How can Kb be used to determine Ka for a conjugate base in chemistry?

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lostsheep
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Hey guys, I am new here. I am a college student that is trying to brush up on some chemistry. I am reading an old textbook that I have, and I didnt understand something.

I was wondering how some would use the Kb of a weak base, how they would determine the value of Ka for the conjugate base?

A sample problem in the book is: A weak acid has a Kb= 1.5 x 10^-9. What is the value of Ka for the conjugate base?


I have read the whole chapter over Acid & Bases, but it says this problem is on the cd-rom that is included with my book. Yet, i never received that cd when I bought my book. I have tried searching but have had no luck. Any help would be great. I am just trying to understand the relationship between Ka and Kb. Thanks again.
 
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K is called a dissociation constant

What K states is that there is a certain amount of dissociation at any given time, and almost everything has one of these numbers. Something like lead chloride will have a K value to say how soluble it is. Here you are talking about water, and K relates to water breaking from HOH into H and OH. For water, the dissociation constant is 10^-14.

[tex][H^+] * [OH^-] = 10^{-14}[/tex]

[tex]K_A * K_B = 10^{-14}[/tex]

[tex]pK_A + pK_B = 14[/tex]