COMPLEX MANGANESE PERIODATES

1960 ◽  
Vol 38 (8) ◽  
pp. 1291-1299 ◽  
Author(s):  
M. W. Lister ◽  
Y. Yoshino
Keyword(s):  
Unpaired Electron ◽  
Magnetic Moment ◽  
Absorption Maximum ◽  
Ferrous Ions ◽  
Complex Ions ◽  
Acid Base ◽  
Iodide Ions ◽  
Reaction Proceeds ◽  
Kinetics Of ◽  
Complex Ion

The preparation of complex periodatomanganates, from manganous salts reacting with sodium (or potassium) hypochlorite and periodate, is described. The products were Na7H4Mn(IO6)3.17H2O and K7H4Mn(IO6)3.8H2O. The manganese was shown to be tetravalent from its redox equivalent in its reaction with iodide and with ferrous ions, and from its magnetic moment, which was 3.87 Bohr magnetons, corresponding to three unpaired electron spins. The ion has an absorption maximum at 483 mμ. Rather complicated pH curves were found for this compound in acid-base titrations. The complex ion decomposes slowly to permanganate and iodate; the kinetics of this reaction have been measured, and a possible mechanism has been suggested. The reaction proceeds in several steps by way of simpler complex ions. The same applies to the reaction between iodide ions and the complex ions when the pH is about 9.

The effect of pressure on complex ion equilibria

1956 ◽  
Vol 9 (1) ◽  
pp. 54 ◽  
Author(s):  
AH Ewald ◽  
SD Hamann
Keyword(s):  
Free Energy ◽  
Dissociation Constant ◽  
Atmospheric Pressure ◽  
Qualitative Agreement ◽  
Complex Ions ◽  
Cobaltous Chloride ◽  
Iodide Ions ◽  
Effect Of Pressure ◽  
Iodide Ion ◽  
Complex Ion

The effect of pressure on the formation of complex ions in solutions of cobaltous chloride and in solutions containing iodine and iodide has been shown to be in qualitative agreement with a theory (Buchanan and Hamann 1953) attributing these effects primarily to changes in the free energy of salvation of the ions. The dissociation constant of tri-iodide ions in water at 22 �C has been shown to decrease from 1.6 x 10-3 mol kg-1 at atmospheric pressure to 1.2 x mol kg-1 at 1500 atm. The enthalpy of dissociation of the tri-iodide ion was found to be approximately -5 kcal mol-1 and to be little affected by a pressure of 1500 atm.

Modeling of sorption kinetics of U(VI) micro-quantities nanostructured materials with anatase mesoporous structures

2021 ◽  
Vol 0 (0) ◽  
Author(s):  
Veniamin Zheleznov ◽  
Aleksey Golikov ◽  
Tatiana Sokolnitskaya ◽  
Sergey Ivannikov
Keyword(s):  
Nanostructured Materials ◽  
Sorption Kinetics ◽  
Uranyl Ion ◽  
Competitive Sorption ◽  
Hydroxyl Groups ◽  
Complex Ions ◽  
The Stability ◽  
Kinetics Of ◽  
Mesoporous Structures ◽  
Ionic Forms

Abstract The sorption kinetics of uranyl ions micro-quantities from fluoride solutions by nanostructured materials with anatase mesoporous structures has been studied. Using the model of competitive sorption of ions and positively charged complexes of uranyl ion on deprotonated hydroxyl groups of an anatase, kinetic curves of changes in the ratio of ionic forms of uranium in solution were calculated. Modeling was carried out under the assumption of a two-stage mechanism of uranium complex ions sorption. The modeling considered the influence of the uranyl ion carbonate complexes formation. The shift in equilibrium among ionic forms of uranyl correlates with the stability of the complexes in solution.

The Effect of Solvent on the Acid-Base Kinetics of the Excited State of β-Naphthol1

1965 ◽  
Vol 69 (6) ◽  
pp. 2044-2059 ◽  
Author(s):  
Norman M. Trieff ◽  
Benson R. Sundheim
Keyword(s):  
Excited State ◽  
Acid Base ◽  
Effect Of Solvent ◽  
Kinetics Of

scholarly journals Kinetics of acid-base parameters in conventional hemodialysis

2019 ◽  
Vol 52 (1) ◽  
Author(s):  
J.R. Lugon ◽  
G.R.M. Pereira ◽  
J.P. Strogoff-de-Matos ◽  
A.J. Peixoto
Keyword(s):  
Acid Base ◽  
Base Parameters ◽  
Kinetics Of ◽  
Conventional Hemodialysis

Solubility and Complex-Ion Equilibria

2021 ◽  
pp. 313-324
Author(s):  
Christopher O. Oriakhi
Keyword(s):  
Metal Complexes ◽  
Solubility Product ◽  
Formation Constants ◽  
Aqueous Systems ◽  
Complex Ions ◽  
Ionic Compounds ◽  
Molar Solubility ◽  
Solubility Product Constant ◽  
Complex Ion

Solubility and Complex-Ion Equilibria broadens the previous chapter’s coverage of equilibria to include aqueous systems containing two or more solutes of slightly soluble ionic compounds and the formation of metal complexes in solution. Solubility equilibria which allow quantitative predictions of how much of a compound will dissolve under given conditions are covered. The meaning of the solubility product constant (K sp) and how to calculate it from molar solubility values is presented. Also discussed is determination of molar solubility from K sp. Calculations demonstrate how to predict the formation of a precipitate by comparing the ion product or solubility quotient (Q) with K sp. Formation constants of complex ions and calculations involving complex ion equilibria are explained.

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