Question 1

Which of the following properties of water is responsible for the formation of raindrops?

Accepted Answer

A)  cohesion property 
B)  adhesion property 
C)  high thermal energy 
D)  high kinetic energy 
A)  cohesion property 
B)  adhesion property 
C)  high thermal energy 
D)  high kinetic energy A

Question 2

Why does a full bathtub have more thermal energy than a pot of freshly brewed coffee (even though the coffee has a higher temperature than the bathwater)?

Accepted Answer

A)  higher; greater volume 
B)  higher; high kinetic energy 
C)  lower; low temperature 
D)  lower; low density 
A)  higher; greater volume 
B)  higher; high kinetic energy 
C)  lower; low temperature 
D)  lower; low density A

Question 3

How many grams of NaCl are required to prepare 50 mL of a solution of 1 M NaCl?
(MW of NaCl=58.44g)

Accepted Answer

A)  2.72g 
B)  2.922g 
C)  5.844g 
D)  58.44g 
A)  2.72g 
B)  2.922g 
C)  5.844g 
D)  58.44g B

Question 4

Which of the following is considered to be a strong base (alkali)?

Accepted Answer

A)  HCl → H+ + Cl- 
B)  NH3 + H+ ⇔ NH4+ 
C)  H2CO3 ⇔ HCO3- + H+ 
D)  NaOH → Na+ + OH- 
A)  HCl → H+ + Cl- 
B)  NH3 + H+ ⇔ NH4+ 
C)  H2CO3 ⇔ HCO3- + H+ 
D)  NaOH → Na+ + OH-

Question 5

Which answer best describes why does ice float in liquid water?

Accepted Answer

A)  The high surface tension of liquid water keeps the ice on top. 
B)  The ionic bonds between the molecules in ice prevent the ice from sinking. 
C)  Stable hydrogen bonds keep water molecules of ice farther apart than water molecules of liquid water. 
D)  The crystalline lattice of ice causes it to be denser than liquid water. 
A)  The high surface tension of liquid water keeps the ice on top. 
B)  The ionic bonds between the molecules in ice prevent the ice from sinking. 
C)  Stable hydrogen bonds keep water molecules of ice farther apart than water molecules of liquid water. 
D)  The crystalline lattice of ice causes it to be denser than liquid water.

Question 6

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) 
  
A) 
  
B) 
  
C) 
  
D)

Question 7

Three moles of the compound in the figure would weigh how many grams? (Note: The atomic masses, in daltons, are approximately 12 for carbon, 1 for hydrogen.)

Accepted Answer

A)  72 
B)  78 
C)  216 
D)  234 
A)  72 
B)  78 
C)  216 
D)  234

Question 8

Consider two solutions: solution X has a pH of 4; solution Y has a pH of 7. From this information, we can reasonably conclude that ________.

Accepted Answer

A)  solution Y has no free hydrogen ions (H+) 
B)  the concentration of hydrogen ions in solution Y is 1000 times as great as the concentration of hydrogen ions in solution X 
C)  the concentration of hydrogen ions in solution X is 3 times as great as the concentration of hydrogen ions in solution Y 
D)  the concentration of hydrogen ions in solution X is 1000 times as great as the concentration of hydrogen ions in solution Y 
A)  solution Y has no free hydrogen ions (H+) 
B)  the concentration of hydrogen ions in solution Y is 1000 times as great as the concentration of hydrogen ions in solution X 
C)  the concentration of hydrogen ions in solution X is 3 times as great as the concentration of hydrogen ions in solution Y 
D)  the concentration of hydrogen ions in solution X is 1000 times as great as the concentration of hydrogen ions in solution Y

Question 9

Increased atmospheric CO2 concentrations might have what effect on seawater?

Accepted Answer

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

Question 10

To act as an effective coolant in a car's radiator, a substance has to have the capacity to absorb a great deal of heat. Which physical property is the best indicator for a good coolant?

Accepted Answer

A)  pH 
B)  density at room temperature 
C)  heat of vaporization 
D)  specific heat 
A)  pH 
B)  density at room temperature 
C)  heat of vaporization 
D)  specific heat

Question 11

How would acidification of seawater affect marine organisms?

