1957
DOI: 10.3109/00365515709101210
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Standard Bicarbonate, its Clinical Significance, and a new Method for its Determination

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Cited by 137 publications
(42 citation statements)
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“…Titration of a buffer mixture over a narrow range of hydrogen ion concentrations could produce such a pattern; whole blood, for example, yields a straight line relationship over a hydrogen ion concentration as wide as that examined here (20)(21)(22)(23). The sittuation in vivo, however, is more complicated, since bicarbonate is generated not only by buffers in the extracellular fluid but also (and to an even larger extent) by sources outside this compartment (1).…”
Section: Resultsmentioning
confidence: 99%
“…Titration of a buffer mixture over a narrow range of hydrogen ion concentrations could produce such a pattern; whole blood, for example, yields a straight line relationship over a hydrogen ion concentration as wide as that examined here (20)(21)(22)(23). The sittuation in vivo, however, is more complicated, since bicarbonate is generated not only by buffers in the extracellular fluid but also (and to an even larger extent) by sources outside this compartment (1).…”
Section: Resultsmentioning
confidence: 99%
“…WVhole-blood pH, and the pH of separated plasma equilibrated at 380 C with a known CO2 tension (40 mm Hg), were determined at once, using the 'Radiometer' pH meter and Astrup apparatus (Astrup & Schroder, 1956; from these two pH determinations the 'standard' bicarbonate in separated plasma, and the plasma CO2 tension, were calculated as described by Astrup (1956); in three studies arterial oxygen saturation was determined spectrophotometrically (Nahas, 1951). (J0rgensen & Astrup, 1957). Although small increases occurred at variable times during diffusion respiration, the 'standard' bicarbonate concentration did not exceed 24 m-mole/l.…”
Section: R a Millarmentioning
confidence: 99%
“…The form of in vivo titration curves in man and animal are significantly different from those obtained in vitro (Cunningham, et al, 1962;Cohen, et al, 1964;Brackett et al, 1965;Linden &Norman, 1966;Norman, 1969). Alsoit has been shown by in vitro measurements that, whereas the apparent first dissociation constant of carbonic acid (pK') varies inversely with pK (Severinghaus, Stupfel & Bradley, 1956) the in vivo measurements show pK' to vary directly with pH Linden &Norman, 1966;Linden & Norman, 1970). In addition a large significant variation in pK' at any one pH and temperature has been observed in studies on the whole animal (Norman, 1969;Linden & Norman, 1970).…”
Section: H + + B a -E H B Amentioning
confidence: 93%
“…Previous methods of assessing acid-base balance (Singer & Hastings, 1948 ;Davenport, 1958 ;Astrup, Jorgensen, Siggaard Andersen & Engel, 1960;Campbell, 1962;Owen, Dudley & Masterton, 1965) have depended upon the use of the Henderson-Hasselbalch equation linking pH to the molar concentrations of carbonic acid and bicarbonate ions in plasma. It is now appreciated that the constants in this equation cannot be predicted with sufficient accuracy to warrant its use (Linden & Norman, 1966;Trenchard, Noble & Guz, 1967;Norman, 1969;Linden & Norman, unpublished observations). Finally some of the existing concepts (buffer base, standard bicarbonate, base excess and base deficit) which have evolved from studies conducted on blood in vitro are at best misleading and at their worst frankly untenable when applied to changing states within the whole animal.…”
mentioning
confidence: 94%
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