Name _________________
AP Biology Study Guide
Chapter 3: Water and the Fitness of the Environment
Concept 3.1 The polarity of water molecules results in hydrogen bonding
1.
Study the water molecules at the right. On the
central molecule, label oxygen (O) and hydrogen (H).
2.
What is a polar molecule?
Why is water considered polar?
3.
4.
Now, add + and – signs to indicate the charged regions of
each molecule. Then, indicate the hydrogen bonds.
Explain hydrogen bonding.
How many hydrogen bonds can a single water molecule form?
Concept 3.2 Four emergent properties of water contribute to Earth’s fitness for life
Hydrogen bonding accounts for the unique properties of water. Let’s look at several.
Cohesion
5.
Distinguish between cohesion and adhesion.
6.
What is demonstrated when you see beads of water on a waxed car hood?
7.
Describe what surface tension is and explain what feature of hydrogen bonds causes it.
8.
Which property explains the ability of a water strider to walk on water?
Moderation of Temperature
9.
The calorie is a unit of heat. Define calorie.
10.
Water has high specific heat. What does this mean?
How does water’s specific heat compare to alcohol’s?
11.
Explain how hydrogen bonding contributes to water’s high specific heat.
12.
Summarize how water’s high specific heat contributes to the moderation of temperature.
13.
How is this property important to life?
Define evaporation.
What is heat of vaporization?
Explain at least three effects of this property on living organisms.
Expansion upon Freezing
14.
Ice floats! So what? Consider what would happen if ponds and other bodies of water accumulated ice
at the bottom.
Describe why this property of water is important.
15.
Now, explain why ice floats.
Why is 4oC the critical temperature in this phenomenon?
Solvent of Life
16.
Review and define these terms:
solvent
solution
solute
17.
Consider coffee to which you have added sugar. Which is the solvent? The solute?
18.
Explain why water is such a fine solvent.
19.
Define hydrophobic and hydrophilic.
20.
Now, let’s do a little work that will enable you to prepare solutions. Read the section on solute
concentrations carefully, and show the calculations here for preparing a 1-molar solution of sucrose.
Steps to help you do this follow. The first step is done for you. Fill in the rest.
Steps to prepare a solution:
a. Here is the molecular formula. C12H22O11
b. Use your periodic table to calculate the mass of each element. Multiply by the number of atoms of
the element. (For example, O has a mass of 16. Therefore, one mole of O has a mass of 16 x 11 = 176
g/mole.)
c. Add the masses of each element in the molecule.
21.
d. If you add this mass of the compound to water to bring it to a volume of 1 liter. This makes 1 liter of
a 1-M (1 molar) solution.
Can you prepare 1 liter of a 0.5-molar glucose solution? Show your work here.
22.
Define molarity.
Concept 3.3 Acidic and basic conditions affect living organisms
23.
Label the diagram below to demonstrate the dissociation (ionization) of the water molecule and then
relate this diagram to pH.
23.
What two ions form when water dissociates?
You should have answered “hydronium (H3O+) and hydroxide ions (OH–)” in the preceding question. However,
by convention, we will represent the hydronium ion as H+.
24.
What is the concentration of each ion in pure water at 25 oC?
25.
Water has a pH of 7. pH is defined as the negative log of the hydrogen ion concentration [H+]. Can you
now see how water is assigned a pH of 7?
26.
To go a step further, the product of H+ and OH– concentrations is constant at 10–14.
[H+}[OH–} = 10–14.
27.
Water, which is neutral with a pH of 7, has an equal number of H+ and OH– ions. Now, define
acid
base
Because the pH scale is logarithmic, each numerical change represents a 10X change in ion
concentration.
a. So, how many times more acidic is a pH of 3 compared to a pH of 5?
28.
b. How many times more basic is a pH of 12 compared to a pH of 8?
c. Explain difference between a pH of 8 and a pH of 12 in terms of H+ concentration.
29.
On the pH chart, label pH 1–14. Label neutral, acid, base.
Indicate the locations of pure water, urine, gastric (stomach)
juice, and bleach.
30.
The carbonic acid/bicarbonate system is an important bio­
logical buffer. Label the molecules and ions in this equation and
indicate which is the H+ donor and which is the acceptor.
In which direction will this reaction proceed
a. when the pH of a solution begins to fall?
b. when the pH rises above normal level?
31.
Even a slight change in pH can be harmful! How do buffers
moderate pH change?
32.
Exercise will result in the production of CO2, which will
acidify the blood. Explain the buffering system that minimizes
blood pH changes.
MULTIPLE CHOICE: Choose the one best answer.
1.
Each water molecule is capable of forming
a. one hydrogen bond.
b. three hydrogen bonds.
c. four hydrogen bonds.
d. two covalent bonds and two hydrogen bonds.
e. two ionic bonds and two hydrogen bonds.
2.
The polarity of water molecules
a. promotes the formation of hydrogen bonds.
b. helps water to dissolve nonpolar solutes.
c. lowers the heat of vaporization and leads to evaporative cooling.
d. creates a crystalline structure in liquid water.
e. does all of the above.
3.
