How does the value of Ka and Kb compare with the concentrations of hydronium ion and hydroxide ion?

Ka X Kb = [H3O+][OH-]

Ka X Kb> [H3O+][OH-]

Ka X Kb< [H3O+]+[OH-]

Ka X Kb + [H3O]/[OH-]

Assuming that we are given the values of Ka and Kb, these can be rewritten and represented by the concentration of the Hydronium ion and Hydroxide Ion:

Hydronium ion: [H3O+]

Hydroxide ion: [OH-]

Ka is the equilibrium constant of an acid which dissociates to a hydronium ion and its cation.

Kb is the equilibrium constant of a base which dissociates to a hydroxide ion and its anion.

So,

Ka x Kb = [H3O+][OH-]