2. 1. The Molecule That Supports All of Life
• Water is the biological medium on Earth
• Most cells are surrounded by water, and cells
themselves are about 70-95% water
3. 2. Four emergent properties of water contribute
to Earth’s fitness for life
• Four of water’s properties that facilitate an
environment for life:
Cohesive behavior
Ability to moderate temperature
Expansion upon freezing
Versatility as a solvent
4. 3. Evaporative Cooling
• Evaporation is transformation of a substance from
liquid to gas
• Heat of vaporization is the heat a liquid must absorb
for 1 gram to be converted to gas
• As a liquid evaporates, its remaining surface cools, a
process called evaporative cooling
• Evaporative cooling of water helps stabilize
temperatures in organisms and bodies of water
5. 4. Insulation of Bodies of Water by
Floating Ice
• Ice floats in liquid water because hydrogen bonds in ice
are more “ordered,” making ice less dense
• If ice sank, all bodies of water would eventually freeze
solid, making life impossible on Earth
6. 5. The Solvent of Life
• A solution is a liquid that is a homogeneous mixture of
substances
• A solvent is the dissolving agent of a solution
• The solute is the substance that is dissolved
• Water is a versatile solvent due to its polarity
• An aqueous solution is one in which water is the
solvent
7. • Water is an effective solvent because it readily forms
hydrogen bonds
• When an ionic compound is dissolved in water, each
ion is surrounded by a sphere of water molecules, a
hydration shell
9. • Water can also dissolve compounds made of nonionic
polar molecules
• Even large polar molecules such as proteins can
dissolve in water if they have ionic and polar regions
12. Hydrophilic and Hydrophobic
Substances
• A hydrophilic substance is one that has an affinity for
water
• A hydrophobic substance is one that does not have an
affinity for water
• Oil molecules are hydrophobic because they have
relatively nonpolar bonds
• A colloid is a stable suspension of fine particles in a
liquid
13. Solute Concentration in Aqueous
Solutions
• Most biochemical reactions occur in water
• Chemical reactions depend on collisions of molecules
and therefore on the concentration of solutes in an
aqueous solution
14. 6. Dissociation of water molecules leads to acidic
and basic conditions that affect living organisms
• A hydrogen atom in a hydrogen bond between two
water molecules can shift from one to the other:
– The hydrogen atom leaves its electron behind and is
transferred as a proton, or hydrogen ion (H+)
– The molecule with the extra proton is now a
hydronium ion (H3O+)
– The molecule that lost the proton is now a
hydroxide ion (OH-)
16. • The process can be described in a simplified way as the
separation of a water molecule into a hydrogen ion (H+)
and a hydroxide ion (OH-)
• Though statistically rare, the dissociation of water
molecules has a great effect on organisms
• Changes in concentrations of H+ and OH- can drastically
affect the chemistry of a cell
17. Effects of changes in pH
• Concentrations of H+ and OH- are equal in pure water
• Adding certain solutes, called acids and bases, modifies
the concentrations of H+ and OH-
• The pH scale describes how acidic or basic (the
opposite of acidic) a solution is
18. Acids and Bases
• An acid is any substance that increases the H+
concentration of a solution
• A base is any substance that reduces the H+
concentration of a solution
19. The pH Scale
• The pH of a solution is determined by the relative
concentration of hydrogen ions
• Acidic solutions have pH values less than 7
• Basic solutions have pH values greater than 7
• Most biological fluids have pH values in the range of 6
to 8
20. • In any aqueous solution at 25°C the product of
H+ and OH– is constant and can be written as
[H+][OH–] = 10–14
• The pH of a solution is defined by the negative
logarithm of H+ concentration, written as
pH = –log [H+]
• For a neutral aqueous solution
[H+] is 10–7 = –(–7) = 7
21. • What would be the pH of a solution with a
hydroxide ion [OH-] concentration of 10-12 M?
A) pH 2
B) pH 4
C) pH 10
D) pH 12
E) pH 14
23. Buffers
• The internal pH of most living cells must remain close
to pH 7
• Buffers are substances that minimize changes in
concentrations of H+ and OH- in a solution
• Most buffers consist of an acid-base pair that reversibly
combines with H+
24. 8. The Threat of Acid Precipitation
• Acid precipitation refers to rain, snow, or fog with a pH
lower than 5.6
• Acid precipitation is caused mainly by the mixing of
different pollutants with water in the air
• Acid precipitation can damage life in lakes and streams
• Effects of acid precipitation on soil chemistry are
contributing to the decline of some forests
25. Property Remarks
Importance to the
environment
1. Physical state
Only substance occurring
naturally in all three phases
as solid, liquid, and gas on
Earth's surface
Transfer of heat between
ocean and atmosphere by
phase change
2. Dissolving ability
Dissolves more substances
in greater quantities than
any other common liquid
Important in chemical,
physical, and biological
processes
3. Density: mass per unit
volume
Density is determined by
(1) temperature, (2)
salinity, and (3) pressure, in
that order of importance.
The temperature of
maximum density for pure
water is 4 °C. For seawater,
the freezing point
decreases with increasing
salinity
Controls oceanic vertical
circulation, aids in heat
distribution, and allows
seasonal stratification
4. Surface tension
Highest of all common
liquids
Controls drop formation in
rain and clouds; important
in cell physiology
26. Property Remarks
Importance to the
environment
5. Conduction of heat
Highest of all common
liquids
Important on the small
scale, especially on cellular
level
6. Heat capacity
Highest of all common
solids and liquids
Prevents extreme range in
Earth's temperatures (i.e.,
great heat moderator)
7. Latent heat of fusion
Highest of all common
liquids and most solids
Thermostatic heat-
regulating effect due to the
release of heat on freezing
and absorption on melting
8. Latent heat of
vaporization
Highest of all common
substances
Immense importance: a
major factor in the transfer
of heat in and between
ocean and atmosphere,
driving weather and
climate
9. Refractive index
Increases with increasing
salinity and decreases with
increasing temperature
Objects appear closer than
in air
27. Property Remarks
Importance to the
environment
10. Transparency
Relatively great for visible
light; absorption high for
infrared and ultraviolet
Important for
photosynthesis
11. Sound transmission
Good compared with other
fluids
Allows for sonar and
precision depth recorders
to rapidly determine water
depth, and to detect
subsurface features and
animals; sounds can be
heard great distances
underwater
12. Compressibility Only slight
Density changes only
slightly with
pressure/depth
13. Boiling and melting
points
Unusually high
Allows water to exist as a
liquid on most of Earth
