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Chemisty Ch. 11 & 12

Chemisty Ch. 11

Question	Answer
1) Identify the characteristics of a liquid.	B) indefinite shape, but definite volume
2) Which one of the following has a low density?	A) gas
3) Which one of the following has a definite shape and volume?	C) solid
4) Give the change in condition to go from a liquid to a gas.	A) increase heat or reduce pressure
5) The forces between polar molecules is known as __________.	C) dipole-dipole forces
6) Which of the following statements is TRUE?	B) The potential energy of molecules decrease as they get closer to one another.
7) What is the strongest type of intermolecular force present in H2?	C) dispersion
8) What is the strongest type of intermolecular force present in CHF3?	D) dipole-dipole
9) What is the strongest type of intermolecular force present in NH2CH3?	C) hydrogen bonding
10) What type of intermolecular force causes the dissolution of NaCl in water?	C) ion-dipole force
11) Choose the molecule or compound that exhibits dispersion forces as its strongest intermolecular force.	A) Cl2
12) Choose the molecule or compound that exhibits dipole-dipole forces as its strongest intermolecular force.	B) SO2
13) Choose the compound that exhibits hydrogen bonding as its strongest intermolecular force.	C) CH3OH
14) Place the following compounds in order of increasing strength of intermolecular forces.	D) F2 < CO2 < NH2CH3
15) Place the following compounds in order of increasing strength of intermolecular forces. CH4 CH3CH2CH3 CH3CH3	E) CH4 < CH3CH3 < CH3CH2CH3
16) Place the following compounds in order of decreasing strength of intermolecular forces. HF O2 CO2	A) HF > CO2 > O2
17) Place the following compounds in order of decreasing strength of intermolecular forces.	B) I > III > II
18) Which has the smallest dipole-dipole forces?	C) O2
19) Which is expected to have the largest dispersion forces?	B) C12H26
20) Identify the compound that does not have dipole-dipole forces as its strongest force.	E) CO2
21) Which of the following compounds exhibits hydrogen bonding?	D) NH3
22) Identify the compound that does not have hydrogen bonding.	A) (CH3)3N
23) Choose the pair of substances that are most likely to form a homogeneous solution.	E) NH3 and CH3OH
24) Choose the pair of substances that are most likely to form a homogeneous solution.	A) C6H14 and C10H20
25) Choose the pair of substances that are most likely to form a homogeneous solution.	B) NF3 and SO2
26) In liquid propanol, CH3CH2CH2OH which intermolecular forces are present?	A) Dispersion, hydrogen bonding and dipole-dipole forces are present.
27) Which of the following compounds exhibits only dispersion and dipole-dipole intermolecular interactions?	B) HI
28) The normal boiling point for H2Se is higher than the normal boiling point for H2S . This can be explained by	B) larger dispersion forces for H2Se .
29) In a liquid, the energy required to increase the surface of the area by a unit amount is called __________.	B) surface tension
30) Choose the substance with the highest surface tension.	A) HOCH2CH2OH
31) Choose the substance with the lowest surface tension.	B) CH3CH2CH2CH3
32) Choose the substance with the highest viscosity.	C) HOCH2CH2CH2CH2OH
33) Choose the substance with the lowest viscosity.	D) ClCH2CH2Cl
34) Choose the substance with the highest viscosity.	D) BeCl2
35) Identify the substance with the highest viscosity.	C) corn syrup
36) Identify the term used to describe the ability of a liquid to flow against gravity up a narrow tube.	A) capillary action
37) Which of the following statements is TRUE?	A) Vapor pressure increases with temperature.
38) Which of the following statements is FALSE?	D) Molecules with hydrogen bonding are more volatile than compounds with dipole-dipole forces.
39) Which substance below has the strongest intermolecular forces?	A) A2X, ΔHvap= 39.6 kJ/mol
40) Define boiling.	A) A liquid becomes a gas.
