Free Kb Calculator
Calculate the base dissociation constant (Kb) from equilibrium concentrations of the conjugate acid, hydroxide ion, and undissociated base.
M
M
M
Kb
0.0010
pKb3.00
Kb vs Concentration of Conjugate Acid [BH⁺]
How to Calculate Kb
Formula
Kb = [BH⁺][OH⁻] / [B]
Where:
Larger Kb indicates a stronger base.
Example Calculation
A 0.1 M ammonia solution has [NH4⁺] = 0.01 M and [OH⁻] = 0.01 M at equilibrium.
- 01Kb = [BH⁺][OH⁻] / [B]
- 02Kb = (0.01)(0.01) / 0.1
- 03Kb = 0.0001 / 0.1
- 04Kb = 1.0 × 10⁻³
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