Final answer:
Bronsted-Lowry bases are compounds that can accept a proton and typically produce hydroxide ions in aqueous solutions. Examples include ammonia, with strong bases completely dissociating to form many hydroxide ions and weak bases partially dissociating.
Step-by-step explanation:
According to the Bronsted-Lowry theory, compounds that are bases in aqueous solutions are those that can accept a proton (hydrogen ion, H+). A Bronsted-Lowry base is characterized by its ability to accept a proton during a chemical reaction. When a base reacts with water, it typically produces hydroxide ions (OH−).
For example, when ammonia (NH3) is dissolved in water, it accepts a proton from a water molecule, leading to the formation of ammonium ions (NH4+) and hydroxide ions (OH−), demonstrating its behavior as a base:
NH3(aq) + H2O(l) → NH4+(aq) + OH−(aq)
Strong bases completely dissociate in water to form a large amount of hydroxide ions, while weak bases partially dissociate, producing only a small amount of hydroxide ions. The strength of a Bronsted-Lowry base can be determined by its base ionization constant (Kb).