Application of Osmotic Coefficient Theory of Electrolyte in Metrology of Physical Chemistry Quantities Including Water Activity

WANG Haifeng; LI Jia

doi:10.12338/j.issn.2096-9015.2024.0191

Article Contents

Article Navigation > Metrology Science and Technology > 2024 > Uncorrected proof

WANG Haifeng, LI Jia. Application of Osmotic Coefficient Theory of Electrolyte in Metrology of Physical Chemistry Quantities Including Water Activity[J]. Metrology Science and Technology. doi: 10.12338/j.issn.2096-9015.2024.0191

Citation:

WANG Haifeng, LI Jia. Application of Osmotic Coefficient Theory of Electrolyte in Metrology of Physical Chemistry Quantities Including Water Activity[J]. Metrology Science and Technology. doi: 10.12338/j.issn.2096-9015.2024.0191

Citation:

PDF( 476 KB)

Application of Osmotic Coefficient Theory of Electrolyte in Metrology of Physical Chemistry Quantities Including Water Activity

doi: 10.12338/j.issn.2096-9015.2024.0191

National Institute of Metrology, Beijing 100029, China

Received Date: 2024-06-15
Accepted Date: 2024-07-08
Rev Recd Date: 2024-07-15

Available Online: 2024-08-02

Abstract

Abstract

Osmotic coefficient (ϕ) is a measure of the deviation of the solvent of electrolyte from the ideal solution. ϕ was usually determined by the manometric method and the electromotive force method. National bureau of standard of United States of America published the reference value of osmotic coefficient equal to the average of many scientific data and its standard deviation based on the statistics. This reference data was expressed as the Debye-Hückel equation. When the molality of the electrolyte was introduced in the equation, and thus the corresponding osmotic coefficient was deduced. ϕ can be used to calculate the water activity, freezing point depression and osmotic pressure concentration of the solution of electrolyte, and thus the reference solution of these quantities were determined and then used to calibrate the instrument of these quantities. Sodium chloride was the most commonly used electrolyte. The reference values specified by the related international or national standard were well consistent with the results calculated using the reference data of ϕ. The reference values of related physical chemistry quantities calculated using the reference data of ϕ were traceable to SI units of vapor pressure or potential of the electromotive force indirectly.
- metrology,
- osmotic coefficient,
- water activity,
- freezing point depression,
- osmolality,
- reference material

FullText(HTML)

References(22)

References

[1]	Hamer, W. J. , Wu, Y. C. Osmotic Coefficients and Mean Activity Coefficients of Uni-univalent Electrolytes in Water at 25°C[J], Journal of Physical and Chemical Reference Data 1, 1047 (1972
[2]	Allrnand, A. J. , Polack, W. G. The free energy of dilution of aqueous sodium chloride solutions [J]. J. Chem. Soc. , Trans. 1919, 1020-1039.
[3]	Harned, H: S. The electromotive forces of uni-univalent halides in concentrated aqueous solutions [J]. J. Am. Chem. Soc. , 1929(2), 416-427.
[4]	Harned, H. S. , Nirns, L. F. The thermodynamic properties of aqueous sodium chloride solutions from 0 to 40° [J]. J. Am. Chem. Soc. , 1932(2), 423-432.
[5]	Brown, A. S. , Macinnes, D. A. The Determination of Activity Coefficients from the Potentials of Concentration Cells with Transference. I. Sodium Chloride at 25° [J]. J. Am. Chem. Soc. 1935(7), 1356-1362.
[6]	Janz, G. J. , Gordon, A. R. The thermodynamics of aqueous solutions of sodium chloride at temperatures from 15-45° from e. m. f. measurements on cells with transference [J]. J. Am. Chem. Soc. , 1943, 218-221.
[7]	Getman, F. H. The activities of the ions in aqueous solutions of some “strong” electrolytes [J]. J. Am. Chem. Soc. 192(8), 1556-1564.
[8]	Stokes, R. H. The Measurement of Vapor Pressures of Aqueous Solutions by Bi-thermal Equilibration Through the Vapor Phase[J]. J. Am. Chem. Soc., 1947(6): 1291-1296.
[9]	Harned, H. S. The Structure of Electrolytic Solutions [B], edited by W. J. Hamer, Chap. 10, John Wiley & Sons, New York, N. Y. , 1959.
[10]	Pearce, J. N. , Nelson, A. F. The vapor pressures of aqueous solutions of lithium nitrate and the activity coefficients of some alkalisalts in solutions of high concentration at 25° [J] J. Am. Chem. Soc. , 1932(9), 3544-3555.
[11]	Olynyk, P. , Gordon, A. R. The Vapor Pressure of Aqueous Solutions of Sodium Chloride at 20, 25 and 30° for Concentrations from 2 Molal to Saturation[J]. J. Am. Chem. Soc., 1943(2): 224-226.
[12]	Petit, M. C. A method for measurement of the activity of electrolytes solutions [J]. J. Chim. Phys-Chim. Biol. , 1965, 1119-1125.
[13]	Hepburn, J. R. I. , The vapour pressure of water over sulphuric acid-water mixtures at 25°C. , and its measurement by an improved dew-point apparatus [J]. Proc. Phys. Soc. 1927(1), 249-256.
[14]	Robinson, R A. , Sinclair, D. A. The Activity Coefficients of the Alkali Chlorides and of Lithium Iodide in Aqueous Solution from Vapor Pressure Measurements [J]. J. Am. Chem. Soc. 1934(9), 1830-1835.
[15]	Scatchard, G. , Hamer, W. J. , Wood, S. E. Isotonic Solutions. I. The chemical potential of water in aqueous solutions of sodium chloride, potassium chloride, sulfuric acid, sucrose, urea and glycerol at 25° [J]. J. Am. Chem. Soc. , 1938(12), 3061-3070.
[16]	Robinson, R. A. The activity coefficients of some alkali halides at 25° [J]. Trans. Faraday Soc. , 1939, 1217-1220.
[17]	Janis, A. A. , Ferguson, J. B. , Sodium chloride solutions as an isopiestic standard [J]. Canadian J. Res. , 1939(8), 215-230.
[18]	Robinson, R. A. The vapor pressures of solutions of potassium chloride and sodium chloride [J] Trans. Proc. Roy. Soc. New Zealand, 1945(2), 203 -217.
[19]	International standard organization. microbiology of food and animal feeding stuffs-determination of water activity: ISO 21807[S]. Geneva: International standard organization, 2004-09-29.
[20]	郑涵, 王海峰, 张艾蕊, 等. 系列水分活度标准物质的研制[J]. 化学试剂, 2024(3): 105-111.
[21]	国家标准化委员会. 食品安全国家标准生乳冰点的测定: GB 5413.38-2016 [S]. 北京: 中国标准出版社, 2016.
[22]	The United States Pharmacopeial Convention. United States Pharmacopeia, Physical tests, 785, Osmolality and osmolarity, USP 41, 6527-6529 [S]. Rockville: The United States Pharmacopeial Convention, 2024.