41) Give the term for the temperature at which the gas and liquid phases form a supercritical fluid.	D) critical temperature
42) Choose the substance with the highest vapor pressure at a given temperature.	D) BF3
43) Choose the substance with the lowest vapor pressure at a given temperature.	B) BeCl2
44) Place the following substances in order of increasing boiling point. Ne Cl2 O2	E) Ne < O2 < Cl2
45) Place the following substances in order of increasing boiling point. CH3CH2OH Ar CH3OCH3	A) Ar < CH3OCH3 < CH3CH2OH
46) Choose the substance with the highest boiling point.	B) KI
47) Choose the substance with the lowest boiling point.	C) F2
48) Which of the following substances would you predict to have the highest ΔHvap?	C) HOCH2CH2OH
49) Which of the following substances would you predict to have the highest ΔHvap?	D) Br2
50) How much energy is required to vaporize 48.7 g of dichloromethane (CH2Cl2) at its boiling point, if its ΔHvap is 31.6 kJ/mol?	E) 18.1 kJ
51) How much energy is required to vaporize 98.6 g of ethanol (C2H5OH) at its boiling point, if its ΔHvap is 40.5 kJ/mol?	A) 86.7 kJ
52) How much energy is required to vaporize 158 g of butane (C4H10) at its boiling point, if its ΔHvap is 24.3 kJ/mol?	B) 66.1 kJ
53) Based on the figure above, the boiling point of diethyl ether under an external pressure of 1.32 atm is __________°C.	D) 40
54) Based on the figure above, the boiling point of ethyl alcohol under an external pressure of 0.0724 atm is __________°C.	E) 20
55) Based on the figure above, the boiling point of water under an external pressure of 0.316 atm is __________°C.	A) 70
56) Place the following substances in order of increasing vapor pressure at a given temperature. SF6 SiH4 SF4	D) SF4 < SF6 < SiH4
57) Place the following substances in order of decreasing vapor pressure at a given temperature. PF5 BrF3 CF4	E) CF4 > PF5 > BrF3
58) Place the following substances in order of increasing vapor pressure at a given temperature. NF3 NH3 BCl3	A) NH3 < NF3 < BCl3
59) Place the following substances in order of decreasing vapor pressure at a given temperature. BeF2 CH3OH OF2	C) OF2 > CH3OH > BeF2
60) Place the following substances in order of decreasing boiling point. H2O N2 CO	C) H2O > CO > N2
61) Place the following substances in order of decreasing boiling point. N2 O2 H2	D) O2 > N2 > H2
62) Place the following substances in order of decreasing boiling point. He Ar H2	D) Ar > He > H2
63) Which of the following compounds has the highest boiling point?	A) H2O
64) Determine ΔHvap for a compound that has a measured vapor pressure of 24.3 torr at 273 K and 135 torr at 325 K.	C) 24 kJ/mol
65) Determine the normal boiling point of a substance whose vapor pressure is 55.1 mm Hg at 35°C and has a ΔHvap of 32 .1 kJ/mol.	D) 390. K
66) Determine the vapor pressure (in mm Hg) of a substance at 29°C, whose normal boiling point is 76°C and has a ΔHvap of 38.7 kJ/mol.	E) 96 mm Hg
67) Determine the vapor pressure (in torr) of a substance at 36°C, whose normal boiling point is 84°C and has a ΔHvap of 22.1 kJ/mol.	A) 239 torr
68) Define deposition.	C) A gas becomes a solid.
69) Define sublimation.	A) the phase transition from solid to gas
70) Define freezing.	E) the phase transition from liquid to solid
71) At atmospheric pressure, dry ice __________.	C) sublimes
72) The melting point of water is __________.	A) 0°C
73) The freezing point of water is __________.	A) 0°C
74) The boiling point of water is __________.	D) 100°C
75) The heat of vaporization of water at 100°C is 40.66 kJ/mol. Calculate the quantity of heat that is absorbed/released when 9.00 g of steam condenses to liquid water at 100°C.	B) 20.3 kJ of heat are released.
