Solubility Of Iodine Research Articles

Electrolysis of ammonium iodide solution in a Na 2CO 3I 2 hybrid cycle

The electrolysis step in the following hybrid cycle Na 2CO 3+I 2→2NaI+CO 2 1 2 O 2 2NaI+2NH 3+2CO 2+2H 2O→2NaHCO 3 +2NH 4I 2NaHCO 3→Na 2CO 3+CO 2+H 2O ▪ was studied. The solubility of iodine in the anolyte (NH 4I-I 2 solution), steady state compositions of the catholyte (NH 4I-NH 3 solution), polarization characteristics for both electrolyte solutions and the nature of ion-exchange membranes was examined. The polarizations of the anode were very small, in a range up to 1000 mA cm −2, and those of the cathode were also relatively small. An advantageous feature of this electrolysis over NaI electrolysis [1] is that a large current density is obtainable. Decomposition voltages assumed from the polarization curves are small compared with NaI electrolysis. This improvement arises from greater solubilities of electrolytes. Among the ion-exchange membranes tested, Nafion was usable because of durability of the electrolyte solution and low permeation of iodine.

An improved model for fission product behavior in nuclear fuel under normal and accident conditions

A theoretical model for the prediction of the behavior of the gaseous and volatile fission products in nuclear fuels under normal and transient conditions has undergone substantial improvements. The major improvements have been in the atomistic and bubble diffusive flow models, in the models for the behavior of gas bubbles on grain surfaces, and in the model for iodine solubility. The theory has received extensive verification over a wide range of fuel operating conditions, and can be regarded as a state-of-the-art model based on our current level of understanding of fission product behavior. Because of existing uncertainties in both materials properties and mechanisms of fission product response, any verified mechanistic description of fission product release entails assumptions in these areas. The diffusivity of fission gas bubbles during transient conditions, the effect of irradiation induced grain boundary gas-atom re-solution on intragranular diffusive flow rates, and the effect of iodine solubility on iodine release rates are aspects of fission product behavior that are currently clouded with uncertainty. The assumptions that have been made in the theory have been evaluated and are discussed in relation to the model verification, uncertainties in the existing data base, and other theoretical descriptions of fission product behavior.

Thermochemical investigations of nearly idial binary solvents. 6. Solubilities of iodine and benzil in systems of nonspecific interactions

Solubilities have been determined at 25°C for iodine in binary mixtures of carbon tetrachloride with cyclohexane, n-hexane, n-heptane, and octamethylcyclotetrasiloxane (OMCTS) and in mixtures of cyclohexane with n-hexane and OMCTS; and for benzil in binary mixtures of carbon tetrachloride with cyclohexane, n-hexane, and n-heptane, mixtures of n-hexane with cyclohexane and n-heptane, and mixtures of benzene with cyclohexane and toluene. With the exception of the benzene+cyclohexane system, the nearly ideal binary solvent model predicts these solubilities with a maximum deviation of 6% and an overall standard deviation of 2.4%. The model correctly predicts minima for solubility (mole fraction) of iodine in the OMCTS systems, and predicts solubilities within 4% for benzil in the carbon tetrachloride+n-hexane system, in which the solubility changes by a factor of 14. The failure of the model for predicting solubilities of benzil in mixtures of benzene and cyclohexane (maximum error of 25% for and 18-fold range of solubilities) is possibly due to specific interactions between benzil and benzene.

Solubility of iodine in mixed solvents

Solubility of iodine in mixed solvents

Solubility of iodine in electron-donating solvents at various temperatures

ADVERTISEMENT RETURN TO ISSUEPREVArticleNEXTSolubility of iodine in electron-donating solvents at various temperaturesCheng Zhang Jiang, Fu Juan Hsu, and Vojtech FriedCite this: J. Chem. Eng. Data 1983, 28, 1, 75–78Publication Date (Print):January 1, 1983Publication History Published online1 May 2002Published inissue 1 January 1983https://doi.org/10.1021/je00031a022RIGHTS & PERMISSIONSArticle Views198Altmetric-Citations3LEARN 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 (438 KB) Get e-Alerts Get e-Alerts

Vapor pressure, iodine solubility, and hydrogen solubility of hydrogen iodide-iodine solutions

