Question

An acid has an acid dissociation constant of 2.8 10–9. What is the base dissociation constant of its conjugate base?

Answer 1

The answer is 3.6 x 10^-6

Answer 2

Answer: The base dissociation constant for a conjugate base is
`3.5* 10^(-6)`

Step-by-step explanation:

To calculate the base dissociation constant for the given acid dissociation constant, we use the equation:

`K_w=K_b* K_a`

where,

`K_w` = Ionic product of water =
`10^(-14)`

`K_a` = Acid dissociation constant =
`2.8* 10^(-9)`

`K_b` Base dissociation constant = ?

Putting values in above equation, we get:

`10^(-14)=2.8* 10^(-9)* K_b\\\\K_b=0.35* 10^(-5)=3.5* 10^(-6)`

Hence, the base dissociation constant for a conjugate base is
`3.5* 10^(-6)`