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Buffer Standards for Physiological pH of the Buffer N-(2-Acetamido)-2-aminoethanesulfonic Acid from 5°C to 55°C

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DOI: 10.4236/ojpc.2011.13016    3,371 Downloads   6,152 Views   Citations

ABSTRACT

Electromotive force (emf) measurements of the Cell Pt(s), H2(g)|ACES(m1) + NaACES(m2) + NaCl (m3)| AgCl, Ag(s) have been carried out from 5°C to 55°C . The agreement of pH values between two calculated (extended Debye-Hückel and liquid junction correction) is very good. Two buffer solutions without the chloride ion and seven buffer solutions with NaCl, at an ionic strength (I = 0.16 mol.kg-1) similar to that of physiological fluids, have been studied. The pH values for these buffer solutions have been evaluated in the temperature range of 5°C to 55°C using the extended Debye-Hückel equation of the Bates-Guggenheim convention. Values of the residual liquid junction potential (δEj) between the ACES solutions and the saturated KCl calomel electrode solution have been estimated at 25°C and 37°C from the previously determined Ej values using the flowing junction cell to determine the operational pH values at 25°C and 37°C. These ACES buffer solutions are recommended as secondary standard reference solutions for pH measurements in the range of physiological applicati on at I = 0.16 mol.kg-1.

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B. Bodendorfer, Z. Downs, I. Henson, L. Roy, R. Roy, J. Stegner, J. Veliz and J. Wollen, "Buffer Standards for Physiological pH of the Buffer N-(2-Acetamido)-2-aminoethanesulfonic Acid from 5°C to 55°C," Open Journal of Physical Chemistry, Vol. 1 No. 3, 2011, pp. 118-123. doi: 10.4236/ojpc.2011.13016.

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, 1980, pp. 300-310. doi:10.1016/0003-2697(80)90079-2
[3] R. N. Roy, J. Bice, J. Greer, J. A. Carlsten, J. Smithson, W. S. Good, L. N. Roy and K. M. Kuhler, “Buffers for the Physiological pH Range: Acidic Dissociation Constants of Zwitterionic Compounds (ACES and CHES) in Water from 5?C to 55?C,” Journal of Chemical & Engineering Data, Vol. 42, No. 1, 1997, pp. 41-44. doi:10.1021/je960279s
[4] 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, 1961, pp. 267-270.
[5] R. A. Durst and B. R. Staples, “Tris/Tris HCl: Standard Buffer for Use in the Physiological pH Range,” Clinical Chemistry, Vol. 18, 1972, pp. 206-208.
[6] 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, No. 13, 1989, pp. 1400-1405. doi:10.1021/ac00188a019
[7] 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, No. 8, 1993, pp. 1084-1087. doi:10.1021/ac00056a023
[8] 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-Morpho- lino)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
[9] R. G. Bates, C. A. Vega and D. R. White Jr., “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
[10] R. G. Bates, “Determination of pH,” 2nd Edition, Wiley & Sons, New York, 1973.
[11] 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-Di methyl-2-hydroxymethyl)-amino]-2-hydroxypropanesulfonic Acid from 278.15 to 328.15 K,” Journal of Chemical & Engineering Data, Vol. 54, 2009, pp. 428-435.
[12] L. N. Roy, R. N. Roy, C. E. Denton, S. R. LeNoue, C. N. Roy, S. Ashkenazi, T. B. Williams, D. R. Church, M. S. Fuge and K. N. Sreepada, “Second Dissociation Constant of Bis-[(2-hydroxyethyl)amino]acetic Acid (BICINE) and pH of Its Buffer Solutions from 5?C - 55?C,” Journal of Solution Chemistry, Vol. 35, No. 4, 2006, pp. 605-624. doi:10.1007/s10953-005-9009-6
[13] 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-ethanesulfonic Acid (HEPES) for I = 0.16 mol?kg–1 from 5?C to 55?C,” Journal of Solution Chemistry, Vol. 38, No. 4, 2009, pp. 449-458. doi:10.1007/s10953-009-9378-3
[14] W. M. Latimer, “Oxidation Potentials,” 2nd Edition, Prentice-Hall, New York, 1952.
[15] 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, 1976, pp. 1293-1296.
[16] R. G. Bates and E. A. Guggenheim, “Report on the Standardization of pH and Related Terminology,” Pure and Applied Chemistry, Vol. 1, 1960, pp. 163-168. doi:10.1351/pac196001010163
[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] M. I. A. Ferra, “A Pitzer Theory Approach to Assignment of pH to Standard Buffer Solutions,” Electrochimica Acta, Vol. 16, 1998, pp. 133-142.

  
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