An explanation regarding the correct choice of p K a values for the given ammonium cations is to be stated. Concept introduction: According to Bronsted-Lowry theory, when an acid donates a proton the species formed is known as conjugate base and when the base accepts a proton the species formed is known as conjugate acid. The equilibrium constant of an acid dissociation reaction depends on the strength of an acid involved in the reaction. The K a value is large for strong acids and small for weak acids. The stronger acid has a lower value of p K a and the weaker acid has a higher p K a value.

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Chapter 2, Problem 2.52P

Interpretation Introduction

Interpretation: An explanation regarding the correct choice of pKa values for the given ammonium cations is to be stated.

Concept introduction: According to Bronsted-Lowry theory, when an acid donates a proton the species formed is known as conjugate base and when the base accepts a proton the species formed is known as conjugate acid.

The equilibrium constant of an acid dissociation reaction depends on the strength of an acid involved in the reaction. The Ka value is large for strong acids and small for weak acids. The stronger acid has a lower value of pKa and the weaker acid has a higher pKa value.

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