Why is #HF# a strong acid?
In aqueous solution, hydrogen fluoride is in fact a weak acid.
For hydrogen chloride, hydrogen bromide, hydrogen iodide, the given equilibrium lies strongly, almost quantitatively to the right.
I do not have the
Now in all of this, I have assumed an aqueous solution. There are other solvent systems, for instance liquid ammonia, or even liquid hydrogen fluoride. This, however, is the preserve of the specialist. I am perfectly justified in confining discussion to aqueous media.