Question 1

A solution containing less solute 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 2

Explain why the van't Hoff factor for MgCl2 is less than its predicted value.

Accepted Answer

The hydrated Mg²⁺ and Cl⁻ ions

Question 3

What is the expected freezing point of a 0.50 mol kg-1 solution of Li2SO4 in water? Kf for water is 1.86 °C m-1.

Accepted Answer

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

Question 4

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 5

What is the mole fraction of I2 in a solution made by dissolving 55.6 g of I2 in 245 g of hexane, C6H14?

Accepted Answer

A)  0. 0715 
B)  0. 0770 
C)  0. 133 
D)  0. 154 
A)  0. 0715 
B)  0. 0770 
C)  0. 133 
D)  0. 154

Question 6

What is the weight percent of a caffeine solution made by dissolving 8.35 g of caffeine, C8H10N4O2, in 75 g of benzene, C6H6?

Accepted Answer

A)  0.0 10% 
B)  0.0 11% 
C)  10% 
D)  11% 
A)  0.0 10% 
B)  0.0 11% 
C)  10% 
D)  11%

Question 7

Parts per billion requires a multiplication factor of ________.

Accepted Answer

A)  10-6 
B)  10-3 
C)  103 
D)  106 
E)  109 
A)  10-6 
B)  10-3 
C)  103 
D)  106 
E)  109

Question 8

To make a 0.500 mol L-1 solution, one could take 0.500 moles of solute and add ________.

Accepted Answer

A)  1.00 L of solvent 
B)  1.00 kg of solvent 
C)  enough solvent to make 1.00 L of solution 
D)  enough solvent to make 1.00 kg of solution 
A)  1.00 L of solvent 
B)  1.00 kg of solvent 
C)  enough solvent to make 1.00 L of solution 
D)  enough solvent to make 1.00 kg of solution

Question 9

Why isn't pentanol (CH3CH2CH2CH2CH2OH) very soluble in water?

Accepted Answer

Even though the pentanol molecule contai

Question 10

An aqueous solution is 0.387 mol L-1 in HCl. What is the molality of the solution if the density is 1.23 g mL-1?

Accepted Answer

A)  0.115 mol kg-1 
B)  0.387 mol kg-1 
C)  0.315 mol kg-1 
D)  0.411 mol kg-1 
E)  0.318 mol kg-1 
A)  0.115 mol kg-1 
B)  0.387 mol kg-1 
C)  0.315 mol kg-1 
D)  0.411 mol kg-1 
E)  0.318 mol kg-1

Question 11

Which of the following compounds is highly soluble at room temperature?

Accepted Answer

A)  Na2SO4 
B)  K2Cr2O7 
C)  KNO3 
D)  KClO3 
E)  NaCl 
A)  Na2SO4 
B)  K2Cr2O7 
C)  KNO3 
D)  KClO3 
E)  NaCl

Question 12

Choose the statement below that is TRUE.

Accepted Answer

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. 
B)  A solution will form between two substances if the solute-solvent interactions are small enough to be overcome by the solute-solute and solvent-solvent interactions. 
C)  A solution will form between two substances if the solute-solute interactions are strong enough to overcome the solvent-solvent interactions. 
D)  A solution will form between two substances only if the solvent-solvent interactions are weak enough to overcome the solute-solvent interactions. 
E)  None of the above 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. 
B)  A solution will form between two substances if the solute-solvent interactions are small enough to be overcome by the solute-solute and solvent-solvent interactions. 
C)  A solution will form between two substances if the solute-solute interactions are strong enough to overcome the solvent-solvent interactions. 
D)  A solution will form between two substances only if the solvent-solvent interactions are weak enough to overcome the solute-solvent interactions. 
E)  None of the above is true.

Question 13

Equal masses, 5.00 g, of pentane (C5H12) and hexane (C6H14) are mixed. Calculate the vapour pressure of the resulting solution. The vapour pressures of pure pentane and hexane are 425 Torr and 151 Torr, respectively. Assume ideal behaviour.

