Question 1

Which pair of dispersed phases and dispersing media can never form a colloid?

Accepted Answer

A)  solid and gas 
B)  liquid and gas 
C)  solid and solid 
D)  liquid and liquid 
E)  gas and gas 
A)  solid and gas 
B)  liquid and gas 
C)  solid and solid 
D)  liquid and liquid 
E)  gas and gas

Question 2

Which process defines how an ionic compound breaks apart into its constituent ions upon dissolution?

Accepted Answer

A)  electrolysis 
B)  dissociation 
C)  division 
D)  ionization 
E)  decomposition 
A)  electrolysis 
B)  dissociation 
C)  division 
D)  ionization 
E)  decomposition

Question 3

________ colloids are solutions containing extremely large molecules such as proteins. These colloids are also termed "water loving".

Accepted Answer

A)  Hydrophobic 
B)  Aerosol 
C)  Hydrophilic 
D)  Emulsion 
E)  Solid sol 
A)  Hydrophobic 
B)  Aerosol 
C)  Hydrophilic 
D)  Emulsion 
E)  Solid sol

Question 4

The ________ ________ is the scattered light that is caused by the dispersed phase of a colloid that has a beam of light passed through it.

Accepted Answer

The answer of The ________ ________ is the scattered light...

Question 5

Cadmium bromide is used in photography and lithography. What is the molality of a solution prepared by dissolving 45.38 g of CdBr2 in 375.0 g of water?

Accepted Answer

A)  0.03035 m 
B)  0.01600 m 
C)  0.1210 m 
D)  0.4446 m 
E)  16.00 m 
A)  0.03035 m 
B)  0.01600 m 
C)  0.1210 m 
D)  0.4446 m 
E)  16.00 m

Question 6

What is the molarity of a solution that is 26.0% by mass phosphoric acid (H3PO4) and that has a density of 1.155 g/mL?

Accepted Answer

A)  2.30 × 10 -3 M 
B)  2.30 M 
C)  2.65 M 
D)  3.06 M 
E)  0.265 M 
A)  2.30 × 10 -3 M 
B)  2.30 M 
C)  2.65 M 
D)  3.06 M 
E)  0.265 M

Question 7

What mass of water is required to dissolve 27.8 g of ammonium nitrate NH4NO3 in order to prepare a 0.452 m solution?

Accepted Answer

A)  0.0615 kg 
B)  0.100 kg 
C)  0.177 kg 
D)  0.768 kg 
E)  1.30 kg 
A)  0.0615 kg 
B)  0.100 kg 
C)  0.177 kg 
D)  0.768 kg 
E)  1.30 kg

Question 8

What is the name given to a solution that contains the maximum amount of solute that will dissolve in a solvent at a specific temperature?

Accepted Answer

A)  Saturated 
B)  Unsaturated 
C)  Solvent 
D)  Solute 
E)  Supersaturated 
A)  Saturated 
B)  Unsaturated 
C)  Solvent 
D)  Solute 
E)  Supersaturated

Question 9

From the following list of aqueous solutions and water, select the one with the highest boiling point.

Accepted Answer

A)  1.0 M KNO3 
B)  0.75 M NaCl 
C)  0.75 M CuCl2 
D)  2.0 M C12H22O11 (sucrose) 
E)  pure water 
A)  1.0 M KNO3 
B)  0.75 M NaCl 
C)  0.75 M CuCl2 
D)  2.0 M C12H22O11 (sucrose) 
E)  pure water

Question 10

When 12.1 g of the sugar sucrose (a nonelectrolyte) are dissolved in exactly 800 g of water, the solution has a freezing point of -0.082°C. What is the molar mass of sucrose? (Kf of water is 1.86°C/m.)

Accepted Answer

A)  426 g/mol 
B)  99.2 g/mol 
C)  178 g/mol 
D)  266 g/mol 
E)  343 g/mol 
A)  426 g/mol 
B)  99.2 g/mol 
C)  178 g/mol 
D)  266 g/mol 
E)  343 g/mol

Question 11

What volume of ethanol (density = 0.7893 g/cm3) should be added to 450. mL of water in order to have a solution that freezes at -15.0°C? Assume the density of water is 1.0 g/mL. (For water, Kf = 1.86 °C/m.)

