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2H2O(l)⇄H3O+(aq)+OH−(aq)ΔH°=+56kJ/molrxnThe endothermic autoionization of pure water is represented by the chemical equation shown above. The pH of pure water is measured to be 7.00 at 25.0°C and 6.02 at 100.0°C. Which of the following statements best explains these observations?AAt the higher temperature water dissociates less, [H3O+]<[OH−], and the water becomes basic.BAt the higher temperature water dissociates less, [H3O+]=[OH−], and the water remains neutral.CAt the higher temperature water dissociates more, [H3O+]>[OH−], and the water becomes acidic.DAt the higher temperature water dissociates more, [H3O+]=[OH−], and the water remains neutral.
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