Maintaining relation between [H3O+] and [OH-]

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Sarah Kiamanesh 1D
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Joined: Fri Sep 28, 2018 12:22 am

Maintaining relation between [H3O+] and [OH-]

Postby Sarah Kiamanesh 1D » Mon Jan 14, 2019 8:33 pm

The textbook emphasizes that because Kw is an equilibrium constant, the product of the concentrations of H3O+ and OH- ions in any aqueous solution is always equal to Kw and that when the concentration of one increases, the other decreases, and vice versa, to maintain this proportion. What is the process that allows this to happen?

Jayasuriya Senthilvelan 4I
Posts: 31
Joined: Thu Jan 10, 2019 12:17 am

Re: Maintaining relation between [H3O+] and [OH-]

Postby Jayasuriya Senthilvelan 4I » Mon Jan 14, 2019 8:46 pm

The reaction or process is 2H2O (l) <---> H3O+ (aq) + OH- (aq)
The Kc value for such a reaction at some temperature is Kc = H3O+ * OH-
Since the Kc is the same for some temperature, for the K value to be constant, H3O and OH vary inversely.

Patrick Cai 1L
Posts: 93
Joined: Fri Sep 28, 2018 12:25 am

Re: Maintaining relation between [H3O+] and [OH-]

Postby Patrick Cai 1L » Mon Jan 14, 2019 8:54 pm

The specific process by which this happens was discussed in class today by Dr. Lavelle, autoprotolysis. Water (H2O) occasionally, and spontaneously, pronates other water molecules, thus forming hydronium (H3O+) and hydroxide (OH-) ions.


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