Question 1

moles of hydroxyl ions [OH⁻] per litre. Which of the following best describes this solution?

Accepted Answer

A) acidic: H⁺ acceptor 
B) basic: H⁺ acceptor 
C) acidic: H⁺ donor 
D) basic: H⁺ donor 
E) neutral 
A) acidic: H⁺ acceptor 
B) basic: H⁺ acceptor 
C) acidic: H⁺ donor 
D) basic: H⁺ donor 
E) neutral

Question 2

Which of the following takes place as an ice cube cools a drink?

Accepted Answer

A) Molecular collisions in the drink increase. 
B) Kinetic energy in the drink decreases. 
C) A calorie of heat energy is transferred from the ice to the water of the drink. 
D) The specific heat of the water in the drink decreases. 
E) Evaporation of the water in the drink increases. 
A) Molecular collisions in the drink increase. 
B) Kinetic energy in the drink decreases. 
C) A calorie of heat energy is transferred from the ice to the water of the drink. 
D) The specific heat of the water in the drink decreases. 
E) Evaporation of the water in the drink increases.

Question 3

Water is densest at

Accepted Answer

A) ⁻4°C. 
B) 0°C. 
C) 2°C. 
D) 4°C. 
E) 8°C. 
A) ⁻4°C. 
B) 0°C. 
C) 2°C. 
D) 4°C. 
E) 8°C.

Question 4

What is the major area of biological concern regarding acidification of the oceans?

Accepted Answer

A) They will become too acidic for life. 
B) There will not be enough carbonate available for organisms to make calcium carbonate. 
C) There will be too much bicarbonate, making the oceans basic. 
D) There will be too much CO₂ released back into the atmosphere. 
E) They will become too polluted for human use. 
A) They will become too acidic for life. 
B) There will not be enough carbonate available for organisms to make calcium carbonate. 
C) There will be too much bicarbonate, making the oceans basic. 
D) There will be too much CO₂ released back into the atmosphere. 
E) They will become too polluted for human use.

Question 5

The molecular weight of water is 18 daltons. What is the molarity of 1 litre of pure water? (Hint: What is the mass of 1 litre of pure water?)

Accepted Answer

A) 55.6 M 
B) 18 M 
C) 37 M 
D) 0.66 M 
E) 1.0 M 
A) 55.6 M 
B) 18 M 
C) 37 M 
D) 0.66 M 
E) 1.0 M

Question 6

What is the hydrogen ion [H⁺] concentration of a solution of pH 8?

Accepted Answer

A) 8 M 
B) 8 x 10⁻⁶ M 
C) 0.01 M 
D) 10⁻⁸ M 
E) 10⁻⁶ M 
A) 8 M 
B) 8 x 10⁻⁶ M 
C) 0.01 M 
D) 10⁻⁸ M 
E) 10⁻⁶ M

Question 7

When an ionic compound such as sodium chloride (NaCl)is placed in water, the component atoms of the NaCl crystal dissociate into individual sodium ions (Na⁺)and chloride ions (Cl⁻). In contrast, the atoms of covalently bonded molecules (e.g., glucose, sucrose, glycerol)do not generally dissociate when placed in aqueous solution. Which of the following solutions would be expected to contain the greatest number of solute particles (molecules or ions)?

Accepted Answer

A) 1 L of 0.5 M NaCl 
B) 1 L of 0.5 M glucose 
C) 1 L of 1.0 M NaCl 
D) 1 L of 1.0 M glucose 
E) 1 L of 1.0 M NaCl and 1 L of 1.0 M glucose will contain equal numbers of solute particles. 
A) 1 L of 0.5 M NaCl 
B) 1 L of 0.5 M glucose 
C) 1 L of 1.0 M NaCl 
D) 1 L of 1.0 M glucose 
E) 1 L of 1.0 M NaCl and 1 L of 1.0 M glucose will contain equal numbers of solute particles.

Question 8

The reason water has a high specific heat is that

Accepted Answer

A) the adhesive property of water resists heat absorption. 
B) ionic bonds require a lot of energy to be broken. 
C) a lot of heat needs to be absorbed to disrupt hydrogen bonds. 
D) the covalent bonds resist splitting. 
E) water cools very quickly. 
A) the adhesive property of water resists heat absorption. 
B) ionic bonds require a lot of energy to be broken. 
C) a lot of heat needs to be absorbed to disrupt hydrogen bonds. 
D) the covalent bonds resist splitting. 
E) water cools very quickly.

Question 9

Increased atmospheric CO₂ concentrations might have what effect on sea water?

