Dissociation Constants of Thiomalic Acid in Aqueous Potassium Chloride Solutions.
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Keywords:
Acid dissociation constant
Dissociation constant
Hydrogen chloride
Hydrochloric acid
Solvation shell
Coordination sphere
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Hydrometallurgy
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The effects of equal concentrations of the alkali and alkaline earth chlorides and of hydrogen chloride on the absorption spectra of aqueous cobalt chloride solutions have been studied. Solutions prepared both on the molar and on the molal bases were used. In all cases, the absorption bands widen with an increase in concentration of the added salt. The increase in width of the absorption bands varies directly as the ionic charge and inversely as the ionic volume of the added cation. The inadequacy of existing explanations of the well-known color changes in cobalt chloride solutions is discussed and a new explanation is offered.
Molality
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A series of concentrated aqueous solutions of ferric chloride with different chloride:iron(III) ratios has been studied by means of EXAFS to determine the structure around the iron(III) ion of the dominating species in such solutions. The dominating species in dilute acidic aqueous solution of ferric chloride, at less than 1 mmol·dm−3, are the hydrated iron(III) and chloride ions, while in concentrated aqueous solution and in solutions with an excess of chloride ions, up to 1.0 mol·dm−3, it is the trans-[FeCl2(H2O)4]+ complex. Possible higher chloroferrate(III) or dimeric [Fe2Cl6] complexes at room temperature, as proposed in the literature, were not observed in any of the studied solutions in spite of an excess of chloride ions of 1 mol·dm−3.
Iron(III) chloride
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In part 1 of this study, I reported that the Debye-Hückel limiting law and the smaller-ion shell (SiS) model of strong electrolyte solutions fit nicely with the experimental mean ionic activity coefficient (γ(±)) of aqueous sulfuric acid as a function of concentration and of temperature when the acid is assumed to be a strong 1-3 electrolyte. Here, I report that the SiS-derived activity coefficient of H(+), γ(H(+)), of the 1-3 acid is comparable to that of aqueous HCl. This agrees with titration curves showing, as well-known, that sulfuric acid in water is parallel in strength to aqueous HCl. The calculated pH is in good accord with the Hammett acidity function, H(0), of aqueous sulfuric acid at low concentration, and differences between the two functions at high concentration are discussed and explained. This pH-H(0) relation is consistent with the literature showing that the H(0) of sulfuric acid (in the 1-9 M range) is similar to those of HCl and the other strong mineral monoprotic acids. The titration of aqueous sulfuric acid with NaOH does not agree with the known second dissociation constant of 0.010 23; rather, the constant is found to be ~0.32 and the acid behaves upon neutralization as a strong diprotic acid practically dissociating in one step. A plausible reaction pathway is offered to explain how the acid may transform, upon base neutralization, from a dissociated H(4)SO(5) (as 3H(+) and HSO(5)(3-)) to a dissociated H(2)SO(4) even though the equilibrium constant of the reaction H(+) + HSO(5)(3-) ↔ SO(4)(2-) + H(2)O, at 25 °C, is 10(-37) (part 1).
Acid dissociation constant
Dissociation constant
Acidity function
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ADVERTISEMENT RETURN TO ISSUEPREVArticleNEXTThe Activity Ratio of Zwitterions and Uncharged Molecules in Ampholyte Solutions. The Dissociation Constants of Amino Acid EstersJohn T. Edsall and Muriel H. BlanchardCite this: J. Am. Chem. Soc. 1933, 55, 6, 2337–2353Publication Date (Print):June 1, 1933Publication History Published online1 May 2002Published inissue 1 June 1933https://pubs.acs.org/doi/10.1021/ja01333a019https://doi.org/10.1021/ja01333a019research-articleACS PublicationsRequest reuse permissionsArticle Views666Altmetric-Citations110LEARN ABOUT THESE METRICSArticle Views are the COUNTER-compliant sum of full text article downloads since November 2008 (both PDF and HTML) across all institutions and individuals. These metrics are regularly updated to reflect usage leading up to the last few days.Citations are the number of other articles citing this article, calculated by Crossref and updated daily. Find more information about Crossref citation counts.The Altmetric Attention Score is a quantitative measure of the attention that a research article has received online. Clicking on the donut icon will load a page at altmetric.com with additional details about the score and the social media presence for the given article. Find more information on the Altmetric Attention Score and how the score is calculated. Share Add toView InAdd Full Text with ReferenceAdd Description ExportRISCitationCitation and abstractCitation and referencesMore Options Share onFacebookTwitterWechatLinked InRedditEmail Other access optionsGet e-Alertsclose Get e-Alerts
Dissociation constant
Acid dissociation constant
Zwitterion
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The mobility of cation vacancies and the equilibrium concentration of cation and anion vacancies in solid potassium chloride are calculated from measurements of the electrical conductivity of pure potassium chloride and solid solutions of strontium chloride in potassium chloride.
Strontium chloride
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Dissociation constant
Acid dissociation constant
Aqueous medium
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It is shown that the growth behavior of potassium chloride crystals from aqueous solution is consistent with the Frank growth mechanism. The growth behavior is altered by the presence of a few parts per million of lead chloride. It is imputed that the rate of growth at unit steps is inhibited and that the rate of two-dimensional nucleation is markedly increased by the presence of lead chloride. The effects are consistent with complete line adsorption of a complex lead containing ion at growth steps.
Lead chloride
Potassium sulfate
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