Solutions Of Lithium Salts Research Articles

Effect of cation size on the enthalpy of dilution of alkali-metal salts of carboxymethylcellulose

The intermediate and integral enthalpies of dilution of aqueous solutions of lithium, sodium, potassium, ammonium and caesium salts of carboxymethylcellulose have been measured at 25 °C. Constant values for the intermediate enthalpies of dilution are obtained with the lithium and sodium salts within the concentration range investigated, but the potassium, ammonium and caseium salts give progressively more exothermic values as the initial concentration is reduced. The integral enthalpies of dilution are in the order Li+ > Na+ K+= NH+4= Cs+. Comparison with the corresponding series of salts of polyacrylic acid and poly(styrenesulphonic acid) shows a greater similarity with the latter group of salts.

Crystal structure, and the infrared and Raman spectra, of tripotassium methanetrisulphonate hydrate, K3[CH(SO3)3]·H2O

The crystal structure of the title compound has been determined using three-dimensional X-ray diffraction data, from 839 reflections; crystals are orthorhombic, space group P212121, with unit-cell dimensions a= 9.405(1), b= 9.405(1), c= 12.321(1)A, Z= 4. The structure has been solved using direct methods and refined by fullmatrix least squares to R 0.045. The S–C–S angles (ca. 113°) indicate an expansion from tetrahedral stereochemistry and the S–C bond lengths (ca. 1.81 A) are appreciably longer than those for K2[CH2(SO3)2](1.77 A) and Ca[CH3SO3]2(1.75 A). The i.r. (4 000–50 cm–1) and Raman spectra of K3[CH(SO3)3]·H2O and K3[CD(SO3)3]·D2O at 77 K are reported and interpreted according to the crystal structure. To assist with the assignment, spectra of the anhydrous salt, K3[CH(SO3)3], and of aqueous solutions of the soluble lithium salts, have also been recorded. The SO3 groups show their characteristic group frequencies: νsym(C–S) and νasym(C–S) are assigned to 762 and 820 cm–1, respectively; δsym(CS3) and δasym(CS3) to 170 and ca. 210 cm–1, respectively. I.r. spectra of samples containing the isotopically dilute HDO species confirm the presence of two types of hydrogen bond per water molecule.

Solutions of lithium salts in liquid lithium: preparation and X-ray crystal structure of the dilithium salt of carbodi-imide (cyanamide)

The salt Li2[NCN] has been prepared by the solid-state reaction of Li2C2 with Li3N at 600 °C. When the reaction is carried out in molten lithium, colourless single crystals of the salt form on evaporation of the metal. This reaction is pertinent to the purification of liquid lithium for fusion reactors and to corrosion and dissolution of containment metals. An X-ray diffraction study has shown that the structure of Li2[NCN] is tetragonal, space group I4/mmm, with unit-cell dimensions a=b= 3.687(3), c= 8.668(5)A, for Z= 2. Full matrix least-squares refinement with anisotropic temperature factors for each atom converged to give an R value of 0.036. The lattice is composed of Li+ and centrosymmetric [NCN]2– ions [r(C–N) 1.230(3)A]. Each Li+ ion is at the centre of a squashed tetrahe-dron of N atoms [r(Li–N) 2.068(l)A, N–Li–N 101.85(5) and 126.1 1(13)°]. The i.r. spectrum of the solid consists of bands at 2000 (ν3, Σu+) and 690 cm–1(ν2, πu,) for the [NCN]2– ion. Comparisons are made with the crystal structures of the analogous compounds MNCN (M = Ca, Sr, or Pb) and H2NCN. The i.r. spectrum is compared with those of the compounds M2NCN (M = Na, K, Ag, or Tl) and MNCN (M = Zn or Pb).

Solutions of lithium salts in liquid lithium. The electrical resistivity of solutions of nitride, hydride and deuteride

The electrical resistivities, ρ, of solutions of lithium nitride, lithium hydride and lithium deuteride in liquid lithium have been determined for concentrations, x, up to 2.77, 5.68 and 2.22 mol % non-metal over the temperature ranges 200–450, 257–551 and 276–500°C, respectively. For each solute, resistivity increases linearly with increasing concentration, except for very dilute solutions, and the coefficient, dρ/dx increases with increasing temperature. Nitride causes the greatest increase in resistivity [dρ/dx= 7.0 × 10–8Ωm (mol % N)–1 at 400°C], and hydride and deuteride show no detectable isotope effect [dρ/dx= 4.9 × 10–8Ωm (mol % H or D)–1 at 400°C]. The resistivities of mixtures of nitride and hydride in lithium are additive, thereby showing lack of association between these solutes. Ammonia vapour reacts with the metal to form hydride and nitride which dissolve to increase the resistivity by their characteristic amounts.

