Weak base

A Brønsted–Lowry base that reacts only partially with water, establishing an equilibrium between the base and its conjugate acid.

Base ionization constant: The equilibrium constant describing a base’s reaction with water to form its conjugate acid and hydroxide ions. It quantifies how far a weak base’s proton-transfer reaction proceeds.
Brønsted–Lowry acid–base theory: A theory defining acids as proton donors and bases as proton acceptors. It supplies the proton-acceptance definition used for weak bases.
Ammonia: A nitrogen hydride, NH₃, that accepts a proton from water to form ammonium and hydroxide. Ammonia is a standard example of a weak base in aqueous chemistry.
Strong base: A base that reacts essentially completely with water or dissociates completely to produce hydroxide ions. Its near-complete reaction contrasts with a weak base’s partial protonation.
Conjugate acid: The species formed when a base accepts a proton. Its strength determines the equilibrium position for protonation of the weak base.
Chemical equilibrium: A dynamic state in which forward and reverse reaction rates are equal. A weak base’s partial reaction with water is an equilibrium, not a one-way conversion.
Pyridine: An aromatic nitrogen-containing heterocycle whose ring nitrogen can accept a proton. Its protonation illustrates how molecular structure affects weak-base behavior.
Weak acid: A Brønsted–Lowry acid that donates protons only partially in water, establishing an equilibrium with its conjugate base. It is the proton-donating counterpart to a weak base’s proton acceptance.
Water autoionization: The equilibrium in which water molecules transfer protons, producing hydronium and hydroxide ions. It supplies the hydroxide reference needed to relate base strength to conjugate-acid strength.
Equilibrium constant: A quantity expressing the ratio of product and reactant activities at chemical equilibrium. The equilibrium constant distinguishes partial reaction from near-complete proton transfer.

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