Abstract
pH is one of the fundamental physiological variables. In fact, serious illness is usually associated with deviations of blood pH only a few tenths from the normal value, 7.4. It is very unlikely that the effects of abnormal pH result from the destructive chemical action of protons or hydroxide; if this were the case, a blood pH of 6.8, say, would not be dangerous. It is more likely that the sensitivity of organisms to pH results chiefly from the influence of pH upon the stability and reactivity of the many biomolecules that possess acidic and basic chemical groups. If this is correct, then the ill effects of abnormal pH values should become substantial for pH changes that correspond to free energy changes equal to the thermal energy, ~ RT. Given that ΔΔG = ωpH(RT/loge) = ΔpH(RT/0.43) [1], the critical pH change should be about 0.4. In fact, this defines quite well the range of blood pH values that are tolerable to humans.
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Gilson, M.K. (1997). Modeling protonation equilibria in biomolecules. In: van Gunsteren, W.F., Weiner, P.K., Wilkinson, A.J. (eds) Computer Simulation of Biomolecular Systems. Computer Simulations of Biomolecular Systems, vol 3. Springer, Dordrecht. https://doi.org/10.1007/978-94-017-1120-3_7
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