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THE IMPORTANCE OF WATER TO LIFE

THE IMPORTANCE OF WATER TO LIFE. Hydrogen Bonds Give Water Unique Properties. Water molecules are polar molecules Unequal sharing of electrons & V-like shape They can thus form hydrogen bonds with each other and with other polar molecules Each hydrogen bond is very weak

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THE IMPORTANCE OF WATER TO LIFE

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  1. THE IMPORTANCE OF WATER TO LIFE

  2. Hydrogen Bonds Give Water Unique Properties • Water molecules are polar molecules • Unequal sharing of electrons & V-like shape • They can thus form hydrogen bonds with each other and with other polar molecules • Each hydrogen bond is very weak • However, the cumulative effect of enormous numbers can make them quite strong • Hydrogen bonding is responsible for many of the physical properties of water

  3. HYDROGEN BONDING: DRAW 2-3 MOLECULES OF WATER & INDICATE THE HYDROGEN BONDS Not effective over long distances WEAK BONDS Formed by the attraction of opposite partial electric charges between two polar molecules

  4. COHESIVE PROPERTIES

  5. Heat vs Temperature • Heat= is a measure of the total amount of kinetic energy due to molecular motion in a body of matter. • Calorie= the amount of heat it takes to raise the temperature of 1g of water by 10C • Kilocalorie= 1,000 calories • Joule (J) one joule = 0.239 calories and 1 calorie= 4.184J • Temperature= the intensity of heat due to the average kinetic energy of the molecules. • We will use Celsius to indicate temperature

  6. THERMAL PROPERTIES High Heat of Vaporization High Specific Heat Water absorbs a lot of heat, hydrogen bonds break, then water turns to vapor & then evaporates. Water can absorb or release a lot of heat without changing its own temperature by very much. It’s ability to store heat Makes water a good coolant Have to add a lot of heat to change its temp. Heat needed for the evaporation of water in sweat is taken from the tissues of the skin Helps keep oceans relatively stable

  7. WATER AS ICE, FLOATS Ice Liquid water

  8. SOLVENT PROPERTIES Most of the important molecules in and out of the cell are polar molecules. These molecules create solutions that enable for biochemical processes to occur. Water is a versatile solvent because of its polarity Protein synthesis & glycolysis Gas Exchange Salt dissolves when all ions have separated from the crystal Water forms a hydration shell around each solute ion. Light independent processes of photosynthesis

  9. HYDROPHILLIC vs HYDROPHOBIC Hydrophillic Hydrophobic Molecules that “fear” water Do not have positive or negative charges & are nonpolar • Molecules that “love” water • With positive or negative charges including polar molecules EX: all substances that dissolve in water like glucose EX: all substances that do not dissolve in water like fats & oils If substances are soluble in water can be freely transported in the blood plasma. Ex: glucose amino acids, & sodium chloride If they are hydrophobic they are transported inside a lipoprotein complex. EX: fats and cholesterol

  10. Solute Concentration in Aqueous Solutions • Molecular mass: sum of the masses of all the atoms in a molecule. = number of daltons • Measuring is done in moles=6.02 x 1023 • Once the molecular mass of a molecule is determined, that number is used with a unit in grams.

  11. How would you make 1 liter of a 1M solution of sucrose (C12H22O11) • Review Avogadro’s number (a mole) • There are 6.02 x 1023 daltons in 1g. Carbon has an atomic mass of 12 & there are 12 carbons so 12 x 12 = 144 Hydrogen has an atomic mass of 1& there are 22 hydrogens so 1 x 22 = 22 Oxygen has an atomic mass of 16& there are 11 oxygens so 16x 11 = 176 For a total of ….342 daltons So, this means you would need 342g of sucrose in a liter of 1M sucrose solution

