What is this pressure expressed in units of Pa?
	A) 0.0232 Pa B) 3.09 Pa C) 2.38 × 108 Pa D) 1.62 × 107 Pa
	Ans: D Difficulty: Medium

7.	A birthday balloon contains helium at a pressure of 815 torr. What is this pressure expressed in units of mm Hg?
	A) 815 mm Hg B) 1.07 mm Hg C) 0.815 mm Hg D) 6.19 × 105 mm Hg
	Ans: A Difficulty: Easy

8.	A sample of neon gas has a volume of 5.0 mL at a pressure of 1.50 atm. What is the pressure exerted by the gas if the volume is increased to 30.0 mL, at constant temperature?
	A) 0.25 atm B) 9.0 atm C) 1.5 atm D) 0.21 atm
	Ans: A Difficulty: Medium

9.	Which gas law describes the relationship between the volume and temperature of a sample of gas at constant pressure?
	A) Boyle’s law B) Avogadro’s law C) Charles’s law D) Gay-Lussac’s law
	Ans: C Difficulty: Easy

10.	A balloon that contains 0.500 L of helium at 25 °C is cooled to 11 °C, at a constant pressure. What volume does the balloon now occupy?
	A) 0.22 L B) 1.1 L C) 0.477 L D) 0.525 L
	Ans: C Difficulty: Medium

11.	A 54.2 L sample of gas at 115 K is heated to 345 K, at constant pressure. What volume does the gas now occupy?
	A) 2.15 × 106 L B) 163 L C) 18.1 L D) 732 L
	Ans: B Difficulty: Medium

12.	The temperature of a 0.750-L gas sample at 25 °C and 2.00 atm is changed to 250 °C. What is the final pressure of the system, at constant volume?
	A) 20.0 atm B) 0.200 atm C) 3.51 atm D) 0.427 atm
	Ans: C Difficulty: Medium

13.	A weather balloon contains 233 L of helium at 22 °C and 760. mm Hg. What is the volume of the balloon when it ascends to an altitude where the temperature is –54 °C and 511 mm Hg?
	A) 2.24 × 107 L B) 467 L C) 116 L D) 257 L
	Ans: D Difficulty: Difficult

14.	A gas cylinder containing 6.38 mol of neon has a pressure of 491 mm Hg at 295 K. If 3.22 mol of helium is added to this cylinder, at constant temperature and volume, what will be the pressure in the cylinder?
	A) 9.73 mm Hg B) 739 mm Hg C) 1460 mm Hg D) 248 mm Hg
	Ans: B Difficulty: Difficult

15.	How many moles are contained in 5.33 L of O2 at standard temperature and pressure?
	A) 5.33 mol of O2 B) 22.4 mol of O2 C) 0.238 mol of O2 D) 1.00 mol of O2
	Ans: C Difficulty: Easy

16.	Which cylinder at STP will contain the greatest number of gas particles?
	A)	A 5.0-L cylinder of neon
	B)	A 5.0-L cylinder of helium
	C)	A 5.0-L cylinder of nitrogen
	D)	A 5.0-L cylinder of hydrogen
	E)	All of the cylinders above contain the same number of gas particles.
	Ans: E Difficulty: Easy

17.	Which cylinder at STP will contain the greatest mass of gas particles?
	A)	A 5.0-L cylinder of neon
	B)	A 5.0-L cylinder of helium
	C)	A 5.0-L cylinder of nitrogen
	D)	A 5.0-L cylinder of hydrogen
	E)	All of the cylinders above contain the same mass of gas particles.
	Ans: C Difficulty: Medium

18.	Consider the balanced reaction: Zn(s) + 2 HCl(aq) ® ZnCl2(aq) + H2(g). What volume of H2(g) at STP can be generated when 134 g of zinc reacts?
	A) 2.05 L B) 45.9 L C) 5.98 L D) 3.00 × 103 L
	Ans: B Difficulty: Difficult

19.	How many moles of gas are contained in a scuba diver’s 12.6-L tank filled with 3422 psi of air at 25 °C?
	A) 1760 moles B) 2.10 × 104 moles C) 120. moles D) 1430 moles
	Ans: C Difficulty: Difficult

20.	A sample of gas contains four gases with the following partial pressures: He (113 mm Hg), Ne (184 mm Hg), Ar (35 mm Hg), and Xe (445 mm Hg). What is the total pressure of the sample?
	A) 777 mm Hg B) 760. mm Hg C) 445 mm Hg D) 332 mm Hg
	Ans: A Difficulty: Easy

