http://www.cquestrate.com/general/conversations-about-cquestrate Developing an open source solution to climate change Sun, 11 Jul 2010 17:59:15 +0100 http://wordpress.org/?v=abc hourly 1 http://www.cquestrate.com/general/conversations-about-cquestrate/comment-page-1#comment-5034 Alberto Mon, 03 Aug 2009 11:35:55 +0000 http://www.cquestrate.com/?p=373#comment-5034 Sorry Tom, but as Calcium Bicarbonate and Calcium Carbonate have very different solubility values, as soon as there is some Ca++ in a Carbonic acid solution this will precipitate CaCO3 crystal. Discussing of Calcium bicarbonate is like "what if" questions... interesting, but useless because not existing. Sorry Tom, but as Calcium Bicarbonate and Calcium Carbonate have very different solubility values, as soon as there is some Ca++ in a Carbonic acid solution this will precipitate CaCO3 crystal.
Discussing of Calcium bicarbonate is like “what if” questions… interesting, but useless because not existing.

]]> http://www.cquestrate.com/general/conversations-about-cquestrate/comment-page-1#comment-1905 Tom Wed, 19 Nov 2008 23:27:06 +0000 http://www.cquestrate.com/?p=373#comment-1905 CO2 in water solution exists as a carbonic acid radical H(HCO3). Adding CaO doesn't make any difference to this - the Ca++ simply displaces the hydrogen radicals when it forms calcium bicarbonate. On its own, this would increase the pH value - except that when the CO2 released by burning the limestone reaches the water and reacts to form carbonic acid, the effect will be cancelled out. Moreover, calcium bicarbonate only exists in solution. If you attempt to precipitate or crystalize it, one CO2 is shed and it turns back into calcium carbonate. See among others: http://www.nationmaster.com/encyclopedia/Calcium-bicarbonate CO2 in water solution exists as a carbonic acid radical H(HCO3). Adding CaO doesn’t make any difference to this – the Ca++ simply displaces the hydrogen radicals when it forms calcium bicarbonate. On its own, this would increase the pH value – except that when the CO2 released by burning the limestone reaches the water and reacts to form carbonic acid, the effect will be cancelled out.
Moreover, calcium bicarbonate only exists in solution. If you attempt to precipitate or crystalize it, one CO2 is shed and it turns back into calcium carbonate.
See among others: http://www.nationmaster.com/encyclopedia/Calcium-bicarbonate

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