Question 1

Ideally,colligative properties depend only on the:

Accepted Answer

A)  relative number of solute and solvent particles in a solution. 
B)  molar masses of the solute particles in a solution. 
C)  density of a solution. 
D)  hydrated radii of the molecules or ions dissolved in a solution. 
E)  partial pressure of the gases above the surface of a solution. 
A)  relative number of solute and solvent particles in a solution. 
B)  molar masses of the solute particles in a solution. 
C)  density of a solution. 
D)  hydrated radii of the molecules or ions dissolved in a solution. 
E)  partial pressure of the gases above the surface of a solution.

Question 2

If 11.7 g of naphthalene,C10H8,is dissolved in 104.2 g of chloroform,CHCl3,what is the molality of the solution?

Accepted Answer

A)  0.0914 m 
B)  13.4 m 
C)  0.877 m 
D)  0.101 m 
E)  0.105 m 
A)  0.0914 m 
B)  13.4 m 
C)  0.877 m 
D)  0.101 m 
E)  0.105 m

Question 3

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)

Accepted Answer

A)    mol/kg⋅mmHg 
B)    mol/kg⋅mmHg 
C)    mol/kg⋅mmHg 
D)    mol/kg⋅mmHg 
E)    mol/kg⋅mmHg 
A)    mol/kg⋅mmHg 
B)    mol/kg⋅mmHg 
C)    mol/kg⋅mmHg 
D)    mol/kg⋅mmHg 
E)    mol/kg⋅mmHg

Question 4

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.

Accepted Answer

A)  5.1 °C 
B)  2.6 °C 
C)  -5.1 °C 
D)  0.0 °C 
E)  -2.6 °C 
A)  5.1 °C 
B)  2.6 °C 
C)  -5.1 °C 
D)  0.0 °C 
E)  -2.6 °C

Question 5

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?

Accepted Answer

A)  232 g 
B)  75.2 g 
C)  716 g 
D)  44.8 g 
E)  157 g 
A)  232 g 
B)  75.2 g 
C)  716 g 
D)  44.8 g 
E)  157 g

Question 6

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

Accepted Answer

A)  1 m 
B)  0 m 
C)  14 m 
D)  1 m.. 
E)  84.0 m 
A)  1 m 
B)  0 m 
C)  14 m 
D)  1 m.. 
E)  84.0 m

Question 7

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

Accepted Answer

A)  0.1 m NaCl 
B)  0.05 m CH3COOH 
C)  0.05 m Al2(SO4)3 
D)  0.1 m BaCl2 
E)  0.25 m C6H12O6 
A)  0.1 m NaCl 
B)  0.05 m CH3COOH 
C)  0.05 m Al2(SO4)3 
D)  0.1 m BaCl2 
E)  0.25 m C6H12O6

Question 8

What is the concentration unit used in the calculation of osmotic pressure of a dilute solution?

Accepted Answer

A)  Molality 
B)  Weight percent 
C)  Mass fraction 
D)  Mole fraction 
E)  Molarity 
A)  Molality 
B)  Weight percent 
C)  Mass fraction 
D)  Mole fraction 
E)  Molarity

Question 9

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)

Accepted Answer

A)  1.4 × 10-9 M 
B)  1.8 × 10-5 M 
C)  4.6 × 10-4 M 
D)  7.7 × 10-4 M 
E)  7.9 × 10-4 M 
A)  1.4 × 10-9 M 
B)  1.8 × 10-5 M 
C)  4.6 × 10-4 M 
D)  7.7 × 10-4 M 
E)  7.9 × 10-4 M

Question 10

Colloids are described by all of the following except:

Accepted Answer

A)  The particles in a colloid are so small that settling is negligible. 
B)  The mixture appears cloudy. 
C)  Only combinations of liquids and gases can form colloids. 
D)  Colloids are not suspensions or homogeneous mixtures. 
E)  Mayonnaise,whipped cream and fog are all examples of colloids. 
A)  The particles in a colloid are so small that settling is negligible. 
B)  The mixture appears cloudy. 
C)  Only combinations of liquids and gases can form colloids. 
D)  Colloids are not suspensions or homogeneous mixtures. 
E)  Mayonnaise,whipped cream and fog are all examples of colloids.

Question 11

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?

Accepted Answer

A)  0.0 bar 
B)  19.0 bar 
C)    bar 
D)    bar 
E)  37.0 bar 
A)  0.0 bar 
B)  19.0 bar 
C)    bar 
D)    bar 
E)  37.0 bar

Question 12

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.

