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( Strong acid) A strong acid is an acid that ionizes completely in an aqueous solution (not in the case of sulfuric acid as it is diprotic), or in other terms, with a pK_a < -1.74. This generally means that in aqueous solution at standard temperature and pressure, the concentration of hydronium ions is equal to the concentration of strong acid introduced to the solution. While strong acids are generally assumed to be the most corrosive, this is not always true. The carborane superacid (H(CHB₁₁Cl₁₁), which is one million times stronger than sulfuric acid, is entirely non-corrosive, whereas the weak acid hydrofluoric acid (HF) is extremely corrosive and can dissolve, among other things, glass and all metals except iridium. The equation for complete dissociation of an acid in aqueous solution is as follows

In all other acid-water reactions, dissociation is not complete, so will be represented as an equilibrium, not a completed reaction. The typical definition of a weak acid is any acid that does not dissociate completely. The difference separating the acid dissociation constants of strong acids from all other acids is so small that this is a reasonable demarcation.

Due to the complete dissociation of strong acids in aqueous solution, the concentration of hydronium ions in the water is equal to the re-duplication of the acid introduced to solution [HA] = [H⁺] = [A^-]; pH = -log[H⁺].

The strength of an acid, in comparison to other acids, can be determined without the use of pH calculations by observing the following characteristics

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