Chemistry, Life and Water II Think/Pair/Share What properties of water enabled evolution of life on earth? Life Importance of water What properties of water enabled evolution of life on earth? Water dissolves most things – Because water is polar, it is an excellent solvent Water keeps its cool – Water’s heat capacity is among the highest of all materials – resists temperature change – Oceans warm and cool much more slowly than the atmosphere What properties of water enabled evolution of life on earth? As water approaches freezing, water gets less dense – Freezes from the top down (floats when frozen) Cohesiveness Hydrogen bonds between water molecules Ice, water, and steam Hydrogen-Bond Lattice of Water Water lattice – Neighboring water molecules form hydrogen bonds temporarily – Difficult for nonpolar substances to penetrate the lattice – Polar or charged substances penetrate easily Ice Lattice Ice lattice – A rigid, crystalline structure – Water molecules in the ice lattice are spread farther apart than in liquid water – Ice is less dense than water and floats Hydrogen-Bond Lattice of Water Fig. 2-12, p. 33 Animation: Structure of water What properties of water enabled evolution of life on earth? Water dissolves most things – Because water is polar, it is an excellent solvent Water is the solvent of life Water is the solvent of life Hydrophilic – water loving Hydrophobic – water repelling – Non-ionic, non-polar Polar (hydrophilic) regions at the surface of the micelle Nonpolar (hydrophobic) ends are oriented toward the interior of the micelle 15 Hydration Layer Water forms hydration layer over surfaces of polar and charged biological molecules, particularly proteins Separates ions and molecules from each other so they can enter a solution – Water = solvent – Dissolved substance = solute Hydration Layer Hydration layers around Na+ and Cl– ions keep salt in solution Fig. 2-14, p. 34 Animation: Spheres of hydration What properties of water enabled evolution of life on earth? Water keeps its cool – Water’s heat capacity is among the highest of all materials – resists temperature change – Oceans warm and cool much more slowly than the atmosphere High Specific Heat Water temperature increases slowly as heat is added – Must break hydrogen bonds to allow water molecules to move faster – Helps moderate and stabilize temperature of organisms and environment – c (calorie) = heat to raise 1g of water 1°C – C (Calorie) = 1,000 calories = 1 kilocalorie (kcal) Water moderates temperatures on Earth Water can absorb or release a large amount of heat with only a slight change in its own temperature Water’s high specific heat – Water, 1 cal/g/C – Iron, 0.1 cal/g/ C High Heat of Vaporization Water absorbs a large amount of heat to break loose from liquid water and form a gas – Some animals sweat (water evaporation cools skin and underlying blood vessels) – Plants evaporate water from leaves (cools heat absorbed from sunlight) What properties of water enabled evolution of life on earth? As water approaches freezing, water gets less dense – Freezes from the top down (floats when frozen) Ocean and lakes do not freeze solid What properties of water enabled evolution of life on earth? Cohesiveness – Hydrogen bonds hold the water molecules together – Organisms depend on the cohesion of water molecules – Ex. Water transport in plants Water Molecules Resist Separation Cohesion – Attraction between water molecules Adhesion – Attraction of water molecules to surfaces with charged or polar molecules Surface Tension Forms at surface of water in contact with air Hydrogen bonds resist stretching, giving surface strength Fig. 2-15, p. 36 Water has an unusually high specific heat. This is directly related to which one of the following? 1. At its boiling point, water changes from liquid to vapor. 2. More heat is required to raise the temperature of water. 3. Ice floats in liquid water. 33% 1 33% 2 33% 3 Which of the following explains what is happening when sodium chloride dissolves in water? 1. More hydrogen bonds are forming between water molecules. 2. Sodium and chloride atoms are separating from one another. 3. Hydration shells are forming around the sodium and chloride ions. 33% 1 33% 2 33% 3 Predict how life on earth would be different if water were less polar. Which one of the following would result if organisms lived in and consisted of a less polar medium than water? Heavier insects than water striders would be able to walk on the surface of a pond. 2. Sweating would be a less effective means of keeping cool. 3. The water temperature of ponds and pools would increase more slowly when in sunlight. 1. 33% 1 33% 2 33% 3 Water, Lipids, and Membranes Membrane molecules have one polar end and one nonpolar (lipid) end In water, lipid molecules are forced into a double layer (bilayer) that forms the membrane – Hydrophilic ends face water – Hydrophobic ends associate inside Membranes: The Lipid Bilayer Fig. 2-13, p. 34 Water Ionization and Acids, Bases, and Buffers Substances act as acids or bases by altering the concentrations of H+ and OH− ions in water Buffers help keep pH under control Water Ionization Water dissociates to form ions: H2O ↔ H+ + OH– H+ (protons) = hydrogen ions OH– = hydroxide ions In pure water, concentration of H+ = OH– Acids and Bases Acids release H+ as they dissolve in water – Solution becomes acidic HCl ↔ H+ + Cl– Acids and Bases Bases gather H+ or release OH− in solution – Solution becomes basic NaOH ↔ Na+ + OH– pH Scale Measures relative concentrations of H+ and OH− (acidity) in a water solution on a scale of 0 to 14 pH = –log10[H+] Pure water: [H+] = [OH−] = 1 X 10-7 M – pH 7 (neutral) = –log10[1 X 10-7] – pH < 7 is acidic, pH > 7 is basic pH Scale Fig. 2-16, p. 37 pH animation pH sliding scale The hydrogen ion concentration of a solution whose pH is 9.0 is greater than that of blood whose pH is 7.3.? 1. True 50% 50% 2. False 1 2 In humans, blood pH is around 7.4, and a decrease in blood pH to 6.4 would be fatal. A drop by 1 pH unit represents which of these? 1. twice as many H+ ions in the solution 2. 1/10 as many H+ ions in the solution 3. ten times as many H+ ions in the solution 33% 1 33% 2 33% 3 The hydrogen ion concentration of a solution whose pH is 9.0 is greater than that of blood whose pH is 7.3. Is this statement true or false? Explain. Buffers Regulate pH of living cells Absorb or release H+ to compensate for changes in H+ concentration Biocarbonate ion (HCO3–), important base H2CO3 ↔ HCO3– + H+ Buffers If cell is too acidic – Push reaction to the left – Remove some H+ ions If cell is too basic – Push reaction to the right – Add more H+ ions Help keep cells close to neutral pH Blood pH critical Blood pH 7.35 – 7.45 Breathing too fast removes buffering capacity from the blood Carbonic acid-bicarbonate system Fig. 2-18, p. 39