productivity and the coral symbiosis iii
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Productivity and the Coral Symbiosis III. Overall productivity of the reef: 4.1 - 14.6 gC/m 2 /d this is organic carbon production must also consider carbonate production (deposition of physical structure of the reef) Get about half of this from the coral symbiosis - PowerPoint PPT PresentationTRANSCRIPT
Productivity and the Coral Symbiosis III
• Overall productivity of the reef: 4.1 - 14.6 gC/m2/d
• this is organic carbon production
• must also consider carbonate production (deposition of physical structure of the reef)
– Get about half of this from the coral symbiosis
– the rest from the calcareous green & reds algae
CALCAREOUS ALGAE (greens & reds) are major contributors to reef calcification– the more flexible magnesian calcite
• last 25 years - role of these algae receive more attention– play a much bigger role in calcium deposition than
previously thought
• 10% of all algae CALCIFY (about 100 genera)
Calcification - growth of the reef
• In ocean, mostly find 3 forms of CaC03
• Calcite– Mostly of mineral origin
• Aragonite– Fibrous, crystalline form, mostly from corals
• Magnesian calcite– Smaller crystals, mostly plant origin
Calcification
Calcite Aragonite
Magnesian calcite (Mg carbonate)
• Examples:
organism CaCO3
Molluscs calcite & aragoniteCorals just aragoniteSome green algae just aragoniteRed algae magnesian calciteSponges aragonite (with silica)Some bryozoans all 3
Corals
• remove Ca++ & CO3-- from seawater
• Combines them to CaCO3
• transports them to base of polyp
– Calcicoblastic epidermis• minute crystals secreted from base of polyp
• Energy expensive– Energy from metabolism of algal PS products
Calcification
CO2 and seawater
• What forms of C are available to the coral ?
• Organic and inorganic forms
• DIC - dissolved inorganic carbon– CO2 (aq)
– HCO3-
– CO3--
• DIC comes from:
– Weathering– dissolution of oceanic rock– Run-off from land– Animal respiration– Atmosphere– etc.
• DIC in ocean constant over long periods
• Can change suddenly on local scale– E.g. environmental change, pollution
• Average seawater DIC = 1800-2300 mol/Kg
• Average seawater pH = 8.0 - 8.2
• pH affects nature of DIC
Carbon and Seawater
• normal seawater - more HCO3- than CO3
--
• when atmospheric CO2 dissolves in water
– only 1% stays as CO2
– rest dissociates to give HCO3- and CO3
--
H2O + CO2 (aq) H2CO3 HCO3- + H+ (1)
HCO3- CO3
-- + H+ (2)
equilibrium will depend heavily on [H+] = pH
relative amounts of different ions will depend on pH
dissolved carbonate removed by corals to make aragonite
Ca++ + CO3--
CaCO3 (3)
pulls equilibrium (2) over, more HCO3- dissociates to CO3
--
HCO3- CO3
-- + H+ (2)
removes HCO3-, pulls equilibrium in eq (1) to the right
H2O + CO2 (aq) H2CO3 HCO3- + H+ (1)
more CO2 reacts with water to replace HCO3-, thus more CO2 has to
dissolve in the seawater
Can re-write this carbon relationship:
2 HCO3- CO2 + CO3
-- + H2O
• used to be thought that
– symbiotic zooxanthellae remove CO2 for PS– pulls equation to right– makes more CO3
-- available for CaCO3 production by polyp
• No
• demonstrated by experiments with DCMU – stops PS electron transport, not CO2 uptake
• removed stimulatory effect of light on polyp CaCO3 deposition
• therefore, CO2 removal was not playing a role
• also, in deep water stony corals– if more food provided, more CaCO3 was deposited
– more energy available for carbonate uptake & CaCO3 deposition
• Now clear that algae provide ATP (via CHO) to allow polyp to secrete the CaCO3 and its
organic fibrous matrix
• Calcification occurs 14 times faster in open thanin shaded corals
• Cloudy days: calcification rate is 50% of rate on sunny days
• There is a background, non-algal-dependent rate
Environmental Effects of Calcification
• When atmospheric [CO2] increases, what happens to calcification rate ?
– goes down
– more CO2 should help calcification ?– No
• Add CO2 to water– quickly converted to carbonic acid– dissociates to bicarbonate:
H2O + CO2 (aq) H2CO3 HCO3- + H+ (1)
HCO3- CO3
-- + H+ (2)
• Looks useful - OK if polyp in control, removing CO3--
• Add CO2 to water– quickly converted to carbonic acid– dissociates to bicarbonate:
H2O + CO2 (aq) H2CO3 HCO3- + H+ (1)
HCO3- CO3
-- + H+ (2)
• Looks useful - OK if polyp in control, removing CO3--
• BUT, if CO2 increases, pushes eq (1) far to right
• [H+] increases, carbonate converted to bicarbonate
• So, as more CO2 dissolves,
• more protons are released• acidifies the water
• the carbonate combines with the protons• produces bicarbonate
• decreases carbonate concentration
• Also, increase in [CO2] – leads to a less stable reef structure– the dissolving of calcium carbonate
H2O + CO2 + CaCO3 2HCO3- + Ca++
• addition of CO2 pushes equilibrium to right– increases the dissolution of CaCO3
• anything we do to increase atmospheric [CO2] leads to various deleterious effects on the reef:
• Increases solubility of CaCO3
• Decreases [CO3--] decreasing calcification
• Increases temperature, leads to increased bleaching
• Increases UV - DNA, PS pigments etc.