Dissociation Constants for Bases (HSC SSCE Chemistry): Quizzes

Extent of weak base splitting in water

$K_b = \frac{[\text{BH}^+][\text{OH}^-]}{[\text{B}]}$

Larger $K_b$ indicates a stronger base

Nearly 100%

$[\text{OH}^-] = [\text{NH}_4^+]$

$K_a \times K_b = K_w$

$[\text{OH}^-] = 10^{-\text{pOH}}$

Equilibrium $[\text{B}] \approx$ initial $[\text{B}]$

Phosphate ion ($K_b = 5.9 \times 10^{-3}$)

$1.8 \times 10^{-5}$