1. Water and the Fitness of the Environment Chapter 3

2. Water Life depends on water Human body and cells  70- 95% water Abundance of water  Earth can support life Water exists in three possible states: ice, liquid, and vapor

3. Properties of Water Polar Molecule Cohesion- Adhesion High Surface Tension High Specific Heat Low Density of ice Excellent solvent

4. Structure of Water Water is a polar molecule  uneven distribution of charge between the hydrogen and oxygen atoms  regions of partial + and – charges Each water molecule can form H- bonds with up to 4 neighbors.

5. Structure of Water

6. Cohesion - Adhesion Cohesion  tendency of molecules of the same kind to stick together. Strongest in water. Adhesion  attraction between unlike molecules

7. Cohesion - Adhesion

8. Surface Tension Surface Tension  a measure of how difficult it is to stretch or break the surface of a liquid At the surface water molecules are H- bonded to one another and to the water molecules below  resist stretching or breaking the surface Water behaves as if covered by an invisible film.

9. Water Moderates Temperatures on Earth Water stabilizes air temperatures  absorbing heat from warmer air and releasing heat to cooler air. Water is a heat bank  can absorb or release relatively large amounts of heat with only a slight change in its own temperature

10. Heat and Temperature Kinetic Energy  the energy of motion Heat is a measure of the total quantity of kinetic energy due to molecular motion in a body of matter. Temperature measures the intensity of heat due to the average kinetic energy of molecules When two object of different temperature meet, heat passes from the warmer to the cooler until the two are the same temperature.

11. Temperature is measured on the Celsius scale ( o C).  At sea level, water freezes at O o C and boils at 100 o C.  Human body temperature averages 37 o C. Heat energy = calorie (cal)  One calorie is the amount of heat energy necessary to raise the temperature of 1 g of water by 1 o C.  Biological processes  the kilocalorie (kcal) A kilocalorie is the amount of heat energy necessary to raise the temperature of 1000g of water by 1 o C. The joule (J), is equivalent to 0.239 cal

12. High Specific Heat Water’s high specific heat is due to hydrogen bonding Water resists changes in temperature because it takes a lot of energy to speed up its molecules.

13. Evaporative Cooling As a liquid evaporates, the surface of the liquid that remains behind cools - evaporative cooling.  This occurs because the most energetic molecules are the most likely to evaporate, leaving the lower kinetic energy molecules behind. Evaporative cooling moderates temperature in lakes and ponds and prevents terrestrial organisms from overheating.  Evaporation of water from the leaves of plants or the skin of humans removes excess heat.

14. Low Density of Ice Water is unusual because it is less dense as a solid than as a liquid. Ice floats on the cool water below. This has important consequences for life.

15. Low Density of Ice If ice sank  all ponds, lakes, and oceans would freeze solid. The surface layer of ice insulates liquid water below, preventing it from freezing and allowing life to exist under the frozen surface.

16. Water is the Solvent of Life A liquid that is a completely homogeneous mixture of two or more substances is called a solution The dissolving agent is the solvent and the substance that is dissolved is the solute. In an aqueous solution, water is the solvent.

17. Water as an Aqueous Solution C 6 H 12 O 6  6(12)+12(1)+6(16)=180g= MW 180g =1 mole of glucose Add 1L H2O Avogadro's number 6.02x10 23 molecules /mole

18. Water surrounds and separates the positive and negative ions

19. The Dissociation of Water A hydrogen atom shared by two water molecules shifts from one molecule to the other.  leaves its electron behind and is transferred as a single proton - a hydrogen ion (H + ).  molecule that lost a proton is now a hydroxide ion (OH - ).

20. Dissociation of Water Water molecule dissociates into a hydrogen ion and a hydroxide ion:  H 2 O H + + OH - (reaction is reversible) At equilibrium the concentration of water molecules greatly exceeds that of H + and OH In pure water only one water molecule in every 554 million is dissociated.  At equilibrium the concentration of H + or OH - is 10 -7 M (25°C)  Adding acids or bases can change this equilibrium and modify the the conc. of H + and OH -

21. Acids and Bases Acid  compound that donates H+ ions Hydrochloric acid, added to water, hydrogen ions dissociate from chloride ions:  HCl -> H + + Cl - Addition of an acid makes a solution more acidic

22. Acids and Bases Base  compounds that donate OH- ions or removes H+ ions Some bases reduce H + directly by accepting hydrogen ions. Ammonia (NH 3 ) acts as a base when the nitrogen’s unshared electron pair attracts a hydrogen ion from the solution, creating an ammonium in (NH 4 + ).  NH 3 + H + NH 4 + Other bases reduce H + indirectly by dissociating to OH - that combines with H + to form water.  NaOH -> Na + + OH - OH - + H + -> H 2 O Solutions with more OH - than H + are basic solutions.

23. pH Scale The scale that describes how acid or basic a solution is. Ranges from 0-14 pH 2 is 10X more acidic than pH 3 pH 7 is neutral

24. pH Scale In any solution the product of their H + and OH - concentrations is constant at 10 -14. pH = -log[H + ]  [H + ] [OH - ] = 10 -14  If [H + ] = 10 -5 M,then [OH - ] = 10 -9 M  In a neutral solution, [H + ] = 10 -7 M and [OH - ] = 10 -7 M, pH =7

25. pH Scale The pH of a neutral solution is 7. Acidic solutions have pH values less than7 and basic solutions have pH values more than 7. Most biological fluids have pH values in the range of 6 to 8. However, pH values in the human stomach can reach 2. Each pH unit represents a tenfold difference in H + and OH - concentrations. A small change in pH actually indicates a substantial change in H + and OH - concentrations

26. Buffers Substances that can prevent or resist sharp changes in pH Important – because molecules in cells are very sensitive to concentrations of H+ or OH- ions. Even the slightest maybe harmful to living things

27. Buffers typically consist of a weak acid and its corresponding base Buffer in human blood and other biological solutions is carbonic acid.  The chemical equilibrium between carbonic acid and bicarbonate acts at a pH regulator.  The equilibrium shifts left or right as other metabolic processes add or remove H + from the solution.

28. Carbonate-bicarbonate buffer

29. Acid Precipitation Uncontaminated rain has a slightly acidic pH of 5.6. The acid is a product of the formation of carbonic acid from carbon dioxide and water. Acid precipitation occurs when rain, snow, or fog has a pH that is more acidic than 5.6. Effects of acid rain??