The Relation between the Rate of Production of Gastric Juice and its Electrolyte Concentrations

1970 ◽  
Vol 39 (1) ◽  
pp. 61-75 ◽  
Author(s):  
M. Hobsley ◽  
W. Silen
Keyword(s):  
Linear Relationship ◽  
Gastric Juice ◽  
Chloride Ion ◽  
Hydrogen Ion ◽  
Ion Concentration ◽  
Hydrogen Ion Concentration ◽  
Acid Component ◽  
Volume Rate ◽  
Fixed Composition ◽  
Analytical Errors

1. Repeated 15-min collections of gastric juice were made during the plateau of response to an intravenous infusion of histamine diphosphate 0·01 mg h−1 kg−1 and the samples measured and their electrolyte concentrations estimated. A linear relationship was found between chloride output and the volume-rate of overall secretion and between hydrogen ion output and the same rate of secretion, while a multivariate linear relationship was also found between all three variables. 2. A mathematical analysis of these results suggests that if gastric secretion consists of an acid and a non-acid component, each of fixed composition, then the acid component has the composition H = 143 mEq/l, K = 16 mEq/l, Cl = 169 mEq/l, and the non-acid component is secreted at the same rate in different subjects under these circumstances. 3. The data enable gross sampling and analytical errors to be detected; in particular, the volume-rate of secretion can be predicted from hydrogen ion concentration, better from chloride ion concentration, and best from the concentrations of both ions. 4. For single samples such predictions appear to be superior to the direct measurement of volume.

THE ELECTRODE POTENTIAL OF IRON IN RELATION TO HYDROGEN ION CONCENTRATION

1936 ◽  
Vol 14b (1) ◽  
pp. 31-40 ◽  
Author(s):  
J. W. Shipley ◽  
J. H. Shipley
Keyword(s):  
Electrode Potential ◽  
Chloride Ion ◽  
Hydrogen Ion ◽  
Ion Concentration ◽  
Iron Electrode ◽  
General Corrosion ◽  
Citrate Buffer ◽  
Hydrogen Ion Concentration ◽  
Electrically Conducting ◽  
Ph Values

The electrode potential of iron immersed in phosphate, borate and citrate buffers of varying hydrogen ion concentration was measured, using a normal calomel electrode as the second half of the cell. Breaks in the potential of the iron electrode amounting to as much as 0.7 volts were found to occur at definite pH values for each series of buffers. The electrode exhibited an "initial" and "final" potential depending on the pH of the electrolyte and the time of immersion, the "final" value requiring several days to become established. The "final" break in the electrode potential of 0.74 volts in the pure phosphate buffer occurred between a pH of 3.1 and 4.0, that in the pure borate buffer, of 0.75 volts, occurred between a pH of 4.3 and 4.6, and in the pure citrate buffer, of 0.77 volts, between a pH of 10.1 and 10.9. The effect of chloride ion and de-aeration on the electrode potential was observed. It is suggested that the potential of the iron electrode is determined by the presence or absence of a non electrically conducting film or deposit on the iron, the formation of which is a function of the nature of the electrolyte and its hydrogen ion concentration. De-aeration apparently had no effect on the electrode potential, but the presence of chloride ion affected the establishing of the "final" potential and caused the break in voltage to appear irregularly at a much lower hydrogen ion concentration.At pH values below that at which the break in potential occurred, corrosion of the iron electrode was marked, and the electrode potential remained high, while, at pH values above the break, corrosion was virtually inhibited or confined to local spots on the electrode, and the electrode potential remained low. The presence of the chloride ion stimulated local corrosion and permitted general corrosion to proceed at a lower hydrogen ion concentration.

THE MECHANISM OF THE ALCOHOLYSIS OF ALIPHATIC NITRITES: II. ACID-CATALYZED ALCOHOLYSIS OF 1-METHYLHEPTYL NITRITE

1961 ◽  
Vol 39 (4) ◽  
pp. 947-953 ◽  
Author(s):  
A. D. Allen ◽  
G. R. Schonbaum
Keyword(s):  
Reaction Rate ◽  
Chloride Ion ◽  
Hydrogen Ion ◽  
Ion Concentration ◽  
Lithium Salts ◽  
Hydrogen Ion Concentration ◽  
First Order ◽  
Low Concentrations ◽  
Acid Catalyzed ◽  
Asymmetric Carbon

The acid-catalyzed alcoholysis of 1-methylheptyl nitrite has been studied kinetically. The reaction rate is first order with respect to both the nitrite and the hydrogen ion concentration, and the reaction does not involve the asymmetric carbon center. Addition of lithium salts (chloride and perchlorate) indicates catalysis by chloride ion. Addition of water in low concentrations inhibits the reaction strongly. These results and the mechanism of the reactions are discussed in terms of the properties of the alcohols and the dissociation of the acid catalysts in the alcohols used.

Effect of acute changes in the PaCO2 on acid–base parameters in normal dogs and dogs with metabolic acidosis or alkalosis

1983 ◽  
Vol 61 (2) ◽  
pp. 166-173 ◽  
Author(s):  
M. Bercovici ◽  
C. B. Chen ◽  
M. B. Goldstein ◽  
B. J. Steinbaugh ◽  
M. L. Halperin
Keyword(s):  
Metabolic Acidosis ◽  
Linear Relationship ◽  
Regression Line ◽  
Hydrogen Ion ◽  
Ion Concentration ◽  
Hydrogen Ion Concentration ◽  
Gastrointestinal Fluid ◽  
Wide Range ◽  
State Formula ◽  
Acute Changes

There is a linear relationship between the [Formula: see text] and blood hydrogen ion concentration in normal dogs, but for theoretical reasons to be discussed, we questioned whether this relationship would apply in animals with metabolic acidosis or alkalosis. To study this in more detail, animals were divided into three groups: normal, metabolically acidotic, and metabolically alkalotic. Following anesthesia and bilateral ureteral ligation, dogs were intubated and ventilated to produce acute steady-state [Formula: see text] values corresponding to the range observed during disease states. Changes in the volume and electrolyte composition of the gastrointestinal fluid and urine as well as the concentration and distribution of lactate were evaluated in all experiments. We observed the previously described linear relationship between the [Formula: see text] and blood hydrogen ion concentration in normal dogs, but the slope of the regression line differed significantly from those of dogs with metabolic acidosis and metabolic alkalosis. On the other hand, there was a consistent relationship between the ratio of the [Formula: see text] values, but not the absolute [Formula: see text], and the change in the plasma bicarbonate concentration over a wide range of [Formula: see text] values in all groups of dogs. The chemical basis for these observations will be discussed.

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