76) Calculate the total quantity of heat required to convert 25.0 g of liquid CCl4(l) from 35.0°C to gaseous CCl4 at 76.8°C (the normal boiling point for CCl4). The specific heat of CCl4(l) is 0.857 J/(g · °C), its heat of fusion is 3.27 kJ/mol, and its	C) 5.74 kJ
77) The enthalpy change for converting 1.00 mol of ice at -50.0°C to water at 70.0°C is __________ kJ. The specific heats of ice, water, and steam are 2.09 J/gK, 4.18 J/gK, and 1.84 J/gK, respectively. For H2O, ΔHfus = 6.01 kJ/mol, and ΔHvap = 40.67 kJ	C) 13.16
78) The enthalpy change for converting 10.0 g of ice at -25.0°C to water at 80.0°C is __________ kJ. The specific heats of ice, water, and steam are 2.09 J/gK, 4.18 J/gK, and 1.84 J/gK, respectively. For H2O, ΔHfus = 6.01 kJ/mol, and ΔHvap = 40.67 kJ/mo	D) 7.21
79) The fluorocarbon C2Cl3F3 has a normal boiling point of 47.6°C. The specific heats of C2Cl3F3(l) and C2Cl3F3 (g) are 0.91 J/gK and 0.67 J/gK, respectively. The heat of vaporization of the compound is 27.49 kJ/mol. The heat required to convert 50.0 g of	E) 10.36
80) Ethanol (C2H5OH) melts at -114°C. The enthalpy of fusion is 5.02 kJ/mol. The specific heats of solid and liquid ethanol are 0.97 J/gK and 2.3 J/gK, respectively. How much heat (kJ) is needed to convert 25.0 g of solid ethanol at -135°C to liquid ethan	C) 6.91 kJ
81) Ethyl chloride, C2H5Cl, is used as a local anesthetic. It works by cooling tissue as it vaporizes; its heat of vaporization is 26.4 kJ/mol. How much heat could be removed by 20.0 g of ethyl chloride?	A) 8.18 kJ
enthalpy of vaporization of water is 40.67 kJ/mol, the enthalpy of fusion for water is 6.01 kJ/mol, the molar heat capacity of liquid water is 75.4 J/(mol ∙ °C), and the molar heat capacity of ice is 36.4 J/(mol ∙ °C).	C) 319 kJ
83) How much energy is required to heat 36.0 g H2O from a liquid at 65°C to a gas at 115°C? The following physical data may be useful.	B) 87.7 kJ
84) How much energy must be removed from a 125 g sample of benzene (molar mass= 78.11 g/mol) at 425.0 K to liquify the sample and lower the temperature to 335.0 K? The following physical data may be useful.	C) 67.7 kJ
85) How much energy is required to heat 87.1 g acetone (molar mass=58.08 g/mol) from a solid at -154.0°C to a liquid at -42.0°C? The following physical data may be useful.	D) 29.4 kJ
86) How much energy must be removed from a 94.4 g sample of benzene (molar mass= 78.11 g/mol) at 322.0 K to solidify the sample and lower the temperature to 205.0 K? The following physical data may be useful.	E) 29.4 kJ
87) Identify triple point.	C) The temperature and pressure where liquid, solid, and gas are equally stable and are in equilibrium.
88) Assign the appropriate labels to the phase diagram shown below.	B) A = gas, B = solid, C = liquid, D = triple point
89) Consider the phase diagram shown. Choose the statement below that is TRUE.	C) The solid phase of this substance is higher in density than the liquid phase.
90) Consider the phase diagram below. If the dashed line at 1 atm of pressure is followed from 100 to 500°C, what phase changes will occur (in order of increasing temperature)?	D) fusion, followed by vaporization
91) Why is water an extraordinary substance?	E) All of the above.
