## 12.45 [ENDORSED]

Acidity $K_{a}$
Basicity $K_{b}$
The Conjugate Seesaw $K_{a}\times K_{b}=K_{w}$

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Kayla Ikemiya 1E
Posts: 56
Joined: Fri Sep 29, 2017 7:04 am

### 12.45

So the back of the book has two different ways of arriving at the fact that 2,4,6 trichlorophenol. Is it enough to just look at which compound has a greater Ka value or do we need to know that the chlorine atoms have a greater withdrawing power?

Hannah Chew 2A
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Joined: Fri Sep 29, 2017 7:05 am
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### Re: 12.45  [ENDORSED]

I'm assuming you are referring to 12.43 instead of 12.45, but I would use the "withdrawing power" or electronegativity differences to explain why 2,4,6 trichlorophenol has a larger Ka. You would use the Ka to identify which is stronger, but to "account for the difference in acid strength," you would have to look at the structure itself.

Humza_Khan_2J
Posts: 56
Joined: Thu Jul 13, 2017 3:00 am

### Re: 12.45

If the attached atoms to an O-H bond have a higher electronegativity, they delocalize the charge on the O- and make it more stable. If anion of an acid post-ionization is more stable, then it will be more acidic because this molecular with ionize more than others, simply due to the anion being more stable than other anions.

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