Arrhenius, Bronsted-Lowry and Lewis acids and bases, conjugate pairs, the ionisation of water, the pH scale, and the ionisation constants of weak acids and bases.
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Created by StemPy LabArrhenius called an acid anything that gives in water, and a base anything that gives . Bronsted and Lowry widened this: an acid gives a proton and a base takes one, so every acid has a conjugate base. Lewis widened it again to electron pairs. Strong acids ionise fully in water, weak acids only partly.
Water ionises very slightly into and . The product of their concentrations, , is at . The pH, minus the logarithm of the hydronium concentration, turns these tiny numbers into a scale from about 0 to 14. For a strong acid or base the concentration gives the pH at once.
A weak acid ionises only partly, and its ionisation constant measures how far. When little ionises, and the degree of ionisation is about . Weak bases follow the same rules with . For a conjugate pair, .
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