1. 3 Water and Life Lecture Presentation by Nicole Tunbridge and3
Water and Life
Lecture Presentation by Nicole Tunbridge and
Kathleen Fitzpatrick

2. Figure 3.1 What role does the chemistry of water play in the development of whooper swans?
Figure 3.1 How does the habitat of a whooper swan depend on the chemistry of water?

3. Figure 3.2 Explain how four (4) hydrogen bonds can occur between five (5) water molecules.−
Hydrogen bond +
Polar covalent bonds − + − + −
Figure 3.2 Hydrogen bonds between water molecules +

4. Two types of water- conducting cells
Figure 3.3 Explain the role of cohesion, adhesion, evaporation, and transpiration on the transport of water in plants.
H2O
Adhesion
Two types of water- conducting cells
Figure 3.3 Water transport in plants
Direction of water movement
Cohesion
300 m
H2O
H2O

5. Figure 3.4 Explain the role surface tension plays in this water strider’s ability to walk on water.
Figure 3.4 Walking on water

6. Los Angeles (Airport) 75° Santa Ana 84° Palm Springs 106° 70s (F) 80s
Figure 3.5a Explain how water’s high specific heat helps moderate inland temperature. Why is this important in the distribution of organisms?
San Bernardino 100°
Burbank 90°
Santa Barbara 73°
Riverside 96°
Los Angeles (Airport) 75°
Santa Ana
84°
Palm Springs 106°
70s (F)
80s
90s
100s
Pacific Ocean 68°
Figure 3.5 Temperatures for the Pacific Ocean and Southern California on an August day
San Diego 72°
40 miles

7. Figure 3.5b Explain how water’s high heat of vaporization, evaporative cooling, and the release of water molecules on the surface of skin (sweat) contributes to regulation of internal body temperature (thermoregulation). (Critical thinking question!)

8. Liquid water: Hydrogen bonds break and re-form
Figure 3.6 Discuss the role hydrogen bonding plays in the ability of water to be a solid and a liquid.
Hydrogen bond
Liquid water: Hydrogen bonds break and re-form
Ice: Hydrogen bonds are stable
Figure 3.6 Ice: crystalline structure and floating barrier

9. Figure 3.6a How would this organism’s life be different if ice was denser than water?
Figure 3.6a Ice: crystalline structure and floating barrier (part 1: krill)

10. − Na+ + + − − + − − Na+ − + + Cl– Cl− + − − + − + − −
Figure 3.7 In this figure, identify the solute and solvent. Explain how the number of hydration shells would change if the solution were heated for a long time? −
Na+ + + − − + − −
Na+ − + +
Cl–
Cl− + − − + − + −
Figure 3.7 Table salt dissolving in water −

11. Figure 3. 8a Why is water an ideal biological solvent
Figure 3.8a Why is water an ideal biological solvent? Explain whether this protein is hydrophilic or hydrophobic. δ+ δ− δ− δ+
Figure 3.8 A water-soluble protein

12. Figure 3.8b Glucose is a molecule used by the mitochondria to generate ATP. The molar mass of glucose is g/mol. Explain how to make 500ml of a 0.80M glucose solution in water.
Figure 3.9 Evidence for subsurface liquid water on Mars

13. Hydronium ion (H3O+) Hydroxide ion (OH−)
Figure 3.UN01 What is the conventional term for a hydronium ion? Write it below the hydronium ion represented in this figure. What is the concentration of each ion in pure water? + −
2 H2O
Hydronium ion (H3O+)
Hydroxide ion (OH−)
Figure 3.UN01 In-text figure, dissociation of water, p. 51

14. H+ OH− OH− H+ OH− OH− H+ OH− H+ H+ H+ OH− OH− OH− OH− OH− OH− OH− H+
Figure 3.10a Identify each solution as acidic, basic, or neutral. Explain your reasoning. H+
OH−
OH− H+
OH−
OH− H+
OH− H+ H+ H+
OH−
OH−
OH−
OH−
OH−
OH−
OH− H+ H+
OH− H+
OH− H+ H+ H+ H+ H+
Figure 3.10a The pH scale and pH values of some aqueous solutions (part 1: ions)

15. Increasingly Acidic [H+] > [OH−] Increasingly Basic [H+] < [OH−]
Figure 3.10a Write out the formula for determining the pH of a solution. What is the difference in hydrogen ion concentration between tomato juice and household ammonia. Does this represent an increase or decrease in hydroxide ion concentration?
pH Scale 1 2 3 4 5 6 7 8 9 10 11 12 13 14
Battery acid
Gastric juice, lemon juice H+ H+ H+
Vinegar, wine, cola H+
OH–
OH– H+ H+
Increasingly Acidic [H+] > [OH−] H+ H+
Acidic solution
Tomato juice Beer
Black coffee Rainwater
Urine
Saliva
OH–
OH–
Neutral [H+] = [OH−]
Pure water
Human blood, tears H+ H+
OH–
OH–
OH– H+ H+ H+
Seawater Inside of small intestine
Neutral solution
Figure 3.10 The pH scale and pH values of some aqueous solutions
Increasingly Basic [H+] < [OH−]
Milk of magnesia
OH–
OH–
OH– H+
OH–
Household ammonia
OH–
OH– H+
OH–
Basic solution
Household bleach
Oven cleaner

16. Figure 3.10b Write the chemical reaction of carbonic acid in response to a rise and drop in pH. How would the reaction shift if HCl was added? NaOH? How do buffers moderate pH change?
Figure 3.UN04 Summary of key concepts: pH scale

17. Figure Explain how the burning of fossil fuels is contributing to the ocean acidification process.
CO2
CO2 + H2O → H2CO3
H2CO3 → H+ + HCO3−
H+ + CO32− → HCO3−
Figure 3.11 Atmospheric CO2 from human activities and its fate in the ocean
CO32− + Ca2+ → CaCO3