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Combining free energy equilibrium and water auto-ionization. In our treatment of acid-base equilibria we have used the value of the autoionization constant of water Kw = 1.0 x 10^-14, which is appropriate at 25°C. However, this value varies with temperature and is different for deuterated of “heavy water” D2O. In this problem, you will use thermodynamics to explore these differences. Thermochemical Information at 298 K. Using the above data, determine the pH of pure water at the boiling point 100°C, and compare your value to the pH of pure water at 25C. How does this change relate to Le Chatelier’s Principle? I don't understand what is circled in red. I didn't know there was a direct relationship between Kw and e??