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Chem II > Ch 13 > Flashcards

Ch 13 Flashcards

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1
Q

A surfactant used for cleaning is called a(n) ________.

A

detergent

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2
Q

For a dilute solution of (NH4)2SO4, the van’t Hoff factor (i) would be approximately ___.
Group of answer choices

1
2
3
4
5

A

b.

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3
Q

For the following gas-liquid equilibrium for an aqueous system at a constant partial pressure of CO2,
CO2(g)

D

CO2(aq)
what is the effect on the equilibrium composition of the liquid when the temperature of the liquid is increased?

A

b.

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4
Q

If the solubility of O2 at 0.300 bar and 25°C is 12.5 g/100 g H2O, what is the solubility of O2 at a pressure of 1.64 bar and 25°C?

A

a.

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5
Q

What is the vapor pressure at 20°C of an ideal solution prepared by the addition of 4.50 g of the nonvolatile solute urea, CO(NH2)2, to 22.7 g of methanol, CH3OH? The vapor pressure of pure methanol at 20°C is 89.0 mmHg.

A

d.

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6
Q

The lattice enthalpy of LiCl is −834 kJ/mol and the enthalpy of solution of LiCl is –37 kJ/mol. Calculate the enthalpy of hydration of LiCl(s).

A

c.

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7
Q

A solution in which there is more dissolved solute than in a saturated solution is known as a(n) ________ solution.

A

saturated

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8
Q

Two nonpolar solvents, such as hexane and carbon tetrachloride, may be miscible even though the enthalpy of mixing of these liquids might be small. A reason that mixing occurs is that mixtures have a greater dispersal of energy relative to pure solvents. The tendency toward greater dispersal of energy is a thermodynamic function ____.

A

not b.

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9
Q

If the concentration of sodium carbonate in water is 12.8 ppm, what is the molarity of Na2CO3(aq)? The molar mass of Na2CO3 is 106.0 g/mol. Assume the density of the solution is 1.00 g/mL.

A

b.

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10
Q

Assuming ideal behavior, which of the following aqueous solutions should have the highest boiling point?

1.00 m LiBr
0.75 m K2SO4
0.50 m Ca(NO3)2
0.75 m NaCl
1.25 m C6H12O6

A

b.

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11
Q

What is the mass of H2SO4 in a 38.2-mL sample of concentrated sulfuric acid that has a density of 1.84 g/mL and consists of 98.3% H2SO4?

37.6 g
69.1 g
4.73 g
1.81 g
20.4 g

A

not a. or e.

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12
Q

A 15 meter by 12 meter pool of water has a depth of 2.2 meters. What mass of silver ion is present in the reservoir if the concentration of silver ion is 0.14 ppm? (1 m3 = 1000 L; assume the density of the solution is 1.00 g/mL)

A

e.

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13
Q

The volume of a 32.4% (by mass) solution is 179.1 mL. The density of the solution is 1.296 g/mL. What is the mass of solute in this solution?
232 g
75.2 g
716 g
44.8 g
157 g

A

b.

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14
Q

For the following gas-aqueous liquid equilibrium for a closed system at a constant temperature,
N2(g)

D

N2(aq)
what is the effect on the equilibrium composition of the liquid when the partial pressure of N2 gas above the liquid is decreased?

A

a.

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15
Q

What is the freezing point of an aqueous 1.38 m NaCl solution? (Kfp for water is 1.858°C/m.) Assume no ion pairing occurs.

5.1 °C
2.6 °C
–5.1 °C
0.0 °C
–2.6 °C

A

c.

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16
Q

Which of the following solutions would have the highest osmotic pressure?
0.2 M C6H12O6, glucose
0.15 M MgCl2, magnesium chloride
0.15 M KCl, potassium chloride
0.2 M CH3OH, methanol
0.2 M C12H22O11, sucrose

A

b.

