pH is a measure of the acidity or alkalinity of a solution. Solutions with a pH less than seven are considered acidic, while those with a pH greater than seven are considered basic (alkaline). pH 7 is considered neutral because it is the accepted pH of pure water at 25 °C, although, due to the self-ionization of water, this is not completely accurate. pH is formally dependent upon the activity of hydrogen  ions (H⁺), but for very pure dilute solutions, the morality may be used as a substitute with some sacrifice of accuracy. Because pH is dependent on activity, a property which cannot be measured easily or predicted theoretically, it is difficult to determine an accurate value for the pH of a solution. The pH reading of a solution is usually obtained by comparing unknown solutions to those of known pH, and there are several ways of doing this.

The concept of pH was first introduced by Danish chemist S. P. L. Sørensen in 1909. The name, pH, has been purported to come from a variety of places including: pondus hydrogenii (Latin), potentiel hydrogène (French), and potential of hydrogen (English). However pH is actually a shorthand for its mathematical approximation: in chemistry a small p is used in place of writing − log₁₀ and the H should more correctly be [H⁺], standing for concentration of hydrogen ions.

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