scholarly journals IV.—The magnetic rotation of hydrogen chloride in different solvents: and also of sodium chloride, lithium chloride, and of chlorine

1894 ◽  
Vol 65 (0) ◽  
pp. 20-28 ◽  
Author(s):  
W. H. Perkin
Keyword(s):  
Sodium Chloride ◽  
Hydrogen Chloride ◽  
Lithium Chloride ◽  
Magnetic Rotation

LITHIUM CHLORIDE CATALYZED DECARBOXYLATION OF OXALACETIC ACID IN ETHANOL

1964 ◽  
Vol 42 (12) ◽  
pp. 2806-2810 ◽  
Author(s):  
G. W. Kosicki ◽  
S. N. Lipovac ◽  
R. G. Annett
Keyword(s):  
Hydrogen Chloride ◽  
Lithium Chloride ◽  
Pyruvic Acid ◽  
Metal Salt ◽  
Enol Form ◽  
Absorption Peak ◽  
Oxalacetic Acid ◽  
Monovalent Metal

The monovalent metal salt lithium chloride promotes the decarboxylation of oxalacetic acid in ethanol. The absorption peak which appears at 230 mμ during the reaction is interpreted to be the enol form of pyruvic acid. Hydrogen chloride has a similar effect on the decarboxylation.

RECIPROCAL SALT PAIRS, INVOLVING THE CATIONS Li2, Na2, AND K2, THE ANIONS SO4, AND Cl2, AND WATER, AT 25 °C

1958 ◽  
Vol 36 (11) ◽  
pp. 1511-1517 ◽  
Author(s):  
A. N. Campbell ◽  
E. M. Kartzmark ◽  
E. G. Lovering
Keyword(s):  
Sodium Chloride ◽  
Potassium Chloride ◽  
Mole Fraction ◽  
Lithium Chloride ◽  
Invariant Point ◽  
Double Salt ◽  
Potassium Sulphate ◽  
Lithium Sulphate ◽  
Solid Phases ◽  
Chloride Monohydrate

In the reciprocal salt pair Li2, K2, Cl2, SO4, and water, at 25 °C there are large areas in which potassium sulphate and potassium lithium sulphate (KLiSO4) are separately in equilibrium with solution. Two incongruent invariant points exist. At one of these the composition of the solution is 0.917 mole fraction chloride, 0.437 mole fraction lithium, and 19.4 moles of water per total mole of salt, the equilibrium solid phases being potassium chloride, potassium sulphate, and the double salt. At the second, the composition of the solution is 0.967 mole fraction chloride, 0.870 mole fraction lithium, and 13.8 moles of water per mole of salt, the solid phases being potassium chloride, double salt, and lithium sulphate monohydrate. One congruent invariant point exists, at which the composition of the solution is 1.00 mole fraction chloride, 0.960 mole fraction lithium, and 9.6 moles of water per mole of salt, the solid phases being lithium sulphate monohydrate, lithium chloride monohydrate, and potassium chloride.In the reciprocal salt pair Li2, Na2, Cl2, SO4, and water, at 25 °C there is an incongruent invariant point at which the composition of the solution is 0.873 mole fraction chloride, 0.668 mole fraction lithium, and 15.1 moles water per total mole of salt, the solid phases being sodium chloride, solid solution of sodium and lithium sulphates, and lithium sulphate monohydrate. A congruent invariant point exists, at which the composition of the solution is practically entirely lithium chloride, the solid phases present being lithium chloride monohydrate, lithium sulphate monohydrate, and sodium chloride.

Inhibition of Glyceraldehyde Phosphate Dehydrogenase by Salts other than Lithium Chloride

Development ◽  
1956 ◽  
Vol 4 (1) ◽  
pp. 93-95
Author(s):  
Richard G. Ham ◽  
Robert E. Eakin
Keyword(s):  
Sodium Chloride ◽  
Lithium Chloride ◽  
Specific Effect ◽  
Lithium Ion ◽  
Developmental Changes ◽  
Lithium Ions ◽  
Sodium Salts ◽  
Glyceraldehyde Phosphate Dehydrogenase ◽  
Typical Data ◽  
Enzyme Study

Lallier (1954) has shown that 0·4 M lithium chloride strongly inactivates glyceraldehyde phosphate dehydrogenase—a finding which might partially explain some of the developmental changes found in lithium-treated embryos. In an attempt to establish an enzymatic basis for the morphological effects of lithium ion on Hydra which have been observed in this laboratory (Ham & Eakin, 1955), we have repeated the enzyme study with lithium chloride and extended it to include a number of other salts as controls. From typical data (Table 1), it is obvious that the inhibition of glyceraldehyde phosphate dehydrogenase activity is in no way a specific effect due to lithium ions. Both sodium chloride and potassium chloride produced a greater inhibition than did lithium chloride. From the various sodium salts tested, it was found that the anion may be of more importance than the cation in determining the degree of inhibition, although the cation also has some effect.

Osmotic coefficients of aqueous lithium chloride and potassium chloride from their isopiestic ratios to sodium chloride at 45.degree.C

1985 ◽  
Vol 30 (4) ◽  
pp. 432-434 ◽  
Author(s):  
Thomas M. Davis ◽  
Lisa M. Duckett ◽  
Judith F. Owen ◽  
C. Stuart Patterson ◽  
Robert Saleeby
Keyword(s):  
Sodium Chloride ◽  
Potassium Chloride ◽  
Lithium Chloride ◽  
Osmotic Coefficients

A simplified form of Stokes–Robinson equation

1976 ◽  
Vol 54 (1) ◽  
pp. 9-11 ◽  
Author(s):  
Chai-Fu Pan
Keyword(s):  
Sodium Chloride ◽  
Hydrogen Chloride ◽  
Activity Coefficients ◽  
Aqueous Electrolyte ◽  
Electrolyte Solutions ◽  
Solvent Interactions ◽  
Interionic Interactions ◽  
Two Parameter ◽  
Robinson Equation ◽  
Existing Data

In non-associated dilute aqueous electrolyte solutions, the deviation from ideality is principally attributed to the interionic interactions and hydration of ions. Stokes and Robinson combined Bjerrum's thermodynamic treatment of ion–solvent interactions with Debye–Hückel treatment of interionic interactions to obtain a two-parameter equation. In very dilute regions, the Stokes and Robinson's equation reduces to a much simpler form, i.e.[Formula: see text]Activity coefficients of an electrolyte at lower concentrations, say up to 0.1 m, can be calculated from the equation provided suitable values of &([a-z]+); and h are available. Solutions of hydrogen chloride and sodium chloride were chosen as examples. The results agree with the existing data very satisfactorily.

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