Accepted Answer

A)  It will increase dissolved carbonate concentrations and promote faster growth of corals and shell-building animals. 
B)  It will decrease dissolved carbonate concentrations and promote faster growth of corals and shell-building animals. 
C)  It will increase dissolved carbonate concentrations and hinder growth of corals and shell-building animals. 
D)  It will decrease dissolved carbonate concentrations and hinder growth of corals and shell-building animals. 
A)  It will increase dissolved carbonate concentrations and promote faster growth of corals and shell-building animals. 
B)  It will decrease dissolved carbonate concentrations and promote faster growth of corals and shell-building animals. 
C)  It will increase dissolved carbonate concentrations and hinder growth of corals and shell-building animals. 
D)  It will decrease dissolved carbonate concentrations and hinder growth of corals and shell-building animals.

Question 12

A solution contains 0.0000001 (10-7) moles of hydrogen ions [H+] per liter. Which of the following best describes this solution?

Accepted Answer

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

Question 13

The nutritional label on a box of cookies says "150 kilocalories/cookie." How many joules of energy each cookie contains when 1 cal = 4.16 J?

Accepted Answer

A)  6.24 × 105 J 
B)  6.24 × 106 J 
C)  624 J 
D)  150 J 
A)  6.24 × 105 J 
B)  6.24 × 106 J 
C)  624 J 
D)  150 J

Question 14

Melting of ice and thus reduced feeding opportunities for polar bears is occurring because of the ________.

Accepted Answer

A)  increase in phytoplankton population 
B)  drying up of lakes and streams 
C)  constant breaking and reforming of hydrogen bonds in water 
D)  increase in CO2 and other greenhouse gases in the atmosphere 
A)  increase in phytoplankton population 
B)  drying up of lakes and streams 
C)  constant breaking and reforming of hydrogen bonds in water 
D)  increase in CO2 and other greenhouse gases in the atmosphere

Question 15

Which of the following statements is true for water in its liquid state?

Accepted Answer

A)  It is less dense than ice. 
B)  It has a specific heat lower than most other substances. 
C)  It has a heat of vaporization higher than most other substances. 
D)  It is nonpolar. 
A)  It is less dense than ice. 
B)  It has a specific heat lower than most other substances. 
C)  It has a heat of vaporization higher than most other substances. 
D)  It is nonpolar.

Question 16

What is the reason why Hydrochloric acid is such a strong acid?

Accepted Answer

A)  HCl dissociates completely to H+(aq) and Cl-(aq) in water 
B)  HCl does not dissociate at all when it is dissolved in water 
C)  HCl produces a gaseous product when it is neutralized 
D)  aqueous solutions of HCl contain equal concentrations of H+(aq) and OH-(aq) 
A)  HCl dissociates completely to H+(aq) and Cl-(aq) in water 
B)  HCl does not dissociate at all when it is dissolved in water 
C)  HCl produces a gaseous product when it is neutralized 
D)  aqueous solutions of HCl contain equal concentrations of H+(aq) and OH-(aq)

Question 17

Which of the following best defines 'one kilocalorie'?

Accepted Answer

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

Question 18

Measurements show that the pH of a particular lake is 4.0. What is the hydrogen ion concentration of the lake?

Accepted Answer

A)  4.0M 
B)  10-10M 
C)  10-4M 
D)  104M 
A)  4.0M 
B)  10-10M 
C)  10-4M 
D)  104M

Question 19

A beaker contains 100 milliliters (mL) of NaOH solution at pH = 13. A technician carefully pours into the beaker 10 mL of HCl at pH = 1. Which of the following statements correctly describes the result of this mixing?

Accepted Answer

A)  The concentration of Na+ ions will rise. 
B)  The pH of the beaker's contents will increase. 
C)  The pH of the beaker's contents will be neutral. 
D)  The pH of the beaker's contents will decrease. 
A)  The concentration of Na+ ions will rise. 
B)  The pH of the beaker's contents will increase. 
C)  The pH of the beaker's contents will be neutral. 
D)  The pH of the beaker's contents will decrease.

