The results of comprehensive equilibrium and kinetic studies of the iron(III)-sulfate system in aqueous solutions at I = 1.0 M (NaClO4), in the concentration ranges of TFeIII = 0.15-0.3 mM, T SO42- = 3-30 mM, and at pH 0.7-2.5 are presented. The iron(III)-containing species detected are FeOH2+ (=FeH-1), (FeOH)24+ (=Fe2H-2), FeSO 4+, and Fe(SO4)2- with formation constants of log βFeH-1 = -2.84, log βFe2H-2 = -2.88, log βFeSO4+ = 2.32, and log βFe(sO4)2- = 3.83. The formation rate constants of the stepwise formation of the sulfate complexes are k1a = 4.4 × 10 3 M-1 s-1 for the Fe3+ + SO 42- ⇌k1a FeSO4+ step and k2 = 1.1 × 103 M-1 s -1 for the FeSO4+ + SO42- ⇌k2 Fe(SO4)2- step. The mono-sulfate complex is also formed in the Fe(OH)2+ + SO 42- →k1b FeSO4+ reaction with the k1b = 2.7 × 105 M-1 s-1 rate constant. The most surprising result is, however, that the 2 FeSO4+ ⇌ Fe3+ + Fe(SO4) 2- equilibrium is established well before the system as a whole reaches its equilibrium state, and the main path of the formation of Fe(SO4)2- is the above fast (on the stopped flow scale) equilibrium process. The use and advantages of our recently elaborated programs for the evaluation of equilibrium and kinetic experiments are briefly outlined.
ASJC Scopus subject areas
- Physical and Theoretical Chemistry
- Organic Chemistry
- Inorganic Chemistry