|MadSci Network: Chemistry|
I understand that Henry's Law defines the relationship between a gases pressure above a liquid and it's concentration within that liquid. And, Henry's Law Constants seem to be, in essence, an empirically determined value which quantifies this relationship. But, what is the "driving force" (logic) behind this balance? Does understanding this logic make it possible to determine the gases concentration within the liquid, knowing it's pressure above, without knowing the Henry's Law Constant? In Message ID # 923925416.Ot, Mr. Kingsley refers to a beer bottle at equalibrium, saying "the partial pressures of the carbon dioxide in the air and in the liquid are the same". This is an interesting thought, yet it confused me. First, how do you determine the partial pressure of the gas in the liquid? And, wouldn't this infer that the dissolved gas concentration is dependent on pressure only? Wouldn't that, in turn, make Henry's Law Constants the same for all gases? Please help...I feel like I'm missing something obvious...
Re: What's the relationship between gases and dissolved gases?
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