1. Ch. 3 Warm-Up
What property of water allows a water strider to “walk” on water?
Contrast adhesion and cohesion. Give an example of each.
Contrast hydrophobic and hydrophilic substances. Give an example of each.

2. Water and the Fitness of the Environment
Chapter 2.5
Water and the Fitness of the Environment

3. You Must Know
The importance of hydrogen bonding to the properties of water.
Four unique properties of water, and how each contributes to life on Earth.
How to interpret the pH scale.
The importance of buffers in biological systems.

4. 1. Polarity of H2O
O- will bond with H+ on a different molecule of H2O = hydrogen bond
H2O can form up to 4 bonds

5. 2. Properties of H2O Cohesion = H-bonding between like molecules
Surface Tension = measure of how difficult it is to break or stretch surface of liquid

6. Adhesion = bonding between unlike molecules
2. Properties of H2O
Adhesion = bonding between unlike molecules
Adhesion of H2O to vessel walls counters ↓ pull of gravity

7. H2O clings to each other by cohesion; cling to xylem tubes by adhesion
2. Properties of H2O
C. Transpiration = movement of H2O up plants
H2O clings to each other by cohesion; cling to xylem tubes by adhesion

8. 3. Moderation of temperature
Heat = Total amount of KE in system Temperature = measure intensity of heat due to average KE of molecules Which has higher temp? More heat?

9. 3. Moderation of temperature
Water’s high specific heat
Change temp less when absorbs/loses heat
Large bodies of water absorb and store more heat  warmer coastal areas
Create stable marine/land environment
Humans ~65% H2O  stable temp, resist temp. change

10. 3. Moderation of temperature
Evaporative Cooling
Water has high heat of vaporization
Molecules with greatest KE leave as gas
Stable temp in lakes & ponds
Cool plants
Human sweat

11. 3. Moderation of temperature
Insulation by ice – less dense, floating ice insulates liquid H2O below
Life exists under frozen surface (ponds, lakes, oceans)
Ice = solid habitat (polar bears)

13. A meniscus is the curve of water inside a test tube
A meniscus is the curve of water inside a test tube. Based on what you know about the properties of water, choose the answer that BEST describes how this phenomenon works

14. 4. Solvent of life
Solution = liquid, homogeneous mixture of 2+ substances
Solvent = dissolving agent (liquid)
Solute = dissolved substance
Water = versatile solvent

15. Hydrophilic Hydrophobic
4. Solvent of life
“like dissolves like”
Hydrophilic
Hydrophobic
Affinity for H2O
Repel H2O
Polar, ions
Nonpolar
Cellulose, sugar, salt
Oils, lipids
Blood
Cell membrane

16. What dissolves in water?
Hydrophilic
substances have attraction to H2O
polar or non-polar?
Hydrophilic
substances have attraction to H2O

17. What doesn’t dissolve in water?
Hydrophobic
substances that don’t have an attraction to H2O
polar or non-polar?
Oh, look hydrocarbons!
Hydrophobic
substances that don’t have an attraction to H2O
fat (triglycerol)

18. Figure 3.8 A water-soluble protein

19. Making solutions Find the mass of the compound (molar mass)
Multiply the atomic mass of an element by the number of atoms of that element in a compound
Add all of the masses together = total mass of the compound
Dilute the molar mass to the required volume with distilled water (Molarity)

20. Calculating Concentrations
CiVi=CfVf
C= concentration
V= volume
i= initial
f= final

21. Practice
53.4 mL of a 1.50 M solution of NaCl is on hand, but you need some M solution. How many mL of M can you make?
(1.50 mol/L) (53.4 mL) = (0.800 mol/L) (x)
x = 100. mL

22. 5. Acids and Bases
H2O H+ + OH- (gains proton) H+ + H2O  H3O+ (hydronium ion) (loses proton) H2O – H+  OH- (hydroxide ion)

23. 7 14 Basic Acidic pH Scale 5. Acids and Bases
Acid = increases H+ concentration (HCl)
Base = reduces H+ concentration (NaOH)
Most biological fluids are pH 6-8 7 14
Basic
Acidic
pH Scale

24. pH Scale H+ Ion Concentration Examples of Solutions pH
10–1
H+ Ion
Concentration
Examples of Solutions
Stomach acid, Lemon juice 1 pH
100
Hydrochloric acid
10–2 2
10–3
Vinegar, cola, beer 3
10–4
Tomatoes 4
10–5
Black coffee, Rainwater 5
10–6
Urine, Saliva 6
10–7
Pure water, Blood 7
10–8
Seawater 8
10–9
Baking soda 9
10–10
Great Salt Lake 10
10–11
Household ammonia 11
10–12
Household bleach 12
10–13
Oven cleaner 13
10–14
Sodium hydroxide 14
tenfold change in H+ ions
pH1  pH2
10-1  10-2
10 times less H+
pH8  pH7
10-8  10-7
10 times more H+
pH10  pH8
10-10  10-8
100 times more H+
In pure water only 1 water molecule in every 554 million is dissociated
tenfold change in H+ ions
pH1  pH2
10-1  10-2
10 times less H+
pH8  pH7
10-8  10-7
10 times more H+
pH10  pH8
10-10  10-8
100 times more H+

25. Figure 3.10 The pH scale and pH values of some aqueous solutions

26. Calculating pH -log 10-2 = -(-2) = 2 Therefore, pH = 2 [H+] = 10-4
[H+][OH-] = 10-14
If [H+] = 10-6 M, then [OH-] = 10-8
pH = -log [H+]
If [H+] = 10-2
-log 10-2 = -(-2) = 2
Therefore, pH = 2
If [OH-] = 10-10
[H+] = 10-4
-log 10-4 = -(-4) = 4
Therefore, pH = 4

27. H2CO3 (carbonic acid)  HCO3- (bicarbonate) + H+
5. Acids and Bases
Buffers: minimize changes in concentration of H+ and OH- in a solution (weak acids and bases)
Buffers keep blood at pH ~7.4
If blood drops to 7 or up to 7.8, then death
Carbonic Acid – Bicarbonate System: important buffers in blood plasma
H2CO3 (carbonic acid)  HCO3- (bicarbonate) + H+

28. Ocean acidification threatens coral reef ecosystems
CO2 mixed with seawater  Carbonic acid (lowers ocean pH)

29. The effects of acid precipitation on a forest

30. Examples of Benefits to Life
H2O Property
Chemical Explanation
Examples of Benefits to Life
Cohesion
polar
H-bond
like-like
↑gravity plants, trees
Adhesion
unlike-unlike
plants xylem
bloodveins
Surface Tension
diff. in stretch
break surface
bugswater
Specific Heat
Absorbs & retains E
oceanmod temp protect marine life
Evaporation
liquidgas KE
Cooling
Homeostasis
Universal Substance
Polarityionic
Good dissolver
solvent