Ionic Equilibrium

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An Arrhenius acid is a substance that dissociates in aqueous solution to produce hydrogen ions (H⁺). Example: HCl → H⁺(aq) + Cl⁻(aq).

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An Arrhenius base is a substance that dissociates in aqueous solution to produce hydroxide ions (OH⁻). Example: NaOH → Na⁺(aq) + OH⁻(aq).

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It only applies to aqueous solutions and cannot explain acidic or basic behavior of substances without H⁺ or OH⁻, such as AlCl₃ (acidic) or NH₃ (basic).

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A Brønsted-Lowry acid is a proton (H⁺) donor; a base is a proton acceptor. Example: In NH₃ + H₂O ⇌ NH₄⁺ + OH⁻, H₂O is acid (donates H⁺), NH₃ is base (accepts H⁺).

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Acid: HF, Base: H₂O; Conjugate acid: H₃O⁺, Conjugate base: F⁻. Pairs: HF/F⁻ and H₃O⁺/H₂O.

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Two species differing by one proton. Example: NH₃ (base) and NH₄⁺ (conjugate acid); F⁻ (base) and HF (conjugate acid).

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H⁺ has high charge density and cannot exist freely in water. It bonds with H₂O to form H₃O⁺, known as hydronium ion.

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Lewis acid: electron pair acceptor (e.g., BF₃). Lewis base: electron pair donor (e.g., NH₃). Reaction: BF₃ + NH₃ → F₃B←NH₃ (adduct).