Question 1

Calculate the freezing point of a solution of 500.0 g of ethylene glycol (C2H6O2)dissolved in 500.0 g of water.Kf = 1.86°C/m and Kb = 0.512°C/m.

Accepted Answer

A) 30.0°C 
B) -30.0°C 
C) 8.32°C 
D) -8.32°C 
E) 70.2°C 
A) 30.0°C 
B) -30.0°C 
C) 8.32°C 
D) -8.32°C 
E) 70.2°C

Question 2

Determine the solubility of N2 in water exposed to air at 25°C if the atmospheric pressure is 1.2 atm.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 M/atm.

Accepted Answer

A) 1.5 × 10-4 M 
B) 6.5 × 10-4 M 
C) 5.7 × 10-4 M 
D) 1.8 × 10-4 M 
E) 3.6 × 10-4 M 
A) 1.5 × 10-4 M 
B) 6.5 × 10-4 M 
C) 5.7 × 10-4 M 
D) 1.8 × 10-4 M 
E) 3.6 × 10-4 M

Question 3

Which of the following concentration units are temperature dependent?

Accepted Answer

A) mole fraction 
B) molality 
C) mass percent 
D) molarity 
E) none of the above 
A) mole fraction 
B) molality 
C) mass percent 
D) molarity 
E) none of the above

Question 4

Choose the aqueous solution that has the highest boiling point.These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable.

Accepted Answer

A) 0.100 m NaNO3 
B) 0.100 m Li2SO4 
C) 0.200 m C3H8O3 
D) 0.060 m Na3PO4 
E) They all have the same boiling point. 
A) 0.100 m NaNO3 
B) 0.100 m Li2SO4 
C) 0.200 m C3H8O3 
D) 0.060 m Na3PO4 
E) They all have the same boiling point.

Question 5

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

Accepted Answer

The hydrated Mg²^⁺ and Cl^⁻ ions ca

Question 6

Which of the following ions should have the most exothermic ΔHhydration?

Accepted Answer

A) Na⁺ 
B) Mg2⁺ 
C) Al3⁺ 
D) Ca2⁺ 
E) Sr2⁺ 
A) Na⁺ 
B) Mg2⁺ 
C) Al3⁺ 
D) Ca2⁺ 
E) Sr2⁺

Question 7

At a given temperature the vapor pressures of benzene and toluene are 183 mm Hg and 59.2 mm Hg,respectively.Calculate the total vapor pressure over a solution of benzene and toluene with Xbenzene = 0.580.

Accepted Answer

A) 106 mm Hg 
B) 121 mm Hg 
C) 131 mm Hg 
D) 242 mm Hg 
A) 106 mm Hg 
B) 121 mm Hg 
C) 131 mm Hg 
D) 242 mm Hg

Question 8

Which aqueous solution has the highest freezing point?

Accepted Answer

A) 0.10 m AlCl3 
B) 0.10 m NaCl 
C) 0.10 m BaCl2 
D) 0.10 m C6H12O6 
A) 0.10 m AlCl3 
B) 0.10 m NaCl 
C) 0.10 m BaCl2 
D) 0.10 m C6H12O6

Question 9

Calculate the boiling point of a solution of 500.0 g of ethylene glycol (C2H6O2)dissolved in 500.0 g of water.Kf = 1.86°C/m and Kb = 0.512°C/m.Use 100°C as the boiling point of water.

Accepted Answer

A) 108°C 
B) 92°C 
C) 130°C 
D) 70°C 
E) 8.3°C 
A) 108°C 
B) 92°C 
C) 130°C 
D) 70°C 
E) 8.3°C

Question 10

Which of the following should have the largest Henry's law constant (kH)in water?

Accepted Answer

A) Ne 
B) CO 
C) Br2 
D) CH3CH3 
E) CO2 
A) Ne 
B) CO 
C) Br2 
D) CH3CH3 
E) CO2

Question 11

What is the mole fraction of oxygen in a gas mixture that is 37% oxygen and 63% nitrogen by volume?

Accepted Answer

A) 0.34 
B) 0.37 
C) 0.25 
D) 0.52 
A) 0.34 
B) 0.37 
C) 0.25 
D) 0.52

Question 12

Commercial grade HCl solutions are typically 39.0% (by mass)HCl in water.Determine the molarity of the HCl,if the solution has a density of 1.20 g/mL.

Accepted Answer

A) 7.79 M 
B) 10.7 M 
C) 12.8 M 
D) 9.35 M 
E) 13.9 M 
A) 7.79 M 
B) 10.7 M 
C) 12.8 M 
D) 9.35 M 
E) 13.9 M

Question 13

A solution is prepared by dissolving 98.6 g of NaCl in enough water to form 875 mL of solution.Calculate the mass % of the solution if the density of the solution is 1.06 g/mL.