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17
Q

What is the freezing point of a solution containing 2.80 grams benzene (molar mass = 78.11 g/mol) dissolved in 43.0 grams paradichlorobenzene (molar mass = 147.0 g/mol)? The freezing point of pure paradichlorobenzene is 53.0 °C and the freezing point depression constant, Kfp, is –7.10 °C/m.
46.7 °C
47.1 °C
58.9 °C
52.6 °C
58.9 °C

A

b.

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18
Q

What is the mass percent of an aqueous sodium hydroxide solution in which the mole fraction of NaOH is 0.0736?
15.0%
16%
69%
9%
3%

A

a.

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19
Q

Henry’s Law constant is 0.0013 mol/kg⋅bar and 0.034 mol/kg⋅bar for O2 and CO2 respectively at 25°C. What pressure of CO2 is required to achieve the same solubility as 0.711 bar of O2?
Group of answer choices
0.0 bar
19.0 bar
bar
bar
37.0 bar

A

not c. or b. or d.

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20
Q

Which of the following is a colligative property?

Vapor pressure addition
Boiling point depression
Freezing point depression
Osmotic pressure
Melting point elevation

A

c.

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21
Q

What is the mole fraction of calcium chloride in 3.35 m CaCl2(aq)? The molar mass of CaCl2 is 111.0 g/mol and the molar mass of water is 18.02 g/mol.
0.000866
0.0569
0.271
37.2
59.2

A

b.

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22
Q

A concentrated hydrochloric acid solution is 37.2% HCl by mass and has a density of 1.19 g/mL at 25°C. What is the molarity of HCl?
12.1 M
0.0434 M
8.57 M
11.7 M
0.0857 M

A

not e.

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23
Q

All of the following are colloidal dispersions EXCEPT ____.
marshmallow
white wine
milk
whipped cream
cheese

A

b.

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24
Q

What type of colloid is formed when a liquid is dispersed in a gas?
Aerosol
Foam
Gel
Sol
Emulsion

A

a.

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25
Q

The Henry’s law constant for N2 in water at 25 °C is 6.0 × 10–4 mol/kg⋅bar. What is the equilibrium concentration of N2 in water when the partial pressure of N2 is 586 mm Hg? (760 mm Hg = 1 atm = 0.9869 bar)
1.4 × 10–9 M
1.8 × 10–5 M
4.6 × 10–4 M
7.7 × 10–4 M
7.9 × 10–4 M

A

c.

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26
Q

Ideally, colligative properties depend only on the:
Group of answer choices

relative number of solute and solvent particles in a solution.

molar masses of the solute particles in a solution.

density of a solution.

hydrated radii of the molecules or ions dissolved in a solution.

partial pressure of the gases above the surface of a solution.

A

a.

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27
Q

Which of the following statements about soaps and detergents is false?
Group of answer choices

The polar end is attracted to grease and oil.

They have a polar and a nonpolar end.

They are emulsifiers for grease and oil.

Phosphate detergents can produce pollution.

They can be described as surfactants.

A

a.

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28
Q
A
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29
Q

If one of the factors determining the equilibrium of a system is changed, the system adjusts to counteract that change. This is known as ________ principle.

A

maybe Le Chatelier’s

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30
Q

The solubility of 1-pentanol in water is 2.7 g per 100 g of water at 25°C. What is the maximum amount of 1-pentanol that will dissolve in 2.1 g of water at 25°C?
0.057 g
1.3 g
2.7 g
5.7 g
0.013 g

A

a.

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31
Q

What is the Henry’s law constant for O2 if the solubility of O2 in water is 0.590 g/L at a pressure of 15.5 atm?
3.81 × 10-2 L·atm/mol
8.41 × 102 L·atm/mol
2.86 × 10-1 L·atm/mol
1.19 × 10-3 L·atm/mol
None of these

A

b.

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32
Q

If 27.9 g LiCl is dissolved in 175 g H2O, what is the weight percent of LiCl in the solution?
0.376%
6.78%
13.8%
15.9%
19.0%

A

c.

