biological buffers. buffers allow biological fluids to maintain relatively constant ph despite...
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Biological Buffers
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Buffers
• Allow biological fluids to maintain relatively constant pH despite additions of acids or bases.
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For Example: Blood
• Human blood is normally pH 7.4
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• If you added a strong acid to water it could change from pH 7 to pH 2 very quickly.
• When a strong acid is added to blood it only changes from pH 7.4 to 7.3. WHY?
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Buffers• Minimizes the changes in
concentrations of H+ and OH-
Carbonic acid forms when carbon dioxide reacts with water
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What’s the diff?
• ACIDS ARE H+ DONORS• (also remove OH-)
• BASES ARE H+ ACCEPTORS• (also add OH-)
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Acid or Base?
HCl
H2SO4
NaOH
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Acid or Base?
HCl
H2SO4
base acid
acidbase
• NaOH
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Carbonic AcidH2CO3 is an H+ donor (Acid)
Bicarbonate IonHCO3- is an H+ acceptor (Base)
Notice the double arrow in the equation above: that means the reaction can go both ways.
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Buffer Equilibrium• H2CO3 is in equilibrium with HCO3
− + H+
• H2CO3 HCO3− + H+
• (the direction of the reaction will go to making the concentrations even on both sides of the arrows)
• If you have a lot of carbonic acid the reaction will go toward the right.
• If you have a lot of H+ ions the reaction will go to the left.
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If H+ concentration falls,
• That means the pH rises• That means it is becoming more basic• The reaction proceeds to the right as the
carbonic acid dissociates to replenish H+ ions
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If H+ concentration rises,
• That means the pH lowers• That means it is becoming more acidic• The reaction proceeds to the left as the
bicarbonate ion removes the H+ ions from the blood to form carbonic acid
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OCEAN ACIDIFICATION• Carbonic acid is also formed in the ocean when
atmospheric CO2 reacts with water.• This will remove the carbonate ion concentration
in the ocean. NOTE CO2 LEVEL INCREASE.
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But marine animals need carbonate ions for:coral and shells
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What causes the increase of carbon dioxide levels in the atmosphere?
• Burning of fossil fuels is a major source• Carbon Dioxide + rain water carbonic acid• Sulfur oxides + rain water sulfuric acid• Nitrogen oxides + rain water nitric acid
• FORMS ACID PRECIPITATION:• Refers to rain, snow, or fog of a pH lower than 5.2 (NORMAL RAIN IS ABOUT pH 5.6)
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ACID PRECIPITATION
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Why is the pH lower in the East?
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Effects of Acid Precipitation
Thinner egg shells
Thinner snail shells
Fewer songbirds that eat snails
Destroys leaves
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More Negative EffectsFish are very susceptible to pH changes.
Plankton and small invertebrates and young marine life are especially vulnerable.
Erode statues and buildings
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Science Fair Project Ideas
• Acid Rain Effects on Ocean LifeOr local aquatic life or local plants
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CLEAN AIR ACT
• Passed 1990• Motor emission standards• Factory clean emission standards• Aircraft emission standards