Equilibrium constants

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Julia Lindner 1I
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Equilibrium constants

Postby Julia Lindner 1I » Wed Dec 05, 2018 6:00 pm

In general, what are equilibrium constants and what is their significance? Also, what is Kw (the autoprotolysis constant according to the textbook), and what do we need to know about it for the final? Finally, what is the difference between Kw and Ka? Thanks in advance.

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Re: Equilibrium constants

Postby Chem_Mod » Thu Dec 06, 2018 1:59 pm

Equilibrium constants show us if products or reactants are favored in a reaction.
If Keq >>>1, then the products are favored more than the reactants. On the other hand, if Keq <<<1, the products are favored less than the reactants.

In terms of acids, a weak acid has a much lower Keq than a strong acid because the weak acid won't dissociate as much as strong acids will.

Kw is the equilibrium constant for water, which is just Kw = [H+][OH-] = 1 x 10-14. Ka is equilibrium constant for acids.

For the final, understand the equations and what situations you could use them in.


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