The term "pKa" is a measure of the strength of an acid in solution. It is defined as the negative base 10 log of the acid dissociation constant. A lower pKa value indicates a stronger acid.
High pKa refers to a weak acid. The strength of an acid refers to its ability to lose a proton. A strong acid has a low pKa whereas a weak acid has a high pKa.
The equation pH = pKa + log is known as the Henderson-Hasselbach equation. In chemistry this equation is often used to prepare buffers in laboratory settings with the availability of weak acids. Weak acids that don't completely disassociate within a solution such as wat...
In chemistry, the main difference between pH and pKa is that pH tells the level of hydrogen ions in a certain medium while pKa value indicates the degree at which an acid dissociates or the side at which equilibrium is favored, according to Tutor Vista.
The pKa of an amino acid depends upon its type, group and side chains. For example, when lysine is part of the carboxylic acid group, it has a pKa of 2.18, compared to a pKa of 8.95 when it is part of the amino group and 10.53 with side chains.
The pKa of benzoic acid is equal to approximately 4.20. The pKa value is a measure of the acidity of a substance, with lower values indicating a stronger acid.
The pka values of carbonic acid are 6.3 for carbonic (I) and 10.3 for carbonic (II). Carbonic (I) has the molecular formula of H2CO3 while carbonic (II) has the molecular formula of HCO3-.