21.	A sample of gas contains four gases (He, Ne, Ar, and Xe) with the following partial pressures: He (43 mm Hg), Ar (835 mm Hg), and Xe (111 mm Hg). If the total pressure in the container is 1355 mm Hg, what is the partial pressure of Ne in the sample?
	A) 989 mm Hg B) 760. mm Hg C) 366 mm Hg D) 323 mm Hg
	Ans: C Difficulty: Easy

22.	What is the volume of 62.3 g of nitrogen gas at STP?
	A) 22.4 L B) 49.8 L C) 99.6 L D) 2.78 L
	Ans: B Difficulty: Medium

23.	What volume does 7.50 × 1020 molecules of O2 occupy at STP?
	A) 22.4 L B) 1.68 × 1022 L C) 0.0279 L D) 2.79 L
	Ans: C Difficulty: Medium

24.	Air pressure at the bottom of Death Valley, at 282 ft below sea level, is 776 mm Hg. What are the partial pressures of O2 and N2, which compose 21% and 78% of the atmosphere, respectively?
	A)	210 mm Hg O2 and 780 mm Hg N2	C)	160 mm Hg O2 and 610 mm Hg N2
	B)	160 mm Hg O2 and 590 mm Hg N2	D)	163 mm Hg O2 and 613 mm Hg N2
	Ans: C Difficulty: Medium

25.	Which gas sample contains the largest number of moles?
	A)	4.0 L of O2 at 273 K and 530 mm Hg
	B)	4.5 L of N2 at 298 K and 610 mm Hg
	C)	3.8 L of He at 250 K and 880 mm Hg
	D)	5.0 L Ar at 300 K and 710 mm Hg
	Ans: C Difficulty: Difficult

26.	Atmospheric pressure in interstellar space is approximately 1 × 10–17 torr at a temperature of –173 °C. How many gas molecules are present in 25,000 L of interstellar space (about the volume of a bedroom)?
	A)	2 × 107 molecules	C)	4 × 10–17 molecules
	B)	2 × 1010 molecules	D)	3 × 10–14 molecules
	Ans: A Difficulty: Difficult

27.	An aerosol spray can with a volume of 350 mL registers a pressure of 4.5 atm at room temperature. What happens to the pressure of the gas inside the can if the can is stored outside during the winter months?
	A)	The pressure of the gas will remain at 4.5 atm.
	B)	The pressure of the gas will be greater than 4.5 atm.
	C)	The pressure of the gas will be less than 4.5 atm.
	D)	It is impossible to predict without knowing the amount of gas present inside the can.
	Ans: C Difficulty: Medium

28.	At rest, the volume of air in the lungs is 615 mL at 760 mm Hg. When the volume of the lungs expands during inhalation, what happens to the pressure inside the lungs?
	A)	The pressure inside the lungs decreases, which draws air into the lungs.
	B)	The pressure inside the lungs increases, which forces air inside the lungs.
	C)	The pressure inside the lungs remains constant, and air readily flows into the lungs.
	D)	The pressure inside the lungs cannot be determined if the weight of the person is unknown.
	Ans: A Difficulty: Medium

29.	Hydrogen peroxide decomposes to give water and oxygen gas according to the equation below. If 3.0 moles of hydrogen peroxide decompose, what volume of oxygen gas is produced at a pressure of 1.0 atm and a temperature of 23 °C? 2 H2O2(l) ® 2 H2O(l) + O2(g)
	A) 1.9 L of O2 B) 2.8 L of O2 C) 24 L of O2 D) 36 L of O2
	Ans: D Difficulty: Difficult

30.	Which statement is not true?
	A)	Chlorofluorocarbons (CFCs) are simple compounds containing carbon, chlorine, and fluorine.
	B)	CF2Cl2 is a chlorofluorocarbon.
	C)	One of the possible long-term effects of a decrease in ozone concentration in the stratosphere is an increase in the incidence of eye cataracts and a reduced immune response.
	D)	CFCs are currently used as refrigerants, solvents, and aerosol propellants in the United States.
	E)	CFCs have been shown to destroy ozone in the upper atmosphere.
	Ans: D Difficulty: Medium

31.	CO2 is a greenhouse gas.
	A) True B) False
	Ans: A Difficulty: Easy

32.	The products of the complete combustion of a hydrocarbon fuel are CO + H2O.
	A) True B) False
	Ans: B Difficulty: Easy

