Salt Effects in the Reactions Between Iodate and Iodide

Indelli, Antonio

doi:10.1021/j100820a011

Cited by 9 publications

(12 citation statements)

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“…The effect of 12 different salts has been investigated by Indelli. 11 For the univalent and divalent anions and cations, the study showed a low effect with a closer conformity to the Bronsted−Debye equation. A larger decrease in rate was also reported when adding sulfate ions and explained by the possible formation of HSO 4…”

Section: Introduction and Bibliographic Reviewsupporting

confidence: 62%

“…Not only is this consideration inconsistent with the value of the second acidity constant (pK a2 = 1.99) but this effect is also increasing with the amount of sulfate salt added, as was observed and underlined by many investigators. 11,32,33 2.1. Partial Ionization of Sulfuric Acid.…”

Section: Kinetic Investigation With the Use Ofmentioning

confidence: 99%

“…However, these results must be taken with certain precautions because acetate and phosphate buffers and HCl were used: for these ions, we actually know that acetate and phosphate ions can catalyze the reaction and that Cl – may enhance iodate reduction reaction. , On the contrary, most of the works observed that an increase in μ led to a decrease in rate. The effect of 12 different salts has been investigated by Indelli . For the univalent and divalent anions and cations, the study showed a low effect with a closer conformity to the Brönsted–Debye equation.…”

Section: Introduction and Bibliographic Reviewmentioning

confidence: 98%

“…The iodide dependence was the subject of a long controversy, but most of the studies provided experimental evidence that the rate order only depends on the iodide concentration range. The order is 1 at a small iodide concentration − ,,,, (i.e., less than 5 × 10 –7 M), while it becomes 2 at concentrations between 5 × 10 –6 M and 10 –3 M. ,,− ,− ,,, At a much higher concentration, it may be less than 2. All of these results are consistent with the fully accepted mechanism, which highlights the importance of the intermediate species I 2 O 2 or its equivalent hydrated form H 2 I 2 O 3 , as written by the following mechanism With The first step, which involves the dissociation equilibrium of iodic acid {eq }, has been early proposed , with the suggestion that the electron-deficient iodyl cation IO 2 + is an intermediate species.…”

Section: Introduction and Bibliographic Reviewmentioning

confidence: 98%

“…The iodide dependence was the subject of a long controversy, but most of the studies provided experimental evidence that the rate order only depends on the iodide concentration range. The order is 1 at a small iodide concentration [6][7][8][9]24,27,29,31 (i.e., less than 5 × 10 −7 M), while it becomes 2 at concentrations between 5 × 10 −6 M and 10 −3 M. 5,6,[10][11][12][13][14][15][16][17][22][23][24]27,28,31 At a much higher concentration, 29 it may be less than 2. All of these results are consistent with the fully accepted mechanism, which highlights the importance of the intermediate species I 2 O 2 or its equivalent hydrated form H 2 I 2 O 3 , as written by the following mechanism 31 (r3) (r4) (r5)…”

Section: Introduction and Bibliographic Reviewmentioning

confidence: 99%

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Villermaux–Dushman Test of Micromixing Characterization Revisited: Kinetic Effects of Acid Choice and Ionic Strength

Guichardon

Baqueiro

Ibaseta

2021

Ind. Eng. Chem. Res.

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The well-known Villermaux−Dushman system is nowadays widely used for examining the micromixing efficiency either in batch or continuous intensified reactors. However, a bibliographic review shows that kinetic data are too scattered for a reliable determination of the micromixing times. The Dushman reaction kinetics is then reexamined with the use of sulfuric and perchloric acids. The results confirm the fifth-order rate law. More precisely, the I − , H + , and IO 3 − dependence orders on the rate law are, respectively, 2, 2, and 1, under any condition. To be more consistent with the reactant concentrations used in the Villermaux− Dushman test, we extend their studied range, namely, 1.

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Section: Introduction and Bibliographic Reviewsupporting

confidence: 62%

Section: Kinetic Investigation With the Use Ofmentioning

confidence: 99%

Section: Introduction and Bibliographic Reviewmentioning

confidence: 98%

Section: Introduction and Bibliographic Reviewmentioning

confidence: 98%

“…The iodide dependence was the subject of a long controversy, but most of the studies provided experimental evidence that the rate order only depends on the iodide concentration range. The order is 1 at a small iodide concentration [6][7][8][9]24,27,29,31 (i.e., less than 5 × 10 −7 M), while it becomes 2 at concentrations between 5 × 10 −6 M and 10 −3 M. 5,6,[10][11][12][13][14][15][16][17][22][23][24]27,28,31 At a much higher concentration, 29 it may be less than 2. All of these results are consistent with the fully accepted mechanism, which highlights the importance of the intermediate species I 2 O 2 or its equivalent hydrated form H 2 I 2 O 3 , as written by the following mechanism 31 (r3) (r4) (r5)…”

Section: Introduction and Bibliographic Reviewmentioning

confidence: 99%

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