Buffer Standards for the Biochemical pH of the Zwitterionic Buffer N-Tris-(Hydroxymethyl) Methyl-2-Aminoethanesulfonic Acid (TES) from 5℃ to 55℃

Rabindra N. Roy, Lakshmi N. Roy, Blake M. Bodendorfer, Zachary M. Downs, Stephen D. Rocchio, Joshua T. Wollen, Jessica M. Stegner, Isaac B. Henson, Nicholas W. Grove, Lauren A. Dieterman

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Hoffman Department of Chemistry, Drury University, Springfield, USA.

DOI: 10.4236/ojpc.2012.21006                

Abstract

The authors have undertaken the determination of pH values for one buffer solution of TES without NaCl and nine buffer solutions with NaCl yielding an ionic strength I = mol.kg^-1. similar to that of blood. These buffer solutions have been evaluated in the temperature range of 5℃ to 55℃ using an extended version of the Debye-Hückel equation. The pH values are reported using 1) the Debye-Hückel extension of the Bates-Guggenheim convention in the tempera- ture range 5℃ to 55℃ and 2) with and without liquid junction correction at 25℃ and 37℃. These TES buffer solutions are recommended as secondary standard references for pH measurements in the range of pH 7.2 to 7.5 for physiological application with an ionic strength of I = 0.16 mol.kg^-1.

Keywords

Ionic Strength; Liquid Junction Potentials; Second Dissociation Constant; Buffer Solutions; Activity Coefficients

Conflicts of Interest

The authors declare no conflicts of interest.

