Question 1

The molecule drawn below is Vitamin D, Calciferol. Would you predict this molecule to be more soluble in water or body fat and explain why?

Accepted Answer

More soluble in fat, as it has only one small polar group (OH). The rest of the molecule is non-polar and would therefore more readily dissolve in fat.

Question 2

Sea water has about 0.46 moles NaCl and 0.065 moles of MgCl2 in every litre. What is the vapour pressure of sea water at 30?C if pure water would have a vapour pressure of 33.2 mm Hg? (Assume there are 1000 grams of water in 1 litre of sea water.)

Accepted Answer

A)  33.2 mm Hg 
B)  32.5 mm Hg 
C)  37.0 mm Hg 
D)  30.3 mm Hg 
E)  32.9 mm Hg 
A)  33.2 mm Hg 
B)  32.5 mm Hg 
C)  37.0 mm Hg 
D)  30.3 mm Hg 
E)  32.9 mm Hg B

Question 3

Benzene and water are immiscible, forming two separate layers when mixed. Samples of the compounds below are shaken in a mixture of benzene and water. Which of the following compounds would you expect to be found in the benzene layer?

Accepted Answer

A)  2 and 4 
B)  2 and 3 
C)  1 and 4 
D)  1 and 3 
E)  1, 3 and 4 
A)  2 and 4 
B)  2 and 3 
C)  1 and 4 
D)  1 and 3 
E)  1, 3 and 4 D

Question 4

Automobile coolant is about 50% by mass ethylene glycol in water. The line structure of ethylene glycol is shown below:   What is the normal boiling point of this solution if Kb for water = 0.512 ˚Cm-1?

Accepted Answer

Question 5

What is the mass percent of an aqueous solution that is 0.569 m CaCl2 (solution density 1.05 g/ml)?

Accepted Answer

A)  5.94 % 
B)  6.32 % 
C)  0.06 % 
D)  5.94 x 10-2 % 
E)  6.32 x10-2% 
A)  5.94 % 
B)  6.32 % 
C)  0.06 % 
D)  5.94 x 10-2 % 
E)  6.32 x10-2%

Question 6

Which of the following molecules would be suitable surfactants?
1)  
2)  
3)  
4)

Accepted Answer

A)  all 
B)  1 and 2 
C)  1 and 3 
D)  2 and 4 
E)  1 and 4 
A)  all 
B)  1 and 2 
C)  1 and 3 
D)  2 and 4 
E)  1 and 4

Question 7

What is the freezing point of a solution made from mixing 39 grams of sugar (MM = 180 g/mol) with 310 grams of water? (Kf = 1.85 ˚Cm-1)?

Accepted Answer

Question 8

What is the mole fraction of ethyl alcohol (C2H6O, density = 0.79 g/ml) in water for a solution made from equal volumes of each?

Accepted Answer

A)  0.235 
B)  0.122 
C)  0.756 
D)  1.11 
E)  17.9 
A)  0.235 
B)  0.122 
C)  0.756 
D)  1.11 
E)  17.9

Question 9

Determine the mole fraction of a solution made from mixing 39 grams of sugar (MM = 180 g/mol) with 310 grams of water.

Accepted Answer

The answer of Determine the mole fraction of a solution...

Question 10

When both solid Na metal and solid NaCl are added to water a colourless solution develops. How are these processes different?

Accepted Answer

Na(s) reacts with water, it is oxidized

Question 11

What is the molality of a radiator solution made by mixing equal volumes of ethylene glycol C2H6O2, (density = 1.11 g/ml) and water?

Accepted Answer

A)  17.9 m 
B)  11.1 m 
C)  1.79 m 
D)  4.60 m 
E)  17.9 M 
A)  17.9 m 
B)  11.1 m 
C)  1.79 m 
D)  4.60 m 
E)  17.9 M

Question 12

Work with and interconvert concentration units (mass %, molarity, molality, mole fraction, ppm, and ppb).

Accepted Answer

The solvent determines the pha

Question 13

A 7.85 g sample of a compound with an empirical formula C1H1 is dissolved in 172 g of benzene. The freezing point of the solution is 1.50$\degree$C below that of pure benzene. Assuming that the compound does not dissociate, what is the molar mass and molecular formula of this compound? The freezing point depression constant for benzene is Kf = 5.12 $\degree$C/m.

Accepted Answer

MM = 156,

Question 14

The boiling point of toluene is 110oC and that of benzene is 80oC. The vapour above a solution that has mole fraction of benzene = 0.5,

Accepted Answer

A)  has mole fraction toluene in 0.5. 
B)  has mole fraction of toluene less than 0.5. 
C)  has mole fraction of toluene greater than 0.5. 
D)  is pure benzene. 
E)  is pure toluene. 
A)  has mole fraction toluene in 0.5. 
B)  has mole fraction of toluene less than 0.5. 
C)  has mole fraction of toluene greater than 0.5. 
D)  is pure benzene. 
E)  is pure toluene.

Question 15

Why was the concentration unit of molality developed?