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33
Q

What mass of ethylene glycol, when mixed with 225 g H2O, will reduce the equilibrium vapor pressure of H2O from 1.00 atm to 0.800 atm at 100 °C? The molar masses of water and ethylene glycol are 18.02 g/mol and 62.07 g/mol, respectively. Assume ideal behavior for the solution.
15.6 g
49.9 g
194 g
969 g
3.10 × 103 g

A

c.

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34
Q

Which of the following statements concerning osmosis is/are correct?
1. Osmosis involves the movement of ions through a semipermeable membrane until the charges on both sides of the membrane are equal.
2. Solvents move from regions of low solute concentration to regions of higher solute concentration.
3. Osmotic pressure is a colligative property.

A

d.

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35
Q

What is the definition of molality?
Group of answer choices

moles of solute per kg of solvent

grams of solute per kg of solution

grams of solute per liter of solution

moles of solute per liter of solvent

moles of solute per liter of solution

A

a.

36
Q

Which action(s) will decrease the equilibrium concentration of an inert gas (such as N2) in water?
1. decreasing the temperature of the water
2. increasing the volume of water
3. decreasing the pressure of the gas above the liquid
Group of answer choices

1 only

2 only

3 only

1 and 3

1, 2, and 3

A

c.

37
Q

What is the equilibrium partial pressure of water vapor above a mixture of 37.5 g H2O and 62.5 g HOCH2CH2OH at 55 °C. The partial pressure of pure water at 55.0 °C is 118.0 mm Hg. Assume ideal behavior for the solution.
Group of answer choices

3.54 mm Hg

31.7 mm Hg

38.5 mm Hg

79.5 mm Hg

175 mm Hg

A

d.

38
Q

What volume of a 0.758 M solution of CaCl2 contains 1.28 g of solute?
Group of answer choices

65.7 mL

15.2 mL

1.69 mL

8.74 mL

84.8 mL

A

b.

39
Q

The standard enthalpy of formation of RbF(s) is –557.7kJ/mol and the standard enthalpy of formation of RbF(aq, 1 m) is –583.8 kJ/mol. Determine the enthalpy of solution of RbF and indicate whether the solution temperature will increase or decrease when RbF is dissolved in water.
Group of answer choices

–26.1 kJ/mol; increase

26.1 kJ/mol; increase

–26.1 kJ/mol; decrease

+1141.5 kJ/mol; increase

–1141.5 kJ/mol; decrease

A

a.

40
Q

Henry’s law states that the solubility of a gas in a liquid is directly proportional to its pressure above the liquid. This law holds true for gases such as nitrogen and oxygen. However, Henry’s law does not hold true for hydrogen chloride gas. Why?

A

Henry’s law only works if the molecules are at equilibrium.

41
Q

A solution consisting of 0.278 mol of methylbenzene, C6H5CH3, in 244 g of nitrobenzene, C6H5NO2, freezes at –2.0°C. Pure nitrobenzene freezes at 6.0°C. What is the freezing-point depression constant of nitrobenzene?
7.1°C/m
29°C/m
14.0°C/m
3.5°C/m
7.0°C/m

A

e.

42
Q

According to the National Institute of Standards webbook, the Henry’s Law constant for O2 gas is 0.0013 mol/kg⋅bar at 25°C What is the Henry’s law constant in units of mol/kg⋅mmHg? (1 bar = 0.9869 atm; 1 atm = 760 mmHg)

mol/kg⋅mmHg

A

a.

43
Q

Which of the following favor(s) the solubility of an ionic solid in a liquid solvent?
Group of answer choices

a small magnitude of the lattice energy of the solute

a large magnitude of the solvation energy of the ions

a large polarity of the solvent

all of the above

none of the above

A

d.

44
Q

What is the osmotic pressure of an aqueous solution that is 0.46% NaCl by weight at 36°C. Assume the density of the solution is 1.0 g/mL. Assume no ion pairing. (R = 0.0821 L · atm/K·mol)
0.20 atm
2.0 atm
2.3 × 102 atm
4.0 atm
0.47 atm

A

d.

