\[K_b=\frac{[BH^+][OH^-]}{[B]}\]
Variables
Kbbase dissociation constant
BH[BH⁺]protonated base concentration (mol/L)
OH[OH⁻]hydroxide ion concentration (mol/L)
Bundissociated base concentration (mol/L)
Description
What is this formula?
The base dissociation constant relation defines the equilibrium constant for the ionization of a weak base in aqueous solution.
When to use it
Use this equation to calculate equilibrium concentrations, determine base strength, analyze weak base solutions, and study buffer systems containing weak bases.
Example
Given:
[BH+] = 2.0×10^-4 mol/L
[OH−] = 2.0×10^-4 mol/L
[B] = 0.10 mol/L
Formula:
Kb = ([BH+][OH−])/[B]
Substitution:
Kb = (2.0×10^-4 × 2.0×10^-4)/0.10
Kb = 4.0×10^-7
Result:
Kb = 4.0×10^-7
Applications
Weak base analysis
Buffer calculations
Analytical chemistry
Environmental chemistry
Chemical equilibrium calculations