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<blockquote data-quote="Peregrini" data-source="post: 55157" data-attributes="member: 2670"><p>Octavusprime;</p><p>Just a small correction.</p><p></p><p>That is not exactly correct. I am not faulting you but your source.</p><p>It's hard to do scientific notation so I hope this still makes sense.</p><p>Carbon dioxide dissolves in water and dissociates 'reversibly' to H2CO3, carbonic acid.</p><p>CO2 + H2O = H2CO3</p><p>H2CO3 is diprotic, that means it has two acid dissociation constants.</p><p>The first one for the dissociation into the bicarbonate ion HCO3-... H2CO3 = HCO3- + H+ : Ka1 = 2.5×10-4 ; pKa1 = 3.6 at 25 C</p><p>The second for the dissociation into the carbonate ion CO3 2-... HCO3- = CO3 2- + H+ : Ka2 = 4.69×10-11 ; pKa2 = 10.329 at 25 C</p><p>A simple quick analysis of how much of something dissociates is how large the negative notation is or the larger the pKa number. A larger negative notation or larger pKa means LESS dissolution.</p><p>The Kh, hydration constant,(at 25 C) of carbonic acid is [H2CO3]/[CO2] = 1.70×10-3: This means the majority of the carbon dioxide is not converted into carbonic acid. It remains as CO2 molecules disolved in the water but not by a chemical reaction and not affecting the pH. H2CO3 is an amphoteric substance and can act as an acid or base, oddly enough, depending on pH of the solution. The oceans are mildly alkaline. A typical pH = 8.2 to 8.5, sea water contains about 120 ppm of bicarbonate ion.</p><p>So, the concentrations of H2CO3, and the ions HCO3-, bicarbonate, and CO3 2-, carbonate, depend on the pH of the solution they are dissociated in. Also the presence of "other" ions in the Ocean act as a buffer further reducing the action of CO2, not to mention, increased temperature (Global Warming) reduces the amount of CO2 'uptake' by the ocean.</p><p>In short, anthropogenic CO2 has very little (almost zero) to do with Ocean pH. There are far too many other sources to blame it on humans.</p><p> </p><p>If you want to know more about atmospheric CO2 and the Oceans you can look here;</p><p><a href="http://ocean.mit.edu/~mick/Papers/McKinleyetalGBC2004.pdf" target="_blank">http://ocean.mit.edu/~mick/Papers/McKinleyetalGBC2004.pdf</a></p></blockquote><p></p>
[QUOTE="Peregrini, post: 55157, member: 2670"] Octavusprime; Just a small correction. That is not exactly correct. I am not faulting you but your source. It's hard to do scientific notation so I hope this still makes sense. Carbon dioxide dissolves in water and dissociates 'reversibly' to H2CO3, carbonic acid. CO2 + H2O = H2CO3 H2CO3 is diprotic, that means it has two acid dissociation constants. The first one for the dissociation into the bicarbonate ion HCO3-... H2CO3 = HCO3- + H+ : Ka1 = 2.5×10-4 ; pKa1 = 3.6 at 25 C The second for the dissociation into the carbonate ion CO3 2-... HCO3- = CO3 2- + H+ : Ka2 = 4.69×10-11 ; pKa2 = 10.329 at 25 C A simple quick analysis of how much of something dissociates is how large the negative notation is or the larger the pKa number. A larger negative notation or larger pKa means LESS dissolution. The Kh, hydration constant,(at 25 C) of carbonic acid is [H2CO3]/[CO2] = 1.70×10-3: This means the majority of the carbon dioxide is not converted into carbonic acid. It remains as CO2 molecules disolved in the water but not by a chemical reaction and not affecting the pH. H2CO3 is an amphoteric substance and can act as an acid or base, oddly enough, depending on pH of the solution. The oceans are mildly alkaline. A typical pH = 8.2 to 8.5, sea water contains about 120 ppm of bicarbonate ion. So, the concentrations of H2CO3, and the ions HCO3-, bicarbonate, and CO3 2-, carbonate, depend on the pH of the solution they are dissociated in. Also the presence of "other" ions in the Ocean act as a buffer further reducing the action of CO2, not to mention, increased temperature (Global Warming) reduces the amount of CO2 'uptake' by the ocean. In short, anthropogenic CO2 has very little (almost zero) to do with Ocean pH. There are far too many other sources to blame it on humans. If you want to know more about atmospheric CO2 and the Oceans you can look here; [url="http://ocean.mit.edu/~mick/Papers/McKinleyetalGBC2004.pdf"]http://ocean.mit.edu/~mick/Papers/McKinleyetalGBC2004.pdf[/url] [/QUOTE]
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