Accepted Answer

A) 11.3% 
B) 12.7% 
C) 9.4% 
D) 10.6% 
E) 11.9% 
A) 11.3% 
B) 12.7% 
C) 9.4% 
D) 10.6% 
E) 11.9%

Question 14

A solution is prepared by dissolving 7.00 g of glycerin (C3H8O3)in 201 g of ethanol (C2H5OH).The freezing point of the solution is ________°C.The freezing point of pure ethanol is -114.6°C at 1 atm.The molal-freezing-point-depression constant (Kf)for ethanol is 1.99°C/m.The molar masses of glycerin and of ethanol are 92.1 g/mol and 46.1 g/mol,respectively.

Accepted Answer

A) -121.3 
B) 0.752 
C) -107.9 
D) -113.8 
E) -115.4 
A) -121.3 
B) 0.752 
C) -107.9 
D) -113.8 
E) -115.4

Question 15

Identify the compound that would have the highest osmotic pressure when dissolved in water.

Accepted Answer

A) NaCl 
B) K2SO4 
C) MgCl2 
D) FeCl3 
E) MgSO4 
A) NaCl 
B) K2SO4 
C) MgCl2 
D) FeCl3 
E) MgSO4

Question 16

Determine the partial pressure of oxygen necessary to form an aqueous solution that is 4.1 × 10-4 M O2 at 25°C.The Henry's law constant for oxygen in water at 25°C is 1.3 × 10-3 M/atm.

Accepted Answer

A) 1.9 atm 
B) 0.53 atm 
C) 0.24 atm 
D) 0.77 atm 
E) 0.32 atm 
A) 1.9 atm 
B) 0.53 atm 
C) 0.24 atm 
D) 0.77 atm 
E) 0.32 atm

Question 17

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

Accepted Answer

A) an unsaturated solution 
B) a solute 
C) a supersaturated solution 
D) a saturated solution. 
E) a solvent 
A) an unsaturated solution 
B) a solute 
C) a supersaturated solution 
D) a saturated solution. 
E) a solvent

Question 18

Calculate the freezing point of a solution of 40.0 g methyl salicylate,C7H6O2,dissolved in 800.g of benzene,C6H6.Kf for benzene is 5.10°C/m and the freezing point is 5.50°C for benzene.

Accepted Answer

A) -2.09°C 
B) 2.09°C 
C) 3.41°C 
D) 7.59°C 
A) -2.09°C 
B) 2.09°C 
C) 3.41°C 
D) 7.59°C

Question 19

Which of the following statements is true?

Accepted Answer

A) In general,the solubility of a solid in water decreases with increasing temperature. 
B) In general,the solubility of a gas in water decreases with increasing temperature. 
C) The solubility of a gas in water usually increases with decreasing pressure. 
D) The solubility of an ionic solid in water decreases with increasing temperature. 
E) None of the above statements are true. 
A) In general,the solubility of a solid in water decreases with increasing temperature. 
B) In general,the solubility of a gas in water decreases with increasing temperature. 
C) The solubility of a gas in water usually increases with decreasing pressure. 
D) The solubility of an ionic solid in water decreases with increasing temperature. 
E) None of the above statements are true.

Question 20

Calculate the mole fraction of CaI2 in an aqueous solution prepared by dissolving 0.400 moles of CaI2 in 850.0 g of water.

Accepted Answer

A) 0.00841 
B) 0.0270 
C) 0.00900 
D) 0.0252 
E) 0.0167 
A) 0.00841 
B) 0.0270 
C) 0.00900 
D) 0.0252 
E) 0.0167

Calculate the freezing point of a solution of 500.0 g of ethylene glycol (C₂H₆O₂)dissolved in 500.0 g of water.K_f = 1.86°C/m and K_b = 0.512°C/m.

Determine the solubility of N₂ in water exposed to air at 25°C if the atmospheric pressure is 1.2 atm.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 M/atm.

Which of the following concentration units are temperature dependent?

Choose the aqueous solution that has the highest boiling point.These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable.

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

Which of the following ions should have the most exothermic ΔH_hydration?

At a given temperature the vapor pressures of benzene and toluene are 183 mm Hg and 59.2 mm Hg,respectively.Calculate the total vapor pressure over a solution of benzene and toluene with X_benzene = 0.580.

Which aqueous solution has the highest freezing point?

Calculate the boiling point of a solution of 500.0 g of ethylene glycol (C₂H₆O₂)dissolved in 500.0 g of water.K_f = 1.86°C/m and K_b = 0.512°C/m.Use 100°C as the boiling point of water.

Which of the following should have the largest Henry's law constant (k_H)in water?

What is the mole fraction of oxygen in a gas mixture that is 37% oxygen and 63% nitrogen by volume?

Commercial grade HCl solutions are typically 39.0% (by mass)HCl in water.Determine the molarity of the HCl,if the solution has a density of 1.20 g/mL.

