Question 1

List the following solutions in order of increasing boiling point: 0.15m NaI, 0.10m K3PO4, 0.20 ethylene glycol

Accepted Answer

ethylene g

Question 2

The osmotic pressure of a 0.010 M MgSO4 solution at 25°C is 0.318 atm.Calculate i, the van't Hoff factor, for this MgSO4 solution.

Accepted Answer

A) 0.013 
B) 1.3 
C) 1.5 
D) 2.0 
E) 76.8 
A) 0.013 
B) 1.3 
C) 1.5 
D) 2.0 
E) 76.8

Question 3

Calculate the molality of a 15.0% by mass solution of MgCl2 in H2O.The density of this solution is 1.127 g/mL.

Accepted Answer

A) 0.0134 m 
B) 0.157 m 
C) 1.58 m 
D) 1.86 m 
E) 11.8 m 
A) 0.0134 m 
B) 0.157 m 
C) 1.58 m 
D) 1.86 m 
E) 11.8 m

Question 4

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°C.Pure benzene freezes at 5.444°C and has a Kf of 5.12°C/m.What is the molar mass of thyroxine?

Accepted Answer

Question 5

What is the mass % of K2SO4 in an aqueous solution that has a mole fraction of K2SO4, X = 0.350?

Accepted Answer

Question 6

For water Kf = 1.86°C/m.Therefore, the freezing points of 1.0 M aqueous KCl and C2H5OH (ethanol)solutions are the same.

Accepted Answer

A) True 
 B)False

Question 7

A saturated solution

Accepted Answer

A) contains more solute than solvent. 
B) contains more solvent than solute. 
C) contains equal moles of solute and solvent. 
D) contains the maximum amount of solute that will dissolve in that solvent at that temperature. 
E) contains a solvent with only sigma bonds and no pi bonds (i.e.only single bonds, with no double or triple bonds). 
A) contains more solute than solvent. 
B) contains more solvent than solute. 
C) contains equal moles of solute and solvent. 
D) contains the maximum amount of solute that will dissolve in that solvent at that temperature. 
E) contains a solvent with only sigma bonds and no pi bonds (i.e.only single bonds, with no double or triple bonds).

Question 8

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

Accepted Answer

A) 0.1°C 
B) 99.9 °C 
C) 100.1°C 
D) 102.2 °C 
E) 105.7 °C 
A) 0.1°C 
B) 99.9 °C 
C) 100.1°C 
D) 102.2 °C 
E) 105.7 °C

Question 9

An endothermic 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 10

The solubility of oxygen in lakes high in the Rocky Mountains is affected by the altitude.If the solubility of O2 from the air is 2.67 × 10-4 M at sea level and 25°C, what is the solubility of O2 at an elevation of 12,000 ft where the atmospheric pressure is 0.657 atm? Assume the temperature is 25°C, and that the mole fraction of O2 in air is 0.209 at both 12,000 ft and at sea level.

Accepted Answer

A) 3.66 × 10-5 M 
B) 1.75 × 10-4 M 
C) 2.67 × 10-4 M 
D) 4.06 × 10-4 M 
E) None of the above. 
A) 3.66 × 10-5 M 
B) 1.75 × 10-4 M 
C) 2.67 × 10-4 M 
D) 4.06 × 10-4 M 
E) None of the above.

Question 11

What is the freezing point of a solution that contains 10.0 g of glucose (C6H12O6)in 100.g of H2O? Kf for water is 1.86°C/m.

Accepted Answer

A) +0.10°C 
B) +0.186°C 
C) -0.10°C 
D) -0.186°C 
E) -1.03°C 
A) +0.10°C 
B) +0.186°C 
C) -0.10°C 
D) -0.186°C 
E) -1.03°C

Question 12

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 13

What is the freezing point of an aqueous solution of a nonvolatile solute that has a boiling point of 102.5°C? For water Kf = 1.86°C/m and Kb = 0.52°C/m.

Accepted Answer

A) 8.94°C 
B) 0.99°C 
C) -0.99°C 
D) -8.94°C 
E) -366°C 
A) 8.94°C 
B) 0.99°C 
C) -0.99°C 
D) -8.94°C 
E) -366°C

Question 14

Calculate the approximate freezing point of a solution made from 21.0 g NaCl and 1.00 × 102 g of H2O.[Kf of water is 1.86°C/m.]

Accepted Answer

A) -13.4°C 
B) -6.68°C 
C) -3.59°C 
D) 3.59°C 
E) 6.68°C 
A) -13.4°C 
B) -6.68°C 
C) -3.59°C 
D) 3.59°C 
E) 6.68°C

Question 15

What is the mole fraction of NaOH in a 32.0 % by mass NaOH aqueous solution?

Accepted Answer

The answer of What is the mole fraction of NaOH...

Question 16

The term "proof" is defined as twice the percent by volume of pure ethanol in solution.A solution that is 95% ethanol is 190 proof.What is the molarity of ethanol in a 92-proof ethanol/water solution? (Given: density of ethanol = 0.80 g/cm3; density of water = 1.0 g/cm3)

Accepted Answer

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 100.mL sample of water is taken from the Great Salt Lake, and the water is allowed to evaporate.The salts that remain (mostly NaCl)have a mass of 31.9 g Calculate the original concentration of NaCl, in g per liter, in each water sample.

