The reactions of hydroxymethylated 2-methoxy-4, 6-diamino-s-triazine (MMT) molecules in an acidic aqueous solution were studied kinetically. The average molar number of formaldehyde (F) combined (n) in the samples used were 1.43 (Sample I) and 1.56 (Sample II). The reactions involved are both dissociation of methylol groups and condensation (methylene bond formation) reaction of methylol with amino groups. The reaction rates were measured by employing both iodometric and sulfite methods in pH's varying from 3.56 to 2.75 at 25°C.
The rate of the dissociation reaction v
d and that of the condensation v
c are expressed as follows,
v
d=k
d (na-x-y)
v
c=k
c (na-x-y) (ma-x+y)
where, k
d is the rate constant of the dissociation, a the initial concentration of MMT, na the initial concentration of methylol groups, x the concentration of methylene bonded F, y the concentration of liberated F and amino groups (mol/l, respectively), k
c the rate constant of the condensation reaction, m the average molar number of amino groups and ma the initial concentration of amino groups (mol/l).
Until over ca. 15% of the initial methylol groups condensed, k
d and k
c were nearly constant. The maximum value of k
c (max) was obtained at[H
3O
+]=[H
2O]/K
1 (K
1: the equlibrium constant of the reaction between MMT and acid), and k
d increased with decreasing pH. Then, the rate constant (k) or condensation reaction, for which y was neglected, was examined. In the range of reaction where k was nearly constant, the difference between k
c and k was comparatively small. Consequently, the rate constant of condensation reaction between MMT molecules having n below 1.56 might be represented approximately by k in the initial stage of the reaction.
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