The Heat of Solution and Solvation Number of Lithium Salts in Water–Alcohol Mixtures

Abstract The solvation numbers of LiCl and LiI, and of KI for comparison, in water–MeOH mixtures and water–i-PrOH mixtures were determined at an infinite dilution at 25 °C from the adiabatic compressibility. The heats of solution of these salts were also determined. In general, with an increase in the concentration of alcohol the solvation number increases initially to reach a maximum at 10–30 mol% alcohol, then it decreases to a minimum and increases again from about 75 mol% alcohol. The maximum solvation numbers of the salts determined are as follows: LiCl 11.2 mol/mol at 30 mol% MeOH; LiCl 11.5 mol/mol at 15 mol% i-PrOH; LiI 8.2 mol/mol at 12 mol% i-PrOH and KI 14.0 mol/mol at 10 mol% i-PrOH. The larger the cation, the larger the solvation number. Also, the composition of the solvant where the salt containing larger ions has a maximum solvation number has a lower concentration of alcohol. The maximum solvation number of LiI containing a larger anion is smaller than that of LiCl because an iodide ion has a much larger structure-breaking effect than a chloride ion. By the way, there seems to be difference in the structure of the mixed solvent before and after the maximum solvation number.

Isotopieeffekte in der Grenzschicht anorganischer Lösungen / Isotope Effects at the Surface of Inorganic Solutions

Isotope effects were investigated at the surface of aqueous lithium and calcium salt solutions. The dependence on the temperature in the gas phase was determined. The surfaces of the solutions were isolated by spray experiments. In the case of calcium salt solutions an enrichment of the lighter isotope 40Ca in relation to the heavier isotopes 44Ca and 48Ca was found at the solution surface. The experiments with lithium fluoride and lithium iodide gave inverse isotope effects. The calcium isotope effect could be qualitatively explained by the Gibbs theorem. The isotope separation of lithium possibly can be referred to the more covalent bonding character than the ionic one of lithium compounds at the solution surface.

The Equivalent Conductivity of Aqueous Solutions of Salts of Carboxymethylcellulose: A Test of Manning's Limiting Law

Measurements of the equivalent conductivity of aqueous solutions of lithium, sodium, potassium, and cesium salts of carboxymethylcellulose (CMC) at 25 °C are reported. The degree of substitution of the CMC used was 0.86, concentrations of the four salts were varied from 5 × 10−4 to 5 × 10−2 equiv l−1. Results show a decrease of Λ with increasing concentration in each case. In the lower concentration range (up to 10−2N) this decrease is in close agreement with a limiting law for conductivity recently developed by Manning. Above 10−2N the decrease in Λ is less than the decrease predicted by the limiting law. The counterion dependence of Λ is accurately predicted by the theory, and a qualitative agreement is obtained when the theory is used to compare conductance data of polyelectrolytes with different charge densities.

Ultrasonic relaxation in aqueous solutions of lithium salts and sodium poly(α,L-glutamic acid)

An ultrasonic relaxation process is observed in aqueous solutions of sodium poly(α, L-glutamic acid) containing high concentrations of LiCl and LiClO4. It arises from an equilibrium involving hydrated lithium ions and the carbonyl group of the peptide bond.

Lithium Anode Cells Operating at Room Temperature in Inorganic Electrolytic Solutions

Lithium anode electrochemical cells have been operated at room temperature using electrolytic solutions of lithium salts in inorganic solvents such as phosphorus oxychloride, thionyl chloride, and sulfuryl chloride. Lithium metal can be electrodeposited from these solutions accompanied, in the case of chlorine‐containing electrolytes, by the simultaneous electrogeneration of chlorine at the positive electrode. The resulting lithium/chlorine electrochemical cells have open‐circuit potentials of 4.0–4.3V, depending on the presence of excess Lewis acid in the electrolyte. The solvents are compatible with both lithium metal and with strong oxidants including chlorine (Cl2), cupric fluoride , polycarbon monofluoride , and tungsten trioxide which can be used as cathode materials. The solvents themselves, while difficult to oxidize, can be electrochemically reduced at various catalytic surfaces (such as carbon black and metals) and act as cathode depolarizers. This catalytic solvent reduction process leads to cells with exceptionally stable voltages and energy densities in excess of 500 W‐hr/kg.

Calculational indices of operation efficiency for one-stage absorption cooling assembly operating on an aqueous solution of lithium salts

Calculational indices of operation efficiency for one-stage absorption cooling assembly operating on an aqueous solution of lithium salts

Preferential solvation of S-cysteinyl bovine serum albumin in aqueous solutions of lithium salts.

ADVERTISEMENT RETURN TO ISSUEPREVArticleNEXTPreferential solvation of S-cysteinyl bovine serum albumin in aqueous solutions of lithium saltsMilton E. NoelkenCite this: Biochemistry 1970, 9, 21, 4122–4128Publication Date (Print):October 13, 1970Publication History Published online1 May 2002Published inissue 13 October 1970https://doi.org/10.1021/bi00823a014RIGHTS & PERMISSIONSArticle Views33Altmetric-Citations19LEARN 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 (682 KB) Get e-Alerts Get e-Alerts

On the hydration of DNA. II. Base composition dependence of the net hydration of DNA.

