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The autoprotolysis of water can be used to link the concentrations of H3O+ and OH- in an aqueous solution via the autoprotolysis constant, Kw. Because Kw is essentially an equilibrium constant, if [H3O+] increases due to acid being added into a solution, [OH-] must decrease in order to keep Kw the same, and vice versa, producing the equation: [H3O+][OH-] = Kw = 10^-14. (You can exclude H2O from the constant because it is basically a pure liquid, and its concentration does not change in any measurable way.
In a similar fashion, Kw links pOH and pH in an aqueous solution in the equation pH + pOH = 14 (which you can find by taking the negative log of the previous equation).
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