On May 18, 2:08 am, Mark & Juanita wrote:
Han wrote:
"Garage_Woodworks" .@. wrote in
:

"Garage_Woodworks" .@. wrote in message
. ..

CO2(g)------ CO2(aq) ---- H2CO3----- HCO3-1 ------ CO3-2.
---increasing pH------

The opposite is also true. As CO2(aq) goes to CO2(g) and leaves the
ocean the equilibrium shifts to the left and the CO2(aq)
concentration doesn't change. And the pH rises.

ABOVE should have read equilibrium shifts to the right. pH rises
(more basic) shifts to right. pH falls (more acidic) shifts to left.

Yes. In principle this is a very simple set of equations. The
difficulty is that oceans are not homogeneous, and we do not exactly know
where in the oceans their is really a good totaal capacity to dissolve
more gaseous CO2 (whether as truely dissolved gas or transformed into
bicarbonate and carbonate). Also, it is not yet known whether ocean
acidification will indeed kill off corals or not. Or whether more
dissolved CO2 in whatever form will enhance coral growth. Very
complicated indeed, mostly because ocean mixing is still hotly discussed
science. What effects chanes in salinity will have is also important
when more arctic and antarctic ice will melt, and mix into the oceans.

Sanity check time. Find the volume of water contained in the world's
oceans, take the absolute worst-case CO2 concentrations that are being
bandied around. Determine the amount of CO2 required to have even a
measureable effect upon that volume of water.


Go ahead and show us. I'll check your arithmetic.

These people have a done a little work in the area:

http://www.pmel.noaa.gov/co2/OA/

http://www.pmel.noaa.gov/co2/OA/Ocea...on%20FINAL.pdf

http://www.ipsl.jussieu.fr/~jomce/ac...ature04095.pdf

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FF