Question

State whether the following statement is true or false for the given equation.
$N{H_3} + N{H_3} \rightleftarrows N{H_4}^+ + N{H_2}^-$
“This type of reaction is an acid-base reaction in terms of Bronsted Lowry protonic concept”
a) True
b) False

Answer 1

In the given reaction a proton is being transferred from one ammonium molecule to another and the reaction is at equilibrium. Check whether this reaction satisfies the Bronsted Lowry protonic concept of acids and bases.

Complete answer:
According to Bronsted Lowry protonic concept, any compound that can transfer a proton to another compound in a reaction is an acid and the compound that accepts the proton is a base.
In our given reaction, two ammonia molecules are reacting with each other to form $N{H_4}^ +$ and $N{H_2}^ -$. For this reaction to be in equilibrium, we need to have a proton transfer in the reaction. It is clear to us that ${H^+}$ is being transferred from one ammonium molecule to another.
The molecule that donates the proton becomes $N{H_2}^-$ and is an acid according to the Bronsted Lowry protonic concept. The molecule that accepts the proton becomes $N{H_4}^+$ and is a base.

**Therefore, we can conclude that the given statement is true i.e. option (a) is correct.

Note:**
In Bronsted Lowry theory or protonic theory of acids and bases, a proton donor is basically an acid and a proton acceptor is a base. Here, in the reaction given to us one ammonium molecule is donating a proton and the other is accepting that proton. Hence, according to the theory one is an acid and the other is a base.