Deck 3: Water and the Fitness of the Environment

Question 1

Which type of bond must be broken for water to vaporize?

A)ionic bonds
B)nonpolar covalent bonds
C)polar covalent bonds
D)hydrogen bonds
E)covalent bonds

Answer 1

D

Question 2

What gives rise to the cohesiveness of water molecules?

A)hydrophobic interactions
B)nonpolar covalent bonds
C)ionic bonds
D)hydrogen bonds
E)both A and C

Answer 2

D

Question 3

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 particles (molecules or ions)?

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)C and D will contain equal numbers of particles.

Answer 3

C

Question 4

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

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

Question 5

At what temperature is water at its densest?

A)0°C
B)4°C
C)32°C
D)100°C
E)212°C

Question 6

How many molecules of glucose (C₆H₂O₆ molecular mass =180 daltons)would be present in one mole of glucose?

A)24
B)342
C)23 × 10¹⁴
D)180 × 10¹⁴
E)6)02 × 10²³

Question 7

The slight negative charge at one end of one water molecule is attracted to the slight positive charge of another water molecule. What is this attraction called?

A)a covalent bond
B)a hydrogen bond
C)an ionic bond
D)a hydrophilic bond
E)a hydrophobic bond

Question 8

Water is able to form hydrogen bonds because

A)oxygen has a valence of 2.
B)the water molecule is shaped like a tetrahedron.
C)the bonds that hold together the atoms in a water molecule are polar covalent bonds.
D)the oxygen atom in a water molecule has a weak positive charge.
E)each of the hydrogen atoms in a water molecule is weakly negative in charge.

Question 9

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

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 10

Why does ice float in liquid water?

A)The liquid water molecules have more kinetic energy and thus support the ice.
B)The ionic bonds between the molecules in ice prevent the ice from sinking.
C)Ice always has air bubbles that keep it afloat.
D)Hydrogen bonds stabilize and keep the molecules of ice farther apart than the water molecules of liquid water.
E)The crystalline lattice of ice causes it to be denser than liquid water.

Question 11

Water's high specific heat is mainly a consequence of the

A)small size of the water molecules.
B)high specific heat of oxygen and hydrogen atoms.
C)absorption and release of heat when hydrogen bonds break and form.
D)fact that water is a poor heat conductor.
E)inability of water to dissipate heat into dry air.

Question 12

The following question is based on Figure 3.1: solute molecule surrounded by a hydration shell of water.

Figure 3.1
Based on your knowledge of the polarity of water molecules, the solute molecule is most likely

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

Question 13

Hydrophobic substances such as vegetable oil are

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.

Question 14

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

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 15

An example of a hydrogen bond is the bond between

A)C and H in methane (CH₄).
B)the H of one water molecule and the O of another water molecule.
C)Na⁺and Cl⁻ in salt.
D)the two hydrogen atoms in a molecule of hydrogen gas (H₂).
E)Mg⁺and Cl⁻ in MgCl₂.

Question 16

Which of the following effects is produced by the high surface tension of water?

A)Lakes don't freeze solid in winter, despite low temperatures.
B)A water strider can walk across the surface of a small pond.
C)Organisms resist temperature changes, although they give off heat due to chemical reactions.
D)Water can act as a solvent.
E)The pH of water remains exactly neutral.

Question 17

The nutritional information on a cereal box shows that one serving of a dry cereal has 200 kilocalories. If one were to burn one serving of the cereal, the amount of heat given off would be sufficient to raise the temperature of 20 kg of water how many degrees Celsius?

A)0)2°C
B)1)0°C
C)2)0°C
D)10.0°C
E)20.0°C

Question 18

Which of the following statements correctly defines a kilocalorie?

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

Question 19

One mole (mol)of a substance is

A)6)02 × 10²³ molecules of the substance.
B)1 g of the substance dissolved in 1 L of solution.
C)the largest amount of the substance that can be dissolved in 1 L of solution.
D)the molecular mass of the substance expressed in grams.
E)A and D only

Question 20

How many molecules of glycerol (C₃H₈O₃)would be present in 1 L of a 1 M glycerol solution?

