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

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SUMMARY

The discussion centers on the mechanisms that maintain the alkalinity of seawater despite the presence of carbon dioxide (CO2). Marine organisms, such as coral and shellfish, create calcium carbonate (CaCO3) structures, which theoretically should acidify the ocean by consuming bicarbonate ions (HCO3-). However, the ocean remains slightly alkaline due to complex equilibria involving bicarbonate, carbonate ions (CO32-), and dissolved CO2. The equilibrium reactions, along with geological processes like rock weathering, contribute to a buffering system that stabilizes seawater pH over millions of years.

PREREQUISITES
  • Understanding of carbonate chemistry, including bicarbonate (HCO3-) and carbonate ions (CO32-).
  • Knowledge of oceanic pH dynamics and buffering systems.
  • Familiarity with the role of marine organisms in biogeochemical cycles.
  • Basic principles of chemical equilibrium and reactions involving acids and bases.
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  • Research the role of bicarbonate and carbonate ions in ocean chemistry.
  • Study the impact of rock weathering on ocean alkalinity and pH levels.
  • Explore the biochemical processes used by marine organisms to produce calcium carbonate.
  • Investigate the effects of atmospheric CO2 levels on ocean acidity and alkalinity.
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Marine biologists, oceanographers, environmental scientists, and anyone interested in the chemical processes that regulate ocean acidity and 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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