Bear in mind if a couple equations was added to render a step threerd, the fresh harmony ongoing in the 3rd picture translates to the item of one’s balance constants of your first two equations. (Point fifteen.3)

Thus, the product of K_{a} and K_{b} is the ion-product constant for water, K_{w} (Equation ). We expect this result because adding Equations and gave us the autoionization equilibrium for water, for which the equilibrium constant is K_{w}.

As the strength of an acid increases (K_{a} gets larger), the strength of its conjugate base must decrease (K_{b} gets smaller) so that the product K_{a} ? K_{b} remains 1.0 ? 10 –1cuatro at 25 °C. TABLE 16.5 demonstrates this relationship.

By using Equation , we can calculate K_{b} for any weak base if we know K_{a} for its conjugate acid. Similarly, we can calculate K_{a} for a weak acid if we know K_{b} for its conjugate base. As a practical consequence, ionization constants are often listed for only one member of a conjugate acid–base pair. For example, Appendix D does not contain K_{b} values for the anions of weak acids because they can be readily calculated from the tabulated K_{a} values for their conjugate acids.

If you look up the values for acid-or base-dissociation constants in a chemistry handbook, you may find them expressed as pK_{a} or pK_{b} (that is, –log K_{a} or –log K_{b}) (Section 16.4). Equation can be written in terms of pK_{a} and pK_{b} by taking the negative logarithm of both sides:

Many low-molecular-weight amines have a fishy odor. Amines and NH_{3} are produced by the anaerobic (absence of O_{2}) decomposition of dead animal or plant matter.