Question 1

The solubility of gases in water usually increases with

Accepted Answer

A)  increasing pressure and increasing temperature. 
B)  increasing temperature and decreasing pressure. 
C)  decreasing temperature and increasing pressure. 
D)  decreasing temperature and decreasing pressure. 
E)  increasing temperature only. 
A)  increasing pressure and increasing temperature. 
B)  increasing temperature and decreasing pressure. 
C)  decreasing temperature and increasing pressure. 
D)  decreasing temperature and decreasing pressure. 
E)  increasing temperature only.

Question 2

Which of the following gives the molarity of a 17.0% by mass solution of sodium acetate, CH3COONa (molar mass = 82.0 g/mol) in water The density of the solution is 1.09 g/mL.

Accepted Answer

A)  2.26 * 10-6 M 
B)  0.207 M 
C)  2.07 M 
D)  2.26 M 
E)  2.72 M 
A)  2.26 * 10-6 M 
B)  0.207 M 
C)  2.07 M 
D)  2.26 M 
E)  2.72 M

Question 3

Calculate the percent by mass of potassium nitrate in a solution made from 45.0 g KNO3 and 295 mL of water. The density of water is 0.997 g/mL.

Accepted Answer

A)  1.51 % 
B)  7.57 % 
C)  13.3 % 
D)  15.2 % 
E)  None of these 
A)  1.51 % 
B)  7.57 % 
C)  13.3 % 
D)  15.2 % 
E)  None of these

Question 4

What is the molarity of a solution that is 5.50 % by mass oxalic acid (C2H2O4) and has a density of 1.0244 g/mL

Accepted Answer

A)  0.626 M 
B)  0.646 M 
C)  0.666 M 
D)  0.686 M 
E)  None of the above 
A)  0.626 M 
B)  0.646 M 
C)  0.666 M 
D)  0.686 M 
E)  None of the above

Question 5

A 9.50 % by mass solution of acetone (C3H6O) in water has a density of 0.9849 g/mL at 20$\circ$C. What is the molarity of this solution

Accepted Answer

A)  0.621 M 
B)  1.61 M 
C)  1.66 M 
D)  1.71 M 
E)  16.9 M 
A)  0.621 M 
B)  1.61 M 
C)  1.66 M 
D)  1.71 M 
E)  16.9 M

Question 6

Arrange the following aqueous solutions in order of increasing boiling points: 0.300m C6H12O6, 0.110m K2CO3, and 0.050m Al(ClO4)3.

Accepted Answer

A)  C6H12O6 2CO3 4)3 
B)  Al(ClO4)3 6H12O6 2CO3 
C)  C6H12O6 4)3 2CO3 
D)  K2CO3 6H12O6 4)3 
E)  K2CO3 4)3 6H12O6 
A)  C6H12O6 2CO3 4)3 
B)  Al(ClO4)3 6H12O6 2CO3 
C)  C6H12O6 4)3 2CO3 
D)  K2CO3 6H12O6 4)3 
E)  K2CO3 4)3 6H12O6

Question 7

Which of the following gases is expected to have a higher solubility in water than what is predicted using Henry's law

Accepted Answer

A)  N2 
B)  CH4 
C)  Ar 
D)  NH3 
E)  H2 
A)  N2 
B)  CH4 
C)  Ar 
D)  NH3 
E)  H2

Question 8

Calculate the mass percent of HOCH2CH2OH in a solution made by dissolving 3.2 g of HOCH2CH2OH in 43.5g of water.