What accounts for the movement of water up the veins of a tall tree?
a. cohesion
b. hydrogen bonding
c. adhesion
d. hydrophilic cell walls
e. all of the above
4.
Climates tend to be moderate near large bodies of water because
a. a large amount of solar heat is absorbed during the gradual rise in temperature of the water.
b. water releases heat to the environment as it cools.
c. the high specific heat of water helps to moderate air temperatures.
d. a great deal of heat is absorbed and released as hydrogen bonds break or form.
e. of all of the above.
5.
Temperature is a measure of
a. specific heat.
b. average kinetic energy of molecules.
d. Celsius degrees.
e. joules.
6.
c. total kinetic energy of molecules.
Evaporative cooling is a result of
a. a low heat of vaporization.
b. the release of heat during the breaking of hydrogen bonds when water molecules escape.
c. the absorption of heat as hydrogen bonds break.
d. the reduction in the average kinetic energy of a liquid after energetic water molecules
enter the gaseous state.
e. both a and b.
7.
Ice floats because
a. air is trapped in the crystalline lattice.
b. the formation of hydrogen bonds releases heat; warmer objects float.
c. it has a smaller surface area than liquid water.
d. it insulates bodies of water so they do not freeze from the bottom up.
e. hydrogen bonding spaces the molecules farther apart, creating a less dense structure.
8.
The molarity of a solution is equal to
a. Avogadro's number of molecules in 1 liter of solvent.
b. the number of moles of a solute in 1 liter of solution.
c. the molecular mass of a solute in 1 liter of solution.
d. the number of solute molecules in 1 liter of solvent.
e. 342 g if the solute is sucrose.
9.
Some archaea are able to live in lakes with pH values of 11. How does pH 11 compare with the pH 7
typical of your body cells?
a. It is four times more acidic than pH 7.
b. It is four times more basic than pH 7.
c. It is a thousand times more acidic than pH 7.
d. It is a thousand times more basic than pH 7.
e. Itis ten thousand times more basic than pH 7.
10.
A buffer
a. changes pH by a magnitude of 10.
d. is often a weak acid-base pair.
11.
b. releases excess OH-.
c. releases excess H+.
e. always maintains a neutral pH.
Which of the following is least soluble in water?
a. polar molecules
b. nonpolar molecules
d. hydrophilic molecules
e. anions
c. ionic compounds
12.
Which would be the best method for reducing acid precipitation?
a. Raise the height of smokestacks so that exhaust enters the upper atmosphere.
b. Add buffers and bases to bodies of water whose pH has dropped.
c. Use coal-burning generators rather than nuclear power to produce electricity.
d. Tighten emission control standards for factories and automobiles.
e. Reduce the concentration of heavy metals in industrial exhaust.
13.
What bonds must be broken for water to vaporize?
a. polar covalent bonds
b. nonpolar covalent bonds
c. hydrogen bonds
d. ionic bonds
e. polar covalent and hydrogen bonds
14.
How would you make a 0.1M solution of glucose (C6H1206)? The mass numbers for these elements are
approximately: C = 12, 0 = 16, H = 1.
a. Mix 6 g C, 12 g H, and 6 g O in 1liter of water.
b. Mix 72 g C, 12 g H, and 96 g O in 1liter of water.
c. Mix 18 g of glucose with enough water to yield 1liter of solution.
d. Mix 29 g of glucose with enough water to yield 1liter of solution.
e. Mix 180 g of glucose with enough water to yield 1liter of solution.
15.
How many molecules of glucose would be in the 1liter 0.1M solution made in question 14?
a. 0.1
b. 6
c. 60
d. 6 x 1023
e. 6 X 1022
16.
Why is water such an excellent solvent?
a. As a polar molecule, it can surround and dis­ solve ionic and polar molecules.
b. It forms ionic bonds with ions, hydrogen bonds with polar molecules, and hydrophobic interac­
tions with nonpolar molecules.
c. It forms hydrogen bonds with itself.
d. It has a high specific heat and a high heat of vaporization.
e. It is wet and has a great deal of surface tension.
17.
Which of the following, when mixed with water, would form a colloid?
a. a large hydrophobic protein
b. a large hydrophilic protein
c. sugar
d. cotton
e. NaCl
18.
Adding a base to a solution would
a. raise the pH.
b. lower the pH.
c. decrease [H+].
d. do both a and c.
e. do both b and c.
19.
A hydration shell is most likely to form around
a. an ion.
d. both a and c.
b. a fat.
e. both b and c.
c. a sugar.
20.
The following are the pH values for each item: cola-2; orange juice-3; beer-4; coffee-5;
human blood-7.4. Which of these liquids has the highest molar concentration of OH-?
a. cola
b. orange juice
c. beer
d. coffee
e. human blood
21.
Comparing the [H+] of orange juice and coffee, the [H+] of
a. orange juice is 10 times higher.
b. orange juice is 100 times higher.
c. orange juice is 1,000 times higher.
d. coffee is 2 times higher.
e. coffee is 100 times higher.
22.
The ability of water molecules to form hydrogen bonds accounts for water's
a. high specific heat.
b. evaporative cooling.
c. high heat of vaporization.
d. cohesiveness and surface tension.
e. All of the above result from water's hydrogen­ bonding capacity.