Accepted Answer

A) Sea water will become more acidic, and bicarbonate concentrations will decrease. 
B) Sea water will become more alkaline, and carbonate concentrations will decrease. 
C) There will be no change in the pH of sea water, because carbonate will turn to bicarbonate. 
D) Sea water will become more acidic, and carbonate concentrations will decrease. 
E) Sea water will become more acidic, and carbonate concentrations will increase. 
A) Sea water will become more acidic, and bicarbonate concentrations will decrease. 
B) Sea water will become more alkaline, and carbonate concentrations will decrease. 
C) There will be no change in the pH of sea water, because carbonate will turn to bicarbonate. 
D) Sea water will become more acidic, and carbonate concentrations will decrease. 
E) Sea water will become more acidic, and carbonate concentrations will increase.

Question 10

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

Accepted Answer

A) a decrease in the concentration of H₂CO₃ and an increase in the concentration of HCO₃⁻. 
B) an increase in the concentration of H₂CO₃ and a decrease in the concentration of HCO₃⁻. 
C) a decrease in the concentration of HCO₃⁻ and an increase in the concentration of H⁺. 
D) an increase in the concentration of HCO₃⁻ and a decrease in the concentration of OH⁻. 
E) a decrease in the concentration of HCO₃⁻ and an increase in the concentration of both H₂CO₃ and H⁺. 
A) a decrease in the concentration of H₂CO₃ and an increase in the concentration of HCO₃⁻. 
B) an increase in the concentration of H₂CO₃ and a decrease in the concentration of HCO₃⁻. 
C) a decrease in the concentration of HCO₃⁻ and an increase in the concentration of H⁺. 
D) an increase in the concentration of HCO₃⁻ and a decrease in the concentration of OH⁻. 
E) a decrease in the concentration of HCO₃⁻ and an increase in the concentration of both H₂CO₃ and H⁺.

Question 11

How many molecules of glucose (C₆H₁₂O₆ molecular mass = 180 daltons)would be present in 90 grams of glucose?

Accepted Answer

A) 90 × 10²³ 
B) (6.02/180)× 10²³ 
C) (6.02/90)× 10²³ 
D) (90 × 6.02)× 10²³ 
E) (90/180)× 6.02 × 10²³ 
A) 90 × 10²³ 
B) (6.02/180)× 10²³ 
C) (6.02/90)× 10²³ 
D) (90 × 6.02)× 10²³ 
E) (90/180)× 6.02 × 10²³

Question 12

A strong acid like HCl

Accepted Answer

A) ionizes completely in an aqueous solution. 
B) increases the pH when added to an aqueous solution. 
C) reacts with strong bases to create a buffered solution. 
D) is a strong buffer at low pH. 
E) both ionizes completely in aqueous solutions and is a strong buffer at low pH. 
A) ionizes completely in an aqueous solution. 
B) increases the pH when added to an aqueous solution. 
C) reacts with strong bases to create a buffered solution. 
D) is a strong buffer at low pH. 
E) both ionizes completely in aqueous solutions and is a strong buffer at low pH.

Question 13

Which of the following ionizes completely in solution and is considered to be a strong base (alkali)?

Accepted Answer

A) NaCl 
B) HCl 
C) NH₃ 
D) H₂CO₃ 
E) NaOH 
A) NaCl 
B) HCl 
C) NH₃ 
D) H₂CO₃ 
E) NaOH

Question 14

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.
-How many grams of acetic acid (C₂H₄O₂)would you use to make 10 L of a 0.1 M aqueous solution of acetic acid? (Note: The atomic masses, in daltons, are approximately 12 for carbon, 1 for hydrogen, and 16 for oxygen.)

Accepted Answer

A) 10 g 
B) 0.1 g 
C) 6.0 g 
D) 60 g 
E) 0.6 g 
A) 10 g 
B) 0.1 g 
C) 6.0 g 
D) 60 g 
E) 0.6 g

Question 15

moles of hydrogen ions [H⁺] per litre. Which of the following best describes this solution?

Accepted Answer

A) acidic: will accept H⁺ from both strong and weak acids 
B) basic: will accept H⁺ from both strong and weak acids 
C) acidic: will give H⁺ to weak acids, but accept H⁺ from strong acids 
D) basic: will give H⁺ to weak acids, but accept H⁺ from weak acids 
E) acidic: will give H⁺ to both strong and weak acids 
A) acidic: will accept H⁺ from both strong and weak acids 
B) basic: will accept H⁺ from both strong and weak acids 
C) acidic: will give H⁺ to weak acids, but accept H⁺ from strong acids 
D) basic: will give H⁺ to weak acids, but accept H⁺ from weak acids 
E) acidic: will give H⁺ to both strong and weak acids

Question 16

Carbon dioxide (CO₂)is readily soluble in water, according to the equation CO₂ + H₂O ↔ H₂CO₃. Carbonic acid (H₂CO₃)is a weak acid. If CO₂ is bubbled into a beaker containing pure, freshly distilled water, which of the following graphs correctly describes the results?

