What Keeps Sea Water Alkaline Despite the Presence of Carbon Dioxide?

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Marine organisms like coral and shellfish produce calcium and magnesium carbonate structures, raising questions about ocean alkalinity despite the presence of dissolved CO2, which should acidify seawater. The primary forms of carbon in the ocean are bicarbonate ions, which are in equilibrium with dissolved CO2 and carbonate ions. The discussion highlights that while the process of forming calcium carbonate releases protons, the ocean remains slightly alkaline due to various buffering systems and geological processes, including rock weathering. Participants debate the role of these buffering systems and the dynamics of calcium and bicarbonate in maintaining pH stability over millions of years. Ultimately, the conversation emphasizes the complexity of marine chemistry and the need for further clarification on how these processes interact to sustain ocean alkalinity.
  • #31
Besides temperature influencing CO2 in the oceans.
There is also CO2 partial pressures in ocean and atmosphere , Henry's Law
to consider.
There is local salinity to consider.
There is CO2 uptake by marine phytoplankton and algae to consider.
Although all your posts are correct in a strict inorganic chemistry context
the carbon dioxide cycle in the oceans is more complex and synergistic than inorganic chemistry alone.
 
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  • #32
morrobay said:
the carbon dioxide cycle in the oceans is more complex and synergistic than inorganic chemistry alone.

So why do you try to answer the initial question with single nonsensical reaction equations?
 
  • #33
Borek said:
So why do you try to answer the initial question with single nonsensical reaction equations?

You don't seem to understand that a single reaction can have products that are
influenced by more than one factor in the surroundings;

Ca++ + 2HCO3- <> Ca(HCO3)2 <> CaCO3 + H2O + CO2
Here is the reaction with products that are influenced by temperature, partial pressures,
salinity and photosynthesis . Do you understand that marine plants consume the CO2 in the above product and hence stop this reaction:
CO2 + H2O > H+ + HCO3-
thereby maintaining alkalinity ?
Mabey you should reread the OP and brush up on photosynthesis
 
  • #34
You are just trolling, and I am telling it for the second (and last) time. You showed you have no idea about the system much earlier, in many ways, proposing presence of Ca(OH)2:

morrobay said:
Ca(OH)2 + CO2 >>shellfish> CaCO3 + H2O

suggesting existence of metallic calcium:

morrobay said:
Ca + 2 H2O ---> Ca(OH)2 + H2

calcium oxide:

morrobay said:
CaO + H2O --> Ca(OH)2

later you suggested that reaction which produces carbon dioxide - acid anhydride:

morrobay said:
Ca++ + 2HCO3- --> Ca(HCO3)2 --> CaCO3 +H2O + CO2

doesn't change pH, now you call for photosynthesis to explain what happens to carbon dioxide. Trick is, if carbon dioxide is produced and then consumed, and speeds of both reactions are identical so that pH is maintained, that's a classic example of a steady state system, different from the one I was thinking about - but conceptually similar.
 
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