How does a Brønsted-Lowry acid form its conjugate base when dissolved in water? How is the water involved in this process?
The Brønsted-Lowry acid-base theory designates
We may take a tank of
In each case this is a REPRESENTATION of what occurs in solution. If we bleed enuff gas in, we achieve saturation at a concentration of approx.
As far as anyone knows, the actual acidium ion in solution is
Note that the
Of course, tunnelling, proton transfer, is more likely in a cluster of water molecules, so the analogy might not be particularly apt in that there is definite transfer of a ball in a maul, but a charge in a water cluster is conceivably tunnelled. The same applies to the transfer of an hydroxide ion. For this reason both
And we know that hydroxide/hydronium ions obey the following equilibrium in aqueous solution under standard conditions of temperature and pressure........
Depending at which level you are at (and I don't know!, which is part of the problem in answering questions on this site), you might not have to know the details at this level of sophistication. The level I have addressed here is probably 1st/2nd year undergrad.........