What is the difference between Kb and pKb.

The terms "Kb" and "pKb" are related to the strength of a base, specifically in the context of chemistry and chemical reactions. Here's the breakdown:

Kb (Base Dissociation Constant):

Kb represents the equilibrium constant for the dissociation of a base in water. It measures the strength of a base in aqueous solution.
Mathematically, Kb is defined as the ratio of the concentrations of the products (the conjugate acid and hydroxide ions) to the concentration of the reactant (the undissociated base) when the base is dissolved in water.
The higher the value of Kb, the stronger the base.
pKb (Negative Logarithm of Kb):

pKb is simply the negative logarithm (base 10) of Kb. It's a way of expressing the strength of a base on a logarithmic scale.
The formula for calculating pKb is: pKb = -log(Kb).
Just like pH (which measures the acidity of a solution) is the negative logarithm of the hydrogen ion concentration (pH = -log[H+]), pKb gives a measure of the basicity of a compound.
The lower the value of pKb, the stronger the base.
In summary, Kb is the actual numerical value representing the strength of a base, while pKb is a logarithmic transformation of Kb, often used to simplify calculations and comparisons between bases.