Question 1

would be present in 1 L of a 1 M glycerol solution?

Accepted Answer

A) 1 × 10⁶ 
B) 14 × 6.02 × 10²³ 
C) 92 × 6.02 × 10²³ 
D) 6.02 × 10²⁶ 
E) 6.02 × 10²³ 
A) 1 × 10⁶ 
B) 14 × 6.02 × 10²³ 
C) 92 × 6.02 × 10²³ 
D) 6.02 × 10²⁶ 
E) 6.02 × 10²³

Question 2

A 0.01 M solution of a substance has a pH of 2. What can you conclude about this substance?

Accepted Answer

A) It is a strong acid that ionizes completely in water. 
B) It is a strong base that ionizes completely in water. 
C) It is a weak acid. 
D) It is a weak base. 
E) It is neither an acid nor a base. 
A) It is a strong acid that ionizes completely in water. 
B) It is a strong base that ionizes completely in water. 
C) It is a weak acid. 
D) It is a weak base. 
E) It is neither an acid nor a base.

Question 3

Which of the following statements is true about buffer solutions?

Accepted Answer

A) They maintain a constant pH when bases are added to them but not when acids are added to them. 
B) They maintain a constant pH when acids are added to them but not when bases are added to them. 
C) They maintain a relatively constant pH of approximately 7 when either acids or bases are added to them. 
D) They maintain a relatively constant pH when either acids or bases are added to them. 
E) They are found only in living systems and biological fluids. 
A) They maintain a constant pH when bases are added to them but not when acids are added to them. 
B) They maintain a constant pH when acids are added to them but not when bases are added to them. 
C) They maintain a relatively constant pH of approximately 7 when either acids or bases are added to them. 
D) They maintain a relatively constant pH when either acids or bases are added to them. 
E) They are found only in living systems and biological fluids.

Question 4

In a single molecule of water, two hydrogen atoms are bonded to a single oxygen atom by

Accepted Answer

A) hydrogen bonds. 
B) nonpolar covalent bonds. 
C) polar covalent bonds. 
D) ionic bonds. 
E) van der Waals interactions. 
A) hydrogen bonds. 
B) nonpolar covalent bonds. 
C) polar covalent bonds. 
D) ionic bonds. 
E) van der Waals interactions.

Question 5

Use the following information to answer the questions below.
You live in Atlantic Canada and you are Skyping a friend in Manitoba. You are both complaining about the weather as both regions are being subjected to the same arctic air mass. As you discuss it, however, it becomes clear that she is experiencing a bitter cold that you are not. You realize that you had pretty much the same conversation last summer when it was much hotter in Manitoba than at home.
-Many mammals control their body temperature by sweating. Which property of water is most directly responsible for the ability of sweat to lower body temperature?

Accepted Answer

A) water's change in density when it condenses 
B) water's ability to dissolve molecules in the air 
C) the release of heat by the formation of hydrogen bonds 
D) the absorption of heat by the breaking of hydrogen bonds 
E) water's high surface tension 
A) water's change in density when it condenses 
B) water's ability to dissolve molecules in the air 
C) the release of heat by the formation of hydrogen bonds 
D) the absorption of heat by the breaking of hydrogen bonds 
E) water's high surface tension

Question 6

Use the following figure to answer the questions below.
  
-How many grams of the compound in the figure above would be required to make 1 L of a 0.5 M solution? (carbon = 12, oxygen = 16, hydrogen = 1)

Accepted Answer

A) 29 
B) 30 
C) 60 
D) 150 
E) 342 
A) 29 
B) 30 
C) 60 
D) 150 
E) 342

Question 7

Use the following information to answer the questions below.
You live in Atlantic Canada and you are Skyping a friend in Manitoba. You are both complaining about the weather as both regions are being subjected to the same arctic air mass. As you discuss it, however, it becomes clear that she is experiencing a bitter cold that you are not. You realize that you had pretty much the same conversation last summer when it was much hotter in Manitoba than at home.
-The bonds that are broken when water vaporizes are

Accepted Answer

A) ionic bonds. 
B) hydrogen bonds between water molecules. 
C) covalent bonds between atoms within water molecules. 
D) polar covalent bonds. 
E) nonpolar covalent bonds. 
A) ionic bonds. 
B) hydrogen bonds between water molecules. 
C) covalent bonds between atoms within water molecules. 
D) polar covalent bonds. 
E) nonpolar covalent bonds.

