Question

Of the following anions, the strongest Bronsted base is:
A. $Cl{O^ - }$
B. $Cl{O_2}^ -$
C. $Cl{O_3}^ -$
D. $Cl{O_4}^ -$

Answer 1

To solve this question, first we will discuss the acids of the given respective conjugate or bronsted base. And compare the acids on the basis of oxygen atoms of the compounds. And then only we will conclude the order of given bases and that’s how we will choose our strongest bronsted base.

Complete step-by-step answer:
As we know,
$HCl{O_4}$ is the strongest acid among $HClO$ , $HCl{O_2}$ , $HCl{O_3}$ and $HCl{O_4}$ as more the number of oxygen atoms attached, more is the acidity of the molecule order of acidity is :
$HClO > HCl{O_2} > HCl{O_3} > HCl{O_4}$
When the acid is strong, the corresponding conjugate base will be weak as acids give up their protons, because the resulting conjugate base becomes more stable and does not react.
So, the conjugate or bronsted order will be just reverse:
$Cl{O^ - } > Cl{O_2}^ - > Cl{O_3}^ - > Cl{O_4}^ -$
So, the strongest bronsted base is $Cl{O^ - }$ .

Hence, the correct option is (A.) $Cl{O^ - }$ .

Note: The Bronsted-Lowry corrosive base hypothesis (or Bronsted Lowry hypothesis) recognizes solid and frail acids and bases dependent on whether the species acknowledges or gives protons or $H +$ . As indicated by the hypothesis, an acid and base respond with one another, making the corrosive structure its form base and the base to frame its form corrosive by trading a proton.