Accepted Answer

The answer of A 100.mL sample of water is taken...

Question 19

Some KCl is dissolved in water at 25°C, where it completely dissociates.The vapor pressure of pure water at 25°C is 28.3 mmHg.On the graph below, sketch the vapor pressure above the salt solution as a function of the mole fraction of H2O, assuming that Raoult's law is obeyed.Explain how you arrived at your graph.

Accepted Answer

@#IMG-DLM& Pure water has a vapor pressu

Question 20

An aqueous fructose solution having a density of 1.049 g/cm3 is found to have an osmotic pressure of 17.0 atm at 25°C.Find the temperature at which this solution freezes.[Given: for water Kf = 1.86 °C/m; molecular mass of fructose = 180.16 g/mol]

Accepted Answer

A) -1.30°C 
B) -1.41°C 
C) -1.52°C 
D) -1.57°C 
E) -1.69°C 
A) -1.30°C 
B) -1.41°C 
C) -1.52°C 
D) -1.57°C 
E) -1.69°C

Exam 12: Physical Properties of Solutions

List the following solutions in order of increasing boiling point: 0.15m NaI, 0.10m K3PO4, 0.20 ethylene glycol

The osmotic pressure of a 0.010 M MgSO4 solution at 25°C is 0.318 atm.Calculate i, the van't Hoff factor, for this MgSO4 solution.

Calculate the molality of a 15.0% by mass solution of MgCl2 in H2O.The density of this solution is 1.127 g/mL.

What is the mass % of K2SO4 in an aqueous solution that has a mole fraction of K2SO4, X = 0.350?

For water Kf = 1.86°C/m.Therefore, the freezing points of 1.0 M aqueous KCl and C2H5OH (ethanol)solutions are the same.

A saturated solution

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

An endothermic solution process is described by which of the following?

What is the freezing point of a solution that contains 10.0 g of glucose (C6H12O6)in 100.g of H2O? Kf for water is 1.86°C/m.

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 freezing point of an aqueous solution of a nonvolatile solute that has a boiling point of 102.5°C? For water Kf = 1.86°C/m and Kb = 0.52°C/m.

Calculate the approximate freezing point of a solution made from 21.0 g NaCl and 1.00 × 102 g of H2O.[Kf of water is 1.86°C/m.]

What is the mole fraction of NaOH in a 32.0 % by mass NaOH aqueous solution?

The term "proof" is defined as twice the percent by volume of pure ethanol in solution.A solution that is 95% ethanol is 190 proof.What is the molarity of ethanol in a 92-proof ethanol/water solution? (Given: density of ethanol = 0.80 g/cm3; density of water = 1.0 g/cm3)

An exothermic solution process is described by which of the following?

A 100.mL sample of water is taken from the Great Salt Lake, and the water is allowed to evaporate.The salts that remain (mostly NaCl)have a mass of 31.9 g Calculate the original concentration of NaCl, in g per liter, in each water sample.

An aqueous fructose solution having a density of 1.049 g/cm3 is found to have an osmotic pressure of 17.0 atm at 25°C.Find the temperature at which this solution freezes.[Given: for water Kf = 1.86 °C/m; molecular mass of fructose = 180.16 g/mol]

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 Orbitals

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 Metal Chemistry and Coordination Compounds

Organic Chemistry

Synthetic and Natural Organic Polymers

Filters

List the following solutions in order of increasing boiling point: 0.15m NaI, 0.10m K₃PO₄, 0.20 ethylene glycol

The osmotic pressure of a 0.010 M MgSO₄ solution at 25°C is 0.318 atm.Calculate i, the van't Hoff factor, for this MgSO₄ solution.

Calculate the molality of a 15.0% by mass solution of MgCl₂ in H₂O.The density of this solution is 1.127 g/mL.

What is the mass % of K₂SO₄ in an aqueous solution that has a mole fraction of K₂SO₄, X = 0.350?

For water K_f = 1.86°C/m.Therefore, the freezing points of 1.0 M aqueous KCl and C₂H₅OH (ethanol)solutions are the same.

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 °C/m)

What is the freezing point of a solution that contains 10.0 g of glucose (C₆H₁₂O₆)in 100.g of H₂O? K_f for water is 1.86°C/m.

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 freezing point of an aqueous solution of a nonvolatile solute that has a boiling point of 102.5°C? For water K_f = 1.86°C/m and K_b = 0.52°C/m.

Calculate the approximate freezing point of a solution made from 21.0 g NaCl and 1.00 × 10² g of H₂O.[K_f of water is 1.86°C/m.]

The term "proof" is defined as twice the percent by volume of pure ethanol in solution.A solution that is 95% ethanol is 190 proof.What is the molarity of ethanol in a 92-proof ethanol/water solution? (Given: density of ethanol = 0.80 g/cm³; density of water = 1.0 g/cm³)

An aqueous fructose solution having a density of 1.049 g/cm³ is found to have an osmotic pressure of 17.0 atm at 25°C.Find the temperature at which this solution freezes.[Given: for water K_f = 1.86 °C/m; molecular mass of fructose = 180.16 g/mol]