Question 8

Coastal regions tend to have more moderate climates than land-locked areas due to the

Accepted Answer

A) high specific heat of water. 
B) heat of vaporization of water. 
C) amount of solutes in ocean water. 
D) high thermal energy in the atmosphere. 
E) latitude on which it is dependent; landmass has no effect. 
A) high specific heat of water. 
B) heat of vaporization of water. 
C) amount of solutes in ocean water. 
D) high thermal energy in the atmosphere. 
E) latitude on which it is dependent; landmass has no effect.

Question 9

One idea to mitigate the effects of burning fossil fuels on atmospheric CO₂ concentrations is to pipe liquid CO₂ into the ocean at depths of 2500 feet or greater. At the high pressures at such depths, CO₂ is heavier than water. What potential effects might result from implementing such a scheme?

Accepted Answer

A) increased photosynthetic carbon fixation because of the increased dissolved carbon dioxide in the deep water 
B) increased carbonate concentrations in the deep waters 
C) reduced growth of corals from a change in the carbonate-bicarbonate equilibrium 
D) no effect because carbon dioxide is not soluble in water 
E) both increased acidity of the deep waters and changes in the growth of bottom-dwelling organisms with calcium carbonate shells 
A) increased photosynthetic carbon fixation because of the increased dissolved carbon dioxide in the deep water 
B) increased carbonate concentrations in the deep waters 
C) reduced growth of corals from a change in the carbonate-bicarbonate equilibrium 
D) no effect because carbon dioxide is not soluble in water 
E) both increased acidity of the deep waters and changes in the growth of bottom-dwelling organisms with calcium carbonate shells

Question 10

One of the buffers that contribute to pH stability in human blood is carbonic acid (H₂CO₃). Carbonic acid is a weak acid that dissociates into a bicarbonate ion (HCO₃⁻)and a hydrogen ion (H⁺). Thus, H₂CO₃ ↔ HCO₃⁻ + H⁺ If the pH of the blood drops, one would expect

Accepted Answer

A) a decrease in the concentration of H₂CO₃ and an increase in the concentration of HCO₃⁻. 
B) the concentration of hydroxide ion (OH⁻)to increase. 
C) the concentration of bicarbonate ion (HCO₃⁻)to increase. 
D) the HCO₃⁻ to act as a base and remove excess H⁺ with the formation of H₂CO₃. 
E) the HCO₃⁻ to act as an acid and remove excess H⁺ with the formation of H₂CO₃. 
A) a decrease in the concentration of H₂CO₃ and an increase in the concentration of HCO₃⁻. 
B) the concentration of hydroxide ion (OH⁻)to increase. 
C) the concentration of bicarbonate ion (HCO₃⁻)to increase. 
D) the HCO₃⁻ to act as a base and remove excess H⁺ with the formation of H₂CO₃. 
E) the HCO₃⁻ to act as an acid and remove excess H⁺ with the formation of H₂CO₃.

Question 11

Use the following information to answer the questions below.
You live in Atlantic Canada and you are Skyping a friend in Manitoba. You are both complaining about the weather as both regions are being subjected to the same arctic air mass. As you discuss it, however, it becomes clear that she is experiencing a bitter cold that you are not. You realize that you had pretty much the same conversation last summer when it was much hotter in Manitoba than at home.
-The best explanation for this difference is that

Accepted Answer

A) your climate is moderated by the Atlantic Ocean. 
B) it is just much colder in the middle of the country. 
C) it rains more in central Canada. 
D) your friend just doesn't adjust well to changes in temperature. 
E) she must be at a higher latitude. 
A) your climate is moderated by the Atlantic Ocean. 
B) it is just much colder in the middle of the country. 
C) it rains more in central Canada. 
D) your friend just doesn't adjust well to changes in temperature. 
E) she must be at a higher latitude.

Question 12

The molar mass of glucose is 180 g/mol. Which of the following procedures should you carry out to make a 1 M solution of glucose?

Accepted Answer

A) Dissolve 1 g of glucose in 1 L of water. 
B) Dissolve 180 g of glucose in 1 L of water. 
C) Dissolve 180 g of glucose in 180 g of water. 
D) Dissolve 180 milligrams (mg)of glucose in 1 L of water. 
E) Dissolve 180 g of glucose in 0.8 L of water, and then add more water until the total volume of the solution is 1 L. 
A) Dissolve 1 g of glucose in 1 L of water. 
B) Dissolve 180 g of glucose in 1 L of water. 
C) Dissolve 180 g of glucose in 180 g of water. 
D) Dissolve 180 milligrams (mg)of glucose in 1 L of water. 
E) Dissolve 180 g of glucose in 0.8 L of water, and then add more water until the total volume of the solution is 1 L.

