1. Ch.3 Life on Earth is Aqueous!

2. Predominance of Water -3/4 of earth covered with water (liquid & solid) -cells are 70-95% water -all organisms require water for survival ~ 1 week survival time for human without water

3. LE 3-2 Hydrogen bonds

4. Key properties of water defines behavior -Polarity: partial positive and negative charges -Hydrophilic nature: attracted to other water molecules and charged particles

5. Four of water’s properties Cohesive behavior Ability to moderate temperature Expansion upon freezing Versatility as a solvent

6. LE 3-3 Water-conducting cells 100 µm Cohesion & Adhesion During Transpiration H2OH2O >100 ft

7. Cohesion Water molecules hold together through H-bonds to other water molecules Example Cohesion helps transport water against gravity in plants from roots to stems during transpiration Adhesion Water’s attraction to other charged surfaces Example Water’s attraction to cell walls helps upward transport against gravity

8. Surface Tension: Strong ordered film-like structure at interface of water and atmosphere Held together through H-bonds Strength creates surface for small organisms to move across

9. Consequence –Lessens temperature fluctuations to within limits that permit life –Heat is absorbed to hydrogen bonds break –Heat is released when hydrogen bonds form High specific heat 1 cal/g/ o C Amount of heat gained or lost to change the temperature of 1g of water by 1ºC Compare to alcohol: specific heat of 0.6 cal/g/ o C

10. Evaporative Cooling –transformation of a substance from liquid to gas –Heat of vaporization the heat a liquid must absorb for 1 gram to be converted to gas (water: ~580 cal/g at 25 o C) remaining surface cools during evaporation, a process called evaporative cooling Consequence Evaporative cooling of water helps stabilize temperatures in organisms and bodies of water Perspiration: sensation?

11. Solid water (ice) : less dense than liquid because H-bonds more stable and ordered; expansion occurs Consequence: Ice floats on liquid water Insulates; prevents temperature fluctuations Example: ponds and lakes in wintertime aquatic organisms survive in the liquid water beneath ice

13. Polar solvent Dissolves other polar or charged solutes Examples: salts, polar proteins, nucleic acids Creates an aqueous solution -through Hydration shells H-bonds

14. LE 3-6 Na + Cl – + + + + + + + + – – – – – – – – – – – Hydration shells form around cations and anions Causes salt crystals to dissolve In H 2 O

15. LE 3-7a Lysozyme molecule in a nonaqueous environment.

16. LE 3-7b Lysozyme molecule in a aqueous environment.

17. Hydrophilic –an affinity for water due to charged or polar nature e.g. salts (ionic) Hydrophobic -repelled by water due to nonpolar nature e.g. oils, fats (nonpolar) Important when considering the plasma membrane. Concepts of Hydrophilic and Hydrophobic

18. Most biochemical reactions occur in water Reactions require collisions of molecules - dependent on concentration of solutes in an aqueous solution Example: increase the concentration of enzyme in an reaction and the rate of the reaction will increase. Cells can regulate how much enzyme they make to control reaction rates. Aqueous chemistry in biological systems

19. Results: –molecule with the extra proton is now a hydronium ion (H 3 O + ) –The molecule that lost the proton is now a hydroxide ion (OH - ) Water Dissociation - Hydrogens involved in H-bonds in H 2 O can lose electrons -H+ (proton) can bond with another H 2 O molecule

20. LE 3-UN53 Hydronium ion (H 3 O + ) Hydroxide ion (OH – ) Simplified to H+

21. Dissociation of water molecules Rare in pure water (25 o C) » [H+]=10^-7 M »[OH-]=10^-7 M » Changes in concentrations of H + and OH - drastically affect the chemistry of a cell Such changes alter the pH

22. pH -measures molar concentration of H+ in solution pH= -log[H+] -adding acid to a solution increases the [H+] more acidic e.g. HCl -adding base to a solution increases the [OH-] more basic (alkali) e.g. NaOH -pH scale measures level of acidity or alkalinity

23. The pH Scale pH 7 occurs when [H+] =[OH-] Acidic solutions pH < 7 Basic solutions pH > 7 Most biological fluids: pH 6-8

24. LE 3-8 pH Scale 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14 Oven cleaner Household bleach Household ammonia Milk of magnesia Seawater Pure water Human blood Urine Rainwater Black coffee Tomato juice Vinegar, beer, wine, cola Digestive (stomach) juice, lemon juice Battery acid Neutral [H + ] = [OH – ] Increasingly Acidic [H + ] > [OH – ] Increasingly Basic [H + ] < [OH – ]

25. Given: pH= -log[H+] Water ion product 10^-14= [H+][OH-] Calculating pH What is the pH of a solution containing 10^-7 M H+? In the same solution, what is the concentration of OH-? Determine the concentration of H+ and OH- at pH 3.

26. Buffers pH of most living cells must remain close to pH 7 Buffers minimize changes in [H +] and [OH - ]in a solution Most buffers consist of an acid-base pair that reversibly combines with H + H 2 CO 3 HCO 3 - + H+ carbonic acid bicarbonate

27. The Damage of Acid Precipitation Acid precipitation refers to rain, snow, or fog with a pH lower than 5.6 Caused by the mixing of different pollutants with water in the air e.g. sulfur and nitrogen oxides Main source: combusted fossil fuels Acid precipitation can damage life in lakes and streams –Leaches geological buffers from soils –Solubilizes toxic heavy metals e.g. aluminum

28. LE 3-9 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14 More basic Normal rain More acidic Acid rain