Accepted Answer

A)  2.9% 
B)  6.9% 
C)  7.4% 
D)  22% 
E)  29% 
A)  2.9% 
B)  6.9% 
C)  7.4% 
D)  22% 
E)  29%

Question 9

The vapor pressure of water at 45.0 $\circ$C is 71.93 mmHg. What is the vapor pressure of water over a solution prepared from 75.0 g of citric acid (C6H8O7) in 0.420 kg of water at this temperature

Accepted Answer

A)  1.22 mmHg 
B)  42.3 mmHg 
C)  43.0 mmHg 
D)  70.7 mmHg 
E)  73.2 mmHg 
A)  1.22 mmHg 
B)  42.3 mmHg 
C)  43.0 mmHg 
D)  70.7 mmHg 
E)  73.2 mmHg

Question 10

What is the boiling point of a solution of 11.0 g of lactose (C12H22O11) in 145.0g of water (Kb (H2O) = 0.52 $\circ$C/m)

Accepted Answer

A)  0.1$\circ$C 
B)  99.9 $\circ$C 
C)  100.1$\circ$C 
D)  102.2 $\circ$C 
E)  105.7 $\circ$C 
A)  0.1$\circ$C 
B)  99.9 $\circ$C 
C)  100.1$\circ$C 
D)  102.2 $\circ$C 
E)  105.7 $\circ$C

Question 11

A solution that contains 55.0 g of ascorbic acid (Vitamin C) in 250. g of water freezes at -2.34$\circ$C. Calculate the molar mass (in units of g/mol) of the solute. Kf of water is 1.86$\circ$C/m.

Accepted Answer

A)  1.26 
B)  10.9 
C)  43.6 
D)  175 
E)  277 
A)  1.26 
B)  10.9 
C)  43.6 
D)  175 
E)  277

Question 12

Using your knowledge of osmosis or osmotic pressure decide if the following statement is true or false:
-Meat that is salted before cooking tends to dry out.

Accepted Answer

A) True 
 B)False

Question 13

What is the percent CdSO4 by mass in a 1.00 m aqueous CdSO4 solution

Accepted Answer

A)  1.00 * 10-3 % 
B)  0.100 % 
C)  17.2 % 
D)  20.8 % 
E)  24.4 % 
A)  1.00 * 10-3 % 
B)  0.100 % 
C)  17.2 % 
D)  20.8 % 
E)  24.4 %

Question 14

A 15.00 % by mass solution of lactose (C12H22O11, 342.30 g/mol) in water has a density of 1.0602 g/mL at 20$\circ$C. What is the molarity of this solution

Accepted Answer

A)  0.03097 M 
B)  0.4133 M 
C)  0.4646 M 
D)  1.590 M 
E)  3.097 M 
A)  0.03097 M 
B)  0.4133 M 
C)  0.4646 M 
D)  1.590 M 
E)  3.097 M

Question 15

What is the molality of a solution that is 3.68 % by mass calcium chloride

Accepted Answer

A)  0.0332 m 
B)  0.332 m 
C)  0.344 m 
D)  0.464 m 
E)  0.506 m 
A)  0.0332 m 
B)  0.332 m 
C)  0.344 m 
D)  0.464 m 
E)  0.506 m

Question 16

Maple syrup is mostly a solution of sucrose in water. Calculate the molality of the syrup if a sample freezes at -0.50$\circ$C, assuming the solute is pure sucrose. [For water, Kf is 1.86$\circ$C/m.]

Accepted Answer

A)  0.17 m 
B)  0.27 m 
C)  0.37 m 
D)  047 m 
E)  None of the above 
A)  0.17 m 
B)  0.27 m 
C)  0.37 m 
D)  047 m 
E)  None of the above

Question 17

An exothermic solution process is described by which of the following

Accepted Answer

A) ($\Delta$H) > 0, solution feels cold B) ($\Delta$H) > 0, solution feels hot C) ($\Delta$H) < 0, solution feels cold D) ($\Delta$H) < 0, solution feels hot E) ($\Delta$H) = 0 A) ($\Delta$H) > 0, solution feels cold B) ($\Delta$H) > 0, solution feels hot C) ($\Delta$H) < 0, solution feels cold D) ($\Delta$H) < 0, solution feels hot E) ($\Delta$H) = 0

Question 18

A research chemist isolates a new compound with an empirical formula C3H3O2. Dissolving 2.51 g of the compound in 100. g of water produces a solution with a freezing point of -0.325$\circ$C. What is the molecular formula of the compound (For water, Kf = 1.86$\circ$C/m.)

