Kb Rechner — Formel
## How to Calculate Kb
### Formula
**Kb = [BH⁺][OH⁻] / [B]**
Where:
- **Kb** = base dissociation constant
- **[BH⁺]** = concentration of conjugate acid at equilibrium
- **[OH⁻]** = hydroxide ion concentration at equilibrium
- **[B]** = concentration of undissociated base at equilibrium
Larger Kb indicates a stronger base.
### Formula
**Kb = [BH⁺][OH⁻] / [B]**
Where:
- **Kb** = base dissociation constant
- **[BH⁺]** = concentration of conjugate acid at equilibrium
- **[OH⁻]** = hydroxide ion concentration at equilibrium
- **[B]** = concentration of undissociated base at equilibrium
Larger Kb indicates a stronger base.
Lösungsbeispiel
A 0.1 M ammonia solution has [NH4⁺] = 0.01 M and [OH⁻] = 0.01 M at equilibrium.
- Kb = [BH⁺][OH⁻] / [B]
- Kb = (0.01)(0.01) / 0.1
- Kb = 0.0001 / 0.1
- Kb = 1.0 × 10⁻³