Accepted Answer

A)  371 mL 
B)  470 mL 
C)  212 mL 
D)  132 mL 
E)  167 mL 
A)  371 mL 
B)  470 mL 
C)  212 mL 
D)  132 mL 
E)  167 mL

Question 12

What is defined as the selective passage of solvent molecules through a porous membrane from a more dilute solution to a more concentrated solution?

Accepted Answer

A)  Permeability 
B)  Semipermeability 
C)  Osmotic pressure 
D)  Osmosis 
E)  Vapor pressure 
A)  Permeability 
B)  Semipermeability 
C)  Osmotic pressure 
D)  Osmosis 
E)  Vapor pressure

Question 13

What is defined as a solution that has a lower concentration of dissolved substances than plasma?

Accepted Answer

A)  Hypotonic 
B)  Hypertonic 
C)  Aplasmic 
D)  Plasmic 
E)  Colloidal 
A)  Hypotonic 
B)  Hypertonic 
C)  Aplasmic 
D)  Plasmic 
E)  Colloidal

Question 14

________ is the term used for a water fearing substance.

Accepted Answer

The answer of ________ is the term used for a...

Question 15

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

Accepted Answer

A) True 
 B)False

Question 16

Dissolving a solute such as KOH in a solvent such as water results in

Accepted Answer

A)  an increase in the melting point of the liquid. 
B)  a decrease in the boiling point of the liquid. 
C)  a decrease in the vapor pressure of the liquid. 
D)  no change in the boiling point of the liquid. 
A)  an increase in the melting point of the liquid. 
B)  a decrease in the boiling point of the liquid. 
C)  a decrease in the vapor pressure of the liquid. 
D)  no change in the boiling point of the liquid.

Question 17

What is the vapor pressure above a solution prepared by dissolving 0.500 mol of a nonvolatile solute in 275 g of hexane (86.18 g/mol) at 49.6°C? P°hexane = 400.0 torr at 49.6°C.

Accepted Answer

A)  54 torr 
B)  154 torr 
C)  246 torr 
D)  346 torr 
E)  400. torr 
A)  54 torr 
B)  154 torr 
C)  246 torr 
D)  346 torr 
E)  400. torr

Question 18

Which law describes the quantitative relationship between the solubility of a gas and its partial pressure?

Accepted Answer

A)  Entropy 
B)  Henry's law 
C)  Enthalpy 
D)  Boyle's law 
E)  Avogadro's law 
A)  Entropy 
B)  Henry's law 
C)  Enthalpy 
D)  Boyle's law 
E)  Avogadro's law

Question 19

What volume of water (d = 1.00 g/mL) should be added to 600. mL of ethanol in order to have a solution that boils at 95.0°C? (For ethanol, Kb = 1.22 °C/m; density = 0.789 g/cm3; boiling point = 78.4°C)

Accepted Answer

A)  186 mL 
B)  245 mL 
C)  518 mL 
D)  116 mL 
E)  322 mL 
A)  186 mL 
B)  245 mL 
C)  518 mL 
D)  116 mL 
E)  322 mL

Question 20

Barbiturates are synthetic drugs used as sedatives and hypnotics. Barbital (184.2 g/mol) is one of the simplest of these drugs. What is the boiling point of a solution prepared by dissolving 42.5 g of barbital in 825 g of acetic acid? (For pure acetic acid, Kb = 3.07°C/m; boiling point of pure acetic acid = 117.9°C)

Accepted Answer

A)  117.0°C 
B)  117.7°C 
C)  118.1°C 
D)  118.8°C 
E)  120.4°C 
A)  117.0°C 
B)  117.7°C 
C)  118.1°C 
D)  118.8°C 
E)  120.4°C

Exam 13: Physical Properties of Solutions

Which pair of dispersed phases and dispersing media can never form a colloid?

Which process defines how an ionic compound breaks apart into its constituent ions upon dissolution?

________ colloids are solutions containing extremely large molecules such as proteins. These colloids are also termed "water loving".

