The two acid dissociation constants for carbonic acid,H₂CO₃,are 4.3 $\times$ 10^-⁷ and 4.8 $\times$ 10^-¹¹ at 25°C.The base constant,K_b,or hydrolysis constant for HCO₃^- is: A)4.3 $\times$ 10^-⁷ B)4.8 $\times$ 10^-¹¹ C)2.1 $\times$ 10^-¹⁷ D)2.3 $\times$ 10^-⁸ E)6.2 $\times$ 10^-²²

Question

Quizplus · Accepted Answer

The base constant for hydrolysis of HCO₃ can be calculated using the relation: KB = Kw / Ka2 where Kw is the ion product constant of water (1.0 x 10^-14) and Ka2 is the second acid dissociation constant for carbonic acid. Substituting the given values: KB = (1.0 x 10^-14) / (4.8 x 10^-11) KB = 2.1 x 10^-4 Therefore, the best choice is C: 2.1 x 10^-4.

The Two Acid Dissociation Constants for Carbonic Acid,H2CO3,are 4 ×\times× 10-7 and 4

The Two Acid Dissociation Constants for Carbonic Acid,H₂CO₃,are 4 $\times$ 10^-⁷ and 4