Chapter 17, Problem 17.4QP

Interpretation Introduction

Interpretation:

The increasing orders for acids strength for given acids namely $\text{HX,}\text{HY}\text{and}\text{HZ}$ should be determined using the given $p{K}_b$ values.

Concept Introduction:

$\text{Bronsted-Lowry Acids}$: If a species loses a proton then it is considered as $\text{Bronsted-Lowry acid}\text{.}$

$\text{Bronsted-Lowry Base}$: If a species receives one proton, then it is considered as $\text{Bronsted-Lowry base}\text{.}$

Strong Acids: Acids that dissociates into ions completely which results in easy donation of protons are considered as strong acids. Strong acid forms weaker conjugated base.

Strong Base: Bases that has strong attraction towards protons and accepts readily. Strong base forms weaker conjugated acid.

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

Base dissociation constant ${\text{K}}_{\text{b}}$ represents how strong the base is in a solution.

  $p{K}_b=-\log K_b$

The strength of base decreases as the value of $p{K}_b$ increases