Vapor pressure, iodine solubility, and hydrogen solubility of hydrogen iodide-iodine solutions

Solubility of iodine in mixed solvents. A case study of preferential solvation in nonpolar and associated solutions

Solubility of iodine in mixed solvents. A case study of preferential solvation in nonpolar and associated solutions

Solubility of HI

Oak Ridge National Laboratory is curtently engaged in the development of methods for reprocessing spent nuclear fuel. One of the major problems encountered in the development of suitable flow sheets for this purpose is the need to provide a means for retaining essentially all of the radioiodine released during the reprocessing. A promising technique (the lodex Process) ( 7 , 2 ) involves trapping the iodine in concentrated nitric acid, where it is ultimately oxidized to the pentavalent form. Earlier work by Unger et al. (4) showed that the solubility of 1 5 + in nitric acid depended both on the temperature and the concentration of the acid, with the heat of solution being largely independent of the nitric acid concentration over the range 13-17M. Data scatter precluded accurate determination of the heat of solution, and the solid phase was not identified at that time. Later, however, it was determined to be H1308. Solubilities at 25°C in 12.5 and 14.3M HN03 can be found in the literature (3). In the studies reported in this paper, we measured the solubility of pentavalent iodine in 12-20M HNO3 over the temperature range 25-100°C. The solid phase was isolated and identified.

The impedance of the Pt/Ag4RbI5 and C/Ag4RbI5 interphases at anodic potentials

Impedance measurements have been made on the Pt/Ag4RbI5 and C/Ag4RbI5 interphases. Rate constants for the electrochemical oxidation of I− to I2 on Pt have been determined. Steady-state measurements have enabled calculation of the solubility and diffusion coefficient of iodine in Ag4RbI5. The variation of these characteristics with pressure and particle size of electrolyte has also been investigated. The results are in agreement with those obtained from transient measurements.

The impedance of the Pt/Ag 4RbI 5 and C/Ag 4RbI 5 interphases at anodic potentials

Impedance measurements have been made on the Pt/Ag 4 RbI 5 and C/Ag 4 RbI 5 interphases. Rate constants for the electrochemical oxidation of I − to I 2 on Pt have been determined. Steady-state measurements have enabled calculation of the solubility and diffusion coefficient of iodine in Ag 4 RbI 5 . The variation of these characteristics with pressure and particle size of electrolyte has also been investigated. The results are in agreement with those obtained from transient measurements.

DETERMINATION OF SOLUBILITY PARAMETER FOR SILOXANE SEGMENT

The solubility of iodine in PDS (polydimethylsiloxane) has been measured for varying degrees of polymerization (number of silicon atoms) from 2 to 470. The data obtained show good agreement with a solubility equation derived on the basis of the following two assumptions : (1) a PDS molecule is composed of several completely freely oriented segments, and (2) the mixture of these segments and iodine can be treated as a regular solution as far as enthalpy calculation is concerned. A constant segment solubility parameter δS, which is about 7.5 cal1/2/cm3/2, is obtained regardless of degree of polymerization by the use of this solubility equation. This value is nearly the same as that of silicon rubber from swelling data. On the basis of the discussions above, it is concluded that the size of a segment is nearly equal to that of a siloxane unit. The molecular-attraction constant for a siloxane unit is found to be 580-600 cal1/2•cm3/2/mol.

