Constantes de stabilité de thiocomplexes et produits de solubilité de sulfures de métaux. II Sulfure de zinc

1967 ◽  
Vol 45 (18) ◽  
pp. 2101-2108 ◽  
Author(s):  
A. O. Gubeli ◽  
J. Ste-Marie
Keyword(s):  
Ionic Strength ◽  
Zinc Sulfide ◽  
Formation Constant ◽  
Solubility Product ◽  
Acidic Solution ◽  
Theoretical Method ◽  
Formation Constants ◽  
Mathematical Treatment ◽  
Ph Scale

A mathematical treatment of solubility curves of sulfides is introduced for the determination of formation constants of complexes in solution. As an example, this theoretical method is used in the determination of the species in equilibrium in solution with a precipitate of zinc sulfide (β-ZnS). The excess of sulfide in solution varies from 0.0004 M to 0.01 M. The presence of Zn2+ is noted in acidic solution, followed by the presence of ZnS.H2O or Zn(HS)(OH) for the rest of the pH scale. The solubility product of ZnS and the formation constant of Zn(HS)(OH) are given for an ionic strength 1.0 (NaClO4) at 25 °C.

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.

Constantes de stabilité de cyano-complexes d'argent et produit de solubilité de AgCN

1972 ◽  
Vol 50 (8) ◽  
pp. 1144-1148 ◽  
Author(s):  
A. O. Gübeli ◽  
P. A. Côté
Keyword(s):  
Solubility Product ◽  
Formation Constants ◽  
Slope Method ◽  
Cyano Complexes

The slope method has been applied to the determination of the cumulative formation constants of [Formula: see text] and Ag(OH)CN− and to the measure of the solubility product of AgCN, in 1 M NaClO4, at 25 °C.

scholarly journals Titrimetrische Analyse von Ionenaustauschgleichgewichten bei Unvollständigkeit der Titrationskurven / Titrimetric Analysis of Ion-Exchange Equilibria in the Case of Incomplete Titration Curves

1993 ◽  
Vol 48 (4) ◽  
pp. 471-477 ◽  
Author(s):  
Uwe Hilgers ◽  
Rüdiger Blume
Keyword(s):  
Ion Exchange ◽  
Titration Curve ◽  
Formation Constant ◽  
Formation Constants ◽  
Ion Exchangers ◽  
Eriochrome Black T ◽  
Titration Curves ◽  
Titrimetric Determination

A method is described which allows the titrimetric determination of the pH of decomplexation and of the formation constant of chelating ion-exchangers, although the titration curve is not complete. Iterative linearization leads to the formation constants and allows the completion of the titration curves. The studied systems are of the type MeL and MeL2, where the metals Me are zinc, copper and manganese, and the ligand L is Eriochrome Black T. The method may also be used for the determination of the number of ligands in a complex of the type MeLn.

scholarly journals Study of Complex Formation Between Iodoquinol (IQ) and Co2+, Mn2+, Cd2+, Pb2+and Zn2+Cations in Binary Aqueous / Non-aqueous Solvent Using Spectrophotometry

2007 ◽  
Vol 4 (4) ◽  
pp. 581-586 ◽  
Author(s):  
A. Nezhadali ◽  
H. A. Hosseini ◽  
P. Langara
Keyword(s):  
Ionic Strength ◽  
Complex Formation ◽  
Stability Constants ◽  
Spectrophotometric Method ◽  
Formation Constants ◽  
The Other ◽  
Aqueous Solvent ◽  
The Stability ◽  
Complexation Reactions

The complexation reactions between iodoquinol and Co2+, Mn2+, Cd2+, Pb2+and Zn2+cations were studied in different DMF/H2O binary mixtures at the ionic strength of 0.1(using NaNO3).The spectrophotometric method was used for the determination of formation constants and the stoichiometries. The stoichiometry of the complexes is established 1:1 by Job's and mole ratio methods. It was found that the stability constants of the complex formed between the ligand (IQ) and the cations in the all cases increase with increasing of the non-aqueous solvent. In the most cases the maximum formation constants between Zn2+ion and IQ were obtained respect to the other cations.

scholarly journals The Behavior of Americium in Aqueous Carbonate Systems

1983 ◽  
Vol 26 ◽  
Author(s):  
R. J. Silva
Keyword(s):  
Experimental Data ◽  
Solubility Product ◽  
Computer Code ◽  
Formation Constants ◽  
Solid Materials ◽  
X Ray ◽  
Solid Phases ◽  
Diffraction Patterns ◽  
Carbonate Complexes

ABSTRACTThe solubilities of crystalline Am(OH)3 and AmOHCO3 were measured at 25° C in aqueous solutions of 0.1 M NaCl04 by determination of the solution concentrations of Am. Prior to use in the measurements, the solid materials were characterized by their x-ray powder diffraction patterns. The solubility product quotients were calculated from the experimental data. The hydrolysis quotients of Am3+ were also estimated from the hydroxide solubility data. Using the thermodynamic data derived from these experiments and the recently reported formation constants for the Am3+ carbonate complexes, the solid phases and concentrations of solution species of americium in several aqueous carbonate systems were calculated using the computer code MINEQL.

scholarly journals The solubility of Ca(OH)2 in extremely concentrated NaOH solutions at 25°C

2012 ◽  
Vol 10 (2) ◽  
pp. 332-337 ◽  
Author(s):  
Attila Pallagi ◽  
Ágost Tasi ◽  
Attila Gácsi ◽  
Miklós Csáti ◽  
István Pálinkó ◽  
...  
Keyword(s):  
Ionic Strength ◽  
Stability Constant ◽  
Solubility Product ◽  
Hydroxo Complex ◽  
Solubility Data ◽  
Alkaline Solutions ◽  
Conditional Stability ◽  
Experimental Protocol ◽  
Conditional Stability Constant

AbstractThe solubility of Ca(OH)2 in aqueous NaOH solutions up to 12.50 M at 25°C has been determined. The solubility data obtained for NaOH concentrations lower than 3 M was compared with those published in the literature. The solubility of Ca(OH)2 steadily decreases with the increasing NaOH concentration. The solubility data obtained at a constant ionic strength (I = 1 M Na(Cl,OH)) enabled the determination of the conditional solubility product of Ca(OH)2(s) (lgLCa(OH)2 = − 4.10 ± 0.02). Formation of the hydroxo complex CaOH+(aq) was invoked to describe the variation of [Ca2+]T with [OH−]T. Its conditional stability constant was found to be lgKCaOH+ = 0.97 ± 0.02. The experimental protocol employed was proven to be suitable for accurate solubility determinations in rapidly equilibrating systems comprising of highly concentrated, alkaline solutions and containing analytes in the ppm range.

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