Accepted Answer

A)  291 Torr 
B)  284 Torr 
C)  317 Torr 
D)  300 Torr 
E)  342 Torr 
A)  291 Torr 
B)  284 Torr 
C)  317 Torr 
D)  300 Torr 
E)  342 Torr

Question 14

Determine the boiling point of a solution that contains 78.8 g of naphthalene (C10H8, molar mass = 128.16 g mol-1) dissolved in 722 mL of benzene (d = 0.877 g mL-1). Pure benzene has a boiling point of 80.1 °C and a boiling point elevation constant of 2.53 °C m-1.

Accepted Answer

A)  2.2 °C 
B)  2.5 °C 
C)  82.3 °C 
D)  80.4 °C 
E)  82.6 °C 
A)  2.2 °C 
B)  2.5 °C 
C)  82.3 °C 
D)  80.4 °C 
E)  82.6 °C

Question 15

A solution is prepared by dissolving 40.0 g of sucrose, C12H22O11, in 250. g of water at 25 °C. What is the vapour pressure of the solution if the vapour pressure of water at 25 °C is 23.76 mmHg?

Accepted Answer

A)  0. 198 mmHg 
B)  20.5 mmHg 
C)  23.6 mmHg 
D)  24. 0 mmHg 
A)  0. 198 mmHg 
B)  20.5 mmHg 
C)  23.6 mmHg 
D)  24. 0 mmHg

Question 16

Determine the solubility of N2 in water exposed to air at 25 °C if the atmospheric pressure is 1.2 bar. 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 mol L-1 bar-1.

Accepted Answer

A)  1.5 × 10-4 mol L-1 
B)  6.5 × 10-4 mol L-1 
C)  5.7 × 10-4 mol L-1 
D)  1.8 × 10-4 mol L-1 
E)  3.6 × 10-4 mol L-1 
A)  1.5 × 10-4 mol L-1 
B)  6.5 × 10-4 mol L-1 
C)  5.7 × 10-4 mol L-1 
D)  1.8 × 10-4 mol L-1 
E)  3.6 × 10-4 mol L-1

Question 17

A solution of LiCl in water has XLiCl = 0.0 900. What is the molality?

Accepted Answer

A)  4.46 mol kg-1 LiCl 
B)  5.00 mol kg-1 LiCl 
C)  5.49 mol kg-1 LiCl 
D)  9.89 mol kg-1 LiCl 
A)  4.46 mol kg-1 LiCl 
B)  5.00 mol kg-1 LiCl 
C)  5.49 mol kg-1 LiCl 
D)  9.89 mol kg-1 LiCl

Question 18

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 19

Calculate the molality of a solution formed by dissolving 27.8 g of LiI in 500.0 mL of water.

Accepted Answer

A)  0.254 mol kg-1 
B)  0.394 mol kg-1 
C)  0.556 mol kg-1 
D)  0.241 mol kg-1 
E)  0.415 mol kg-1 
A)  0.254 mol kg-1 
B)  0.394 mol kg-1 
C)  0.556 mol kg-1 
D)  0.241 mol kg-1 
E)  0.415 mol kg-1

Question 20

Which cation in each set is expected to have the larger (more negative) hydration energy? I Be2+ or Ca2+
II Rb+ or Zn2+

Accepted Answer

A)  Be2+ in set I and Rb+ in set II 
B)  Be2+ in set I and Zn2+ in set II 
C)  Ca2+ in set I and Rb+ in set II 
D)  Ca2+ in set I and Zn2+ in set II 
A)  Be2+ in set I and Rb+ in set II 
B)  Be2+ in set I and Zn2+ in set II 
C)  Ca2+ in set I and Rb+ in set II 
D)  Ca2+ in set I and Zn2+ in set II

Exam 12: Solutions

A solution containing less solute than the equilibrium amount is called ________.

Explain why the van't Hoff factor for MgCl2 is less than its predicted value.

What is the expected freezing point of a 0.50 mol kg-1 solution of Li2SO4 in water? Kf for water is 1.86 °C m-1.

