chapter 2.4 water—the elixir of life! why are we studying water? all life occurs in water inside...
TRANSCRIPT
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Chapter 2.4Water—The Elixir of Life!
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Why are we studying water? All life occurs in water
inside & outside the cell
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Chemistry of water Water is polar molecule
remember polar covalent bonds + & – poles
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Chemistry of water H2O molecules form H bonds with each
other + attracted to – creates a sticky
molecule
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Cohesion H bonding between H2O creates
cohesion water is “sticky” surface tension drinking straw
can you suck sugar up a straw?
You watch… Sean will try this at
lunch tomorrow!
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How does H2O get to top of tree? Transpiration (much, much later)
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Adhesion H2O molecules form H bonds with other
substances capillary action meniscus water climbs up fiber
ex. paper towel
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Water is the solvent of life H2O is a good solvent due to its polarity
polar H2O molecules surround + & – ions solvents dissolve solutes creating
aqueous solutions
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Hydrophilic Hydrophilic
substances have affinity for H2O polar or non-polar? ionic
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Hydrophobic Hydrophobic
substances do not have affinity for H2O polar or non-polar? non-ionic
fat (triglycerol)
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The special case of ice Most (all?) substances are more
dense when they are solid But not water… Ice floats!
H bonds form a crystal with loose structure
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Ice floats
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Why is “ice floats” important? Oceans & lakes don’t freeze solid
if ice sank… eventually all ponds, lakes & even ocean
would freeze solid during summer, only upper few inches
would thaw surface ice insulates water below
allowing life to survive the winter seasonal turnover of lakes
cycling nutrients
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Specific heat H2O has high specific heat
due to H bonding
H2O resists changes in temperature takes a lot to heat it up takes a lot to cool it down
H2O moderates temperatures on Earth
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Evaporative cooling Organisms rely on
heat of vaporization to remove heat
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Water forms ions Hydrogen ion (H+) splits off from water to
leave a hydroxide ion (-OH)
H2O H+ + -OH
If concentration of 2 ions is equal, water is neutral
If [H+] > [-OH], water is acidic If [-OH] > [H+], water is basic pH scale = how acidic or basic a
solution is
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pH Scale In pure water only 1 water molecule in
every 554 million is dissociated. very small amount of ions [H+] and [OH-] is 10-7M
[H+] [OH-] = 10-14
pH scale is based on this equation
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pH Scale In neutral solution
[H+] = 10-7 pH = 7 Values for pH decline as [H+] increase
Acids adding acid
increases [H+] Bases
adding base increases [OH-]
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pH & Biology pH of a neutral solution = 7 Acidic solutions = pH < 7
Basic solutions = pH > 7 Most biological fluids have pH 6 – 8
pH values in human stomach can reach 2 Each pH unit represents a 10-fold difference
in H+ & OH- concentrations. small change in pH actually indicates a
substantial change in [H+] & [OH-]
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Buffers Resist pH change Is a solution of weak
acid and its corresponding base
ex. HCO3
- + H+ H2CO3
Staying in the buffering range limits pH swings
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Water is a polar molecule The special properties of water make
life on Earth possible The chemical behavior of water
governs how organisms function
Importance of Water
Where we have
found water, we
have found life!
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Any Questions??