Question

How are percent ionization values similar to equilibrium constant values?

Answer 1

We'll take acids for this example
\[\huge \alpha A+ \beta B \rightleftharpoons \gamma C + \phi D\]
The thermodynamic equilibrium constant can be defined as
\[\large K=\frac{\left\{ C \right\} ^{\gamma} \left\{ D \right\}^{\phi}}{\left\{ A \right\}^{\alpha}\left\{ B \right\}^{\beta}}\]
When percentage dissociation/ionisation increases, eg. from weak acid to stronger weak acids, the reactants forms more products before they reach equilibrium. K increases, and vice versa.

Answer 2

I'm still a little confused...

Answer 3

Do you know that strong acids dissociates completely?

Answer 4

Yes

Answer 5

Ok, so that means that when weak acid gets stronger, the reaction goes towards the products increases.