A)1
B)14
C)92
D)1 × 10⁷
E)6)02 × 10²³

Question 21

The molecular weight of water is 18 daltons. What is the molarity of 1 liter of pure water?

A)55.6M
B)18M
C)37M
D)0)66M
E)1)0M

Question 22

A solution contains 0.0000001(10⁻⁷)moles of hydroxyl ions [OH⁻] per liter. Which of the following best describes this solution?

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

Question 23

Which of the following statements is completely correct?

A)H₂CO₃ is a weak acid, and NaOH is a weak base (alkali).
B)H₂CO₃ is a strong acid, and NaOH is a strong base (alkali).
C)NH₃ is a weak base (alkali), and H₂CO₃ is a strong acid.
D)NH₃ is a weak base (alkali), and HCl is a strong acid.
E)NH₃ is a strong base (alkali), and HCl is a weak acid.

Question 24

The molecular mass of glucose (C₆H₁₂O₆)is 180 g. Which of the following procedures should you carry out to make a 0.5 M solution of glucose?

A)Dissolve 0.5 g of glucose in a small volume of water, and then add more water until the total volume of solution is 1 L.
B)Dissolve 90 g of glucose in a small volume of water, and then add more water until the total volume of the solution is 1 L.
C)Dissolve 180 g of glucose in a small volume of water, and then add more water until the total volume of the solution is 1 L.
D)Dissolve 0.5 g of glucose in 1 L of water.
E)Dissolve 180 g of glucose in 1 L of water.

Question 25

How many grams of the molecule in Figure 3.2 would be required to make 1 L of a 0.5 M solution of the molecule?
(Carbon = 12, Oxygen = 16, Hydrogen = 1)

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

Question 26

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

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

Question 27

You have a freshly-prepared 1M solution of glucose in water. You carefully pour out a 100 mL sample of that solution. How many glucose molecules are included in that 100 mL sample?

A)6)02 × 10²³
B)3)01 × 10²³
C)6)02 × 10²⁴
D)12.04 × 10²³
E)6)02 × 10²²

Question 28

What is the pH of a solution with a hydrogen ion [H⁺] concentration of 10⁻⁸ M?

A)pH 2
B)pH 4
C)pH 6
D)pH 8
E)pH 10

Question 29

How many grams of the molecule in Figure 3.2 would be equal to 1 mol of the molecule?
(Carbon = 12, Oxygen = 16, Hydrogen = 1)

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

Question 30

Which of the following solutions has the greatest concentration of hydroxyl ions [OH⁻]?

A)lemon juice at pH 2
B)vinegar at pH 3
C)tomato juice at pH 4
D)urine at pH 6
E)seawater at pH 8

Question 31

You have a freshly-prepared 0.1M solution of glucose in water. Each liter of this solution contains how many glucose molecules?

A)6)02 × 10²³
B)3)01 × 10²³
C)6)02 × 10²⁴
D)12.04 × 10²³
E)6)02 × 10²²

Question 32

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

A)NaCl
B)HCl
C)NH₃
D)H₂CO₃
E)NaOH

Question 33

Which of the following ionizes completely in solution and is considered to be a strong acid?

A)NaOH
B)HCl
C)NH₃
D)H₂CO₃
E)CH₃COOH

Question 34

What is the pH of a solution with a hydroxyl ion [OH⁻] concentration of 10⁻¹² M?

A)pH 2
B)pH 4
C)pH 10
D)pH 12
E)pH 14

Question 35

A given solution contains 0.0001(10⁻⁴)moles of hydrogen ions [H⁺] per liter. Which of the following best describes this solution?

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

Question 36

Which of the following solutions has the greatest concentration of hydrogen ions [H⁺]?

