Inner-sphere mechanisms of oxidation. Stoichiometry and kinetics of the cobalt(III) oxidation of oxalic acid in acid perchlorate solution

1970 ◽  
Vol 9 (12) ◽  
pp. 2735-2739 ◽  
Author(s):  
Geoffrey Davies ◽  
Kay O. Watkins
Keyword(s):  
Oxalic Acid ◽  
Perchlorate Solution ◽  
Inner Sphere ◽  
Kinetics Of

Chromium(II) reduction of the μ-Amido-di-μ-hydroxo-bis[triamminecobalt(III)] complex in aqueous perchlorate solution

1976 ◽  
Vol 29 (4) ◽  
pp. 915
Author(s):  
JD Edwards
Keyword(s):  
Electron Transfer ◽  
Aqua Ligand ◽  
Hydrogen Ion ◽  
Perchlorate Solution ◽  
Inner Sphere ◽  
Kinetics Of

The kinetics of the reduction of [(NH3)3Co,μ(NH2,0H,0H),Co(NH3)3]3+ by chromium(11) ion in aqueous perchlorate solution is reported. The results are interpreted in terms of a rapid pre-equilibrium involving hydrogen-ion catalysed hydroxo bridge cleavage, followed by rate determining inner-sphere reduction. A deprotonated aqua ligand is the bridge for electron transfer.

ChemInform Abstract: STOICHIOMETRY AND KINETICS OF THE COBALT(III) OXIDATION OF L-ASCORBIC ACID IN ACID PERCHLORATE SOLUTION

1977 ◽  
Vol 8 (34) ◽  
pp. no-no
Author(s):  
R. A. RICKMAN ◽  
R. L. SORENSEN ◽  
K. O. WATKINS ◽  
G. DAVIES
Keyword(s):  
Ascorbic Acid ◽  
Perchlorate Solution ◽  
Kinetics Of

The Role of Oxalic Acid in the Ozone Bleaching Kinetics of an Xo-Kraft Pulp

2000 ◽  
Vol 20 (2) ◽  
pp. 147-167 ◽  
Author(s):  
M. Blanca Roncero ◽  
José F. Colom ◽  
Teresa Vidal ◽  
M. [Agrave]ngels Queral
Keyword(s):  
Oxalic Acid ◽  
Kraft Pulp ◽  
Kinetics Of ◽  
Ozone Bleaching

scholarly journals Kinetic Study of the Recovery of Phosphorus from Wastewater by Calcium Hydroxide Solution

2019 ◽  
Vol 25 (6) ◽  
pp. 19-29
Author(s):  
Shams Asem Mahdi ◽  
Raghad Fareed Qasim
Keyword(s):  
Oxalic Acid ◽  
Calcium Hydroxide ◽  
Phosphorus Concentration ◽  
Ambient Conditions ◽  
Residual Phosphorus ◽  
Mixing Speed ◽  
Dissolution Reaction ◽  
Best Value ◽  
Percentage Removal ◽  
Kinetics Of

This research presents a study for precipitating phosphorus (as phosphate ion) from simulated wastewater (5ppm initial concentration of phosphorus) using calcium hydroxide Ca(OH)2 solution. The removal of phosphorus by Ca (OH)2 solution is expected to be very effective since the chemical reaction is of acid-base type but Ca(OH)2 forms complex compound with phosphate ions called. Hydroxyapatite Ca5 (PO4)3OH. hydroxyapatite is slightly soluble in water. This research was directed towards sustainable elements as phosphorus. Kinetics of the dissolution reaction of hydroxyapatite was investigated to find the best factors to recover phosphorus. The effect of concentration of Ca(OH)2 (180- 380 ppm) on phosphorus precipitation on the outputs like the residual phosphorus concentration in the simulated solution, the percentage removal of phosphorus and the weight of the precipitate was also studied. The residual phosphorus decreased with increasing Ca(OH)2 concentration while the percentage removal, as well as the weight of the precipitate, increased with increasing Ca(OH)2 concentration at constant temperature and mixing speed. The best Ca(OH)2 concentration was obtained depending on the lowest amount of the residual phosphorus concentration. The best value obtained was 230 ppm at a fixed mixing speed of 400 rpm and a temperature of 20°C.  The best value for Ca(OH)2 concentration under fixed stirring speed and temperature was applied on a real wastewater taken from the detergent factory. The percentage removal was 30. 69% due to the complexity of the real sample. Oxalic acid was chosen to dissolve hydroxyapatite because it is an organic acid, less hazardous than mineral acids and of less cost. Kinetics of the dissolution reaction of hydroxyapatite in (160 ppm) concentration oxalic acid under ambient conditions (20°C and 1 atm (and mild stirring (200 rpm) was studied using the differential method for determining the order of the reaction which was 0.4296 and the rate constant 0.0743 (L/mg)-0.5704. min-1. The reaction was considered as a rate-controlled reaction.  

scholarly journals Kinetics of non-exchangeable potassium release in selected soil orders of southern Iran

2018 ◽  
Vol 13 (No. 4) ◽  
pp. 200-207
Author(s):  
Zareian Gholamreza ◽  
Farpoor Mohammad Hady ◽  
Hejazi-Mehrizi Majid ◽  
Jafari Azam
Keyword(s):  
Oxalic Acid ◽  
Soil Depth ◽  
Clay Content ◽  
Exchangeable K ◽  
Southern Iran ◽  
Successive Extraction ◽  
Palygorskite Clay ◽  
Kinetics Of ◽  
K Release Rate ◽  
K Release

Non-exchangeable K release can greatly influence soil K fertility. This study was carried out to study the release of non-exchangeable K from 22 surface and subsurface soils of southern Iran using successive extraction with 10 mmol/l of CaCl<sub>2</sub> and oxalic acid in a period of 2−1368 h at 25 ± 1°C. Alfisols, Aridisols, Entisols, Inceptisols, Mollisols, and Histosols were among the studied soil orders. Illite, smectite, chlorite, vermiculite, kaolinite and palygorskite clay minerals were identified. The amount of non-exchangeable K varied from 95 to 506 mg/kg. Results showed that CaCl<sub>2</sub> and oxalic acid released 60 and 55% of non-exchangeable K from soils, respectively. The discontinuity in slope was found when the cumulative amount of released K was plotted versus time, supporting the multi-reactive nature of K exchange sites. The cumulative K release in soils ranged from 87 to 300 mg/kg for CaCl<sub>2</sub> and 78 to 300 mg/kg for oxalic acid which was well described by simplified Elovich and power function equations. The b constant of simplified Elovich as an index of non-exchangeable K release rate was in the range of 10 to 36 mg/kg for CaCl<sub>2</sub> and 11 to 36 mg/kg for oxalic acid. The highest b constant was measured in Inceptisols and Alfisols, while the lowest values were found in Entisols and Histosols. In conclusion, the K release pattern was similar for both extractants and affected by clay content and type, and soil depth.

Study on the kinetics of iron oxide leaching by oxalic acid

2006 ◽  
Vol 80 (2-4) ◽  
pp. 144-152 ◽  
Author(s):  
Suong Oh Lee ◽  
Tam Tran ◽  
Yi Yong Park ◽  
Seong Jun Kim ◽  
Myong Jun Kim
Keyword(s):  
Iron Oxide ◽  
Oxalic Acid ◽  
Kinetics Of
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