Solutions of Nonelectrolytes

Introduction.-The purpose of the authors in writing the following review has been to give a critical account of the more significant papers bearing upon the theory of solutions which have appeared during the year 1949. We have not hesitated to trace certain developments back into 1948, but we are not giving the earlier background as fully as might be desirable if it were not for the expected publication of the third edition of our Solubility of Nonelectrolytes (1) in which the progress in the subject has been brought down to the middle of 1948.1 It would be impossible, in the space at our disposal, to mention all the contributions pertinent to the general topic without turning this review into a mere set of abstracts such as are already available elsewhere; conse· quently, we can only apologize upon these grounds for the failure to report on a number of good pieces of work. Certain topics and types of system have been the subject of particularly active study during the year and have brought to light points of more than ordinary interest. reviews which follow have been grouped accordingly. Iodine solutions.-The investigation of iodine solutions has for many years contributed much to the theory of solubility and has continued during the past year to yield results of considerable significance. Iodine lends itself peculiarly. well to this purpose for several reasons: its solutions can be easily and accurately analyzed; its molecular attractive field is very high, giving an enormous range to its solubilities; its molecules have nearly spherical symmetry; and chemical effects can readily be differentiated from physical effects by departures in color from the violet of iodine vapor. A general review of The Nature of Iodine Solutions by Kleinberg & Davidson (2) covered the subject into 1948. Late in the same year Benesi & Hildebrand (3) published a paper on the solubility of iodine in 1,2. and 1,l-dichloroethanes, cisand trans-dichloroethylenes, and perfluoro-n-hep­ tane. All these solvents give violet solutions in spite of the considerable dipole moments of all but the last two, and the temperature dependence of solu­ bility in all cases fits them into the family of regular solution curves to which all violet solutions of iodine belong, the significance of which is maximum randomness of distribution of iodine molecules; so the entropy of transfer of

SOLUBILITY AND ENTROPY OF SOLUTION OF IODINE IN ETHANOL-CYCLOHEXANE SOLUTIONS

Abstract The solubility of iodine in ethanol-cyclohexane solutions has been measured at 15.0, 25.0 and 35.0°C and the entropy of solution has been evaluated. It is found that the iodine complex formed in the mixed solutions is more stable than that in pure ethanol.

Studies in Solubility Parameter Theory for Mixed Solvent Systems

Data are presented for the saturation solubility and partial molal volume of iodine in a mixed benzene–cyclohexane solvent and for the saturation solubility of stannic iodide in the same solvent mixture. A successful interpretation of these data in terms of solubility parameter theory is possible if we define an effective volume fraction term. This term reflects the immediate solvent environment of the solute molecule with the preferential solvation of the solute by one of the solvent molecules. Data for iodine in a mixed carbon tetrachloride–benzene solvent mixture and for iodine in a carbon tetrachloride–perfluoroheptane mixture are also interpreted in terms of the proposed theory.

The solubility and diffusion of iodine in Ag 4RbI 5

E.m.f. measurments on the cell: Download : Download full-size image show that mixtures of I2 and Ag4RbI5 form at least a two phase system for x2>0.004. From transient and steady state potentiostatic measurements it has been possible to calculate the apparent solubility of iodine in polycrystalline Ag4RbI5 of voidage ≈3% as 4.3×10−7 mol cm−3 with a diffusion coefficient of 1.1×10−5 cm2 s−1. It is suggested that this solubility arises from adsorption of I2 on particle surfaces coupled with diffusion through voids.

The solubility and diffusion of iodine in Ag4RbI5

The solubility and diffusion of iodine in Ag4RbI5

Solubility of iodine in water?Alcohol mixtures comparison with a ternary-solution model

Solubility of iodine in water?Alcohol mixtures comparison with a ternary-solution model

Studies in regular solution theory. Part 1.—Solubolity studies of tetraphenyltin in simple non-polar solvents

The solubility of tetraphenyltin in a number of non-polar solvents is presented. The data are analyzed in terms of Hildebrand's theory of regular solutions. The large molar volume of this solute requires the inclusion of a Flory-Huggins term in the saturation solubility equation. The possible limitation of the interaction-energy geometric-mean rule are examined and a comparison is made with data for the solubility of stannic iodide, iodine and sulphur in a similar set of solvents.

Solubility of iodine in dimethyl sulfoxide

Solubility of iodine in dimethyl sulfoxide

Thermodynamics of Iodine Solubility and Triiodide Ion Formation in Water and in Deuterium Oxide

ADVERTISEMENT RETURN TO ISSUEPREVArticleNEXTThermodynamics of Iodine Solubility and Triiodide Ion Formation in Water and in Deuterium OxideR. W. Ramette and R. W. Sandford Jr.Cite this: J. Am. Chem. Soc. 1965, 87, 22, 5001–5005Publication Date (Print):November 1, 1965Publication History Published online1 May 2002Published inissue 1 November 1965https://doi.org/10.1021/ja00950a005RIGHTS & PERMISSIONSArticle Views2488Altmetric-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 InReddit PDF (545 KB) Get e-Alerts Get e-Alerts