15454-31-6Relevant articles and documents
Kinetics of the Oxidation of chromium(III) by Periodate
Abdel-Khalek, Ahmed A.,Elsemongy, Mahmoud M.
, p. 4407 - 4410 (1988)
The kinetics of oxidation of III(H2O)(TOH)>, (TOH=N-(2-hydroxyethyl)ethylenediamine-N,N',N'-triacetate) by periodate in aqueous solutions has been found to obey the following equation: where k2 is the rate constant for
Disproportionation Kinetics of Hypoiodous Acid As Catalyzed and Suppressed by Acetic Acid-Acetate Buffer
Urbansky, Edward T.,Cooper, Brian T.,Margerum, Dale W.
, p. 1338 - 1344 (1997)
The kinetics of the disproportionation of hypoiodous acid to give iodine and iodate ion (5HOI ? 2I2 + IO3- + H+ + 2H2O) are investigated in aqueous acetic acid-sodium acetate buffer. The rate of iodine formation is followed photometrically at -log [H+] = 3.50, 4.00, 4.50, and 5.00, μ = 0.50 M (NaClO4), and 25.0°C. Both catalytic and inhibitory buffer effects are observed. The first process is proposed to be a disproportionation of iodine(I) to give HOIO and I-; the iodide then reacts with HOI to give I2. The reactive species (acetato-O)iodine(I), CH3CO2I, is postulated to increase the rate by assisting in the formation of I2O, a steady-state species that hydrolyzes to give HOIO and I2. Inhibition is postulated to result from the formation of the stable ion bis(acetato-O)iodate-(I), (CH3CO2)2I-, as buffer concentration is increased. This species is observed spectrophotometrically with a UV absorption shoulder (λ = 266 nm; ∈ = 530 M-1 cm-1). The second process is proposed to be a disproportionation of HOIO to give IO3- and I2. Above 1 M total buffer, the reaction becomes reversible with less than 90% I2 formation. Rate and equilibrium constants are resolved and reported for the proposed mechanism.
Oxidation of hexaaquoiron(II) by periodate in aqueous acidic solution
El-Eziri,Sulfab, Yousif
, p. 15 - 20 (1977)
The oxidation of Fe(II) by periodate in aqueous acidic solutions obeys the rate law (i) {A figure is presented} where [L6]T represents the total periodate concentration. The magnitudes of k0, k′1, k″2 and k3 are 0.235 sec-1, 120 sec-1, 7.5 ± 1.5 sec]-1, and (7.3 ± 0.5) X 104M-2 sec-1 respectively at 25 °C and I = 1.0 M. The terms in equation (i), that are first order in [L-]T, correspond to the oxidation process with possibly one-electron (term showing first order in [Fe(11)] and two electron-transfer (term showing second order in [Fe(II)]. At low [H+] (0.10 M), the pathway first order in [Fe(II)] predominates, whereas at high [H+] (0.80 M), the term second order in [Fe(II)] prevails. An explanation of the term independent of [L-]T is not quite obvious.
Kinetics and Mechanism of the Chlorite-Periodate System: Formation of a Short-Lived Key Intermediate OClOIO3 and Its Subsequent Reactions
Baranyi, Nóra,Cseko, Gy?rgy,Valkai, László,Xu, Li,Horváth, Attila K.
, p. 2436 - 2440 (2016/03/19)
The chlorite-periodate reaction has been studied spectrophotometrically in acidic medium at 25.0 ± 0.1 °C, monitoring the absorbance at 400 nm in acetate/acetic acid buffer at constant ionic strength (I = 0.5 M). We have shown that periodate was exclusive
Photoinduced reaction between chlorine dioxide and iodine in acidic aqueous solution
Rabat, Gyula,Kovacs, Klara M.
, p. 6167 - 6170 (2007/10/03)
Photoinduced reaction between ClO2 and I2 has been discovered under illumination with 460 nm lightband. The photochemical reaction has a variable stoichiometry in acidic aqueous solution because the induced disproportionation of ClO2 to ClO3- and Cl- competes with the oxidation of I2 to IO3- by ClO2 in the illuminated reaction mixture. The reaction rate depends on the light power of illumination and on the concentration of I2, but it is independent of the concentration of ClO2. It is also independent of the pH in the range of 0-2.0 and of the ionic strength in the range of 0.01-1.0 M. Reversible dissociation of I2 has been identified as the primary photochemical process and rate-determining step in the mechanism. Reactive I atoms are considered to initiate fast reaction steps, leading to the formation of products through reactive intermediates such as IClO2, ClO, IO, and HOCl. This mechanism is proposed for explaining the photoresponses of the CDIMA oscillatory reaction system to the illumination with visible light.