92) Identify the compound with the highest boiling point.	E) H2O
93) Give the coordination number for a body-centered cubic cell.	C) 8
94) Determine the radius of an Al atom (in pm) if the density of aluminum is 2.71 g/cm3. Aluminum crystallizes in a face centered cubic structure with an edge length of 2 r.	A) 143 pm
95) A metal crystallizes in a face centered cubic structure and has a density of 11.9 g/cm3. If the radius of the metal atom is 138 pm, what is the identity of the metal?	B) Pd
96) Vanadium crystallizes in a body centered cubic structure and has an atomic radius of 131 pm. Determine the density of vanadium, if the edge length of a bcc structure is 4r/ .	C) 6.11 g/cm3
97) Which of the following is considered a molecular solid?	C) I2
98) Which of the following is considered an ionic solid?	A) (NH4)2CO3
99) Which of the following is considered an atomic solid?	D) Nb
100) Which of the following is considered a nonbonding atomic solid?	A) Ne
101) Identify the type of solid for AgCl.	B) ionic solid
102) Identify the type of solid for ice.	D) molecular solid
103) Identify the type of solid for gold.	A) metallic atomic solid
104) Identify the type of solid for diamond.	E) networking atomic solid
105) Identify the type of solid for argon.	C) nonbonding atomic solid
106) Which of the following substances should have the highest melting point?	E) MgO
107) Which of the following substances should have the highest melting point?	A) Fe
1) What is the edge length of a face-centered cubic unit cell made up of atoms having a radius of 128 pm?	B) 362 pm
2) Nickel has a face-centered cubic structure and has a density of 8.90 g/cm3. What is its atomic radius?	A) 125 pm
3) Gold crystallizes in a face-centered cubic structure. What is the edge length of the unit cell if the atomic radius of gold is 144 pm?	D) 407 pm
4) Cesium has a radius of 272 pm and crystallizes in a body-centered cubic structure. What is the edge length of the unit cell?	D) 628 pm
5) Lithium crystallizes in a body-centered cubic structure. What is the coordination number of each atom?	C) 8
6) Na Cl crystallizes in a cubic unit cell with Cl- ions on each corner and each face. How many Na+ and Cl- ions are in each unit cell of Na Cl?	C) 4 Na+ ions and 4 Cl- ions
7) How many H- ions are around each Na+ ion in NaH, which has a cubic unit cell with H- ions on each corner and each face?	C) 6
8) Which of the following forms a molecular solid?	B) C6H4Cl2
9) Which of the following forms an ionic solid?	C) Rb I
10) Which type of bonding does Sr form upon solidification?	C) metallic
1) Choose the statement below that is TRUE.	A) A solution will form between two substances if the solute-solvent interactions are of comparable strength to the solute-solute and solvent-solvent interactions.
2) Give the major force between ethanol and water.	C) hydrogen bonding
3) Give the major force between acetone and chloroform.	A) dipole-dipole
4) Which of the following compounds will be most soluble in pentane (C5H12)?	B) benzene (C6H6)
5) Which of the following compounds will be most soluble in ethanol (CH3CH2OH)?	C) ethylene glycol (HOCH2CH2OH)
6) Which of the following compounds is most soluble in hexane (CH3CH2CH2CH2CH2CH2CH3)?	E) 1-pentanol
7) Choose the situation below that would result in a ΔHsolution near 0.	D) When \|ΔHsolute\| is close to \|ΔHhydration\|
8) Choose the situation below that would result in an exothermic ΔHsolution.	C) When \|ΔHsolute\| < \|ΔHhydration\|
9) Choose the situation below that would result in an endothermic ΔHsolution.	A) When \|ΔHsolute\| > \|ΔHhydration\|
10) Which of the following ions should have the most exothermic ΔHhydration?	C) Al3⁺
11) Determine DHsolute for KBr if the DHsolution (KBr) = +19.9 kJ/mol and the ΔHhydration(KBr)=-670. kJ/mol.	C) +690 kJ/mol
12) Dynamic equilibrium can be defined as	A) rate of dissolution = rate of deposition
13) Dissolving is	C) rate of dissolution > rate of deposition
14) A solution containing less than the equilibrium amount is called __________.	A) an unsaturated solution
15) A solution is formed at room temperature by vigorously dissolving enough of the solid solute so that some solid remains at the bottom of the solution. Which statement below is TRUE?	C) The solution is considered saturated.
16) Which of the following statements is generally TRUE?	D) The solubility of a solid is highly dependent on temperature.
17) A solid can be purified through what technique?	A) recrystallization
18) Identify the compound whose solubility is least affected by temperature.	E) NaCl
19) Identify the compound whose solubility decreases with increasing temperature.	A) Na2SO4
20) Which of the following statements is TRUE?	C) The solubility of a gas is highly dependent on both pressure and temperature.
21) Which of the following statements is TRUE?	B) In general, the solubility of a gas in water decreases with increasing temperature.
