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For water, is [H3O+] always equal to [OH-]? Because in class Professor Lavelle was saying they're both 1.0x10^-7 which is why Kw is 1.0x10^-14, but the book also mentions the see saw behavior when there's more H3O+, OH- concentration will decrease.
When the concentrations of H30+ and OH- are the same in a given water, they are quite small and equivalent at 10^-7 M each. This leads to a pH of 7, since -log(10^-7) is 7. The reason there exist these concentrations of H30+ and OH- is because due to chance, water may as an amphiprotic compound form brief new covalent bonds in a chemical reaction of autoprotolysis: 2H20 -> H30+ + OH-
the Kw of water remains constant at a given temperature, although the concentrations of hydronium and hydroxide ions can vary. for example, in an acidic solution if [H3O+] is say 1.00 x 10^-2, then using the Kw, we can conclude that the [OH-] is 1.00 x 10^ -12.
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