Accepted Answer

A)  C3H3O2 
B)  C6H6O4 
C)  C9H9O6 
D)  C3H12O4 
E)  None of the above 
A)  C3H3O2 
B)  C6H6O4 
C)  C9H9O6 
D)  C3H12O4 
E)  None of the above

Question 19

Thyroxine, an important hormone that controls the rate of metabolism in the body, can be isolated from the thyroid gland. If 0.455 g of thyroxine is dissolved in 10.0 g of benzene, the freezing point of the solution is 5.144$\circ$C. Pure benzene freezes at 5.444$\circ$C and has a Kf of 5.12$\circ$C/m. What is the molar mass of thyroxine

Accepted Answer

A)  777 g/mol 
B)  787 g/mol 
C)  797 g/mol 
D)  807 g/mol 
E)  None of the above 
A)  777 g/mol 
B)  787 g/mol 
C)  797 g/mol 
D)  807 g/mol 
E)  None of the above

Question 20

A solution is prepared by adding 6.24 g of benzene (C6H6, 78.11 g/mol) to 80.74 g of cyclohexane (C6H12, 84.16 g/mol). Calculate the mole fraction and molality of benzene in this solution.

Accepted Answer

A)  Mole fraction = 0.0769; molality = 0.789 m 
B)  Mole fraction = 0.0869; molality = 0.789 m 
C)  Mole fraction = 0.0769; molality = 0.989 m 
D)  Mole fraction = 0.0869; molality = 0.989 m 
E)  None of the above 
A)  Mole fraction = 0.0769; molality = 0.789 m 
B)  Mole fraction = 0.0869; molality = 0.789 m 
C)  Mole fraction = 0.0769; molality = 0.989 m 
D)  Mole fraction = 0.0869; molality = 0.989 m 
E)  None of the above

Exam 12: Physical Properties of Solutions

The solubility of gases in water usually increases with

Which of the following gives the molarity of a 17.0% by mass solution of sodium acetate, CH3COONa (molar mass = 82.0 g/mol) in water The density of the solution is 1.09 g/mL.

Calculate the percent by mass of potassium nitrate in a solution made from 45.0 g KNO3 and 295 mL of water. The density of water is 0.997 g/mL.

What is the molarity of a solution that is 5.50 % by mass oxalic acid (C2H2O4) and has a density of 1.0244 g/mL

A 9.50 % by mass solution of acetone (C3H6O) in water has a density of 0.9849 g/mL at 20 ∘\circ∘ C. What is the molarity of this solution

Arrange the following aqueous solutions in order of increasing boiling points: 0.300m C6H12O6, 0.110m K2CO3, and 0.050m Al(ClO4)3.

Which of the following gases is expected to have a higher solubility in water than what is predicted using Henry's law

Calculate the mass percent of HOCH2CH2OH in a solution made by dissolving 3.2 g of HOCH2CH2OH in 43.5g of water.

The vapor pressure of water at 45.0 ∘\circ∘ C is 71.93 mmHg. What is the vapor pressure of water over a solution prepared from 75.0 g of citric acid (C6H8O7) in 0.420 kg of water at this temperature

What is the boiling point of a solution of 11.0 g of lactose (C12H22O11) in 145.0g of water (Kb (H2O) = 0.52 ∘\circ∘ C/m)

A solution that contains 55.0 g of ascorbic acid (Vitamin C) in 250. g of water freezes at -2.34 ∘\circ∘ C. Calculate the molar mass (in units of g/mol) of the solute. Kf of water is 1.86 ∘\circ∘ C/m.

Using your knowledge of osmosis or osmotic pressure decide if the following statement is true or false: -Meat that is salted before cooking tends to dry out.

What is the percent CdSO4 by mass in a 1.00 m aqueous CdSO4 solution

A 15.00 % by mass solution of lactose (C12H22O11, 342.30 g/mol) in water has a density of 1.0602 g/mL at 20 ∘\circ∘ C. What is the molarity of this solution

What is the molality of a solution that is 3.68 % by mass calcium chloride

Maple syrup is mostly a solution of sucrose in water. Calculate the molality of the syrup if a sample freezes at -0.50 ∘\circ∘ C, assuming the solute is pure sucrose. [For water, Kf is 1.86 ∘\circ∘ C/m.]

