The Arrhenius theory explains why ammonia, NH₃, is basic, but the Bronsted-Lowry theory does not.

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The Arrhenius theory explains acids and bases in terms of the production of hydrogen ions or hydroxide ions in water. The Bronsted-Lowry theory, however, explains acids and bases in terms of their ability to donate or accept protons (H+), respectively. According to the Bronsted-Lowry theory, ammonia is basic because it can accept a proton (H+) to form ammonium (NH4+), thus providing an explanation for its basic nature.

The Arrhenius Theory Explains Why Ammonia, NH3, Is Basic, but the Bronsted-Lowry

The Arrhenius Theory Explains Why Ammonia, NH₃, Is Basic, but the Bronsted-Lowry