Final answer:
The base dissociation constant Kb for the conjugate base of the unknown acid Ha with Ka = 4.57 x 10×3 is calculated as 2.19 x 10×12.
Step-by-step explanation:
The base dissociation constant Kb for the conjugate base of an acid Ha can be calculated using the relationship Ka × Kb = 1.0 × 10-14. Given that the acid dissociation constant Ka for the unknown acid Ha is 4.57 x 10×3, we can calculate its Kb:
Ka × Kb = 1.0 × 10-14
4.57 x 10×3 × Kb = 1.0 × 10-14
To find Kb, divide both sides by the Ka value:
Kb = × 1.0 × 10-14 / 4.57 x 10×3
Kb = 2.19 x 10×12
The conjugate base's Kb is 2.19 x 10×12, indicating its affinity to accept protons (H+) in water.