33.	The combustion of alkanes and other hydrocarbons obtained from fossil fuels adds a tremendous amount of CO2 to the atmosphere each year.
	A) True B) False
	Ans: A Difficulty: Easy

34.	The size of gas particles is large compared to the space between the particles.
	A) True B) False
	Ans: B Difficulty: Easy

35.	When a sample of gas is compressed from 6.0 L to 2.0 L at a constant temperature, the pressure of the gas doubles.
	A) True B) False
	Ans: B Difficulty: Easy

36.	When a sample of gas is heated from 80. °C to 160. °C at a constant pressure, the volume of the gas doubles.
	A) True B) False
	Ans: B Difficulty: Medium

37.	STP is defined as a pressure of exactly one atmosphere and a temperature of 25 °C.
	A) True B) False
	Ans: B Difficulty: Medium

38.	If 10.3 g of Ne and 10.3 g of N2 are put into a 7.0 L container, the partial pressure of N2 will be less than the partial pressure of Ne in the container.
	A) True B) False
	Ans: A Difficulty: Difficult

39.	When the pressure and temperature are held constant, the volume of a gas is inversely proportional to the number of moles present.
	A) True B) False
	Ans: B Difficulty: Difficult

40.	If the lungs of a child hold 0.11 mol of air in a volume of 2.8 L, then the lungs of an average female adult, with a volume is 4.6 L, can be expected to hold 0.18 mol of air.
	A) True B) False
	Ans: A Difficulty: Medium

41.	A gas cylinder containing 3.88 mol of helium has a pressure of 549 mm Hg at 298 K. If 1.22 mol of neon is added to this cylinder, at constant temperature and volume, the pressure will rise to 1750 mm Hg.
	A) True B) False
	Ans: B Difficulty: Medium

42.	The value of the universal gas constant, R, changes as a function of temperature.
	A) True B) False
	Ans: B Difficulty: Easy

43.	The value of the universal gas constant, R, depends on its units.
	A) True B) False
	Ans: A Difficulty: Easy

44.	When the volume of a sample of gas is doubled and the Kelvin temperature is cut in half, the pressure of a sample remains constant.
	A) True B) False
	Ans: B Difficulty: Difficult

45.	When the volume of a sample of gas is doubled and the Kelvin temperature is doubled, the pressure of a sample remains constant.
	A) True B) False
	Ans: A Difficulty: Difficult

46.	The density of a sample of gas increases if the temperature is increased but the pressure is held constant.
	A) True B) False
	Ans: B Difficulty: Difficult

47.	A sample of 22.4 g of O2 will occupy less than 22.4 L at STP.
	A) True B) False
	Ans: A Difficulty: Easy

48.	The pressure of a gas is proportional to its Kelvin temperature, so increasing the temperature increases the pressure at constant volume.
	A) True B) False
	Ans: A Difficulty: Easy

49.	When 88.4 g of hydrogen gas is put in a 25.8-L container at 300. K the pressure will be 83.7 atm.
	A) True B) False
	Ans: B Difficulty: Difficult

50.	Charles’s law can be used to explain the dangerous condition for scuba divers called “the bends”, which is caused by the formation of nitrogen gas bubbles in the bloodstream.
	A) True B) False
	Ans: B Difficulty: Medium

51.	CHCl2F is classified as a CFC.
	A) True B) False
	Ans: B Difficulty: Medium

52.	The kinetic energy of gas particles _____ with increasing temperature.
	Ans:	increases
	Difficulty: Easy

53.	_____’s law relates the pressure and temperature of a gas sample at constant volume.
	Ans:	Gay–Lussac
	Difficulty: Medium

Chapter 7: Solutions

1.	Which is not an example of a solution?
	A) A dental filling B) Chicken noodle soup C) Gasoline D) Tap water
	Ans: B Difficulty: Easy

2.	Which substance is a nonelectrolyte?
	A) NaCl B) (NH4)2SO4 C) H2O2 D) KOH
	Ans: C Difficulty: Easy

3.	Which substance is a colloid?
	A)	Mayonnaise	C)	A dental filling
	B)	Mint chocolate chip ice cream	D)	Gasoline
	Ans: A Difficulty: Easy

4.	Nonpolar compounds are soluble in
	A)	Ionic compounds.	C)	Polar solvents.
	B)	Electrolytes.	D)	Nonpolar solvents.
	Ans: D Difficulty: Easy

