![]() ![]() I'd be interested in seeing how the problem is completely solved when you are finished. Of course at that point you would need to know the value of k for SO2, and I'm not familiar with using that, or even where to find it. atm/mol for dioxygen (O2) in water at 298 K), p is the partial pressure (atm), and c is the concentration of the dissolved gas in the liquid (mol/L). ![]() Where k is a temperature-dependent constant (for example, 769.2 L Īt that point, you could perhaps use Henry's law, which states that the solubility of a gas in a liquid is directly proportional to the partial pressure of that gas above the liquid, which may be written as: Then if you know the (and assume the is the same), and the Ka value (1.5 x 10 -2 for sulfurous acid) you could calculate the which is the same as. If you know the pH, you could calculate the ( = antilog (-pH) Let's start with the obvious, the lower the pH, the greater the concentration of dissolved SO2 since the SO2 reacts with water according to the equation: ![]()
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