Free Access
J. Chim. Phys.
Volume 96, Number 4, April 1999
Page(s) 610 - 633
DOI: 10.1051/jcp:1999161

J. Chim. Phys. Vol. 96, N°4  p. 610-633

Kinetic study of HMSA formation and decomposition: Tropospheric relevance

J. Lagrange, G. Wenger and P. Lagrange

UMR 7512 du CNRS, Laboratoire de Cinétique et Analyse, ECPM, Université de Strasbourg, 1 rue Blaise Pascal, 67000 Strasbourg, France

The rate law of HMSA (hydroxymethanesulphonic acid) formation is: rate = $\frac{3.5+1.05\times10^6[\rm H^+]}{1.2.19\times10^6[\rm H^+]}$ [ CH 2O] $_{\rm T}$ [ SO 2, aq] $_{\rm T}$ (NaClO 4 1 M, 25  $^{\circ}$C). The formation can occur by two parallel nucleophilic additions of HSO 3- or SO 32- to the formadehyde. In presence of H 2O 2, a slow oxidation process is observed: rate = $1.8\times10^{-10}$ [HMSA] [ H +] -1 (1 M NaClO 4, 25  $^{\circ}$C). Some atmospheric simulations are presented taking into account the salt effects in NaCl and Na 2SO 4.

La formation de HMSA (acide hydroxyméthanesulphonique) suit la loi de vitesse : vitesse = $\frac{3.5+1.05\times10^6[\rm H^+]}{1.2.19\times10^6[\rm H^+]}$ [ CH 2O] $_{\rm T}$ [ SO 2, aq] (NaClO 4 1 M, 25  $^{\circ}$C). Cette formation correspond à deux additions nucléophiles parallèles, soit de HSO 3-, soit de SO 32- au formaldéhyde. Une oxydation lente est observée en présence de H 2O 2 : vitesse = $1.8\times10^{-10}$ [HMSA] [ H +] -1 (1 M NaClO 4 1 M, 25  $^{\circ}$C). Quelques simulations atmosphériques sont présentées en milieu NaCl et Na 2SO 4.

Key words: Atmosphere -- HMSA -- formaldehyde -- acid rains

© EDP Sciences 1999

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