Question 1

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)  2)  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? 
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B)  2)  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? 
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C)  2)  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? 
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D)  2)  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? 
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F) A) and B)

Question 2

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.E) All of the above
F) B) and C)

Question 3

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 heatE) C) and D)
F) B) and D)

Question 4

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.E) B) and D)
F) B) and C)

Question 5

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)   104ME) All of the above
F) A) and C)

Question 6

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 energyE) C) and D)
F) All of the above A

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)   234E) All of the above
F) C) and D)

Question 8

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°CE) A) and C)
F) B) and D)

Question 9

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 densityE) C) and D)
F) B) and D) A

Question 10

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 JE) C) and D)
F) B) and C)

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.E) All of the above
F) A) and D)

Question 12

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-E) B) and D)
F) A) and C)

Question 13

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 YE) A) and D)
F) B) and C)

Question 14

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)   neutralE) None of the above
F) A) and C)

Question 15

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.E) B) and C)
F) C) and D)

Question 16

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)   58.44gE) A) and D)
F) B) and C) B

Question 17

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.E) C) and D)
F) A) and B)

Question 18

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) E) A) and B)
F) B) and C)

Question 19

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 atmosphereE) A) and B)
F) None of the above

Question 20

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.E) None of the above
F) B) and C)

Exam 3: The Chemistry of 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?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

Which of the following statements is incorrect?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedA

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.)

Correct AnswerverifiedShow Answer

Which of the following best defines 'one kilocalorie'?

Correct AnswerverifiedShow Answer

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) ?

Correct AnswerverifiedA

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?

Correct AnswerverifiedShow Answer

How would acidification of seawater affect marine organisms?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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 ________.

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Increased atmospheric CO2 concentrations might have what effect on seawater?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedB

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

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?

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A

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A

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Increased atmospheric CO₂ concentrations might have what effect on seawater?

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B

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