A)gastric juice at pH 2
B)vinegar at pH 3
C)tomato juice at pH 4
D)black coffee at pH 5
E)household bleach at pH 12

Question 37

A small birthday candle is weighed, then lighted and placed beneath a metal can containing 100 mL of water. Careful records are kept as the temperature of the water rises. Data from this experiment are shown on the graph. What amount of heat energy is released in the burning of candle wax?

A)0)5 kilocalories per gram of wax burned
B)5 kilocalories per gram of wax burned
C)10 kilocalories per gram of wax burned
D)20 kilocalories per gram of wax burned
E)50 kilocalories per gram of wax burned

Question 38

Identical heat lamps are arranged to shine on identical containers of water and methanol (wood alcohol), so that each liquid absorbs the same amount of energy minute by minute. The covalent bonds of methanol molecules are non-polar, so there are no hydrogen bonds among methanol molecules. Which of the following graphs correctly describes what will happen to the temperature of the water and the methanol?

A)
B)
C)
D)
E)

Question 39

How many grams of the molecule in Figure 3.2 would be required to make 2.5 L of a 1 M solution of the molecule?
(Carbon = 12, Oxygen = 16, Hydrogen = 1)

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

Question 40

If the pH of a solution is decreased from 9 to 8, it means that the

A)concentration of H⁺ has decreased to one-tenth (1/10)what it was at pH 9.
B)concentration of H⁺ has increased 10-fold (10X)compared to what it was at pH 9.
C)concentration of OH⁻ has increased 10-fold (10X)compared to what it was at pH 9.
D)concentration of OH⁻ has decreased to one-tenth (1/10)what it was at pH 9.
E)Both B and D are correct.

Question 41

You have two beakers. One contains a solution of HCl at pH = 1.0. The other contains a solution of NaOH at pH = 13. Into a third beaker, you slowly and cautiously pour 20 mL of the HCL and 20 mL of the NaOH. After complete stirring, the pH of the mixture will be

A)2)0.
B)12.0.
C)7)0.
D)5)0.
E)9)0.

Question 42

The bonds that are broken when water vaporizes are

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 43

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?

A)1 × 10⁻¹⁰ mol of hydroxyl ion per liter of lake water
B)1 × 10⁻⁴ mol of hydroxyl ion per liter of lake water
C)10.0 M with regard to hydroxyl ion concentration
D)4)0 M with regard to hydroxyl ion concentration
E)both B and D

Question 44

Pure, freshly-distilled water has a pH of 7. This means that

A)there are no H⁺ ions in the water.
B)there are no OH⁻ ions in the water.
C)the concentration of H⁺ ions in the water equals the concentration of OH⁻ ions in the water.
D)the concentration of H⁺ ions in the water is 7 times the concentration of OH⁻ ions in the water.
E)The concentration of OH⁻ ions in the water is 7 times the concentration of H⁺ ions in the water.

Question 45

Equal volumes of vinegar from a freshly-opened bottle are added to each of the following solutions. After complete mixing, which of the mixtures will have the highest pH?

A)100 mL of pure water
B)100 mL of freshly-brewed coffee
C)100 mL of household cleanser containing 0.5M ammonia
D)100 mL of freshly-squeezed orange juice
E)100 mL of tomato juice

Question 46

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?

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 47

Research indicates that acid precipitation can damage living organisms by

A)buffering aquatic systems such as lakes and streams.
B)decreasing the H⁺ concentration of lakes and streams.
C)increasing the OH⁻ concentration of lakes and streams.
D)washing away certain mineral ions that help buffer soil solution and are essential nutrients for plant growth.
E)both B and C

Question 48

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.

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 49

A 100 mL beaker contains 10 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 results of this mixing?

A)The concentration of Na⁺ ion rises.
B)The concentration of Cl⁻ ion falls.
C)The concentration of undissociated H₂O molecules remains unchanged.
D)The pH of the beaker's contents rises.
E)The pH of the beaker's contents falls.

Question 50

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?

A)
B)
C)
D)
E)

Question 51

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

A)4 times more
B)400 times more
C)4,000 times more
D)10,000 times more
E)100,000 times more

Question 52

One liter of a solution pH 9 has how many more hydroxyl ions (OH⁻)than 1 L of a solution of pH 4?