5.	The attraction of an ion with a dipole in a molecule is called
	A)	A dipole-dipole interaction.	D)	Van der Waals forces.
	B)	London dispersion forces.	E)	Hydrogen bonding.
	C)	An ion–dipole interaction.
	Ans: C Difficulty: Easy

6.	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.
	Ans: A Difficulty: Medium

7.	Which ionic compound is not soluble in water?
	A) NaCl B) AgCl C) (NH4)2SO4 D) Ca(CH3CO2)2
	Ans: B Difficulty: Medium

8.	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 above is soluble in water.
	Ans: D Difficulty: Medium

9.	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.
	Ans: A Difficulty: Easy

10.	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	C)	94.3% (w/v) NaCl
	B)	5.72% (w/v) NaCl	D)	0.0572% (w/v) NaCl
	Ans: B Difficulty: Medium

11.	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	D)	0.295% (v/v) ethanol
	B)	0.418% (v/v) ethanol	E)	70.5% (v/v) ethanol
	C)	29.5% (v/v) ethanol
	Ans: C Difficulty: Medium

12.	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	D)	0.016 g NaCl
	B)	529 g NaCl	E)	1.6 g NaCl
	C)	5.3 g NaCl
	Ans: C Difficulty: Medium

13.	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	C)	6.70 mL ethanol
	B)	0.840 mL ethanol	D)	14.9 mL ethanol
	Ans: A Difficulty: Medium

14.	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	C)	140 mL of saline solution
	B)	840 mL of saline solution	D)	7.1 mL of saline solution
	Ans: B Difficulty: Medium

15.	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	D)	4.0 × 103 ppm Ca2+ ions
	B)	4.0 ppm Ca2+ ions	E)	420 ppm Ca2+ ions
	C)	0.42 ppm Ca2+ ions
	Ans: C Difficulty: Medium

16.	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 above contain the same number of moles of sucrose.
	Ans: A Difficulty: Difficult

17.	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
	Ans: C Difficulty: Easy

18.	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
	Ans: C Difficulty: Medium

19.	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
	Ans: D Difficulty: Medium

20.	How many grams of glucose (C6H12O6) are contained in 555 mL of a 1.77 M glucose solution?
	A)	0.982 g C6H12O6	C)	177 g C6H12O6
	B)	0.555 g C6H12O6	D)	0.177 g C6H12O6
	Ans: C Difficulty: Difficult

21.	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
	Ans: C Difficulty: Difficult

22.	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 above have the same mass of solute.
	Ans: C Difficulty: Medium

23.	Which compound will be the least soluble in water?
	A)
	B)
	C)
	D)
	Ans: A Difficulty: Difficult

24.	Which compound will be the most soluble in water?
	A)
	B)
	C)
	D)
	Ans: C Difficulty: Difficult

25.	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
	Ans: B Difficulty: Medium

26.	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
	Ans: A Difficulty: Difficult

27.	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	D)	8.6 mL HCl solution
	B)	240 mL HCl solution	E)	230 mL HCl solution
	C)	7,500 mL HCl solution
	Ans: A Difficulty: Medium

28.	A hypotonic solution has _____ osmotic pressure than/as body fluids.
	A) A higher B) A lower C) The same
	Ans: B Difficulty: Easy

29.	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.
	Ans: B Difficulty: Difficult

30.	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
	Ans: D Difficulty: Difficult

31.	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
	Ans: B Difficulty: Difficult

32.	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
	Ans: B Difficulty: Difficult

33.	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)
	Ans: A Difficulty: Medium

34.	The solubility of a substance is best described by which of the following?
	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
	Ans: C Difficulty: Easy

35.	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.
	Ans: A Difficulty: Easy

36.	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.
	Ans: B Difficulty: Easy

37.	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.
	Ans: A Difficulty: Medium

38.	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
	Ans: B Difficulty: Medium

39.	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	C)	0.967 L of a 1.50 M NaOH solution
	B)	1.09 L of a 1.50 M NaOH solution	D)	967 mL of a 1.50 M NaOH solution
	Ans: A Difficulty: Difficult

40.	Any mixture of two or more components is a solution.
	A) True B) False
	Ans: B Difficulty: Easy

41.	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.
	A) True B) False
	Ans: A Difficulty: Easy

42.	In solution formation, solvation always releases more energy than that required to separate particles, so the overall process is always exothermic.
	A) True B) False
	Ans: B Difficulty: Medium

