Strong acid

A strong acid dissociates nearly completely in a specified solvent at ordinary concentrations. Its strength depends on the solvent and differs from the concentration of the acid solution.

Acid dissociation constant: An equilibrium constant that quantifies an acid’s tendency to donate a proton in a specified solvent. Its very large value corresponds to nearly complete dissociation for strong acids.
Brønsted–Lowry acid–base theory: A theory defining acids as proton donors and bases as proton acceptors. Strong-acid dissociation is proton donation to the surrounding solvent.
Hydrochloric acid: A strong aqueous acid composed of hydrogen chloride dissolved in water. It is a widely used strong acid in laboratories, industry, and biological systems.
Weak acid: An acid that dissociates only partially in a specified solvent at ordinary concentrations. Its limited dissociation contrasts with the near-complete dissociation that defines a strong acid.
Conjugate acid–base pair: Two chemical species related by the gain or loss of a proton. Dissociation produces the acid’s conjugate base and transfers a proton to a base.
Chemical equilibrium: A dynamic state in which forward and reverse reaction rates are equal. Acid dissociation is an equilibrium, even when it lies overwhelmingly toward products.
Sulfuric acid: A diprotic mineral acid whose first dissociation in water is essentially complete. Its first proton makes sulfuric acid a strong acid in aqueous solution.
Superacid: A medium more acidic than pure sulfuric acid under an acidity scale suited to that medium. Superacidity describes acidity beyond familiar aqueous strong acids, often in specialized media.
Hydronium ion: The protonated water ion, H₃O⁺, formed when water accepts a proton. In water, strong acids transfer protons to solvent molecules, producing hydronium.
Activity (chemistry): The effective concentration of a chemical species used in thermodynamic expressions. Acid strength and pH are defined through activities rather than concentration alone.

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