Accepted Answer

A)  Molarity had not been developed yet. 
B)  Morality had not been developed yet. 
C)  Solution volumes changed with temperature. 
D)  Solution volumes changed with pressure. 
E)  Solution masses changed upon mixing. 
A)  Molarity had not been developed yet. 
B)  Morality had not been developed yet. 
C)  Solution volumes changed with temperature. 
D)  Solution volumes changed with pressure. 
E)  Solution masses changed upon mixing.

Question 16

Fahrenheit developed his temperature scale where he set zero degrees as the freezing point for a salt-water solution. What is the concentration of this salt solution in molality (assume NaCl in water)? (Tf = 1.86 ˚C/m)

Accepted Answer

4.78 molal; be caref

Question 17

If you have ever made homemade ice cream you would know that you need to add salt to the ice surrounding the container that you make the ice cream in. By adding the salt to the ice it lowers the temperature of the ice. Explain what is happening to the salt when added to the ice and what you can say about the heat of solvation for sodium chloride.

Accepted Answer

The first process that will occur is tha

Question 18

How can mercury be used in dental fillings?

Accepted Answer

A)  It is a solid at body temperature. 
B)  It forms an amalgam with your tooth enamel. 
C)  It forms an amalgam with other metals. 
D)  It is an insoluble salt in your mouth. 
E)  It forms a compound called brass with copper. 
A)  It is a solid at body temperature. 
B)  It forms an amalgam with your tooth enamel. 
C)  It forms an amalgam with other metals. 
D)  It is an insoluble salt in your mouth. 
E)  It forms a compound called brass with copper.

Question 19

Which of the following are colloidal suspensions: fog, milk, sugar in water, salt in water, styrofoam?

Accepted Answer

A)  fog and milk 
B)  milk, sugar in water, styrofoam 
C)  fog, sugar in water styrofoam 
D)  fog, milk, styrofoam 
E)  fog and styrofoam 
A)  fog and milk 
B)  milk, sugar in water, styrofoam 
C)  fog, sugar in water styrofoam 
D)  fog, milk, styrofoam 
E)  fog and styrofoam

Question 20

Carbon dioxide and O2 are non-polar molecules. Can you provide some rational why CO2 dissolves so much more in water than O2?

Accepted Answer

A)  CO2 can hydrogen bond and O2 cannot. 
B)  CO2 reacts with water and O2 does not. 
C)  O2 reacts with water and CO2 does not. 
D)  CO2 forms a solid with water. 
E)  Water decomposes to O2. 
A)  CO2 can hydrogen bond and O2 cannot. 
B)  CO2 reacts with water and O2 does not. 
C)  O2 reacts with water and CO2 does not. 
D)  CO2 forms a solid with water. 
E)  Water decomposes to O2.

The molecule drawn below is Vitamin D, Calciferol. Would you predict this molecule to be more soluble in water or body fat and explain why?

Sea water has about 0.46 moles NaCl and 0.065 moles of MgCl₂ in every litre. What is the vapour pressure of sea water at 30?C if pure water would have a vapour pressure of 33.2 mm Hg? (Assume there are 1000 grams of water in 1 litre of sea water.)

Benzene and water are immiscible, forming two separate layers when mixed. Samples of the compounds below are shaken in a mixture of benzene and water. Which of the following compounds would you expect to be found in the benzene layer?

Automobile coolant is about 50% by mass ethylene glycol in water. The line structure of ethylene glycol is shown below: What is the normal boiling point of this solution if K_b for water = 0.512 ˚Cm^-1?

What is the mass percent of an aqueous solution that is 0.569 m CaCl₂ (solution density 1.05 g/ml)?

Which of the following molecules would be suitable surfactants? 1) 2) 3) 4)

What is the freezing point of a solution made from mixing 39 grams of sugar (MM = 180 g/mol) with 310 grams of water? (K_f = 1.85 ˚Cm^-1)?

What is the mole fraction of ethyl alcohol (C₂H₆O, density = 0.79 g/ml) in water for a solution made from equal volumes of each?

Determine the mole fraction of a solution made from mixing 39 grams of sugar (MM = 180 g/mol) with 310 grams of water.

When both solid Na metal and solid NaCl are added to water a colourless solution develops. How are these processes different?

What is the molality of a radiator solution made by mixing equal volumes of ethylene glycol C₂H₆O₂, (density = 1.11 g/ml) and water?

Work with and interconvert concentration units (mass %, molarity, molality, mole fraction, ppm, and ppb).

The boiling point of toluene is 110^oC and that of benzene is 80^oC. The vapour above a solution that has mole fraction of benzene = 0.5,

Why was the concentration unit of molality developed?

Fahrenheit developed his temperature scale where he set zero degrees as the freezing point for a salt-water solution. What is the concentration of this salt solution in molality (assume NaCl in water)? (T_f = 1.86 ˚C/m)

How can mercury be used in dental fillings?

Which of the following are colloidal suspensions: fog, milk, sugar in water, salt in water, styrofoam?

Carbon dioxide and O₂ are non-polar molecules. Can you provide some rational why CO₂ dissolves so much more in water than O₂?