Question 13

Sulphur is in the same column of the periodic table as oxygen, but has electronegativity similar to carbon. Compared to water molecules, molecules of H₂S

Accepted Answer

A) will ionize more readily. 
B) will have greater cohesion to other molecules of H₂S. 
C) will have a greater tendency to form hydrogen bonds with each other. 
D) will have a higher capacity to absorb heat for the same change in temperature. 
E) will not form hydrogen bonds with each other. 
A) will ionize more readily. 
B) will have greater cohesion to other molecules of H₂S. 
C) will have a greater tendency to form hydrogen bonds with each other. 
D) will have a higher capacity to absorb heat for the same change in temperature. 
E) will not form hydrogen bonds with each other.

Question 14

You have two beakers. One contains pure water; the other contains pure methanol (wood alcohol). The covalent bonds of methanol molecules are nonpolar, so there are no hydrogen bonds among methanol molecules. You pour crystals of table salt (NaCl)into each beaker. Predict what will happen.

Accepted Answer

A) Equal amounts of NaCl crystals will dissolve in both water and methanol. 
B) NaCl crystals will NOT dissolve in either water or methanol. 
C) NaCl crystals will dissolve readily in water but will not dissolve in methanol. 
D) NaCl crystals will dissolve readily in methanol but will not dissolve in water. 
E) When the first crystals of NaCl are added to water or to methanol, they will not dissolve; but as more crystals are added, the crystals will begin to dissolve faster and faster. 
A) Equal amounts of NaCl crystals will dissolve in both water and methanol. 
B) NaCl crystals will NOT dissolve in either water or methanol. 
C) NaCl crystals will dissolve readily in water but will not dissolve in methanol. 
D) NaCl crystals will dissolve readily in methanol but will not dissolve in water. 
E) When the first crystals of NaCl are added to water or to methanol, they will not dissolve; but as more crystals are added, the crystals will begin to dissolve faster and faster.

Question 15

One mole (mol)of glucose (molecular mass = 180 daltons)is

Accepted Answer

A) 180 × 10²³ molecules of glucose. 
B) 1 kg of glucose dissolved in 1 L of solution. 
C) the largest amount of glucose that can be dissolved in 1 L of solution. 
D) 180 kilograms of glucose. 
E) both 180 grams of glucose and 6.02 × 10²³ molecules of glucose. 
A) 180 × 10²³ molecules of glucose. 
B) 1 kg of glucose dissolved in 1 L of solution. 
C) the largest amount of glucose that can be dissolved in 1 L of solution. 
D) 180 kilograms of glucose. 
E) both 180 grams of glucose and 6.02 × 10²³ molecules of glucose.

Question 16

-Based on your knowledge of the polarity of water molecules, the solute molecule depicted here is most likely

Accepted Answer

A) positively charged. 
B) negatively charged. 
C) without charge. 
D) hydrophobic. 
E) nonpolar. 
A) positively charged. 
B) negatively charged. 
C) without charge. 
D) hydrophobic. 
E) nonpolar.

Question 17

One litre of a solution of pH 2 has how many more hydrogen ions (H⁺)than 1 L of a solution of pH 6?

Accepted Answer

A) 4 times more 
B) 16 times more 
C) 40 000 times more 
D) 10 000 times more 
E) 100 000 times more 
A) 4 times more 
B) 16 times more 
C) 40 000 times more 
D) 10 000 times more 
E) 100 000 times more

Question 18

Plants transport water through their vascular system utilizing what property of water?

Accepted Answer

A) Hydrogen bonds allowing for surface tension. 
B) Hydrogen bonds allowing for increased structure of water. 
C) Hydrogen bonds allowing for adhesion and cohesion of molecules. 
D) Evaporative cooling. 
E) Its ability to function as a solvent. 
A) Hydrogen bonds allowing for surface tension. 
B) Hydrogen bonds allowing for increased structure of water. 
C) Hydrogen bonds allowing for adhesion and cohesion of molecules. 
D) Evaporative cooling. 
E) Its ability to function as a solvent.

Question 19

A dietary calorie equals 1 kilocalorie. Which of the following statements correctly defines? 1 kilocalorie?

