Homework Help :12.43 pg 513

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

John Huang 1G
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Homework Help :12.43 pg 513

The values of Ka for phenol and 2,4,6-trichlorophenol (see following structures) are 1.3x10^10 and 1.0x10^6, respectively. Which is the stronger acid? Account for the difference in acid strength.

By what means are we supposed to determine the strength of the acid? Is it simply a matter of which Ka value is larger or smaller? Or do we have to look at the structures of the compounds?
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Danah Albaaj 1I
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Re: Homework Help :12.43 pg 513

You would want to consider how trichlorophenol has atoms with a higher electronegativity on it, which correlates with its strength as an acid. This is because the bonds of atoms with higher electronegativity typically are weaker therefore increasing the transfer of H+