Question

What is the relationship between \[p{K_a} and p{K_b}\] values where ${K_a} and {K_b}$ represent ionization constants of the acid and its conjugate base respectively?

Answer 1

Hint: To answer this question, we first need to understand what ionization constant is. In a solution or liquid, an ionization constant (abbreviated K) is a constant that depends on the equilibrium between ions and non-ionized molecules. A dissociation constant is another name for an ionization constant.

Complete answer:
Ionization constant - It's the ratio of products to reactants increased to the right stoichiometric powers, or the ratio of concentration product to reactant. Corrosion can be caused by any imbalance in the equation.
Acid - An acid is a molecule or ion that has the ability to donate a proton or establish a covalent connection with an electron pair. The proton donors, also known as Brnsted–Lowry acids, are the first group of acids.
Base - There are three prevalent meanings of the word base in chemistry: Arrhenius bases, Brnsted bases, and Lewis bases. According to all definitions, bases are chemicals that react with acids, as proposed by G.-F. Rouelle in the mid-eighteenth century.
$p{K_a}$ - It is the negative base-10 logarithm of the acid dissociation constant $({K_a})$ of a solution. Because it uses small decimal quantities to explain acid dissociation, $p{K_a}$ is used. Ka values can provide the same type of information, but they are often exceedingly small figures written in scientific notation that are difficult to comprehend for most people.
 $p{K_a} = - \log ({K_a})$
$p{K_b}$ - It is the negative base-10 logarithm of the acid dissociation constant $({K_b})$ of a solution. The stronger the base, the lower the pKb value. The computation of the base dissociation constant, like the computation of the acid dissociation constant, $p{K_b}$ , is an approximation that is only correct in dilute solutions.
$p{K_b} = - \log ({K_b})$
Relation between \[p{K_a}{\kern 1pt} {\kern 1pt} {\kern 1pt} and{\kern 1pt} {\kern 1pt} {\kern 1pt} p{K_b}\] values where ${K_a}{\kern 1pt} \,and{\kern 1pt} {\kern 1pt} {\kern 1pt} {K_b}$ is
$p{K_a} + p{K_b} = p{K_w} = 14$
So, the final answer is $p{K_a} + p{K_b} = p{K_w} = 14$ .

Note:
The pH of an aqueous solution is a measurement of hydrogen ion concentration. Although $p{K_a}$ (acid dissociation constant) and pH are connected, $p{K_a}$ is more specific in that it aids in predicting what a molecule would do at a given pH. The Henderson-Hasselbalch equation describes the link between pH and $p{K_a}$ .