An exothermic solution process is described by which of the following

A research chemist isolates a new compound with an empirical formula C3H3O2. Dissolving 2.51 g of the compound in 100. g of water produces a solution with a freezing point of -0.325 ∘\circ∘ C. What is the molecular formula of the compound (For water, Kf = 1.86 ∘\circ∘ C/m.)

A solution is prepared by adding 6.24 g of benzene (C6H6, 78.11 g/mol) to 80.74 g of cyclohexane (C6H12, 84.16 g/mol). Calculate the mole fraction and molality of benzene in this solution.

Chemistry: The Study of Change

Atoms Molecules and Ions

Mass Relationships in Chemical Reactions

Reactions in Aqueous Solutions

Gases

Thermochemistry

Quantum Theory and the Electronic Structure of Atoms

Periodic Relationships Among the Elements

Chemical Bonding I: Basic Concepts

Chemical Bonding II: Molecular Geometry and Hybridization of Atomic

Intermolecular Forces and Liquids and Solids

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Entropy Free Energy and Equilibrium

Electrochemistry

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Chemistry in the Atmosphere

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Transition Metals Chemistry and Coordination Compounds

Organic Chemistry

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Which of the following gives the molarity of a 17.0% by mass solution of sodium acetate, CH₃COONa (molar mass = 82.0 g/mol) in water The density of the solution is 1.09 g/mL.

Calculate the percent by mass of potassium nitrate in a solution made from 45.0 g KNO₃ and 295 mL of water. The density of water is 0.997 g/mL.

What is the molarity of a solution that is 5.50 % by mass oxalic acid (C₂H₂O₄) and has a density of 1.0244 g/mL

A 9.50 % by mass solution of acetone (C₃H₆O) in water has a density of 0.9849 g/mL at 20^$\circ$C. What is the molarity of this solution

Arrange the following aqueous solutions in order of increasing boiling points: 0.300m C₆H₁₂O₆, 0.110m K₂CO₃, and 0.050m Al(ClO₄)₃.

Calculate the mass percent of HOCH₂CH₂OH in a solution made by dissolving 3.2 g of HOCH₂CH₂OH in 43.5g of water.

The vapor pressure of water at 45.0 ^$\circ$C is 71.93 mmHg. What is the vapor pressure of water over a solution prepared from 75.0 g of citric acid (C₆H₈O₇) in 0.420 kg of water at this temperature

What is the boiling point of a solution of 11.0 g of lactose (C₁₂H₂₂O₁₁) in 145.0g of water (K_b (H₂O) = 0.52 ^$\circ$C/m)

A solution that contains 55.0 g of ascorbic acid (Vitamin C) in 250. g of water freezes at -2.34^$\circ$C. Calculate the molar mass (in units of g/mol) of the solute. K_f of water is 1.86^$\circ$C/m.

What is the percent CdSO₄ by mass in a 1.00 m aqueous CdSO₄ solution

A 15.00 % by mass solution of lactose (C₁₂H₂₂O₁₁, 342.30 g/mol) in water has a density of 1.0602 g/mL at 20^$\circ$C. What is the molarity of this solution

Maple syrup is mostly a solution of sucrose in water. Calculate the molality of the syrup if a sample freezes at -0.50^$\circ$C, assuming the solute is pure sucrose. [For water, K_f is 1.86^$\circ$C/m.]

A research chemist isolates a new compound with an empirical formula C₃H₃O₂. Dissolving 2.51 g of the compound in 100. g of water produces a solution with a freezing point of -0.325^$\circ$C. What is the molecular formula of the compound (For water, K_f = 1.86^$\circ$C/m.)

A solution is prepared by adding 6.24 g of benzene (C₆H₆, 78.11 g/mol) to 80.74 g of cyclohexane (C₆H₁₂, 84.16 g/mol). Calculate the mole fraction and molality of benzene in this solution.