How does the behaviour of a strong acid in water compare to that of a weak acid when both are dissolved in water?
Consider the solution behaviour of an acid, in water.........
In water we know that the following equilbrium operates, the autoprotolysis of water:
An acid is conceived to protonate the solvent, here the water, to form the hydronium ion,
This is an equilibrium reaction, which might be small (i.e. lie on the reactants side), or might be large (lie towards the products), and as with any equilibrium, we may measure its extent by
And again, large values of
And likewise, a
And the moral, a strong acid is an acid that almost completely undergoes this ionization reaction in water, and yet this behaviour is still governed by