22) Identify the gas that is dissolved in carbonated sodas.	A) carbon dioxide
23) Which of the following should have the largest Henry's law constant (kH) in water?	B) CO
24) Determine the solubility of N2 in water exposed to air at 25°C if the atmospheric pressure is 1.2 atm. Assume that the mole fraction of nitrogen is 0.78 in air and the Henry's law constant for nitrogen in water at this temperature is 6.1 × 10-4 M/atm	C) 5.7 × 10-4 M
25) Determine the solubility of CO2 in soda water at 25°C if the pressure of CO2 is 5.2 atm. The Henry's law constant for carbon dioxide in water at this temperature is 3.4 × 10-2 M/atm.	D) 0.18 M
26) Determine the partial pressure of oxygen necessary to form an aqueous solution that is 4.1 × 10-4 M O2 at 25°C. The Henry's law constant for oxygen in water at 25°C is 1.3 × 10-3 M/atm.	E) 0.32 atm
27) Determine the Henry's law constant for ammonia in water at 25°C if an ammonia pressure of 0.022 atm produces a solution with a concentration of 1.3 M.	A) 59 M/atm
28) Calculate the mass of oxygen (in mg) dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air. Assume the mole fraction of oxygen in air to be 0.21 and the Henry's law constant for oxygen in water at this temperature to be 1.3 ×	A) 49.4 mg
29) Give the term for the amount of solute in moles per liter of solution.	B) molarity
30) Give the term for the amount of solute in moles per kilogram of solvent.	A) molality
31) Parts per billion requires a multiplication factor of ________.	E) 10^9
32) Which of the following concentration units are temperature dependent?	D) molarity
33) Identify the colligative property.	E) all of the above
34) Calculate the molality of a solution formed by dissolving 27.8 g of LiI in 500.0 mL of water.	E) 0.415 m
35) What mass (in g) of NH3 must be dissolved in 475 g of methanol to make a 0.250 m solution?	A) 2.02 g
36) How many moles of KF are contained in 347 g of water in a 0.175 m KF solution?	C) 6.07 × 10-2 mol KF
37) How many moles of KF are contained in 244 mL of 0.135 m KF solution? The density of the solution is 1.22 g/mL.	B) 4.02 × 10-2 mol KF
38) Calculate the molality of a solution that is prepared by mixing 25.5 mL of CH3OH (d= 0.792 g/mL) and 387 mL of CH3CH2CH2OH (d= 0.811 g/mL).	D) 2.01 m
39) Determine the molality of a solution prepared by dissolving 0.500 moles of CaF2 in 11.5 moles H2O.	E) 2.41 m
40) Determine the molality of an aqueous solution prepared by dissolving 0.112 moles of LiCl in 13.7 moles of H2O.	A) 0.454 m
41) Commercial grade HCl solutions are typically 39.0% (by mass) HCl in water. Determine the molarity of the HCl, if the solution has a density of 1.20 g/mL.	C) 12.8 M
42) A solution is prepared by dissolving 98.6 g of NaCl in enough water to form 875 mL of solution. Calculate the mass % of the solution if the density of the solution is 1.06 g/mL.	D) 10.6%
43) A solution is prepared by dissolving 49.3 g of KBr in enough water to form 473 mL of solution. Calculate the mass % of KBr in the solution if the density is 1.12 g/mL.	E) 9.31%
44) What mass of CuCl2 is contained in 75.85 g of a 22.4% by mass solution of CuCl2 in water?	A) 17.0 g
45) What mass of NaCl is contained in 24.88 g of a 15.00% by mass solution of NaCl in water?	C) 3.73 g
46) A solution is prepared by dissolving 38.6 g sucrose (C12H22O11) in 495 g of water. Determine the mole fraction of sucrose if the final volume of the solution is 508 mL.	A) 4.09 × 10-3