43.	Methanol (CH3OH) is soluble in water.
	A) True B) False
	Ans: A Difficulty: Easy

44.	Heptane (C7H16) is soluble in water.
	A) True B) False
	Ans: B Difficulty: Easy

45.	For most ionic and molecular solids, solubility generally increases as temperature increases.
	A) True B) False
	Ans: A Difficulty: Easy

46.	The solubility of gases increases with increasing temperature.
	A) True B) False
	Ans: B Difficulty: Medium

47.	The greater the number of dissolved particles in a solution, the lower the solution’s osmotic pressure.
	A) True B) False
	Ans: B Difficulty: Easy

48.	The solubility of helium gas in water is greater at 25 °C than at 50 °C.
	A) True B) False
	Ans: A Difficulty: Medium

49.	The ionic compound (NH4)2SO4 is soluble in water.
	A) True B) False
	Ans: A Difficulty: Easy

50.	The ionic compound CaCO3 is soluble in water.
	A) True B) False
	Ans: B Difficulty: Medium

51.	Ethylene glycol is more soluble in water than propane.
	A) True B) False
	Ans: A Difficulty: Easy

52.	Pure water has an osmotic pressure of 1 atm.
	A) True B) False
	Ans: B Difficulty: Easy

53.	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.
	A) True B) False
	Ans: B Difficulty: Medium

54.	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.
	A) True B) False
	Ans: A Difficulty: Medium

55.	Dialysis is a process that involves the selective passage of water, protein molecules, and ions across a semipermeable membrane.
	A) True B) False
	Ans: B Difficulty: Medium

56.	Adding 356 g of NaCl to a flask that contains 1.00 L of water makes a 6.10 M NaCl solution.
	A) True B) False
	Ans: B Difficulty: Medium

57.	The concentration unit of weight/volume percent concentration, (w/v)%, is the number of grams of solute dissolved in 100 mL of solution.
	A) True B) False
	Ans: A Difficulty: Medium

58.	Nonpolar compounds are soluble in nonpolar solvents and insoluble in polar solvents.
	A) True B) False
	Ans: A Difficulty: Easy

59.	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.
	A) True B) False
	Ans: A Difficulty: Medium

60.	A solution containing the maximum number of grams of solute that can dissolve in the solvent is said to be supersaturated.
	A) True B) False
	Ans: B Difficulty: Easy

61.	Liquid solutions are always transparent and colorless.
	A) True B) False
	Ans: B Difficulty: Medium

62.	Sodium chloride is soluble in nonpolar solvents such as octane (C8H18).
	A) True B) False
	Ans: B Difficulty: Medium

63.	The solubility of Ba(NO3)2 in water is lower at 25 °C than at 50 °C.
	A) True B) False
	Ans: A Difficulty: Medium

64.	A solution can be made less concentrated by adding additional solvent.
	A) True B) False
	Ans: A Difficulty: Easy

65.	An aqueous solution with the label 0.25 M sucrose contains 0.25 grams of sucrose in every 1 L of solution.
	A) True B) False
	Ans: B Difficulty: Medium

66.	Dilution is the addition of solute to decrease the concentration of solvent.
	A) True B) False
	Ans: B Difficulty: Easy

67.	Colligative properties are properties of a solution that depend on the concentration of the solute particles but not their identity.
	A) True B) False
	Ans: A Difficulty: Easy

68.	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.
	A) True B) False
	Ans: B Difficulty: Medium

69.	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.
	A) True B) False
	Ans: B Difficulty: Easy

70.	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 _____.
	Ans:	solute, solvent
	Difficulty: Easy

71.	A solution with water as the solvent is called a(n) _____ solution.
	Ans:	aqueous
	Difficulty: Easy

72.	The process of solvent molecules surrounding solute particles is called _____.
	Ans:	solvation
	Difficulty: Medium

73.	_____ 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.
	Ans:	Osmosis
	Difficulty: Easy

74.	Two solutions with the same osmotic pressure are said to be _____.
	Ans:	isotonic
	Difficulty: Medium

75.	Two conversion factors that can be generated for the concentration 55 ppm Pb2+ are _____ and _____.
	Ans:	and
	Difficulty: Medium

76.	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.
	Ans:	51
	Difficulty: Difficult

77.	In order for a solution to conduct electricity it must contain _____.
	Ans:	ions
	Difficulty: Easy

78.	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 _____.
	Ans:	water
	Difficulty: Easy

79.	Dilution involves adding additional _____ to a solution in order to decrease the concentration of the _____.
	Ans:	solvent, solute
	Difficulty: Medium