NH3 acts as Bronsted-Lowry Base
In 1923, scientists Johannes Bronsted and Thomas Lowry independently suggested new classifications for acids and bases. Instead of addressing both hydrogen and hydroxide ions, they simply considered hydrogen. A Bronsted-Lowry acid is a substance that contributes a hydrogen ion to a chemical process. In contrast, a Bronsted-Lowry base is a substance that accepts a hydrogen ion in a chemical process. Thus, the Bronsted-Lowry definitions of an acid and a base emphasise the movement of hydrogen ions during a chemical reaction, as opposed to the formation of hydrogen ions and hydroxide ions in an aqueous solution.
Bronsted Lowry acid-base reaction example
Let’s take the ammonia-water reaction to illustrate the Bronsted-Lowry definitions of acid and base. Ammonia and water molecules serve as reactants, whereas ammonium ion and hydroxide ion serve as products:
The water molecule is the Bronsted-Lowry acid because it provides a hydrogen ion to the ammonia molecule, whereas the ammonia molecule is the Bronsted-Lowry base because it takes the hydrogen ion. Consequently, ammonia functions as a base in the Bronsted-Lowry perspective.
Frequently asked Questions -FAQ
Why is ammonia a Bronsted-Lowry base but not an Arrhenius base?
The NH3 molecule is a Bronsted-Lowry base, but not an Arrhenius base. According to the Bronsted-Lowry hypothesis, NH3 is a proton acceptor, but according to the Arrhenius theory, it does not raise the concentration of OH when mixed with water.
What is a Brønsted base give an example?
Bronsted base refers to a substance that accepts a proton from another substance. Ammonia NH3 is an example of a Bronsted lowry base.
What is a Bronsted-Lowry acid ?
Bronsted-Lowry acids must donate protons. This would be paired with an atom known as a Bronsted-Lowry base that accepts a proton.