Accepted Answer

A) 1000 calories, or the amount of heat required to raise the temperature of 1 g of water by 1000°C 
B) 100 calories, or the amount of heat required to raise the temperature of 100 g of water by 1°C 
C) 10 000 calories, or the amount of heat required to raise the temperature of 1 kg of water by 1°F 
D) 1000 calories, or the amount of heat required to raise the temperature of 1 kg of water by 1°C 
E) 1000 calories, or the amount of heat required to raise the temperature of 100 g of water by 100°C 
A) 1000 calories, or the amount of heat required to raise the temperature of 1 g of water by 1000°C 
B) 100 calories, or the amount of heat required to raise the temperature of 100 g of water by 1°C 
C) 10 000 calories, or the amount of heat required to raise the temperature of 1 kg of water by 1°F 
D) 1000 calories, or the amount of heat required to raise the temperature of 1 kg of water by 1°C 
E) 1000 calories, or the amount of heat required to raise the temperature of 100 g of water by 100°C

Question 20

Hydrophobic substances such as vegetable oil are

Accepted Answer

A) nonpolar substances that repel water molecules. 
B) nonpolar substances that have an attraction for water molecules. 
C) polar substances that repel water molecules. 
D) polar substances that have an affinity for water. 
E) charged molecules that hydrogen-bond with water molecules. 
A) nonpolar substances that repel water molecules. 
B) nonpolar substances that have an attraction for water molecules. 
C) polar substances that repel water molecules. 
D) polar substances that have an affinity for water. 
E) charged molecules that hydrogen-bond with water molecules.

Exam 3: Water and Life

would be present in 1 L of a 1 M glycerol solution?

A 0.01 M solution of a substance has a pH of 2. What can you conclude about this substance?

Which of the following statements is true about buffer solutions?

In a single molecule of water, two hydrogen atoms are bonded to a single oxygen atom by

Use the following figure to answer the questions below. -How many grams of the compound in the figure above would be required to make 1 L of a 0.5 M solution? (carbon = 12, oxygen = 16, hydrogen = 1)

Coastal regions tend to have more moderate climates than land-locked areas due to the

One of the buffers that contribute to pH stability in human blood is carbonic acid (H₂CO₃). Carbonic acid is a weak acid that dissociates into a bicarbonate ion (HCO₃⁻)and a hydrogen ion (H⁺). Thus, H₂CO₃ ↔ HCO₃⁻ + H⁺ If the pH of the blood drops, one would expect

The molar mass of glucose is 180 g/mol. Which of the following procedures should you carry out to make a 1 M solution of glucose?

Sulphur is in the same column of the periodic table as oxygen, but has electronegativity similar to carbon. Compared to water molecules, molecules of H₂S

You have two beakers. One contains pure water; the other contains pure methanol (wood alcohol). The covalent bonds of methanol molecules are nonpolar, so there are no hydrogen bonds among methanol molecules. You pour crystals of table salt (NaCl)into each beaker. Predict what will happen.

One mole (mol)of glucose (molecular mass = 180 daltons)is

-Based on your knowledge of the polarity of water molecules, the solute molecule depicted here is most likely

One litre of a solution of pH 2 has how many more hydrogen ions (H⁺)than 1 L of a solution of pH 6?

Plants transport water through their vascular system utilizing what property of water?

A dietary calorie equals 1 kilocalorie. Which of the following statements correctly defines? 1 kilocalorie?

Hydrophobic substances such as vegetable oil are

Introduction: Evolution and Themes of Biology

The Chemical Context of Life

Carbon and the Molecular Diversity of Life

The Structure and Function of Large Biological Molecules

A Tour of the Cell

Membrane Structure and Function

An Introduction to Metabolism

Cellular Respiration and Fermentation

Photosynthesis

Cell Communication

The Cell Cycle

Meiosis and Sexual Life Cycles

Mendel and the Gene Idea

The Chromosomal Basis of Inheritance

The Molecular Basis of Inheritance

From Gene to Protein

Regulation of Gene Expression

Viruses

Dna Tools and Biotechnology

Genomes and Their Evolution

Descent With Modification: a Darwinian View of Life

The Evolution of Populations

The Origin of Species

The History of Life on Earth

Phylogeny and the Tree of Life

Bacteria and Archaea

Protists

Plant Diversity I: How Plants Colonized Land

Plant Diversity Ii: the Evolution of Seed Plants

Fungi

An Overview of Animal Diversity

An Introduction to Invertebrates

The Origin and Evolution of Vertebrates

Plant Structure, Growth, and Development

Resource Acquisition and Transport in Vascular Plants

Soil and Plant Nutrition

Angiosperm Reproduction and Biotechnology

Plant Responses to Internal and External Signals

Basic Principles of Animal Form and Function

Animal Nutrition

Circulation and Gas Exchange

The Immune System

Osmoregulation and Excretion

Hormones and the Endocrine System

Animal Reproduction

Animal Development

Neurons, Synapses, and Signalling

Nervous Systems

Sensory and Motor Mechanisms

Animal Behaviour

An Introduction to Ecology and the Biosphere

Population Ecology

Community Ecology

Ecosystems and Restoration Ecology

Conservation Biology and Global Change

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