Question 1

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.

Accepted Answer

A)  0.075 m LiCl 
B)  0.075 m (NH4)3PO4 
C)  0.075 m NaBrO4 
D)  0.075 m KCN 
E)  0.075 m KNO2 
A)  0.075 m LiCl 
B)  0.075 m (NH4)3PO4 
C)  0.075 m NaBrO4 
D)  0.075 m KCN 
E)  0.075 m KNO2

Question 2

Define osmosis.

Accepted Answer

Osmosis is the flow of solvent

Question 3

Soap has an ionic and a polar end.It works well to remove oil by

Accepted Answer

A)  surrounding the oil with the nonpolar end, and the water interacts with the polar end. 
B)  surrounding the oil with the polar end, and the water interacts with the nonpolar end. 
C)  surrounding the oil and water with the polar end. 
D)  surrounding the oil and water with the nonpolar end. 
A)  surrounding the oil with the nonpolar end, and the water interacts with the polar end. 
B)  surrounding the oil with the polar end, and the water interacts with the nonpolar end. 
C)  surrounding the oil and water with the polar end. 
D)  surrounding the oil and water with the nonpolar end.

Question 4

Choose the situation below that would result in an exothermic ΔHsolution.

Accepted Answer

A)  When   >
  
B)  When   is close to
  
C)  When   >
  
E)  There isn't enough information to determine. 
A)  When   >
  
B)  When   is close to
  
C)  When   >
  
E)  There isn't enough information to determine.

Question 5

To increase solubility of a gas into a liquid the most,then

Accepted Answer

A)  increase the temperature and lower the pressure. 
B)  increase the temperature and raise the pressure. 
C)  decrease the temperature and raise the pressure. 
D)  decrease the temperature and lower the pressure. 
E)  neither pressure or temperature affects solubility. 
A)  increase the temperature and lower the pressure. 
B)  increase the temperature and raise the pressure. 
C)  decrease the temperature and raise the pressure. 
D)  decrease the temperature and lower the pressure. 
E)  neither pressure or temperature affects solubility.

Question 6

Solutions having osmotic pressures less than those of body fluids are called

Accepted Answer

A)  isosmotic. 
B)  hyperosmotic. 
C)  hyposmotic. 
D)  neosmotic. 
E)  magnosmotic. 
A)  isosmotic. 
B)  hyperosmotic. 
C)  hyposmotic. 
D)  neosmotic. 
E)  magnosmotic.

Question 7

What mass (in g)of NH3 must be dissolved in 475 g of methanol to make a 0.250 m solution?

Accepted Answer

A)  2.02 g 
B)  4.94 g 
C)  1.19 g 
D)  8.42 g 
E)  1.90 g 
A)  2.02 g 
B)  4.94 g 
C)  1.19 g 
D)  8.42 g 
E)  1.90 g

Question 8

________ is applied to roads in wintertime so that the ice will melt at a lower temperature.

Accepted Answer

A)  Antifreeze 
B)  Water 
C)  Salt 
D)  Dirt 
E)  Syrup 
A)  Antifreeze 
B)  Water 
C)  Salt 
D)  Dirt 
E)  Syrup

Question 9

A solution containing more than the equilibrium amount is called

Accepted Answer

A)  an unsaturated solution. 
B)  a dilute solution. 
C)  a supersaturated solution. 
D)  a concentrated solution. 
E)  a saturated solution. 
A)  an unsaturated solution. 
B)  a dilute solution. 
C)  a supersaturated solution. 
D)  a concentrated solution. 
E)  a saturated solution.

Question 10

Choose the situation below that would result in a ΔHsolution near 0.

Accepted Answer

A) When >> B) When > C) When < D) When is close to E) There isn't enough information to determine. A) When >> B) When > C) When < D) When is close to E) There isn't enough information to determine.

Question 11

What is the expected freezing point of a 0.50 m solution of Li2SO4 in water? Kf for water is 1.86°C/m.

Accepted Answer

A)  -0.93°C 
B)  -1.9°C 
C)  -2.8°C 
D)  -6.5°C 
E)  +1.9°C 
A)  -0.93°C 
B)  -1.9°C 
C)  -2.8°C 
D)  -6.5°C 
E)  +1.9°C

Question 12

What is the molality of a D-mannose solution prepared by dissolving 45.0 g of D-mannose,C6H12O6,in 125.9 g of water?

Accepted Answer

A)  1.98 × 10-3 m 
B)  0.358 m 
C)  1.46 m 
D)  1.98 m 
E)  9.81 × 10-3 m 
A)  1.98 × 10-3 m 
B)  0.358 m 
C)  1.46 m 
D)  1.98 m 
E)  9.81 × 10-3 m

Question 13

Choose the situation below that would result in an endothermic ΔHsolution.

