A Brønsted-Lowry base is defined as a substance that can accept protons (H⁺ ions) in a chemical reaction. This theory, developed by Johannes Brønsted and Thomas Lowry in the early 20th century, expands the concept of bases beyond just hydroxide ions (OH⁻). When a Brønsted-Lowry base accepts a proton, it often forms a corresponding Brønsted-Lowry acid. This interaction is crucial in many chemical processes, including acid-base reactions in solutions. Common examples of Brønsted-Lowry bases include ammonia (NH₃) and sodium bicarbonate (NaHCO₃).