pH, pKa, Ka, pKb, and Kb Explained

A Guide to Acid-Base Equilibrium Constants

person putting pH strip in liquid
The strength of acids and bases are expressed using pH, pka, and pkb. Stephan Zabel/Getty Images

There are related scales in chemistry used to measure how acidic or basic a solution is and the strength of acids and bases. Although the pH scale is most familiar, pKa, Ka, pKb, and Kb are common calculations that offer insight into acid-base reactions. Here's an explanation of the terms and how they differ from each other.

What Does the "p" Mean?

Whenever you see a "p" in front of a value, like pH, pKa, and pKb, it means you're dealing with a -log of the value following the "p".

For example, pKa is the -log of Ka. Because of the way the log function works, a smaller pKa means a larger Ka. pH is the -log of hydrogen ion concentration, and so on.

Formulas and Definitions for pH and Equilibrium Constant

pH and pOH are related, just as Ka, pKa, Kb, and pKb are. If you know pH, you can calculate pOH. If you know an equilibrium constant, you can calculate the others.

About pH

pH is a measure of hydrogen ion concentration, [H+], in an aqueous (water) solution. The pH scale ranges from 0 to 14. A low pH value indicates acidity, a pH=7 is neutral, and a high pH value indicates alkalinity. The pH value can tell you whether you're dealing with an acid or a base, but it offers limited value indicating the true strength of the acid of base. The formula to calculate pH and pOH are:

pH = - log [H+]

pOH = - log [OH-]

At 25 degrees Celsius:

pH + pOH = 14

Understanding Ka and pKa

Ka, pKa, Kb, and pKb are more helpful for predicting whether a species will donate or accept protons at a specific pH value.

They describe the degree of ionization of an acid or base and are true indicators of acid or base strength because adding water to a solution will not change the equilibrium constant. Ka and pKa relate to acids, while Kb and pKb deal with bases. Like pH and pOH, these values also account for hydrogen ion or proton concentration (for Ka and pKa) or hydroxide ion concentration (for Kb and pKb).

Ka and Kb are related to each other through the ion constant for water, Kw:

Kw = Ka x Kb

Ka is the acid dissociation constant. pKa is simply the -log of this constant. Similarly, Kb is the base dissociation constant, while pKb is the -log of the constant. The acid and base dissociation constants are usually expressed in terms of mole per liter (mol/L). Acids and bases dissociate according to general equations:

HA + H2O ⇆ A- + H3O+


HB + H2O ⇆ B+ + OH-

In the formulas, A stands for acid and B for base.

Ka = [H+][A-]/ [HA]

pKa = - log Ka

at half the equivalence point, pH = pKa = -log Ka

A large Ka value indicates a strong acid because it means the acid is largely dissociated into its ions. A Large Ka value also means the formation of products in the reaction is favored. A small Ka value means little of the acid dissociates, so you have a weak acid. The Ka value for most weak acids ranges from 10-2 to 10-14.

The pKa gives the same information, just in a different way. The smaller the value of pKa, the stronger the acid. Weak acids have a pKa ranging from 2-14.

Understanding Kb and pKb

Kb is the base dissociation constant. The base dissociation constant is a measure of how completely a base dissociates into its component ions in water.

Kb = [B+][OH-]/[BOH]

pKb = -log Kb

A large Kb value indicates the high level of dissociation of a strong base. A lower pKb value indicates a stronger base.

pKa and pKb are related by the simple relation:

pKa + pKb = 14

What Is pI?

Another important point is pI. This is the isoelectric point. It is the pH at which a protein (or another molecule) is electrically neutral (has no net electrical charge).

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Your Citation
Helmenstine, Anne Marie, Ph.D. "pH, pKa, Ka, pKb, and Kb Explained." ThoughtCo, Aug. 30, 2017, Helmenstine, Anne Marie, Ph.D. (2017, August 30). pH, pKa, Ka, pKb, and Kb Explained. Retrieved from Helmenstine, Anne Marie, Ph.D. "pH, pKa, Ka, pKb, and Kb Explained." ThoughtCo. (accessed March 23, 2018).