Accepted Answer

A)  When   >
  
B)  When   >
  
E)  There isn't enough information to determine. 
A)  When   >
  
B)  When   >
  
E)  There isn't enough information to determine.

Question 14

Identify the most polar solvent.

Accepted Answer

A)  acetone 
B)  octane 
C)  sodium chloride 
D)  toluene 
E)  carbon tetrachloride 
A)  acetone 
B)  octane 
C)  sodium chloride 
D)  toluene 
E)  carbon tetrachloride

Question 15

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.

Accepted Answer

A)  59 M/atm 
B)  0.017 M/atm 
C)  0.029 M/atm 
D)  35 M/atm 
E)  0.038 M/atm 
A)  59 M/atm 
B)  0.017 M/atm 
C)  0.029 M/atm 
D)  35 M/atm 
E)  0.038 M/atm

Question 16

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 × 10-3 M/atm.

Accepted Answer

A)  49.4 mg 
B)  23.5 mg 
C)  9.87 mg 
D)  27.3 mg 
E)  13.7 mg 
A)  49.4 mg 
B)  23.5 mg 
C)  9.87 mg 
D)  27.3 mg 
E)  13.7 mg

Question 17

Which of the following compounds will be most soluble in ethanol (CH3CH2OH)?

Accepted Answer

A)  trimethylamine (N(CH3)3) 
B)  acetone (CH3COCH3) 
C)  ethylene glycol (HOCH2CH2OH) 
D)  hexane (CH3CH2CH2CH2CH2CH3) 
E)  None of these compounds should be soluble in ethanol. 
A)  trimethylamine (N(CH3)3) 
B)  acetone (CH3COCH3) 
C)  ethylene glycol (HOCH2CH2OH) 
D)  hexane (CH3CH2CH2CH2CH2CH3) 
E)  None of these compounds should be soluble in ethanol.

Question 18

The scattering of light by a colloidal dispersion is known as

Accepted Answer

A)  an emulsion 
B)  an aerosol. 
C)  micelle repulsion. 
D)  Brownian motion. 
E)  Tyndall effect. 
A)  an emulsion 
B)  an aerosol. 
C)  micelle repulsion. 
D)  Brownian motion. 
E)  Tyndall effect.

Question 19

Identify the solute with the lowest van't Hoff factor.

Accepted Answer

A)  nonelectrolyte 
B)  KI 
C)  MgSO4 
D)  CaCl2 
E)  AlCl3 
A)  nonelectrolyte 
B)  KI 
C)  MgSO4 
D)  CaCl2 
E)  AlCl3

Question 20

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 4.90°C/m.

Accepted Answer

A)  4.76°C 
B)  4.17°C 
C)  0.74°C 
D)  1.33°C 
E)  1.68°C 
A)  4.76°C 
B)  4.17°C 
C)  0.74°C 
D)  1.33°C 
E)  1.68°C

Exam 13: Solutions

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.

Define osmosis.

Soap has an ionic and a polar end.It works well to remove oil by

Choose the situation below that would result in an exothermic ΔHsolution.

To increase solubility of a gas into a liquid the most,then

Solutions having osmotic pressures less than those of body fluids are called

What mass (in g)of NH3 must be dissolved in 475 g of methanol to make a 0.250 m solution?

________ is applied to roads in wintertime so that the ice will melt at a lower temperature.

A solution containing more than the equilibrium amount is called

Choose the situation below that would result in a ΔHsolution near 0.

What is the expected freezing point of a 0.50 m solution of Li2SO4 in water? Kf for water is 1.86°C/m.

What is the molality of a D-mannose solution prepared by dissolving 45.0 g of D-mannose,C6H12O6,in 125.9 g of water?

Choose the situation below that would result in an endothermic ΔHsolution.

Identify the most polar solvent.

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.

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 × 10-3 M/atm.

Which of the following compounds will be most soluble in ethanol (CH3CH2OH)?

The scattering of light by a colloidal dispersion is known as

Identify the solute with the lowest van't Hoff factor.

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 4.90°C/m.

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Filters

Choose the situation below that would result in an exothermic ΔH_solution.

What mass (in g)of NH₃ must be dissolved in 475 g of methanol to make a 0.250 m solution?

Choose the situation below that would result in a ΔH_solution near 0.

What is the expected freezing point of a 0.50 m solution of Li₂SO₄ in water? K_f for water is 1.86°C/m.

What is the molality of a D-mannose solution prepared by dissolving 45.0 g of D-mannose,C₆H₁₂O₆,in 125.9 g of water?

Choose the situation below that would result in an endothermic ΔH_solution.

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 × 10^-3 M/atm.

Which of the following compounds will be most soluble in ethanol (CH₃CH₂OH)?

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 4.90°C/m.