45
Q

A 3.0 g sample of a small protein having a molecular weight of 42,000 g/mol is dissolved in 52.8 mL of water at 21°C. What is the osmotic pressure of the solution? (R = 0.0821 L · atm/K·mol, 1 atm = 760 mmHg)

25 mmHg
1900 mmHg
1.8 mmHg
23,000 mmHg
0.033 mmHg

A

a.

46
Q

Which of the following statements is INCORRECT?
Group of answer choices

The solubility of a gas in water decreases with increasing temperature.

The solubility of a gas in water is proportional to the partial pressure of the gas above the water.

The dissolution of a gas in water is usually an exothermic process.

The relationship between the solubility of a gas and its partial pressure is known as Henry’s law.

The solubility of a gas in water is inversely proportional to the molar mass of the gas.

A

e.

47
Q

The osmotic pressure of blood is 7.65 atm at 37 °C. What mass of glucose (C6H12O6, molar mass = 180.2 g/mol) is needed to prepare 2.25 L of solution for intravenous injection? The osmotic pressure of the glucose solution must equal the osmotic pressure of blood. (R = 0.08206 L⋅atm/mol⋅K)
Group of answer choices

0.676 g

0.698 g

5.67 g

122 g

1.02 × 103 g

A

d.

48
Q

The vapor pressure of pure water at 15 °C is 12.8 mm Hg. What is the equilibrium vapor pressure of water above a mixture of 72.0 g ethanol (CH3CH2OH, molar mass = 46.07 g/mol) and 22.0 g water?
Group of answer choices

2.84 mm Hg

5.61 mm Hg

7.19 mm Hg

10.0 mm Hg

12.8 mm Hg

A

b.

49
Q

The following equation is known as ________ law: .

A

maybe Raoult’s

50
Q

Colloids represent a state intermediate between a solution and a suspension. Is this statement true or false?

A

true

51
Q

If an egg’s shell is carefully dissolved using an acid, the egg white and yolk will remain intact inside a membrane. If the egg is then placed in distilled water, it will slowly expand until it bursts. Why?

A

maybe This happens from the hypotonic solution

52
Q

Because ________ particles are relatively large (say, 1000 nm in diameter) they scatter visible light, making the mixtures containing these particles appear cloudy. This scattering is known as the Tyndall effect.

A

maybe colloidal

53
Q

The Henry’s law constant for O2 in water at 25 °C is 1.3 × 10–3 mol/kg⋅bar. What partial pressure of O2 (in atm) is necessary to achieve an equilibrium concentration of 2.9 × 10–3 mol/kg O2? (1 atm = 0.9869 bar)
0.44 atm
0.45 atm
2.1 atm
2.3 atm
3.8 atm

A

d.

54
Q

What mass of Zn(NO3)2 must be diluted to a mass of 1.00 kg with H2O to prepare 97 ppm Zn2+(aq)?
7.8 × 10–6 g
7.8 × 10–3 g
3.3 × 10–2 g
1.3 × 10–1 g
2.8 × 10–1 g

A

e.

55
Q

What is the freezing point of a 0.29 m solution of glucose (C6H12O6) in water? (Kfp for water is 1.858 °C/m.)
0.27 °C
0.54 °C
–0.54 °C
–0.27 °C
–1.08 °C

A

c.

56
Q

If a 15.6-g sample of a nonelectrolyte is dissolved in 100.0 g of water, the resulting solution will freeze at –0.93°C. What is the molar mass of the nonelectrolyte? (Kfp for water is 1.858°C/m.)
81 g/mol
0.31 g/mol
430 g/mol
270 g/mol
310 g/mol

A

e.

57
Q

What is the concentration unit used in the calculation of osmotic pressure of a dilute solution?
Molality
Weight percent
Mass fraction
Mole fraction
Molarity

A

e.

