Sea Salt Solution Research Articles

Ion pair formation model for sea salt solutions

Ion pair formation model for sea salt solutions

Thermodynamic properties of sea salt solutions

AbstractBased on new experimental data presented for the boiling point elevation of natural sea water solutions, smoothed tabular values are presented for boiling point elevation (BPE), osmotic coefficient, water activity, osmotic pressure, and minimum separation energy to 200°C and 12% sea salt.The concentration of sodium chloride solutions having the same water activities as sea salt solutions is also presented.Rigorous thermodynamics and the equations for strong electrolytes by Bromley (1973) were used for the correlation together with previously obtained heat capacity and enthalpy data and equations. A simplified equation is presented for boiling point elevation.

Heat capacities and enthalpies of sea salt solutions to 200.deg.

Heat capacities and enthalpies of sea salt solutions to 200.deg.

The solubility of calcium sulphate in sodium chloride and sea salt solutions

The results of experiments on the solubility of calcium sulphate in sodium chloride solutions and in simulated sea water solutions at temperatures of up to lOO°C are given. They are compared with those of similar experiments by other workers and found to be in satisfactory agreement. A tabulation of the best molal solubility products of CaSO 4 anhydrite in sea salt solutions for the temperature range from 50° to 200°C is given in the appendix.

Thermodynamic properties of sea salt solutions

Thermodynamic properties of sea salt solutions

Calculation of Some Thermodynamic Properties of Sea Salt Solutions at Elevated Temperatures from Data on NaCI Solutions.

ADVERTISEMENT RETURN TO ISSUEPREVArticleNEXTCalculation of Some Thermodynamic Properties of Sea Salt Solutions at Elevated Temperatures from Data on NaCI Solutions.R. W. Stoughton and M. H. LietzkeCite this: J. Chem. Eng. Data 1965, 10, 3, 254–260Publication Date (Print):July 1, 1965Publication History Published online1 May 2002Published inissue 1 July 1965https://doi.org/10.1021/je60026a016RIGHTS & PERMISSIONSArticle Views675Altmetric-Citations50LEARN 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 InReddit PDF (643 KB) Get e-Alerts Get e-Alerts

The nature of ice‐forming nuclei in the atmosphere

AbstractDuring the last decade many experiments have been designed to investigate the initial processes of ice formation in the atmosphere. The results of these experiments are examined for clues as to the identity of the responsible nuclei and the following tentative conclusions are reached: (a) The nuclei which cause freezing between 0°C and −32°C are mainly solid, insoluble particles which are wetted by water and produce ice particles through the freezing of water drops.(b) The nuclei which become operative in the range −32° to −11°C consist of droplets of sea salt solution, ice and salt crystallising out on contaminating foreign particles at a temperature depending on the efficiency of these particles and the rate of expansion of the ambient air.(c) The nuclei effective at just below −41°C consist of droplets of pure salt solution and possibly of “ gaseous” nuclei formed industrially or by the action of ultra‐violet light on the gases of the upper atmosphere.

The Possibility of Transforming Rubber into an Ion Exchanger

Abstract Before taking up the actual subject of the present work, it is well to point out what is meant by an exchange of ions and to define an ion exchanger. An exchange of ions is a chemical reaction which takes place in a heterogeneous medium; when a solid heteropolar substance is immersed in a liquid, usually aqueous, ions belonging to the solid pass into the liquid in exchange for ions of the same polarity in solution in the liquid, and these dissolved ions thereby become fixed on the solid substance in place of the ions which the latter has just given up. As an example, minerals of the type of zeolite (green sand, harmatome, chabasie, etc.) can exchange their alkaline-earth metal ions, i.e., their cations, for sodium ions in an aqueous solution of sea salt which wets them or penetrates through them, and this phenomenon is reversible. Such a reaction is the basis of the detartarizing purification of industrial waters containing lime. Likewise the heteropolarity of exchangers sometimes renders their anions mobile, i.e., some substances give up their anions to liquids which wet them in exhange for the anions of these liquids, which thereby replace the anions liberated from the solids.