PKa, also known as acid dissociation constant, is a measure of the strength of an acid in solution. Specifically, it is the negative logarithm (base 10) of the equilibrium constant for the dissociation of an acid in water.
A lower pKa value indicates a stronger acid as it will have a higher concentration of hydronium ions in solution at equilibrium. Conversely, a higher pKa value indicates a weaker acid as it will have a lower concentration of hydronium ions in solution at equilibrium.
Early studies on pKa were performed in the late 1800s by Swedish chemist Svante Arrhenius, who proposed that acids produce hydronium ions when dissolved in water. Later, American chemist Gilbert N. Lewis developed the concept further by including bases and proposing that acids and bases form conjugate acid-base pairs that differ only by a single proton (H+ ion).
Today, pKa values are widely used in chemistry, biochemistry, and pharmacology to predict the behavior and reactivity of acids and bases in various chemical reactions and biological processes.
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