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• W2414250801 abstract "The principles involved in the definition of pH are discussed in relation to the actual procedures used in its measurement. The assumptions made in the operational definition of pH and the existence of a residual liquid junction potential when pH is measured using a glass electrode and calomel electrode result in an uncertainty of ±0.02 in the pH measured. While of small im­ portance in most uses of pH, this uncertainty is of considerable importance when pH is used to calculate the activity or concentration of hydrogen ions, and when it is used in formulae such as the Henderson-Hasselbalch equation. The measurement of pH using a glass electrode-calomel electrode pair is a com­ mon procedure in the clinical laboratory. Recent improvements in the design and construction of these electrodes and of pH meters have permitted the reliable mea­ surement of pH to ±0.002 in the range of pH of *4 to 9. This excellent reproducibility of pH measurements does not necessarily mean, however, that the accuracy of the pH measurement is equally precise. Ac­ cording to Mattock and Band,6 pH cannot be measured with an accuracy better than ±0.02. Bates,1 without quoting a figure, warns that “no quantitative interpretation of measured pH values should be attempted unless the medium can be classified as a dilute aqueous solution of simple solutes.” Blood and most other biological fluids are therefore excluded by this warning. The reasons for this lack of precise quantitative interpretation of pH measurements can be considered under three headings: the defi­ nition of pH; the standardization of pH; the measurement of pH. T he D efin ition o f pH S0rensen introduced the term pH (p standing for Potenz, i.e., power)9 as a de­ vice for the more convenient expression of hydrogen ion concentrations. He defined it as pH = — logi0cH, cH being the molar con­ centration of hydrogen ions. The concept of activity5 had been introduced a little earlier; eventually pH was redefined10 as pH = —log10aH, where an was the activity of hydrogen ions given by one of the formulae a = yc, a = ym, a = fN, c, m and N being respectively the molarity, molality and mole-fraction of hydrogen ions and y, y and f the corresponding activity coefficients. Although this definition was theoretically sound, it was not really useful in practice, as it defined pH in terms of something that could not be measured, namely the activity of a single ionic species. Ions in solution always occur accompanied by ions of the opposite charge, so that the solution is electrically neutral. Thermodynamic theory shows that what is measurable is the mean" @default.
• W2414250801 created "2016-06-24" @default.
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• W2414250801 date "1973-05-01" @default.
• W2414250801 modified "2023-09-23" @default.
• W2414250801 title "The meaning of pH." @default.
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