References

[1]	N. E. Good, G. D. Winget, W. Winter, T. N. Connolly, S. Izawa and R. M. M. Singh, “Hydrogen Ion Buffers for Biological Research,” Biochemistry, Vol. 5, No. 2, 1966, pp. 467 -477. doi:10.1021/bi00866a011
[2]	W. J. Ferguson, K. L. Braunschweiger, W. R. Braunschweiger, J. R. Smith, J. J. McCormick, C. C. Wasmann, N. P. Jarvis, D. H. Bell and N. E. Good, “Hydrogen Ion Buffers for Biological Research,” Analytical Biochemistry, Vol. 104, No. 2, 1980, pp. 300-310. doi:10.1016/0003-2697(80)90079-2
[3]	L. N. Roy, R. N. Roy, C. E. Denton, S. R. LeNoue, C. A. Himes, S. J. Richards, A. N. Simon and V. S. Somal, “Buffer Standards for the Physiological pH of the Zwitterionic Compound, TAPS, from 5?C to 55?C,” Journal of Solution Chemistry, Vol. 35, 2006, pp. 551-556. doi:10.1007/s10953-005-9010-0
[4]	C. A. Vega and R. G. Bates, “Buffers for the Physiological pH Range: Thermodynamic Constants of Four Substituted Aminoethanesulfonic Acids from 5?C to 50?C,” Analytical Chemistry, Vol. 48, No. 9, 1976, pp. 1293- 1296.
[5]	R. N. Roy, C. P. Moore, J. A. Carlsten, W. S. Good, P. Harris, J. M. Rook, L. N. Roy and K. M. Kuhler, “Second Dissociation Constants of Two Substituted Aminoethanesulfonic Acids (MES) and (TES) in Water from 5?C to 55?C,” Journal of Solution Chemistry, Vol. 26, No. 12, 1997, pp. 1209-1216. doi:10.1023/A:1022937324983
[6]	V. E. Bower, M. Paabo and R. G. Bates, “A Standard for the Measurement of the pH of Blood and Other Physiological Media,” Journal of Research of the National Bureau of Standards, Vol. 65A, No. 3, 1961, pp. 267-270.
[7]	R. A. Durst and B. R. Staples, “Tris/Tris HCl: Standard Buffer for Use in the Physiological pH Range,” Clinical Chemistry, Vol. 18, No. 3, 1972, pp. 206-208.
[8]	D. Feng, W. F. Koch and Y. C. Wu, “Second Dissociation Constant and pH of N-(2-Hydroxyethyl)-piperazine-N’- 2-ethanesulfonic Acid from 0?C to 50?C,” Analytical Chemistry, Vol. 61, 1989, pp. 1400-1405. doi:10.1021/ac00188a019
[9]	Y. C. Wu, P. A. Berezansky, D. Feng and W. F. Koch, “Second Dissociation Constant of 3-(N-Morpholino)-2- hydroxypropanesulfonic Acid and pH of Its Buffer Solutions,” Analytical Chemistry, Vol. 65, 1993, pp. 1084- 1987. doi:10.1021/ac00056a023
[10]	R. N. Roy, D. R. Mrad, P. A. Lord, J. A. Carlsten, W. S. Good, P. Allsup, L. N. Roy, K. M. Kuhler, W. F. Koch and Y. C. Wu, “Thermodynamics of the Second Dissociation Constant and Standards for pH of 3-(N-Mor- pholino)propanesulfonic Acid (MOPS) from 5?C to 55?C,” Journal of Solution Chemistry, Vol. 27, No. 1, 1998, pp. 73-87. doi:10.1023/A:1022692629289
[11]	R. G. Bates, C. A. Vega and D. R. Jr. White, “Standards for pH Measurements in Isotonic Saline Media of Ionic Strength I = 0.16,” Analytical Chemistry, Vol. 50, No. 9, 1978, pp. 1295-1300. doi:10.1021/ac50031a026
[12]	R. G. Bates, “Determination of pH,” 2nd Edition, Wiley, New York, 1973.
[13]	R. N. Roy, L. N. Roy, C. E. Denton, S. R. LeNoue, S. Ashkenazi, M. S. Fuge, C. D. Dunseth, J. L. Durden, C. N. Roy, A. Bwashi, J. T. Wollen and S. J. DeArmon, “Buffer Standards for the Physiological pH of 3-[(1,1-Dimethyl- 2-hydroxymethyl)-amino]-2-hydroxypropanesulfonic Acid from (278.15 to 328.15) K,” Journal of Chemical & Engineering Data, Vol. 54, No. 2, 2009, pp. 428-435.
[14]	W. M. Latimer, “Oxidation Potentials,” 2nd Edition, Prentice-Hall, New York, 1952.
[15]	R. G. Bates and E. A. Guggenheim, “Report on the Standardization of pH and Related Terminology,” Pure and Applied Chemistry, Vol. 1, No. 1, 1960, pp. 163-168. doi:10.1351/pac196001010163
[16]	R. N. Roy, L. N. Roy, S. Ashkenazi, J. T. Wollen, C. D. Dunseth, M. S. Fuge, C. N. Roy, H. M. Hughes, B. T. Morris and K. L. Cline, “Buffer Standards for pH Measurement of N-(2-Hydroxyethyl)piperazine-N’-2-ethanesulfo- nic Acid (HEPES) for I = 0.16 mol?kg?1 from 5?C to 55?C,” Journal of Solution Chemistry, Vol. 38, 2009, pp. 449-458. doi:10.1007/s10953-009-9378-3
[17]	K. S. Pitzer and G. J. Mayorga, “Thermodynamics of Electrolytes. II. Activity and Osmotic Coefficients for Strong Electrolytes with One or Both Ions Univalent,” Journal of Physical Chemistry, Vol. 77, No. 19, 1973, pp. 2300-2307. doi:10.1021/j100638a009
[18]	R. P. Buck, S. Rondinini, A. K. Covington, F. G. K. Baucke, C. M. A. Brett, M. F. Cam?es, M. J. T. Milton, T. Mussini, R. Naumann, K. W. Pratt, P. Spitzer and G. S. Wilson, “Measurement of pH: Definition, Standards, and Procedures,” Pure and Applied Chemistry, Vol. 74, No. 11, 2002, pp. 2169-2200. doi:10.1351/pac200274112169