which example is a bronsted-lowry base but not an arrhenius base?
Which example is a Bronsted-Lowry base but not an Arrhenius base?
Answer: In the context of acid-base theories, it is important to understand the differences between the Bronsted-Lowry and Arrhenius definitions. An Arrhenius base is defined as a substance that increases the concentration of hydroxide ions (OH-) when dissolved in water, while a Bronsted-Lowry base is a substance that accepts a proton (H+) from an acid.
One common example of a Bronsted-Lowry base that is not considered an Arrhenius base is ammonia (NH3). In the Bronsted-Lowry theory, ammonia can accept a proton to form its conjugate acid, ammonium ion (NH4+). However, in the Arrhenius theory, ammonia does not increase the concentration of hydroxide ions in water when dissolved.
So, ammonia is a classic example of a Bronsted-Lowry base, as it has the ability to accept a proton, but it is not categorized as an Arrhenius base since it does not produce hydroxide ions in water.