What determines the magnitude of the equilibrium constant of the autoprotolysis reaction of water? 2H_2O(l) rightleftharpoons H_3O^+ + HO^(-). K_w=10^(-14).

Aug 11, 2017

The strength of the interatomic bond...........

Explanation:

And the stability of the particles formed by such dissociation.....

As you know water undergoes such dissociation, in a so-called autoprotolysis reaction.....

$2 {H}_{2} O r i g h t \le f t h a r p \infty n s {H}_{3} {O}^{+} + O {H}^{-}$

And the extent of this dissociation is very small.......

${K}_{w} = \left[{H}_{3} {O}^{+}\right] \left[H {O}^{-}\right] = {10}^{-} 14$.

On the other hand, hydrogen chloride is a covalent molecule, that is supplied as a gas........

Because it can undergo protolysis, we would represent its dissolution in water as......

$H C l \left(g\right) \stackrel{{H}_{2} O}{\rightarrow} {H}_{3} {O}^{+} + C {l}^{-}$

Even despite such dissociation the $H - X$ bond is covalent to a first approximation, and it can be supplied in a gaseous cylinder....The hydrochloric acid that we use in bottles, when the acid is solvated, has a concentration of approx. $10.6 \cdot m o l \cdot {L}^{-} 1$.