Question

Is ammonium ion a bronsted base

Answer 1

Unlikely. It's unlikely for ammonium ion
`{\text{NH}_4}^(+)` to accept a proton
`\text{H}^(+)` and act as a Bronsted-Lowry Acid.

Step-by-step explanation

What's the definition of Bronsted-Lowry acids and bases?

• Bronsted-Lowry Acid: a species that can donate one or more protons
  `\text{H}^(+)` in a reaction.

• Bronsted-Lowry Base: a species that can accept one or more protons
  `\text{H}^(+)`

Ammonium ions
`{\text{NH}_4}^(+)` are positive. Protons
`\text{H}^(+)` are also positive.

Positive charges repel each other, which means that it will be difficult for
`{\text{NH}_4}^(+)` to accept any additional protons. As a result, it's unlikely that
`{\text{NH}_4}^(+)` will accept any proton and act like a Bronsted-Lowry Base.