AbstractThe dependence of the net hydration of DNA on its base composition has been measured by density gradient ultracentrifugation of three DNA's in a series of cesium and lithium salt solutions of different water activities. Extrapolation to zero water activity showed the dependence of the partial specific volume on base composition to be very small for CsDNA and aero for LiDNA. At least 99% of the dependence of buoyant density on base composition can be accounted for on the basis of a differential hydration, with a mole of adenine–thymine pairs binding about 2 moles more water than a mole of guanine–cytosine pairs in CsCl.

A study of the surface tension of the systems: “Water-lithium soaps and butanol-I”

The surface tension of the solutions of lithium salts of fatty acids in the mixtures of water and butanol-I of varying composition has been studied. It has been suggested that the change in the nature of the micelles takes place at about 50% butanol-I concentration. Up to 50% butanol-I concentration hydrophilic oleomicelles are formed but above 50% butanol-I concentration lipophilic hydromicelles exist. A study of the effect of the concentration of the different soaps on the surface tension suggests that the surface tension of the solutions increases with the increase in the soap concentration. It has also been observed that the surface tension of the soap solutions increases with the increase in the number of carbon atoms in the soap.

A concentration-cell method for the determination of trace amounts of chloride in solutions of lithium salts

A concentration-cell method for the determination of trace amounts of chloride in solutions of lithium salts

An Electrolytic Countercurrent Column for Isotope Separation: a Simplified Theoretical Approximation

IN this communication, the possibility is considered of multiplying a single, electrolytic isotopic separation effect in a continuous process occurring in an electrolyser with a countercurrent flow and conversion of two immiscible liquid phases. The latter consisted of an electrode and an electrolyte. Such a process may—among other applications—be used to the enrichment of lithium. The process is presented schematically in Fig. 1. A solution of the lithium salt chosen is electrolysed during the flow between the immovable anode 1, and the movable cathode 2, which is mercury flowing in countercurrent. During the flow the isotopically enriched lithium is accumulated in the mercury. The resulting amalgam is then decomposed in the converter 3. The solution of the lithium salt obtained and the pure mercury are turned back to the electrolyser. Part of the solution of the salt in the converter can be taken off as the enriched product P. The dilute and isotopically exhausted electrolyte is removed from the device, which, owing to the apparent analogy, may be called the electrolytic column.

Separation factors for lithium isotope exchange on the amberlite IR-120 cation exchange resin

The effect of concentration on the elementary separation factor for various lithium compounds (LiNO/sub 3/, LiCl, Li/sub 2/SO/sub 4/, CH/sub 3/COOLi, and LiOH) Was investigated using the breakthrough technique on an exchange column. Depending on the concentration and the anion, the separation factors varied from 1.019 to 0.999, Li/sup 7/ being enriched in the solution. In cases of the chloride and nitrate solutions distinct maxima at the concentration of 2N (1.019 and 1.014 resp.) were observed. Minima appeared at 3 resp. 4N with factors of 1.007 and 0.999. The solutions of sulfate, acetate, and hydroxide showed factors between 1.0021 and 1.0003 with a less pronounced concentration dependence. Addition of alcohol, glycol, or dioxane to the lithium salt solutions acted in the sense of decreasing the separation parameters. A qualitative explanation is based on ion pair formation. (auth)

Determination of the separation factor of lithium isotopes in ion exchange

The isotopic equilibrium between the solutions of lithium salts (LiOH and LiCl) and SBS, KU-2, and Dowex-50 cationites is investigated. It is shown that, in the first place, the Li7 isotope was concentrated in the solution in all the cases which were investigated; in the second place, there is a dependence of the separation factor value α on the nature of the cationite; in the third place, in 1 N to 5 N solutions of LiCl, the value of a does not depend on the concentration of the solution.

The “HCl Effect” in Anion-Resin Exchange

An explanation is offered for the interesting feature that distribution ratios of anions with strong-base exchange resins are generally lower from concentrated HCI solutions than from comparable LiCl solutions. It is suggested that this behavior is due to the invasion of the resin by non-exchange electrolyte at the high external-solution concentrations and to the partial association of the acid species in the resin phase. That is, because of the nature of the latter phase, normally strong acids are differentiated, the weaker ones partially associating. This does not occur as readily with the lithium salts, and so the preferential association of non-exchange H+ with the weaker- acid anion (Cl- in most of the cases studied) represses the absorption of the other anion as a non-exchange electrolyte. If the anion of interest were the anion of a weaker acid than that of the macroelectrolyte, the reverse of the usual behavior should occur, namely, exchange from acid solution should yield larger distribution ratios than exchange from lithium salt solutions. This is shown to be the case for CI- tracer exchanging with concentrated HBr and LiBr solutions. (auth)

The Supercontraction of Wool in Solutions of Lithium Salts

The supercontraction of various types of wool, modified wool, and other keratins has been studied using concentrated solutions of lithium salts, particularly the bromide. The purity of the lithium bromide has been found to be of considerable importance, traces of bromine in the solution having a profound effect. With bromine concentrations in the range 10-4-10-5 M, marked differences between clean and detergent-treated wools have been observed. Removal of the bromine by means of thiosulfate has enabled quantitative measurements to be made of such variables as concentration of lithium bromide, time and temperature of treatment, etc.