Question

Be sure to answer all parts. Be sure to report your answer to the correct number of significant figures. Determine Kb of the weak base B whose conjugate acid HB+ has Ka 6.6 × 10−4. × 10 Determine the Ka of the weak acid HA whose conjugate base has Kb 2.1 × 10−8.

Answer 1

part 1: Kb of the weak base = 1.5 x 10^-11

part 2: Ka of the weak acid = 4.8 x 10^-7

Step-by-step explanation:

Using the formula Ka x Kb = 1.0 x 10^-14

Part 1:

Ka x Kb = 1.0 x 10^-14

Kb = (1.0 x 10^-14)/Ka = (1.0 x 10^-14)/(6.6 x 10^-4) = 1.5 x 10^-11

Part 2:

Ka x Kb = 1.0 x 10^-14

Ka = (1.0 x 10^-14)/Kb = (1.0 x 10^-14)/(2.1 x 10^-8) = 4.8 x 10^-7