Accepted Answer

A)    
B)    
C)    
D)    
E)    
A)    
B)    
C)    
D)    
E)

Question 17

If a solution has a pH of 7, this means that

Accepted Answer

A) there are no H⁺ ions in the water. 
B) this is a solution of pure water. 
C) the concentration of H⁺ ions in the water equals the concentration of OH⁻ ions in the water. 
D) this is a solution of pure water, and the concentration of H⁺ ions in the water is 10⁻⁷ M. 
E) this is a solution of pure water, and the concentration of H⁺ ions equals the concentration of OH⁻ ions in the water. 
A) there are no H⁺ ions in the water. 
B) this is a solution of pure water. 
C) the concentration of H⁺ ions in the water equals the concentration of OH⁻ ions in the water. 
D) this is a solution of pure water, and the concentration of H⁺ ions in the water is 10⁻⁷ M. 
E) this is a solution of pure water, and the concentration of H⁺ ions equals the concentration of OH⁻ ions in the water.

Question 18

Temperature usually increases when water condenses. Which behaviour of water is most directly responsible for this phenomenon?

Accepted Answer

A) the change in density when it condenses to form a liquid or solid 
B) reactions with other atmospheric compounds 
C) the release of heat by the formation of hydrogen bonds 
D) the release of heat by the breaking of hydrogen bonds 
E) the high surface tension of water 
A) the change in density when it condenses to form a liquid or solid 
B) reactions with other atmospheric compounds 
C) the release of heat by the formation of hydrogen bonds 
D) the release of heat by the breaking of hydrogen bonds 
E) the high surface tension of water

Question 19

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.
-Which of the following is a hydrophobic material?

Accepted Answer

A) paper 
B) table salt 
C) wax 
D) sugar 
E) pasta 
A) paper 
B) table salt 
C) wax 
D) sugar 
E) pasta

Question 20

Assume that acid rain has lowered the pH of a particular lake to pH 4.0. What is the hydroxyl ion concentration of this lake?

Accepted Answer

A) 1 × 10⁻¹⁰ mol of hydroxyl ion per litre of lake water 
B) 1 × 10⁻⁴ mol of hydroxyl ion per litre of lake water 
C) 10.0 M with regard to hydroxyl ion concentration 
D) 4.0 M with regard to hydroxyl ion concentration 
E) 1 × 10⁻⁴ mol of hydroxyl ion per litre of lake water and 4.0 M with regard to hydrogen ion concentration 
A) 1 × 10⁻¹⁰ mol of hydroxyl ion per litre of lake water 
B) 1 × 10⁻⁴ mol of hydroxyl ion per litre of lake water 
C) 10.0 M with regard to hydroxyl ion concentration 
D) 4.0 M with regard to hydroxyl ion concentration 
E) 1 × 10⁻⁴ mol of hydroxyl ion per litre of lake water and 4.0 M with regard to hydrogen ion concentration

Exam 3: Water and Life

moles of hydroxyl ions [OH⁻] per litre. Which of the following best describes this solution?

Which of the following takes place as an ice cube cools a drink?

Water is densest at

What is the major area of biological concern regarding acidification of the oceans?

The molecular weight of water is 18 daltons. What is the molarity of 1 litre of pure water? (Hint: What is the mass of 1 litre of pure water?)

What is the hydrogen ion [H⁺] concentration of a solution of pH 8?

The reason water has a high specific heat is that

Increased atmospheric CO₂ concentrations might have what effect on sea water?

How many molecules of glucose (C₆H₁₂O₆ molecular mass = 180 daltons)would be present in 90 grams of glucose?

A strong acid like HCl

Which of the following ionizes completely in solution and is considered to be a strong base (alkali)?

moles of hydrogen ions [H⁺] per litre. Which of the following best describes this solution?

Carbon dioxide (CO₂)is readily soluble in water, according to the equation CO₂ + H₂O ↔ H₂CO₃. Carbonic acid (H₂CO₃)is a weak acid. If CO₂ is bubbled into a beaker containing pure, freshly distilled water, which of the following graphs correctly describes the results?

If a solution has a pH of 7, this means that

Temperature usually increases when water condenses. Which behaviour of water is most directly responsible for this phenomenon?

Assume that acid rain has lowered the pH of a particular lake to pH 4.0. What is the hydroxyl ion concentration of this lake?

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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