Fundamental Concepts of Chemistry

The Behaviour of Gases

Energy and Its Conservation

Atoms and Light

Atomic Energies and Periodicity

Fundamentals of Chemical Bonding

Theories of Chemical Bonding

Effects of Intermolecular Forces

Organic Chemistrystructure

Organic Chemistryreactions

Spontaneity of Chemical Processes

Kinetics: Mechanisms and Rates of Reactions

Principles of Chemical Equilibrium

Aqueous Acidbase Equilibria

Applications of Aqueous Equilibria

Electron Transfer Reactions

Macromolecules

The Transition Metals

The Main Group Elements

Nuclear Chemistry and Radiochemistry

Filters

Exam 9: Properties of Solutions

The molecule drawn below is Vitamin D, Calciferol. Would you predict this molecule to be more soluble in water or body fat and explain why?

Sea water has about 0.46 moles NaCl and 0.065 moles of MgCl2 in every litre. What is the vapour pressure of sea water at 30?C if pure water would have a vapour pressure of 33.2 mm Hg? (Assume there are 1000 grams of water in 1 litre of sea water.)

Benzene and water are immiscible, forming two separate layers when mixed. Samples of the compounds below are shaken in a mixture of benzene and water. Which of the following compounds would you expect to be found in the benzene layer?

Automobile coolant is about 50% by mass ethylene glycol in water. The line structure of ethylene glycol is shown below: What is the normal boiling point of this solution if Kb for water = 0.512 ˚Cm-1?

What is the mass percent of an aqueous solution that is 0.569 m CaCl2 (solution density 1.05 g/ml)?

Which of the following molecules would be suitable surfactants? 1) 2) 3) 4)

What is the freezing point of a solution made from mixing 39 grams of sugar (MM = 180 g/mol) with 310 grams of water? (Kf = 1.85 ˚Cm-1)?

What is the mole fraction of ethyl alcohol (C2H6O, density = 0.79 g/ml) in water for a solution made from equal volumes of each?

Determine the mole fraction of a solution made from mixing 39 grams of sugar (MM = 180 g/mol) with 310 grams of water.

When both solid Na metal and solid NaCl are added to water a colourless solution develops. How are these processes different?

What is the molality of a radiator solution made by mixing equal volumes of ethylene glycol C2H6O2, (density = 1.11 g/ml) and water?

Work with and interconvert concentration units (mass %, molarity, molality, mole fraction, ppm, and ppb).

The boiling point of toluene is 110oC and that of benzene is 80oC. The vapour above a solution that has mole fraction of benzene = 0.5,

Why was the concentration unit of molality developed?

Fahrenheit developed his temperature scale where he set zero degrees as the freezing point for a salt-water solution. What is the concentration of this salt solution in molality (assume NaCl in water)? (Tf = 1.86 ˚C/m)

How can mercury be used in dental fillings?

Which of the following are colloidal suspensions: fog, milk, sugar in water, salt in water, styrofoam?

Carbon dioxide and O2 are non-polar molecules. Can you provide some rational why CO2 dissolves so much more in water than O2?

Fundamental Concepts of Chemistry

The Behaviour of Gases

Energy and Its Conservation

Atoms and Light

Atomic Energies and Periodicity

Fundamentals of Chemical Bonding

Theories of Chemical Bonding

Effects of Intermolecular Forces

Organic Chemistrystructure

Organic Chemistryreactions

Spontaneity of Chemical Processes

Kinetics: Mechanisms and Rates of Reactions

Principles of Chemical Equilibrium

Aqueous Acidbase Equilibria

Applications of Aqueous Equilibria

Electron Transfer Reactions

Macromolecules

The Transition Metals

The Main Group Elements

Nuclear Chemistry and Radiochemistry

Filters

Sea water has about 0.46 moles NaCl and 0.065 moles of MgCl₂ in every litre. What is the vapour pressure of sea water at 30?C if pure water would have a vapour pressure of 33.2 mm Hg? (Assume there are 1000 grams of water in 1 litre of sea water.)

Automobile coolant is about 50% by mass ethylene glycol in water. The line structure of ethylene glycol is shown below: What is the normal boiling point of this solution if K_b for water = 0.512 ˚Cm^-1?

What is the mass percent of an aqueous solution that is 0.569 m CaCl₂ (solution density 1.05 g/ml)?

What is the freezing point of a solution made from mixing 39 grams of sugar (MM = 180 g/mol) with 310 grams of water? (K_f = 1.85 ˚Cm^-1)?

What is the mole fraction of ethyl alcohol (C₂H₆O, density = 0.79 g/ml) in water for a solution made from equal volumes of each?

What is the molality of a radiator solution made by mixing equal volumes of ethylene glycol C₂H₆O₂, (density = 1.11 g/ml) and water?

The boiling point of toluene is 110^oC and that of benzene is 80^oC. The vapour above a solution that has mole fraction of benzene = 0.5,

Fahrenheit developed his temperature scale where he set zero degrees as the freezing point for a salt-water solution. What is the concentration of this salt solution in molality (assume NaCl in water)? (T_f = 1.86 ˚C/m)

Carbon dioxide and O₂ are non-polar molecules. Can you provide some rational why CO₂ dissolves so much more in water than O₂?