![]() Here we discuss the problems that invalidate this conclusion, the most important being that it is based on the use of the pure liquid standard state (mole fraction = 1) that is quite different from the standard state for acidities determined in dilute solution (molality = 1). ![]() Organic chemists generally defend the use of these values by citing measurements of the equilibrium constant for the water + methoxide acid–base reaction that suggested that methanol (p K a = 15.54) is a stronger acid than water from this, organic chemists have concluded that p K a of water must be 15.74 rather than 14.00. Here we trace this error back to Brønsted’s early contributions in the 1920s to the Brønsted–Lowry Theory of acids and bases. Since at least the 1960s, organic chemistry textbooks have featured p K a tables for organic acids that include values for H 2O and H 3O + (15.74 and −1.74, respectively) that are thermodynamically and chemically indefensible.
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