The ________ ________ is the scattered light that is caused by the dispersed phase of a colloid that has a beam of light passed through it.

Cadmium bromide is used in photography and lithography. What is the molality of a solution prepared by dissolving 45.38 g of CdBr2 in 375.0 g of water?

What is the molarity of a solution that is 26.0% by mass phosphoric acid (H3PO4) and that has a density of 1.155 g/mL?

What mass of water is required to dissolve 27.8 g of ammonium nitrate NH4NO3 in order to prepare a 0.452 m solution?

What is the name given to a solution that contains the maximum amount of solute that will dissolve in a solvent at a specific temperature?

From the following list of aqueous solutions and water, select the one with the highest boiling point.

When 12.1 g of the sugar sucrose (a nonelectrolyte) are dissolved in exactly 800 g of water, the solution has a freezing point of -0.082°C. What is the molar mass of sucrose? (Kf of water is 1.86°C/m.)

What volume of ethanol (density = 0.7893 g/cm3) should be added to 450. mL of water in order to have a solution that freezes at -15.0°C? Assume the density of water is 1.0 g/mL. (For water, Kf = 1.86 °C/m.)

What is defined as the selective passage of solvent molecules through a porous membrane from a more dilute solution to a more concentrated solution?

What is defined as a solution that has a lower concentration of dissolved substances than plasma?

________ is the term used for a water fearing substance.

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

Dissolving a solute such as KOH in a solvent such as water results in

What is the vapor pressure above a solution prepared by dissolving 0.500 mol of a nonvolatile solute in 275 g of hexane (86.18 g/mol) at 49.6°C? P°hexane = 400.0 torr at 49.6°C.

Which law describes the quantitative relationship between the solubility of a gas and its partial pressure?

What volume of water (d = 1.00 g/mL) should be added to 600. mL of ethanol in order to have a solution that boils at 95.0°C? (For ethanol, Kb = 1.22 °C/m; density = 0.789 g/cm3; boiling point = 78.4°C)

Chemistry: the Central Science

Atoms, Molecules, and Ions

Stoichiometry: Ratios of Combination

Reactions in Aqueous Solutions

Thermochemistry

Quantum Theory and the Electronic Structure of Atoms

Electron Configuration and the Periodic Table

Chemical Bonding I: Basic Concepts

Chemical Bonding II: Molecular Geometry and Bonding Theories

Gases

Intermolecular Forces and the Physical Properties of Liquids and Solids

Modern Materials

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Entropy, Free Energy, and Equilibrium

Electrochemistry

Nuclear Chemistry

Environmental Chemistry

Coordination Chemistry

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Organic Chemistry

Filters

The is the scattered light that is caused by the dispersed phase of a colloid that has a beam of light passed through it.

Cadmium bromide is used in photography and lithography. What is the molality of a solution prepared by dissolving 45.38 g of CdBr₂ in 375.0 g of water?

What is the molarity of a solution that is 26.0% by mass phosphoric acid (H₃PO₄) and that has a density of 1.155 g/mL?

What mass of water is required to dissolve 27.8 g of ammonium nitrate NH₄NO₃ in order to prepare a 0.452 m solution?

When 12.1 g of the sugar sucrose (a nonelectrolyte) are dissolved in exactly 800 g of water, the solution has a freezing point of -0.082°C. What is the molar mass of sucrose? (K_f of water is 1.86°C/m.)

What volume of ethanol (density = 0.7893 g/cm³) should be added to 450. mL of water in order to have a solution that freezes at -15.0°C? Assume the density of water is 1.0 g/mL. (For water, K_f = 1.86 °C/m.)

What is the vapor pressure above a solution prepared by dissolving 0.500 mol of a nonvolatile solute in 275 g of hexane (86.18 g/mol) at 49.6°C? P°_hexane= 400.0 torr at 49.6°C.

What volume of water (d = 1.00 g/mL) should be added to 600. mL of ethanol in order to have a solution that boils at 95.0°C? (For ethanol, K_b = 1.22 °C/m; density = 0.789 g/cm³; boiling point = 78.4°C)