The Influence of Salts on the Absorption Spectra of Aqueous Cobalt Chloride Solutions
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Abstract:
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.Keywords:
Molality
Particle (ecology)
Aqueous two-phase system
Qualitative inorganic analysis
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Journal of the Chemical Society Faraday Transactions 1 Physical Chemistry in Condensed Phases (1980)
13 C resonances of carbonyl and methyl groups in amides are shifted down-field on interaction with alkali and alkaline earth metal salts. The magnitude of the shift depends on the ionic potential of the cation. Ions like Li+ bind to the amide carbonyl group both in neat amide solutions as well as in concentrated salt solutions in water.
Amide
Alkaline earth metal
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Carbon fibers
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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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Abstract : Studies on ionic liquids composed of aluminum chloride and 1-ethyl-3-methylimidazolium chloride were carried out, with emphasis on understanding and explaining and in buffered melts. It was found that alkaline earth, as well as alkali metal salts, function as agents, with both showing the latent acidity effect. Both Bronsted and Lewis acidities were investigated in an effort to understand the role of the type and concentration of the buffering alkali or alkaline earth salt. A silver/silver chloride/chloride ion electrode was found to function as a reversible chloride ion indicator over a very narrow range of melt about the neutral point. This electrode, and relative solubility product measurements, were employed in these studies. It was found that the could be explained in terms of the solubility product relationship of the salt, with the salt having the smallest solubility product creating the most acidic melt. Some work was also carried out on non-haloaluminate melts.
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K-absorption edge-shifts of cobalt in CoCl 2 ·6H 2 O, CoSO 4 ·7H 2 O, Co(NO 3 ) 2 ·6H 2 O, Co(en) 3 Cl 3 , Co(en) 3 (SO 4 ) 3 and Co(en) 3 (NO 3 ) 3 in aqueous solutions as well as in polycrystalline form were measured using X-ray absorption spectroscopic technique. Effective charges on cobalt ions are estimated using Gianturco and Coulson method. Comparison of the general features of the absorption spectra in aqueous solution with those observed for the same ion in solid form reveals interesting results. An attempt is made to interpret the results in the light of the available chemical and physical data on these samples.
Absorption edge
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ADVERTISEMENT RETURN TO ISSUEPREVArticleNEXTThe Apparent Molal Volumes of the Alkali Metal Chlorides in Aqueous Solution and Evidence for Salt-Induced Structure TransitionsFred VaslowCite this: J. Phys. Chem. 1966, 70, 7, 2286–2294Publication Date (Print):July 1, 1966Publication History Published online1 May 2002Published inissue 1 July 1966https://pubs.acs.org/doi/10.1021/j100879a034https://doi.org/10.1021/j100879a034research-articleACS PublicationsRequest reuse permissionsArticle Views300Altmetric-Citations106LEARN 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 options Get e-Alerts
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The D/H ratio of hydrogen gas in equilibrium with aqueous alkaline earth (Mg, Ca, Sr or Ba) chloride solutions measured at 25 ◦ C using a hydrophobic platinum catalyst, was found to be higher than the D/H ratio equilibrated with the applied pure water. The hydrogen isotope effect between such solutions and pure water changes with the molality of the solutions. The order of the D/H ratios in alkaline earth chlorides is found to be BaCl 2 > SrCl 2 ≥ CaCl 2 ≥ MgCl 2 . The hydrogen isotope effect in the aqueous chloride solutions of Mg, Ca, Sr or Ba ions is significantly larger than that in the aqueous chloride solutions of Li, Na, K or Cs ions. For MgCl 2 and CaCl 2 solutions, the hydrogen isotope effect is opposite to the oxygen isotope effect. The results are compared with the free energy change of transfer from H 2 O to D 2 O, and are discussed for the vapour pressure ratio of H 2 O and D 2 O of CaCl 2 solutions.
Molality
Alkaline earth metal
Kinetic isotope effect
Hydrogen chloride
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The electrode potentials of the system Th, ThCl 4 (KCl, NaCl) were measured at various concentrations of thorium chloride, and at temperatures between 670 °C and 850 °C, using a silver – silver chloride reference electrode. It was shown by a direct gravimetric method that the reaction,Th (metal) + ThCl 4(melt) = 2ThCl 2(in melt) ,postulated by previous investigators, did not take place.The activity coefficients, and the other partial molal properties of the solutions of ThCl 4 , in the equimolar mixture of potassium and sodium chlorides, were calculated as a function of temperature from the e.m.f. measurements.
Molality
Gravimetric analysis
Polarography
Standard electrode potential
Glass electrode
Tetrachloride
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