A solution is prepared by dissolving 98.6 g of NaCl in enough water to form 875 mL of solution.Calculate the mass % of the solution if the density of the solution is 1.06 g/mL.

Identify the compound that would have the highest osmotic pressure when dissolved in water.

Determine the partial pressure of oxygen necessary to form an aqueous solution that is 4.1 × 10^-4M O₂ at 25°C.The Henry's law constant for oxygen in water at 25°C is 1.3 × 10^-3 M/atm.

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

Calculate the freezing point of a solution of 40.0 g methyl salicylate,C₇H₆O₂,dissolved in 800.g of benzene,C₆H₆.K_f for benzene is 5.10°C/m and the freezing point is 5.50°C for benzene.

Which of the following statements is true?

Calculate the mole fraction of CaI₂ in an aqueous solution prepared by dissolving 0.400 moles of CaI₂ in 850.0 g of water.

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Chemical Bonding I: Lewis Theory

Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and

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Exam 12: Solutions

Calculate the freezing point of a solution of 500.0 g of ethylene glycol (C2H6O2)dissolved in 500.0 g of water.Kf = 1.86°C/m and Kb = 0.512°C/m.

Determine the solubility of N2 in water exposed to air at 25°C if the atmospheric pressure is 1.2 atm.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 M/atm.

Which of the following concentration units are temperature dependent?

Choose the aqueous solution that has the highest boiling point.These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable.

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

Which of the following ions should have the most exothermic ΔHhydration?

At a given temperature the vapor pressures of benzene and toluene are 183 mm Hg and 59.2 mm Hg,respectively.Calculate the total vapor pressure over a solution of benzene and toluene with Xbenzene = 0.580.

Which aqueous solution has the highest freezing point?

Calculate the boiling point of a solution of 500.0 g of ethylene glycol (C2H6O2)dissolved in 500.0 g of water.Kf = 1.86°C/m and Kb = 0.512°C/m.Use 100°C as the boiling point of water.

Which of the following should have the largest Henry's law constant (kH)in water?

What is the mole fraction of oxygen in a gas mixture that is 37% oxygen and 63% nitrogen by volume?

Commercial grade HCl solutions are typically 39.0% (by mass)HCl in water.Determine the molarity of the HCl,if the solution has a density of 1.20 g/mL.

A solution is prepared by dissolving 98.6 g of NaCl in enough water to form 875 mL of solution.Calculate the mass % of the solution if the density of the solution is 1.06 g/mL.

Identify the compound that would have the highest osmotic pressure when dissolved in water.

Determine the partial pressure of oxygen necessary to form an aqueous solution that is 4.1 × 10-4 M O2 at 25°C.The Henry's law constant for oxygen in water at 25°C is 1.3 × 10-3 M/atm.

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

Calculate the freezing point of a solution of 40.0 g methyl salicylate,C7H6O2,dissolved in 800.g of benzene,C6H6.Kf for benzene is 5.10°C/m and the freezing point is 5.50°C for benzene.

Which of the following statements is true?

Calculate the mole fraction of CaI2 in an aqueous solution prepared by dissolving 0.400 moles of CaI2 in 850.0 g of water.

Matter, Measurement, and Problem Solving

Atoms and Elements

Molecules, Compounds and Chemical Equations

Chemical Quantities and Aqueous Reactions

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and

Liquids, Solids, and Intermolecular Forces

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Filters

Calculate the freezing point of a solution of 500.0 g of ethylene glycol (C₂H₆O₂)dissolved in 500.0 g of water.K_f = 1.86°C/m and K_b = 0.512°C/m.

Determine the solubility of N₂ in water exposed to air at 25°C if the atmospheric pressure is 1.2 atm.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 M/atm.

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

Which of the following ions should have the most exothermic ΔH_hydration?

At a given temperature the vapor pressures of benzene and toluene are 183 mm Hg and 59.2 mm Hg,respectively.Calculate the total vapor pressure over a solution of benzene and toluene with X_benzene = 0.580.

Calculate the boiling point of a solution of 500.0 g of ethylene glycol (C₂H₆O₂)dissolved in 500.0 g of water.K_f = 1.86°C/m and K_b = 0.512°C/m.Use 100°C as the boiling point of water.

Which of the following should have the largest Henry's law constant (k_H)in water?

Determine the partial pressure of oxygen necessary to form an aqueous solution that is 4.1 × 10^-4M O₂ at 25°C.The Henry's law constant for oxygen in water at 25°C is 1.3 × 10^-3 M/atm.

Calculate the freezing point of a solution of 40.0 g methyl salicylate,C₇H₆O₂,dissolved in 800.g of benzene,C₆H₆.K_f for benzene is 5.10°C/m and the freezing point is 5.50°C for benzene.

Calculate the mole fraction of CaI₂ in an aqueous solution prepared by dissolving 0.400 moles of CaI₂ in 850.0 g of water.