The mechanism of the nonenzymatic iodination of tyrosine by molecular iodine

Over the pH range 7–10, at very low buffer concentration, the nonenzymatic iodination of tyrosine obeys the rate law[Formula: see text]where k app is the measured second order rate constant based upon the total initial concentrations of molecular iodine and tyrosine and K 2 (units M) is the equilibrium constant for [Formula: see text]. The value of k′ is 3.5 × 10 −8 M∙s −1 . There are three plausible mechanisms that fit the experimental data. One, the simplest, is a concerted process in which hypoiodous acid attacks tyrosine with its phenolic group unionized. The other two involve the formation of an iodinated quinoid reactive intermediate species in a rapid pre-equilibrium between unionized tyrosine and either hypoiodous acid or molecular iodine. The pre-equilibrium, if it occurs, favors the initial reactants. It is followed by a slow step in which the quinoid is converted to mono-iodinated tyrosine. Positive deviations from the rate law for pH dependence indicate that some specific acid catalysis (H 3 O + ) is occurring in the pH range 5–7. In the presence of sufficient buffer, general acid–base catalysis is observed with acetic acid acting as a general acid catalyst in the vicinity of pH 5 and carbonate acting as a general base at pH ~ 9.5. The nonenzymatic iodination of tyrosine occurs more rapidly as the pH is increased, in marked contrast to the peroxidase-catalyzed iodination, which has its optimum at low pH.