47) A solution is prepared by dissolving 76.3 g NaI in 545 g of water. Determine the mole fraction of NaI if the final volume of the solution is 576 mL.	B) 1.65 × 10-2
48) Calculate the mole fraction of total ions in an aqueous solution prepared by dissolving 0.400 moles of MgCl2 in 850.0 g of water.	D) 0.0252
49) Calculate the mole fraction of MgCl2 in an aqueous solution prepared by dissolving 0.400 moles of MgCl2 in 850.0 g of water.	A) 0.00841
50) A 1.00 L sample of water contains 0.0036 g of Cl⁻ ions. Determine the concentration of chloride ions in ppm if the density of the solution is 1.00 g/mL.	C) 3.6 ppm
51) A 4.55 L sample of water contains 0.115 g of sodium ions. Determine the concentration of sodium ions in ppm if the density of the solution is 1.00 g/mL.	D) 25.3 ppm
52) What mass of ethane (CH3CH3) is contained in 50.0 mL of a 13.9% by mass solution of ethane in hexane? The density of the solution is 0.611 g/mL.	E) 4.25 g
53) Commercial grade HCl solutions are typically 39.0% (by mass) HCl in water. Determine the molality of the HCl, if the solution has a density of 1.20 g/mL.	B) 17.5 m
54) A solution is 0.0433 m LiF. What is the molarity of the solution if the density is 1.10 g/mL?	D) 0.0476 M
55) An aqueous solution is 0.387 M in HCl. What is the molality of the solution if the density is 1.23 g/mL?	E) 0.318 m
56) Determine the vapor pressure of a solution at 25°C that contains 76.6 g of glucose (C6H12O6) in 250.0 mL of water. The vapor pressure of pure water at 25°C is 23.8 torr.	C) 23.1 torr
57) Determine the vapor pressure of a solution at 55°C that contains 34.2 g NaCl in 375 mL of water. The vapor pressure of pure water at 55°C is 118.1 torr.	A) 115 torr
58) Determine the freezing point depression of a solution that contains 30.7 g glycerin (C3H8O3, molar mass = 92.09 g/mol) in 376 mL of water. Some possibly useful constants for water are Kf = 1.86°C/m and Kb = 0.512°C/m.	B) 1.65°C
59) Determine the freezing point of a solution that contains 78.8 g of naphthalene (C10H8, molar mass = 128.16 g/mol) dissolved in 722 mL of benzene (d = 0.877 g/mL). Pure benzene has a melting point of 5.50°C and a freezing point depression constant of	C) 0.74°C
60) Calculate the freezing point of a solution of 500.0 g of ethylene glycol (C2H6O2) dissolved in 500.0 g of water. Kf = 1.86°C/m and Kb = 0.512°C/m.	B) -30.0°C
61) Choose the solvent below that would show the greatest boiling point elevation when used to make a 0.10 m nonelectrolyte solution.	A) CCl4, Kb = 29.9°C/m
62) Calculate the boiling point of a solution of 500.0 g of ethylene glycol (C2H6O2) dissolved in 500.0 g of water. Kf = 1.86°C/m and Kb = 0.512°C/m. Use 100°C as the boiling point of water.	A) 108°C
63) The boiling point elevation of an aqueous sucrose solution is found to be 0.39°C. What mass of sucrose (molar mass= 342.30 g/mol) would be needed to dissolve in 500.0 g of water? Kb (water) = 0.512°C/m.	E) 130. g sucrose
64) Determine the boiling point of a solution that contains 78.8 g of naphthalene (C10H8, molar mass = 128.16 g/mol) dissolved in 722 mL of benzene (d = 0.877 g/mL). Pure benzene has a boiling point of 80.1°C and a boiling point elevation constant of 2.5	E) 82.6°C
65) Give the reason that antifreeze is added to a car radiator.	A) The freezing point is lowered and the boiling point is elevated.