58
Q

_____ are colloidal dispersions of one liquid in another.

A

maybe emulsion

59
Q

Colloids are described by all of the following except:
Group of answer choices

The particles in a colloid are so small that settling is negligible.

The mixture appears cloudy.

Only combinations of liquids and gases can form colloids.

Colloids are not suspensions or homogeneous mixtures.

Mayonnaise, whipped cream and fog are all examples of colloids.

A

c.

60
Q

How many milliliters of 11.7 M H2SO4 are needed to prepare 600.0 mL of 0.10 M H2SO4?
0.19 mL
70 mL
5.1 mL
2.6 mL
6.1 mL

A

c.

61
Q

A solution is prepared by dissolving 5.88 g of an unknown nonelectrolyte in enough water to make 0.355 L of solution. The osmotic pressure of the solution is 1.21 atm at 27 °C. What is the molar mass of the solute? (R = 0.08206 L⋅atm/mol⋅K)

0.00297 g/mol
30.3 g/mol
42.5 g/mol
175 g/mol
337 g/mol

A

e.

62
Q

Assuming ideal behavior, which of the following aqueous solutions would be expected to exhibit the smallest freezing-point lowering?

A

a.

63
Q

The change in energy accompanying the equation below is the _____ of MX.

A

b.

64
Q

Two nonpolar solvents, such as hexane and carbon tetrachloride, may be miscible even though the enthalpy of mixing of these liquids might be small. A reason that mixing occurs is that mixtures have a greater dispersal of energy relative to pure solvents. The tendency toward greater dispersal of energy is a thermodynamic function called ____.

A

a.

65
Q

A 12.0% sucrose solution by mass has a density of 1.05 g/cm3. What mass of sucrose is present in a 53.0-mL sample of this solution?

A

a.

66
Q

What concentration of silver nitrate (in ppm) is present in 7.1 × 10–7 M AgNO3(aq)? For very dilute aqueous solutions, you can assume the solution’s density is 1.0 g/mL. The molar mass of AgNO3 is 169.9 g/mol.

A

b.

67
Q

Which of the following equations illustrates the formation of an aqueous solution of KF from its elements in their standard states?
K+(g) + F−(g) → K+(aq) + F−(aq)
KF(s) → KF(aq, 1 m)
K+(g) + F−(g) → KF(s)
K(s) + F2(g) → KF(s)
K(s) + F2(g) → KF(aq, 1 m)

A

e.

68
Q

What partial pressure of oxygen gas is required in order for 0.00284 g of the gas to dissolve in 15.9 mL of pure water? The Henry’s law constant for oxygen gas is 1.3 × 10–3 M atm–1.
2.3 × 10–7 atm
4.3 × 100 atm
1.2 × 10–7 atm
2.3 × 10–1 atm
4.2 × 10–2 atm

A

b.

69
Q

Which of the following liquids are miscible with water in any proportion?
Group of answer choices

Ethanol (CH3CH2OH) and carbon tetrachloride (CCl4)

Carbon tetrachloride (CCl4) and hexane (C6H14)

Ethanol (CH3CH2OH) and formic acid (HCO2H)

Ethanol (CH3CH2OH), carbon tetrachloride (CCl4), and hexane (C6H14)

Carbon tetrachloride (CCl4) and formic acid (HCO2H)

A

c.

70
Q

What is the mole fraction of urea, CO(NH2)2, in a solution prepared by dissolving 4.8 g of urea in 30.3 g of methanol, CH3OH?
0.86
0.14
0.078
0.92
0.23

A

c.

71
Q

What mass of Na2SO4 must be dissolved in 100.0 grams of water to lower the freezing point by 2.50 °C? The freezing point depression constant, Kfp, of water is –1.86 °C/m. Assume the van’t Hoff factor for Na2SO4 is 2.85.
3.77 g
6.36 g
6.70 g
11.3 g
19.1 g

A

c.

