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Ocean Acidification Chemistry

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Ocean Acidification
So, what is it?
• The ongoing decrease in the pH of the Earth's oceans,
caused by the uptake of carbon dioxide (CO2) from the
atmosphere.
• An estimated 30–40% of the carbon dioxide released by
humans into the atmosphere dissolves into oceans, rivers
and lakes.
• To achieve chemical equilibrium, some of it reacts with the
water to form carbonic acid.
• Some of these extra carbonic acid molecules react with a
water molecule to give a bicarbonate ion and a hydronium ion,
thus increasing ocean "acidity" (H+ ion concentration).
So, what is it?
• Between 1751 and 1994 surface
ocean pH is estimated to have
decreased from approximately
8.25 to 8.14, representing an
increase of almost 30% in H+
ion concentration in the
world's oceans.
• Earth System Models project
that within the last decade
ocean acidity exceeded
historical predictions
• Could undermine the functioning
of marine ecosystems and many
ocean goods and services
Estimated change in sea water pH caused by human
created CO2 between the 1700s and the 1990s, from
the Global Ocean Data Analysis Project (GLODAP) and
the World Ocean Atlas
How much CO2 can the ocean
absorb?
• The total amount of any gas seawater can absorb
depends on temperature and salinity
• Salinity is a measure
of the dissolved salt
content of water
Remember this relationship!
Temperature
or
Salinity
Amount of gas
seawater can absorb
Increases in temperature and salinity can decrease the
amount of gas seawater can absorb.
4
From the wikimedia free licensed media file repository
Life on Earth would not be
possible without water
Its chemical and physical
properties actually defy some
fundamental laws of physics
Almost all biochemical reactions
require water!
pH and buffers
• Measure of the acidity or basicity of an aqueous solution.
– Solutions with a pH less than 7 are said to be acidic
– Solutions with a pH greater than 7 are basic or alkaline.
– Pure water has a pH very close to 7
•
•
•
•
Acid
A chemical compound that donates H+ ions to solutions.
Base
A compound that accepts H+ ions and removes them from solution.
• Remember H3O+ and OH-?
• The H3O+ donates H+ to a solution and the OH- removes H+ from a
solution
• If an equal number of these ions are present in a solution the pH
will not change as it is said to be neutral.
The pH scale
• To describe the acidity of
a solution, we use the pH
scale.
• Acids have a low pH, so
they have a high
concentration of H+
• Bases have a high pH, so
they have a low
concentration of H+
Used with permission from purewaterproducts.com
• The ocean absorbs
carbon dioxide from the
atmosphere
• Human activities release
carbon dioxide into the
atmosphere
• Too much carbon dioxide
in the ocean has the
potential to harm marine
organisms and
ecosystems
How is atmospheric CO2 responsible for
ocean acidification?
When CO2 dissolves in seawater, carbonic acid is produced via the reaction:
This carbonic acid dissociates in the water, releasing hydrogen ions and bicarbonate:
The increase in the hydrogen ion concentration causes an increase in acidity, since acidity is
defined by the pH scale, where pH = -log [H+] (so as hydrogen increases, the pH
decreases). This log scale means that for every unit decrease on the pH scale, the
hydrogen ion concentration has increased 10-fold.
One result of the release of hydrogen ions is that they combine with any carbonate ions in
the water to form bicarbonate:
This removes carbonate ions from the water, making it more difficult for
organisms to form the CaCO3 they need for their shells.
“Battle” for carbonate!
• Organisms must use more
energy or make less hard
part material
• Existing hard parts
dissolve (chemical
reaction goes “the wrong
way”)
From the wikimedia free licensed media file
repository
Hgm,
• dgdfg
Ocean acidification: Impacts on individual marine organisms
Reduced fertilization of gametes in corals and other marine organisms
• Deformed flagellum in sperm that impacts their swimming
• Fitness effect: lower population growth
Natural range in the ocean
Albright et al. 2010
Ocean acidification: Impacts on individual marine organisms
Reduced hearing ability in anemone fish (clown fish) larvae
• Deformed morphology of CaCO3 fish ear bones (otoliths)
• Disruption of acid-base balance in neuro-sensory system
• Fitness effect: lower survival due to higher predation.
Simpson et al. 2011
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file repository
Ocean acidification: Impacts on ecological communities
Tropical Oceans Predictions:
• Corals will become increasingly rare
• Algae will become more abundant
• Because coral reefs support so many animals,
biodiversity will decline
Hoegh-Guldberg et al. 2007
Ocean acidification: Impacts on individual marine organisms
Growth
Photosynthesis
Non-calcifying marine algae: Increased photosynthesis and growth
• Lower pH means more dissolved CO2 for photosynthesis to fuel growth
• Fitness effect: higher survival and population growth
Amount of dissolved carbon
Chen & Durbin 1994
The Solutions
What can we do about ocean acidification?
A possible geoengineering solution: Add CaCO3 to the ocean.
Reduce CO32- under-saturation caused by excess CO2 dissolving in ocean water.
2+
2Shells
3 32Shells are
are made
made of
of CaCO
CaCO33 =
= Ca
Ca2+ ++ CO
CO
H+
CO32-
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Sounds great, but……………..
To counteract 2 gigatons of carbon/yr input of CO2, would
need 20 gigatons of CaCO3/yr.
White Cliffs of Dover would be
rapidly consumed.
Limestone Rock (CaCO3)
• Limestone mining would be expensive and would cause
ecological damage.
• All the energy needed to move massive amounts of rock into
the ocean would likely add more CO2 to the atmosphere.
Oh yes,
Stop adding CO2 to the atmosphere!
From the wikimedia free licensed media file repository
A Quick Note
• Buffer Capacity: the extent to which a buffer
can resist changes to the pH of the solution
when an acid or base is added
• The higher the [buffer] in solution, the better
controlled the pH will be when an acid/base is
added
The End!
Any Questions?
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