Question

In the reaction: HCl(g) + NH3(aq) → NH4 +(aq) + Cl– (aq), HCl(g) is acting as a(n):

Answer 1

The correct answer is Bronsted-Lowry Acid

Answer 2

Answer:
`HCl(g)` is acting as a Bronsted acid.

Step-by-step explanation:

According to the Bronsted-Lowry conjugate acid-base theory, an acid is defined as a substance which donates protons and thus forming conjugate base and a base is defined as a substance which accepts protons and thus forming conjugate acid.

For the given chemical equation:

`HCl(g)+NH_3(aq)\rightarrow NH_4^+(aq)+Cl^-(aq)`

Here,
`HCl` is loosing a proton, thus it is considered as a bronsted acid and after losing a proton, it forms
`Cl^-` which is a conjugate base.

And,
`NH_3` is gaining a proton, thus it is considered as a bronsted base and after gaining a proton, it forms
`NH_4^+` which is a conjugate acid.