66) Place the following aqueous solutions of nonvolatile, nonionic compounds in order of decreasing osmotic pressure. I. 0.011 M sucrose II. 0.00095 M glucose III. 0.0060 M glycerin	A) I > III > II
67) Place the following solutions in order of increasing osmotic pressure. I. 0.15 M C2H6O2 II. 0.15 M MgCl2 III. 0.15 M NaCl	E) I < III < II
68) A compound is found to have a molar mass of 598 g/mol. If 35.8 mg of the compound is dissolved in enough water to make 175 mL of solution at 25°C, what is the osmotic pressure of the resulting solution?	B) 6.36 torr
69) A 150.0 mL sample of an aqueous solution at 25°C contains 15.2 mg of an unknown nonelectrolyte compound. If the solution has an osmotic pressure of 8.44 torr, what is the molar mass of the unknown compound?	A) 223 g/mol
70) Identify the solute with the highest van't Hoff factor.	E) FeCl3
71) Identify the solute with the lowest van't Hoff factor.	A) nonelectrolyte
72) Choose the aqueous solution that has the highest boiling point. These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable.	A) 0.100 m AlCl3
73) Choose the aqueous solution that has the highest boiling point. These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable.	B) 0.100 m Li2SO4
74) Choose the aqueous solution with the lowest vapor pressure. These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable.	C) 0.060 m K2CO3
75) Choose the aqueous solution with the highest vapor pressure. These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable.	E) They all have about the same vapor pressure.
76) Choose the aqueous solution below with the lowest freezing point. These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable.	B) 0.075 m (NH4)3PO4
77) Choose the aqueous solution below with the highest freezing point. These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable.	C) 0.200 m HOCH2CH2OH
78) The boiling point of an aqueous 1.83 m (NH4)2SO4 (molar mass = 132.15 g/mol) solution is 102.5°C. Determine the value of the van't Hoff factor for this solute if the Kb for water is 0.512°C/m.	D) 2.7
79) Fluids used for an intravenous transfusion must be __________ with bodily fluids.	A) isosmotic
80) Solutions having osmotic pressures less than those of body fluids are called __________.	C) hyposmotic
81) Define smoke as a colloid.	B) a solid dispersed in a gas
82) Identify the classification of milk.	D) emulsion
83) Identify the classification of opal.	E) solid emulsion
84) Identify the classification of whipped cream.	C) foam
1) Which cation in each set is expected to have the larger (more negative) hydration energy? I Be2+ or Ca2+ II Rb+ or Zn2+	B) Be2+ in set I and Zn2+ in set II
2) The Henry's Law constant of methyl bromide, CH3Br, is k = 0.159 mol/(L ∙ atm) at 25°C. What is the solubility of methyl bromide in water at 25°C and at a partial pressure of 270. mm Hg?	A) 0.0 565 mol/L
3) The Henry's law constant for helium gas in water at 30°C is 3.70 × 10-4 M/atm. When the partial pressure of helium above a sample of water is 0.650 atm, the concentration of helium in the water is __________ M.	D) 2.41 × 10-4
4) What volume of a 0.716 M KBr solution is needed to provide 30.5 g of KBr?	D) 357 mL
5) What volume of 3.00 M CH3OH solution is needed to provide 0. 220 mol of CH3OH?	C) 73.3 mL
6) To make a 0.500 M solution, one could take 0.500 moles of solute and add	C) enough solvent to make 1.00 L of solution.
7) How many grams of KBr are required to make 350. mL of a 0.115 M KBr solution?	C) 4.79 g
8) What is the molality of a glucose solution prepared by dissolving 18.0 g of glucose, C6H12O6, in 125.9 g of water?	D) 0.794 m
9) To make a 2.00 m solution, one could take 2.00 moles of solute and add	B) 1.00 kg of solvent.