  12. Calculate the solutions of sucrose (C12H22O11) 68.4g 1,000mL 136.8g 1,000mL 205.2g 1,000mL 273.6g 1,000mL

  13. + H2O OH– H+ hydroxide ion hydrogen ion Water Ionizes • Covalent bonds within a water molecule sometimes break spontaneously Simplified version • This process of spontaneous ion formation is called ionization • It is not common because of the strength of covalent bonds

  14. BELOW IS A BEAKER OF DISTILLED WATER WHAT IS THE CHEMICAL FORMULA FOR THIS BEAKER OF DISTILLED WATER? H2O +H2 H3O+ + OH- H2O H+ + OH- Simplified version Is the concentration of water in the beaker the same as the total concentration of H+ + OH- ? NO What does it mean to be at equilibrium? The reactions is flowing back & forth, but there is no longer any net gain in either the concentration of the products or the reactants. Which is in higher concentration in this beaker; H2O or H+ + OH- ? H2O

  15. _ pH log [H+] = pH • A convenient way to express the hydrogen ion concentration of a solution • The pH scale is logarithmic • A difference of one unit represents a ten-fold change in H+concentration • Acid • Dissociates in water to increase H+concentration • Base • Combines with H+when dissolved inwater

  16. Remember: • The pH scale is logarithmic. • A change in one pH number actually represents a tenfold change in hydrogen ion concentration • EX: pH of 3 is actually ten times more acidic than a pH of 4.

  17. CALCULATE THE RATIO OF DISSOCIATED TO INTACT WATER MOLECULES IN A BEAKER OF DISTILLED WATER OF pH at 250 C If pH =7, then the concentration of hydrogen [H+ ] = 1 x 10-7 , which is the same as… [H+ ] = 1/10,000,000 , which is the same as Saying there is 1 dissociated molecule of H2 O for every 10 million intact H2 O molecules in the beaker of distilled water on the table. IN OTHER WORDS…. If you could reach in & pick out a single molecule from the beaker of water, 9,999,999 times out of 10,000,000 you would pull out a molecule of H2 O & 1 out of 10,000,000 times you would pick out a hydrogen ion.

  18. pH chart (from WS)

  19. DISCUSSION QUESTIONS Considering the equation H2O H+ + OH- at equilibrium to answer the following questions Does the equation tend to one direction of the other? If so, which direction does it tend to go? This reaction tends towards the left Which is in higher concentration in the above equation: (H2O) or (H+ + OH- ) H2O

  20. DISCUSSION QUESTIONS How many times different is a change in one unit of the pH scale? 10X more or less concentrated What’s the difference in hydrogen concentration between pH5 & pH2? pH2 has 1,000 times the concentration of H+ than a solution of pH5 What is the difference between a strong acid/base & a weak acid/base? A strong acid/base dissociates readily because the differences in the electronegativity of the ions are greater; a weak acid/base has atoms that are not as different in their electronegativity so they don’t tend to the dissociated side of the equation as easily.

  21. DISCUSSION QUESTIONS Which acids/bases are weaker & which are stronger --- HCl, NH3, H2CO3 & NaOH? Cl & Na both have very high electronegativity – they are both in column VII of ther periodic table with nearly full valence shells - & so they tend to dominate the electrons of H+ or OH- since the electronegativity of these atoms are very low. This huge difference in electronegativity causes a strong tendency for NaOH and HCl to dissociate. When the H+ or OH- dissociate from the Na & the Cl they are free to react with other molecules making them strong acids & bases. N & CO3 don’t have as strong of an electronegative difference with H since they are in columns IV-VI. Because of their lower electronegativity they do not dissociate as readily as HCl & NaOH so they are considered weaker acids & bases.

  22. – + + + HCO3– Bicarbonate ion H+ Hydrogen ion H2O CO2 H2CO3 Water in blood plasma Carbon dioxide Carbonic acid Buffers • Hydrogen ion reservoirs that take up or release H+ as needed • The key buffer in blood is an acid-base pair (carbonic acid-bicarbonate buffering system) Response to a rise in pH Response to a drop in pH

  23. Acid Precipitation

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