Question 1

Which of the following concentration units will not change with temperature: molarity, percent mass, mole fraction, and molality.

Accepted Answer

Percent mass, mole f

Question 2

A solution of carbon tetrachloride in benzene, C6H6, at 20°C has a total vapor pressure of 78.50 mmHg. (Assume that this solution is ideal.)The vapor pressure of pure benzene at this temperature is 74.61 mmHg and its density is 0.87865 g/cm3; the vapor pressure of pure carbon tetrachloride is 91.32 mmHg and its density is 1.5940 g/cm3. What percentage of the volume of this solution is due to carbon tetrachloride? (Hint: assume that you have 1.000 L of solution.)

Accepted Answer

A) 75.2% 
B) 76.7% 
C) 14.3% 
D) 24.8% 
E) 23.3% 
A) 75.2% 
B) 76.7% 
C) 14.3% 
D) 24.8% 
E) 23.3%

Question 3

The solubility of a solid always increases with increasing solvent temperature.

Accepted Answer

A) True 
 B)False

Question 4

What is the freezing point of a solution prepared from 50.0 g ethylene glycol (C2H6O2)and 85.0 g H2O? Kf of water is 1.86°C/m.

Accepted Answer

A) 17.6°C 
B) -176°C 
C) -1.50°C 
D) 1.50°C 
E) -17.6°C 
A) 17.6°C 
B) -176°C 
C) -1.50°C 
D) 1.50°C 
E) -17.6°C

Question 5

Which of the following aqueous solutions has the highest osmotic pressure at 25°C?

Accepted Answer

A) 0.2 M KBr 
B) 0.2 M ethanol 
C) 0.2 M Na2SO4 
D) 0.2 M KCl 
A) 0.2 M KBr 
B) 0.2 M ethanol 
C) 0.2 M Na2SO4 
D) 0.2 M KCl

Question 6

Consider a solution made from a nonvolatile solute and a volatile solvent. Which statement is true?

Accepted Answer

A) The vapor pressure of the solution is always greater than the vapor pressure of the pure solvent. 
B) The boiling point of the solution is always greater than the boiling point of the pure solvent. 
C) The freezing point of the solution is always greater than the freezing point of the pure solvent. 
A) The vapor pressure of the solution is always greater than the vapor pressure of the pure solvent. 
B) The boiling point of the solution is always greater than the boiling point of the pure solvent. 
C) The freezing point of the solution is always greater than the freezing point of the pure solvent.

Question 7

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

Question 8

What is the osmotic pressure of a 0.25 M solution of sucrose at 37°C? (R = 0.0821 L.atm/K.mol)

Accepted Answer

A) 6.6 * 10-5 atm 
B) 0.76 atm 
C) 6.4 atm 
D) 100 atm 
E) 940 atm 
A) 6.6 * 10-5 atm 
B) 0.76 atm 
C) 6.4 atm 
D) 100 atm 
E) 940 atm

Question 9

It has been suggested that gold might be recovered from seawater.If seawater contains about 4.0 * 10-9 g/L of dissolved gold, how many liters of seawater would have to be processed to get 1.00 ounce of gold? (1 oz = 28.4 g)

Accepted Answer

7.1 * 10<s

Which of the following concentration units will not change with temperature: molarity, percent mass, mole fraction, and molality.

The solubility of a solid always increases with increasing solvent temperature.

What is the freezing point of a solution prepared from 50.0 g ethylene glycol (C₂H₆O₂)and 85.0 g H₂O? K_f of water is 1.86°C/m.

Which of the following aqueous solutions has the highest osmotic pressure at 25°C?

Consider a solution made from a nonvolatile solute and a volatile solvent. Which statement is true?

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]

What is the osmotic pressure of a 0.25 M solution of sucrose at 37°C? (R = 0.0821 L.atm/K.mol)

It has been suggested that gold might be recovered from seawater.If seawater contains about 4.0 * 10^-9 g/L of dissolved gold, how many liters of seawater would have to be processed to get 1.00 ounce of gold? (1 oz = 28.4 g)

Chemistry: The Study of Change

Atoms, Molecules, and Ions

Mass Relationships in Chemical Reactions

Reactions in Aqueous Solution

Gases

Thermo-Chemistry

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

Chemistry in the Atmosphere

Entropy, Free Energy, and Equilibrium

Electrochemistry

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Transition Metal Chemistry and Coordination Compounds

Nuclear Chemistry

Organic Chemistry

Synthetic and Natural Organic Polymers

Filters

Exam 12: Physical Properties of Solutions

Which of the following concentration units will not change with temperature: molarity, percent mass, mole fraction, and molality.

The solubility of a solid always increases with increasing solvent temperature.

What is the freezing point of a solution prepared from 50.0 g ethylene glycol (C2H6O2)and 85.0 g H2O? Kf of water is 1.86°C/m.

Which of the following aqueous solutions has the highest osmotic pressure at 25°C?

Consider a solution made from a nonvolatile solute and a volatile solvent. Which statement is true?

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]

What is the osmotic pressure of a 0.25 M solution of sucrose at 37°C? (R = 0.0821 L.atm/K.mol)

It has been suggested that gold might be recovered from seawater.If seawater contains about 4.0 * 10-9 g/L of dissolved gold, how many liters of seawater would have to be processed to get 1.00 ounce of gold? (1 oz = 28.4 g)

Chemistry: The Study of Change

Atoms, Molecules, and Ions

Mass Relationships in Chemical Reactions

Reactions in Aqueous Solution

Gases

Thermo-Chemistry

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

Chemistry in the Atmosphere

Entropy, Free Energy, and Equilibrium

Electrochemistry

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Transition Metal Chemistry and Coordination Compounds

Nuclear Chemistry

Organic Chemistry

Synthetic and Natural Organic Polymers

Filters

What is the freezing point of a solution prepared from 50.0 g ethylene glycol (C₂H₆O₂)and 85.0 g H₂O? K_f of water is 1.86°C/m.

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]

It has been suggested that gold might be recovered from seawater.If seawater contains about 4.0 * 10^-9 g/L of dissolved gold, how many liters of seawater would have to be processed to get 1.00 ounce of gold? (1 oz = 28.4 g)