In Chapter 15 of Chemistry: The Central Science, we learned about the equilibrium constant Keq and that if it is greater than 1, equilibrium favors the products and if it's less than 1, equilibrium favors the reactants. I get that part. Why can't Ka (the acid-dissociation constant) be greater than one? There's something I'm not getting. Why wouldn't an aqueous solution of acid in equilibrium with its conjugate base and hydronium favor a higher concentration of products . . . ever? I hope that makes sense. Thanks
Explanation / Answer
Yes because generally the acid dissociation constant fora weak acid is less than 1. Because the degree of dissociationof a weak acid is less. So ,the the equilibruim constant forthe dissociation of a weak acid is less than 1 as the equilibriumlies towards the reactants side. If we consider the Ka value for the dissociation of astrong base, it would be greater than 1 as the acid is almostcompletely dissociated.