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.

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.