= Weak electrolyte
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A <weak electrolyte> yields only a fraction of <ions> from its dissolved substance under the specified conditions, as illustrated by <acetic acid> in <water>.
For a neutral <weak acid>, unconverted <molecules> coexist with <hydronium> and the <conjugate base> at <chemical equilibrium>. The <weak acid dissociation fraction> describes the partition of the dissolved inventory; the <acid dissociation constant> describes the <chemical equilibrium> at fixed <solvent>, <temperature> and <standard states>. A single fraction is not a permanent label for every <concentration>: <dilution> can increase that fraction while the <acid dissociation constant> stays fixed. Calling a substance a <weak electrolyte> does not mean its <chemical solution> must be dilute.<Chemistry 2e by Paul Flowers and others/14.3 Relative Strengths of Acids and Bases>[Chemistry 2e, §14.3, Acid and Base Ionization Constants, percent-ionization discussion preceding Example 14.7]{ref}
The following <ideal weak electrolyte dilution law> makes the distinction quantitative for a <monoprotic acid>. Other <weak electrolytes>, mixed <chemical solutions> and additional proton-transfer steps require their own <chemical equilibrium> and inventory balances.
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