Arrhenius and Bronsted-Lowry acids and bases, and strong vs. weak

There are two common definitions of acids and bases. In the Arrhenius definition, an acid produces hydrogen ions (H+, which exist in water as hydronium, H3O+) when dissolved in water, and a base produces hydroxide ions (OH-). The broader Bronsted-Lowry definition says an acid is a proton (H+) donor and a base is a proton acceptor, which also covers bases like ammonia, NH3, that produce hydroxide by taking a proton from water. Strength describes how completely an acid or base ionizes in water: strong acids like hydrochloric and nitric acid ionize completely, while weak acids like acetic acid in vinegar ionize only partially; sodium hydroxide is a strong base and ammonia a weak one. Strength is not the same as concentration: a dilute strong acid and a concentrated weak acid are both possible.

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