Chapter 16, Problem 16.33AP

Interpretation Introduction

Interpretation:

It should be determined that, whether water is a weaker or stronger base than ammonia.

Concept introduction:

A base donates a pair of electrons to a proton.

Basicity will decrease as an atom becomes more electronegative.

For example: oxygen is more electronegative than nitrogen, therefore its electron are less likely to be donated to a proton.

In the Bronsted – Lowery definition of acid and bases,

• An acid is a $H^{+}$ (proton) donor.
• A base is a proton acceptor.

Conjugate acid formed when the proton is transferred to the base.

In a conjugate base everything that remains of the acid molecule after a proton is lost.

$\begin{array}{l}\text{Conjugate}\text{acid}\text{=}\text{Base}\text{+}{\text{H}}^{\text{+}}\\ \text{Conjugate}\text{base}\text{=}A\text{cid}\text{+}{\text{H}}^{\text{+}}\end{array}$