10) What molality of pentane is obtained by dissolving 15 g pentane, C5H12, in 245.0 g hexane, C6H14?	C) 0.85 m
11) A solution of LiCl in water has XLiCl = 0.0 900. What is the molality?	C) 5.49 m LiCl
12) A solution is prepared by adding 1.43 mol of KCl to 889 g of water. The concentration of KCl is __________ molal.	E) 1.61
13) A solution is prepared by dissolving 16.2 g of benzene (C6H6) in 282 g of carbon tetrachloride (CCl4) The concentration of benzene in this solution is __________ molal. The molar masses of C6H6 and CCl4 are 78.1 g/mol and 154 g/mol, respectively.	B) 0.736
14) What is the weight percent of vitamin C in a solution made by dissolving 6.50 g of vitamin C, C6H8O6, in 55.0 g of water?	C) 10.6%
15) What is the weight percent of a caffeine solution made by dissolving 8.35 g of caffeine, C8H10N4O2, in 75 g of benzene, C6H6?	C) 10%
16) How much water must be added to 40.0 g of CaCl2 to produce a solution that is 35.0 wt% CaCl2?	B) 74.2 g
17) A solution of LiCl in water is 20.0 wt% LiCl. What is the mole fraction of LiCl?	A) 0. 0960
18) What is the mole fraction of ethanol in a solution made by dissolving 29.2 g of ethanol, C2H5OH, in 53.6 g of water?	A) 0. 176
19) What is the mole fraction of I2 in a solution made by dissolving 55.6 g of I2 in 245 g of hexane, C6H14?	A) 0. 0715
20) What is the mole fraction of oxygen in a gas mixture that is 37% oxygen and 63% nitrogen by volume?	B) 0. 37
21) A solution is 2.25% by weight NaHCO3. How many grams of NaHCO3 are in 150.0 g of solution?	B) 3.38 g
22) At 20°C, an aqueous solution that is 24.0% by mass in ammonium chloride has a density of 1.0674 g/mL. What is the molarity of ammonium chloride in the solution? The formula weight of NH4Cl is 53.50 g/mol.	C) 4.79
23) At 20°C, a 2.32 M aqueous solution of ammonium chloride has a density of 1.0344 g/mL. What is the molality of ammonium chloride in the solution? The formula weight of NH4Cl is 53.50 g/mol.	A) 2.55
24) At 20°C, a 0.376 M aqueous solution of ammonium chloride has a density of 1.0045 g/mL. What is the mass % of ammonium chloride in the solution? The formula weight of NH4Cl is 53.50 g/mol.	E) 2.00
25) A solution is prepared by dissolving 40.0 g of sucrose, C12H22O11, in 250. g of water at 25°C. What is the vapor pressure of the solution if the vapor pressure of water at 25°C is 23.76 mm Hg?	C) 23.6 mm Hg
26) A KCl solution is prepared by dissolving 25.0 g KCl in 250.0 g of water at 25°C. What is the vapor pressure of the solution if the vapor pressure of water at 25°C is 23.76 mm Hg?	B) 22.7 mm Hg
27) At a given temperature the vapor pressures of benzene and toluene are 183 mm Hg and 59.2 mm Hg, respectively. Calculate the total vapor pressure over a solution of benzene and toluene with Xbenzene = 0. 580.	C) 131 mm Hg
28) Which of the following solutions will have the lowest freezing point?	D) 0.015 m BaCl2
29) What is the expected freezing point of a 0.50 m solution of Li2SO4 in water? Kf for water is 1.86°C/m.	C) -2.8°C
30) Calculate the freezing point of a solution of 40.0 g methyl salicylate, C7H6O2, dissolved in 800. g of benzene, C6H6. Kf for benzene is 5.10 °C/m and the freezing point is 5.50°C for benzene.	C) 3.41°C
31) What is the freezing point of a solution of 7.15 g MgCl2 in 100 g of water? Kf for water is 1.86 °C/m.	D) - 4.18°C
32) An aqueous solution has a normal boiling point of 103.0°C. What is the freezing point of this solution? For water Kb = 0.51 °C/m and Kf = 1.86 °C/m.	D) - 11°C
33) A solution is prepared by adding 30.00 g of lactose (milk sugar) to 110.0 g of water at 55°C. The partial pressure of water above the solution is __________ torr. The vapor pressure of pure water at 55°C is 118.0 torr. The MW of lactose is 342.3 g/mo	D) 116.3
34) A solution is prepared by dissolving 7.00 g of glycerin (C3H8O3) in 201 g of ethanol (C2H5OH). The freezing point of the solution is __________°C. The freezing point of pure ethanol is -114.6 °C at 1 atm. The molal-freezing-point-depression constant	E) -115.4
35) Calculate the freezing point of a solution containing 5.0 grams of KCl and 550.0 grams of water. The molal-freezing-point-depression constant (Kf) for water is 1.86 °C/m.	A) -0.45 oC
36) The osmotic pressure of a solution formed by dissolving 25.0 mg of aspirin (C9H8O4) in 0.250 L of water at 25°C is __________ atm.	C) 0.0136

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