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Chapter 3 AP Biology

front 1

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

back 1

polar covalent bonds

front 2

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?

back 2

a hydrogen bond

front 3

An example of a hydrogen bond is the bond between

back 3

the H of one water molecule and the O of another water molecule

front 4

Water is able to form hydrogen bonds because

back 4

the bonds that hold together the atoms in a water molecule are polar covalent bonds

front 5

What gives rise to the cohesiveness of water molecules?

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hydrogen bonds

front 6

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

back 6

a water strider can walk across the surface of a small pond

front 7

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

back 7

Kinetic energy in the drink decreases

front 8

Which of the following statements correctly defines a kilocalorie?

back 8

the amount of heat required to raise the temperature of 1kg of water by 1°C

front 9

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 20kg of water how many degrees Celsius?

back 9

10.0°C

front 10

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

back 10

absorption and release of heat when hydrogen bonds break and form

front 11

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

back 11

hydrogen bonds

front 12

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

back 12

the release of heat by the formation of hydrogen bonds

front 13

At what temperature is water at its densest?

back 13

4°C

front 14

Why does ice float in liquid water?

back 14

Hydrogen bonds stabilize and keep the molecules of ice farther apart than the water molecules of liquid water

front 15

The following question is based on the figure of a solute molecule surrounded by a hydration shell of water. Based on your knowledge of the polarity of water molecules, the solute molecule is most likely

back 15

positively charged

front 16

Hydrophobic substances such as vegetable oil are

back 16

nonpolar substances that repel water molecules

front 17

One mole (mol) of a substance is

back 17

6.02E23 molecules of the substance and the molecular mass of the substance expressed in grams

front 18

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

back 18

6.02E23

front 19

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

back 19

6.02E23

front 20

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)?

back 20

1 L of 1.0M NaCl

front 21

The molecular mass of glucose (C6H12O6) is 180g. Which of the following procedures should you carry out to make a 1M solution of glucose?

back 21

Dissolve 180g of glucose in water, and then add more water until the total volume of the solution is 1 L

front 22

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

back 22

Dissolve 90g of glucose in a small volume of water, and then add more water until the total volume of the solution is 1 L

front 23

How many grams of the molecule CH3COOH (C=12, O=16, H=1) would be equal to 1 mol of the molecule?

back 23

60

front 24

How many grams of the molecule CH3COOH would be required to make 1L of a 0.5M solution of the molecule? (C=12, O=16, H=1)

back 24

30

front 25

How many grams of the molecule CH3COOH would be required to make 2.5L of a 1M solution of the molecule? (C=12, O=16, H=1)

back 25

150

front 26

A small birthday candle is weighed, then lighted and placed beneath a metal can containing 100mL 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?

back 26

0.5 kilocalories per gram of wax burned

front 27

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?

back 27

graph

front 28

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

back 28

6.02E24

front 29

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

back 29

55.6M

front 30

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

back 30

6.02E24

front 31

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

back 31

HCl

front 32

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

back 32

NaOH

front 33

Which of the following statements is completely correct?

back 33

NH₃ is a weak base (alkali) and H₂CO₃ is a strong acid

front 34

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

back 34

acidic: H⁺ donor

front 35

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

back 35

neutral

front 36

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

back 36

pH 2

front 37

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

back 37

pH 8

front 38

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

back 38

gastric juice at pH 2

front 39

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

back 39

seawater at pH 8

front 40

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

back 40

concentration of H⁺ has increased 10-fold (10X) compared to what it was at pH9 and concentration of OH⁻ has decreased to one-tenth (1/10) what it was at pH 9

front 41

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

back 41

concentration of OH⁻ is 100 times greater than what it was at pH 5

front 42

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

back 42

10,000 times more

front 43

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

back 43

100,000 times more

front 44

Which of the following statements is true about buffer solutions?

back 44

they maintain a relatively constant pH when either acids or bases are added to them

front 45

Buffers are substances that help resist shifts in pH by

back 45

Donating H⁺ to a solution when they have been depleted and accepting H⁺ when they are in excess

front 46

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

back 46

the HCO₃⁻ to act as a base and remove excess H⁺ with the formation of H₂CO₃

front 47

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

back 47

a decrease in the concentration of H2CO3 and an increase in the concentration of H2O

front 48

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?

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1x10⁻¹⁰ mol of hydroxyl ion per liter of lake water

front 49

Research indicates that acid precipitation can damage living organisms by

back 49

washing away certain mineral ions that help buffer soil solution and are essential nutrients for plant growth

front 50

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

back 50

none of the other answer choices correctly describes these solutions

front 51

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

back 51

the concentration of H+ ions in the water equals the concentration of OH- ions in the water

front 52

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?

back 52

c

front 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?

back 53

blood pH will decrease slightly

front 54

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?

back 54

the pH of the beaker's contents falls

front 55

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?

back 55

100mL of household cleanser containing 0.5M ammonia

front 56

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.

back 56

NaCl crystals will dissolve readily in water but will not dissolve in methanol

front 57

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

back 57

7.0