Accepted Answer

A)  15.6 g 
B)  49.9 g 
C)  194 g 
D)  969 g 
E)  3.10 × 103 g 
A)  15.6 g 
B)  49.9 g 
C)  194 g 
D)  969 g 
E)  3.10 × 103 g

Question 13

All of the following are colloidal dispersions EXCEPT ____.

Accepted Answer

A)  marshmallow 
B)  white wine 
C)  milk 
D)  whipped cream 
E)  cheese 
A)  marshmallow 
B)  white wine 
C)  milk 
D)  whipped cream 
E)  cheese

Question 14

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

Accepted Answer

A)  65.7 mL 
B)  15.2 mL 
C)  1.69 mL 
D)  8.74 mL 
E)  84.8 mL 
A)  65.7 mL 
B)  15.2 mL 
C)  1.69 mL 
D)  8.74 mL 
E)  84.8 mL

Question 15

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?

Accepted Answer

A)  7.1°C/m 
B)  29°C/m 
C)  14.0°C/m 
D)  3.5°C/m 
E)  7.0°C/m 
A)  7.1°C/m 
B)  29°C/m 
C)  14.0°C/m 
D)  3.5°C/m 
E)  7.0°C/m

Question 16

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).

Accepted Answer

A)  -797.0 kJ/mol 
B)  -74.0 kJ/mol 
C)  -871.0 kJ/mol 
D)  797.0 kJ/mol 
E)  871.0 kJ/mol 
A)  -797.0 kJ/mol 
B)  -74.0 kJ/mol 
C)  -871.0 kJ/mol 
D)  797.0 kJ/mol 
E)  871.0 kJ/mol

Question 17

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

Accepted Answer

A)  1 
B)  2 
C)  3 
D)  4 
E)  5 
A)  1 
B)  2 
C)  3 
D)  4 
E)  5

Question 18

What is the mass percent of an aqueous sodium hydroxide solution in which the mole fraction of NaOH is 0.0736?

Accepted Answer

A)  15.0% 
B)  16% 
C)  69% 
D)  9% 
E)  3% 
A)  15.0% 
B)  16% 
C)  69% 
D)  9% 
E)  3%

Question 19

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?

Accepted Answer

A)  37.6 g 
B)  69.1 g 
C)  4.73 g 
D)  1.81 g 
E)  20.4 g 
A)  37.6 g 
B)  69.1 g 
C)  4.73 g 
D)  1.81 g 
E)  20.4 g

Question 20

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.

Accepted Answer

A)  0.0071 ppm 
B)  0.12 ppm 
C)  0.71 ppm 
D)  1.7 ppm 
E)  8.3 ppm 
A)  0.0071 ppm 
B)  0.12 ppm 
C)  0.71 ppm 
D)  1.7 ppm 
E)  8.3 ppm

Exam 14: Solutions and Their Behavior

Ideally,colligative properties depend only on the:

If 11.7 g of naphthalene,C10H8,is dissolved in 104.2 g of chloroform,CHCl3,what is the molality of the solution?

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)

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.

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?

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

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

What is the concentration unit used in the calculation of osmotic pressure of a dilute solution?

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)

Colloids are described by all of the following except:

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?

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.

All of the following are colloidal dispersions EXCEPT ____.

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

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?

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).

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

What is the mass percent of an aqueous sodium hydroxide solution in which the mole fraction of NaOH is 0.0736?

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?

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.

Basic Concepts of Chemistry

Lets Review: The Tools of Quantitative Chemistry

Atoms, molecules, and Ions

Chemical Reactions

Stoichiometry: Quantitative Information About Chemical Reactions

Principles of Chemical Reactivity: Energy and Chemical Reactions

The Structure of Atoms

The Structure of Atoms and Periodic Trends

Bonding and Molecular Structure

Bonding and Molecular Structure Orbital Hybridization and Molecular Orbitals

Gases and Their Properties

Intermolecular Forces and Liquids

The Solid State

Chemical Kinetics: the Rates of Chemical Reactions

Principles of Chemical Reactivity: Equilibria

Principles of Chemical Reactivity: the Chemistry of Acids and Bases

Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria

Principles of Chemical Reactivity: Entropy and Free Energy

Principles of Chemical Reactivity: Electron Transfer Reactions

Environmental Chemistry: Earths Environment, energy, and Sustainability

The Chemistry of the Main Group Elements

The Chemistry of the Transition Elements

Carbon: Not Just Another Element

Biochemistry

Nuclear Chemistry

Filters

If 11.7 g of naphthalene,C₁₀H₈,is dissolved in 104.2 g of chloroform,CHCl₃,what is the molality of the solution?

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)

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

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

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)

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?

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.

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

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?

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

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?

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.