Abstract:
The kinetics of the reaction between vitamin C, L-ascorbic acid, and hexacyanoferrare (III),
Fe(CN)63', in aqueous acidic media at different temperatures has been studied by following
the absorbance with time at 420 nm. The mechanism of the oxidation of L-ascorbic acid
had been proposed to be multi-step and the rate determining step was between ascobate
anion, which would be produced in the initial reversible step, and hexacyanoferrare
(III). This reaction has been well established to be first order with respect to L-ascorbic
acid and Fe(CN)63\ The overall second order rate constant, kobs, was observed to show
an inverse dependence on [H+] for the range of pH studied at temperatures from 293 to
313 K. In this study k2, the rate constant for the rate-determining step, was determined
by its relationship to kobs, the experimentally measured overall rate constant, at various
temperatures and different concentrations of NaN0 3. The experimental value for k2 was
found to vary from 52.6 to 202 dm3 mol'1 min'1 when NaN0 3 concentration was changed
from zero to 0.200 mol dm'3 at 302 K. The effect of ionic strength on the kinetics of this
reaction was investigated by substituting NaN0 3 with KN0 3, K2S04, NaCl, KC1, Na2S0 4,
MgCl, MgSC) , Mg(NO ) , AlfSO.), and Al(NO ) . It was deduced by the primary kinetic
salt effect, that the rate determining step involved species of like charges. Thermodynamic
parameters of activation at different ionic strengths were calculated by using the Eyring
equation.
