Weak acid

A weak acid dissociates only partially in a specified solvent at equilibrium. Its degree of dissociation depends on its acid strength, concentration, and conditions.

Acid dissociation constant: An equilibrium constant that quantifies an acid’s tendency to donate a proton in a specified solvent. Its value measures how strongly a weak acid dissociates.
Brønsted–Lowry acid–base theory: A theory defining acids as proton donors and bases as proton acceptors. It defines weak-acid behavior through reversible proton donation.
Buffer solution: A solution that resists pH change, typically containing a weak acid and its conjugate base. A weak acid paired with its conjugate base provides a practical buffer.
Strong acid: An acid that dissociates nearly completely in a specified solvent under the stated conditions. Its near-complete dissociation contrasts with the equilibrium mixture of a weak acid.
Henderson–Hasselbalch equation: An equation relating a buffer’s pH to its acid dissociation constant and conjugate acid–base ratio. It predicts buffer pH from a weak acid’s equilibrium and its conjugate base.
pH: A logarithmic measure of hydrogen-ion activity in a solution. The hydrogen ions released by a weak acid influence solution pH.
Acid–base titration: A quantitative method that determines solution concentration through a neutralization reaction. Titrating a weak acid produces a characteristic curve and equivalence-point pH.
Weak base: A base that accepts protons only partially in a specified solvent at equilibrium. It shares partial ionization behavior but acts as a proton acceptor.
Conjugate acid–base pair: Two chemical species that differ by one proton and are related by proton transfer. Dissociation converts a weak acid into its conjugate base.
Chemical equilibrium: A dynamic state in which forward and reverse reaction rates are equal. Partial dissociation is an equilibrium between molecular acid and ions.

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