72
Q

What is the boiling-point change for a solution containing 0.251 mol of naphthalene (a nonvolatile, nonionizing compound) in 250. g of liquid benzene? (Kbp = 2.53°C/m for benzene)
2.54 °C
10.08 °C
0.159 °C
2.52 °C
0.635 °C

A

a.

73
Q

Aqueous colloidal solutions can be classified as ________ (water-fearing), or hydrophilic (water-loving).

A

hydrophobic

74
Q

The vapor pressure of water at 90°C is 0.692 atm. What is the vapor pressure (in atm) of a solution made by dissolving 2.91 mole(s) of CsF(s) in 1.00 kg of water? Assume that Raoult’s law applies.
Group of answer choices
0.626 atm
0.658 atm
0.692 atm
0.765 atm
none of these

A

a.

75
Q

What is the molality of a 19.4 M sodium hydroxide solution that has a density of 1.54 g/mL?
12.6 m
19.8 m
25.4 m
29.9 m
50.4 m

A

c.

76
Q

Calculate the molarity of a solution of magnesium chloride with a concentration of 27.0 mg/mL.
0.142 M
3.53 M
0.567 M
0.452 M
0.284 M

A

e.

77
Q

If 11.7 g of naphthalene, C10H8, is dissolved in 104.2 g of chloroform, CHCl3, what is the molality of the solution?
Group of answer choices
0.0914 m
13.4 m
0.877 m
0.101 m
0.105 m

A

not d. or a.

78
Q

A 0.20 M solution of MgSO4 has an observed osmotic pressure of 7.7 atm at 25°C. Determine the observed van’t Hoff factor for this experiment.
Group of answer choices
2.0
1.6
0.31
19
1.8

A

b.

79
Q

Which of the following statements concerning solubility is/are correct?
1. Ionic compounds composed of Group 1A metal ions and halide ions, such as NaCl, are insoluble in nonpolar solvents.
2. The solubility of halogens (Cl2, Br2, and I2) in polar solvents is greater than their solubility in nonpolar solvents.
3. The solubility of polar molecules, such as sugar, in polar solvents is generally greater than their solubility in nonpolar solvents.

A

d.

80
Q

Which of the following statements is/are CORRECT?
1. Solubility is defined as the concentration of solute in equilibrium with undissolved solute in a saturated solution.
2. If two liquids mix to an appreciable extent to form a solution, they are miscible.
3. If two liquids mix completely in any proportion to form a solution, the resulting solution is supersaturated.

A

d.

81
Q

Which of the following solutions has the lowest osmotic pressure?
Group of answer choices

0.10 M Al(NO3)3

0.20 M C6.0H12O6

0.15 M Ba(NO3)2

0.10 M CaBr2

0.15 M Na2Cl

A

b.

82
Q

What is the molality of ethanol (C2H5OH) in an aqueous solution that is 39.8% ethanol by mass?
Group of answer choices

1 m

0 m

14 m

1 m

84.0 m

A

c.

83
Q

Which of the following compounds is not miscible with water?
Group of answer choices

CH3NH2

CH3COOH

CCl4

CH3CN

HOCH2CH2OH

A

c.

84
Q

What is the mole fraction of urea, CH4N2O, in an aqueous solution that is 49% urea by mass?

A

a.

85
Q

What is the mass percent of an aqueous sodium hydroxide solution in which the molality of NaOH is 10.7 m?
Group of answer choices

0%
69%
2%
30.0%
0%

A

d.

86
Q

What mass of an aqueous 18.8% glucose solution contains 85.5 g of water?
Group of answer choices
105 g
19.8 g
14.5 g
16.1 g
85.5 g

A

not b. or c. or d.

87
Q

A concentrated nitric acid solution has a density of 1.41 g/mL at 25°C and is 15.8 M. What is the percent by mass of HNO3 in the solution?
Group of answer choices
70.6% HNO3 by mass
1.12% HNO3 by mass
0.895% HNO3 by mass
1.77% HNO3 by mass
44.7% HNO3 by mass

A

a.

Chem II (13 decks)

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