Question 20

Which of the following statements is incorrect?

Accepted Answer

A)  Water can form hydrogen bonds with compounds that form polar covalent bonds. 
B)  Water can form hydrogen bonds with other water molecules. 
C)  Water can form intramolecular hydrogen bonds. 
D)  Water can form intermolecular hydrogen bonds. 
A)  Water can form hydrogen bonds with compounds that form polar covalent bonds. 
B)  Water can form hydrogen bonds with other water molecules. 
C)  Water can form intramolecular hydrogen bonds. 
D)  Water can form intermolecular hydrogen bonds.

Exam 3: The Chemistry of Water

Which of the following properties of water is responsible for the formation of raindrops?

Why does a full bathtub have more thermal energy than a pot of freshly brewed coffee (even though the coffee has a higher temperature than the bathwater)?

How many grams of NaCl are required to prepare 50 mL of a solution of 1 M NaCl? (MW of NaCl=58.44g)

Which of the following is considered to be a strong base (alkali)?

Which answer best describes why does ice float in liquid water?

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?

Three moles of the compound in the figure would weigh how many grams? (Note: The atomic masses, in daltons, are approximately 12 for carbon, 1 for hydrogen.)

Consider two solutions: solution X has a pH of 4; solution Y has a pH of 7. From this information, we can reasonably conclude that ________.

Increased atmospheric CO2 concentrations might have what effect on seawater?

To act as an effective coolant in a car's radiator, a substance has to have the capacity to absorb a great deal of heat. Which physical property is the best indicator for a good coolant?

How would acidification of seawater affect marine organisms?

A solution contains 0.0000001 (10-7) moles of hydrogen ions [H+] per liter. Which of the following best describes this solution?

The nutritional label on a box of cookies says "150 kilocalories/cookie." How many joules of energy each cookie contains when 1 cal = 4.16 J?

Melting of ice and thus reduced feeding opportunities for polar bears is occurring because of the ________.

Which of the following statements is true for water in its liquid state?

What is the reason why Hydrochloric acid is such a strong acid?

Which of the following best defines 'one kilocalorie'?

Measurements show that the pH of a particular lake is 4.0. What is the hydrogen ion concentration of the lake?

A beaker contains 100 milliliters (mL) of NaOH solution at pH = 13. A technician carefully pours into the beaker 10 mL of HCl at pH = 1. Which of the following statements correctly describes the result of this mixing?

Which of the following statements is incorrect?

Biology and Its Themes

Atoms and Molecules

Carbon: the Basis of Molecular Diversity

Biological Macromolecules and Lipids

Energy and Life

Cell Structure and Function

Cell Membranes

Cellular Signaling

Cell Respiration

Photosynthetic Processes

Mitosis

Sexual Life Cycles and Meiosis

Mendelian Genetics

Linkage and Chromosomes

Nucleic Acids and Inheritance

Expression of Genes

Control of Gene Expression

Dna Technology

The Evolution of Genomes

How Evolution Works

Phylogenetic Reconstruction

Microevolution

Species and Speciation

Macroevolution

Introduction to Viruses

Prokaryotes

The Origin and Evolution of Eukaryotes

Nonvascular and Seedless Vascular Plants

Seed Plants

Introduction to Fungi

An Introduction to Animal Diversity

Invertebrates

Vertebrates

Plant Structure and Growth

Transport in Vascular Plants

Plant Nutrition

Reproduction of Flowering Plants

Plant Signals and Behavior

The Animal Body

Chemical Signals in Animals

Animal Digestive Systems

Animal Transport Systems

Animal Excretory Systems

Animal Reproductive Systems

Development in Animals

Animal Defenses Against Infection

Electrical Signals in Animals

Neural Regulation in Animals

Sensation and Movement in Animals

An Overview of Ecology

Behavioral Ecology

Populations and Life History Traits

Biodiversity and Communities

Energy Flow and Chemical Cycling in Ecosystems

Conservation and Global Ecology

Filters

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?

Increased atmospheric CO₂ concentrations might have what effect on seawater?