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

What is the mole fraction of I2 in a solution made by dissolving 55.6 g of I2 in 245 g of hexane, C6H14?

What is the weight percent of a caffeine solution made by dissolving 8.35 g of caffeine, C8H10N4O2, in 75 g of benzene, C6H6?

Parts per billion requires a multiplication factor of ________.

To make a 0.500 mol L-1 solution, one could take 0.500 moles of solute and add ________.

Why isn't pentanol (CH3CH2CH2CH2CH2OH) very soluble in water?

An aqueous solution is 0.387 mol L-1 in HCl. What is the molality of the solution if the density is 1.23 g mL-1?

Which of the following compounds is highly soluble at room temperature?

Choose the statement below that is TRUE.

Equal masses, 5.00 g, of pentane (C5H12) and hexane (C6H14) are mixed. Calculate the vapour pressure of the resulting solution. The vapour pressures of pure pentane and hexane are 425 Torr and 151 Torr, respectively. Assume ideal behaviour.

Determine the boiling point of a solution that contains 78.8 g of naphthalene (C10H8, molar mass = 128.16 g mol-1) dissolved in 722 mL of benzene (d = 0.877 g mL-1). Pure benzene has a boiling point of 80.1 °C and a boiling point elevation constant of 2.53 °C m-1.

A solution is prepared by dissolving 40.0 g of sucrose, C12H22O11, in 250. g of water at 25 °C. What is the vapour pressure of the solution if the vapour pressure of water at 25 °C is 23.76 mmHg?

Determine the solubility of N2 in water exposed to air at 25 °C if the atmospheric pressure is 1.2 bar. 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 mol L-1 bar-1.

A solution of LiCl in water has XLiCl = 0.0 900. What is the molality?

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

Calculate the molality of a solution formed by dissolving 27.8 g of LiI in 500.0 mL of water.

Which cation in each set is expected to have the larger (more negative) hydration energy? I Be2+ or Ca2+ II Rb+ or Zn2+

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Explain why the van't Hoff factor for MgCl₂ is less than its predicted value.

What is the expected freezing point of a 0.50 mol kg^-1 solution of Li₂SO₄ in water? K_f for water is 1.86 °C m^-1.

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

What is the mole fraction of I₂ in a solution made by dissolving 55.6 g of I₂ in 245 g of hexane, C₆H₁₄?

What is the weight percent of a caffeine solution made by dissolving 8.35 g of caffeine, C₈H₁₀N₄O₂, in 75 g of benzene, C₆H₆?

To make a 0.500 mol L^-1 solution, one could take 0.500 moles of solute and add ________.

Why isn't pentanol (CH₃CH₂CH₂CH₂CH₂OH) very soluble in water?

An aqueous solution is 0.387 mol L^-1 in HCl. What is the molality of the solution if the density is 1.23 g mL^-1?

Equal masses, 5.00 g, of pentane (C₅H₁₂) and hexane (C₆H₁₄) are mixed. Calculate the vapour pressure of the resulting solution. The vapour pressures of pure pentane and hexane are 425 Torr and 151 Torr, respectively. Assume ideal behaviour.

Determine the boiling point of a solution that contains 78.8 g of naphthalene (C₁₀H₈, molar mass = 128.16 g mol^-1) dissolved in 722 mL of benzene (d = 0.877 g mL^-1). Pure benzene has a boiling point of 80.1 °C and a boiling point elevation constant of 2.53 °C m^-1.

A solution is prepared by dissolving 40.0 g of sucrose, C₁₂H₂₂O₁₁, in 250. g of water at 25 °C. What is the vapour pressure of the solution if the vapour pressure of water at 25 °C is 23.76 mmHg?

Determine the solubility of N₂ in water exposed to air at 25 °C if the atmospheric pressure is 1.2 bar. 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 mol L^-1bar^-1.

A solution of LiCl in water has X_LiCl = 0.0 900. What is the molality?

Which cation in each set is expected to have the larger (more negative) hydration energy? I Be²⁺ or Ca²⁺ II Rb⁺ or Zn²⁺