A)5 times more
B)100 times more
C)1,000 times more
D)10,000 times more
E)100,000 times more

Question 53

Carbon dioxide (CO₂)is readily soluble in water, according to the equation CO₂ + H₂O → H₂CO₃. Carbonic acid (H₂CO₃)is a weak acid. Respiring cells release CO₂. What prediction can we make about the pH of blood as that blood first comes in contact with respiring cells?

A)Blood pH will decrease slightly.
B)Blood pH will increase slightly.
C)Blood pH will remain unchanged.
D)Blood pH will first increase, then decrease as CO₂ combines with hemoglobin.
E)Blood pH will first decrease, then increase sharply as CO₂ combines with hemoglobin.

Question 54

Buffers are substances that help resist shifts in pH by

A)releasing H⁺ in acidic solutions.
B)donating H⁺ to a solution when they have been depleted.
C)releasing OH⁻ in basic solutions.
D)accepting H⁺ when the are in excess.
E)Both B and D are correct.

Question 55

Which of the following statements is True about buffer solutions?

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 constant pH of exactly 7 in all living cells and biological fluids.
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 56

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

A)solution Y has no free hydrogen ions (H⁺).
B)the concentration of hydrogen ions in solution X is 30 times as great as the concentration of hydrogen ions in solution Y.
C)the concentration of hydrogen ions in solution Y is 1,000 times as great as the concentration of hydrogen ions in solution X.
D)the concentration of hydrogen ions in solution X is 3 times as great as the concentration of hydrogen ions in solution Y.
E)None of the other answer choices correctly describes these solutions.

Question 57

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

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 58

If the pH of a solution is increased from pH 5 to pH 7, it means that the

A)concentration of H⁺ is twice (2X)what it was at pH 5.
B)concentration of H⁺ is half (1/2)what it was at pH 5.
C)concentration of OH⁻ is 100 times greater than what it was at pH 5.
D)concentration of OH⁻ is one-hundredth (0.01X)what it was at pH 5.
E)concentration of H⁺ is 100 times greater and the concentration of OH⁻ is one-hundredth what they were at pH 5.

Question 59

A slice of pizza has 500 kcal. If we could burn the pizza and use all the heat to warm a 50-L container of cold water, what would be the approximate increase in the temperature of the water? (Note: A liter of cold water weighs about 1 kg.)

A)50°C
B)5°C
C)10°C
D)100°C
E)1°C

Question 60

One of the buffers that contribute 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

A)a decrease in the concentration of H₂CO₃ and an increase in the concentration of H₂O.
B)an increase in the concentration of H₂CO₃ and a decrease in the concentration of H₂O.
C)a decrease in the concentration of HCO₃⁻ and an increase in the concentration of H₂O.
D)an increase in the concentration of HCO₃⁻ and a decrease in the concentration of H₂O.
E)a decrease in the concentration of HCO₃⁻ and an increase in the concentration of both H₂CO₃ and H₂O.

Question 61

We can be sure that a mole of table sugar and a mole of vitamin C are equal in their

A)mass in daltons.
B)mass in grams.
C)number of molecules.
D)number of atoms.
E)volume.

Question 62

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.)

A)10.0 g
B)0)1 g
C)6)0 g
D)60.0 g
E)0)6 g

Question 63

Draw three water molecules and label the atoms. Draw solid lines to indicate covalent bonds and dotted lines for hydrogen bonds. Add partial charge labels as appropriate.

Question 64

Which of the following is a hydrophobic material?

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

Question 65

What is the hydroxide ion concentration of the lake described in question 7?

A)10⁻⁷ M
B)10⁻⁴ M
C)10⁻¹⁰ M
D)10⁻¹⁴ M
E)10 M

Question 66

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

A)4)0 M
B)10⁻¹⁰ M
C)10⁻⁴ M
D)10⁴ M
E)4%