Calculateur de Kb
Calculez la constante de basicité Kb d'une base faible.
Kb
0.0010
Kb vs Concentration of Conjugate Acid [BH⁺]
Formule
## 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.
Exemple Résolu
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
Questions Fréquentes
What does Kb represent?
Kb is the base dissociation constant. It measures the extent to which a base dissociates in water to produce hydroxide ions.
How are Ka and Kb related?
For a conjugate acid-base pair, Ka × Kb = Kw = 1.0 × 10⁻¹⁴ at 25°C.
What is a typical Kb for a weak base?
Weak bases have Kb values between about 10⁻² and 10⁻¹³. Ammonia has Kb = 1.8 × 10⁻⁵.
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