The Arrhenius theory explains why ammonia, NH3, is basic, but the Bronsted-Lowry theory does not.
True or False
False
Both explain how NH3 acts as a base.
False. The Arrhenius theory and the Bronsted-Lowry theory both explain why ammonia, NH3, is basic. According to the Arrhenius theory, a base is a substance that produces hydroxide ions (OH-) when dissolved in water. NH3, when dissolved in water, reacts with water to form NH4+ and OH-. Therefore, according to the Arrhenius theory, NH3 is a base.
On the other hand, the Bronsted-Lowry theory defines a base as a substance that accepts a proton (H+) in a chemical reaction. NH3 can accept a proton to form NH4+. Therefore, according to the Bronsted-Lowry theory, NH3 is also a base.
True. The Arrhenius theory explains that substances like ammonia (NH3) are basic because they produce hydroxide ions (OH-) when dissolved in water. According to the Arrhenius theory, a substance is considered a base if it increases the concentration of hydroxide ions in the aqueous solution.
On the other hand, the Bronsted-Lowry theory, which is a more general theory of acids and bases, defines an acid as a proton (H+) donor and a base as a proton acceptor. In the case of ammonia (NH3), it can act as a base by accepting a proton (H+) from an acid and forming ammonium ion (NH4+). However, the Bronsted-Lowry theory does not explicitly explain the basicity of ammonia by referring to the hydroxide ion (OH-).
Therefore, the statement is true. The Arrhenius theory provides an explanation for the basic nature of ammonia, whereas the Bronsted-Lowry theory does not explicitly do so.