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Carbon dioxide is also soluble in water so perhaps has been reabsorbed?
I would expect the dissolved gas concentration to be close to equilibrium immediately after the experiment, since the decomposition of H2CO3 generated in the first stage of the reaction happens in an almost ideal way to maximise solution of the resulting CO2 in the water.
To the extent that the reaction chills the solution due to the slight overall endothermicity, the equilibrium concentration of dissolved CO2 should fall as the temperature equilibrates to ambient, so more gas should come out of solution.
gbj_tester
Carbon dioxide is also soluble in water so perhaps has been reabsorbed? As above, atmospheric pressure is could well be a factor. In the middle of the recent storms I noticed the difference in some ziplock bags that I'd sealed some time before.