Temperature-induced changes in blood acid-base status: Donnan rCl and red cell volume.

The Donnan ratio for chloride ion (rCl) was determined for human red cells in plasma utilizing 36Cl. The effect of altered PCO2 and pH on rCl was followed in two ways. CO2 partial pressure was varied (1-1.5% CO2 in O2; pH range 7.1-7.9) at 37.5 degrees C (isothermal); PCO2 and pH were also changed by altering temperature (range 5-45 degrees C) at constant CO2 content (temperature induced). At pH 7.4 and 37.5 degrees C, rCl was 0.631 +/- 0.0269 (SE, N = 5); isothermal drcl/dpH = -0.306 +/- 0.0234. When measured under conditions of variable temperature at constant CO2 content (pH range 7.3-7.9), drcl/dpH = .018 +/- 0.0232, significantly different from isothermal response (P less than 0.001). Hematocrit (H) changes with pH for conditions of initial H(7.4) of 0.45, under these conditions were also determined: isothermal dH/dpH = -0.031 +/- 0.0019; temperature induced, -0.004 +/- 0.0009. Temperature change alone at constant carbon dioxide content produces no significant change in distribution of chloride ions or water between erythrocyte and plasma compartments.     

Thermodynamics of ribonuclease T1 denaturation.

Differential scanning calorimetry has been used to investigate the thermodynamics of denaturation of ribonuclease T1 as a function of pH over the pH range 2-10, and as a function of NaCl and MgCl2 concentration. At pH 7 in 30 mM PIPES buffer, the thermodynamic parameters are as follows: melting temperature, T1/2 = 48.9 +/- 0.1 degrees C; enthalpy change, delta H = 95.5 +/- 0.9 kcal mol-1; heat capacity change, delta Cp = 1.59 kcal mol-1 K-1; free energy change at 25 degrees C, delta G degrees (25 degrees C) = 5.6 kcal mol-1. Both T1/2 = 56.5 degrees C and delta H = 106.1 kcal mol-1 are maximal near pH 5. The conformational stability of ribonuclease T1 is increased by 3.0 kcal/mol in the presence of 0.6 M NaCl or 0.3 M MgCl2. This stabilization results mainly from the preferential binding of cations to the folded conformation of the protein. The estimates of the conformational stability of ribonuclease T1 from differential scanning calorimetry are shown to be in remarkably good agreement with estimates derived from an analysis of urea denaturation curves.     

Human whole-blood O2 affinity: effect of CO2

The proton Bohr factor (phi H = alpha log PO2/alpha pH), the carbamate Bohr factor (phi C = alpha log PO2/alpha log PCO2), the total Bohr factor (phi HC = d log PO2/dpH[base excess) and the CO2 buffer factor (d log PCO2/dpH) were determined in the blood of 12 healthy donors over the whole O2 saturation (SO2) range. All three Bohr factors proved to be dependent on SO2, although to a lesser extent than reported in some of the recent literature. At SO2 = 50% and 37 degrees C, we found phi H = -0.428 +/- 0.010 (SE), phi C = 0.054 +/- 0.006, and phi HC = -0.488 +/- 0.007. The values obtained for phi H, phi C, and d log PCO2/dpH were used to calculate phi HC. Calculated and measured values of phi HC proved to be in good agreement. In an additional series of 12 specimens of human blood we determined the influence of PCO2 on phi H and the influence of pH on phi C. At SO2 = 50%, phi H varied from -0.49 +/- 0.009 at PCO2 = 15 Torr to -0.31 +/- 0.010 at PCO2 = 105 Torr and phi C from 0.157 +/- 0.015 at pH = 7.80 to 0.006 +/- 0.009 at pH = 7.00. When on the basis of these data a second-order term is taken into account, a still slightly better agreement between measured and calculated values of phi HC can be attained.     

Hemoglobins of the tadpole of the bullfrog, Rana catesbeiana. Temperature dependence of oxygen binding and pH dependence of subunit dissociation.

The temperature dependence of the oxygen equilibrium of tadpole hemoglobin has been determined between 0 degrees and 32 degrees for the unfractionated but phosphate-free lysate and between 12 degrees and 32 degrees for each of the four isolated components between pH 6 and 10 in 0.05 M cacodylate, Tris, or glycine buffers containing 0.1 M NaCl and 1 mM EDTA. Under these conditions the Bohr effect (defined as deltalog p50/deltapH) of the unfractionated lysate is positive at low temperatures between pH 6 and 8.5 and is negative above pH 8.5 to 8.8 at any temperature. As the temperature rises the Bohr effect below pH 8.5 changes greatly. In the interval pH 7.0 to 7.5, the magnitude of the Bohr effect decreases from + 0.28 at 0 degrees to zero at about 24 degrees and becomes negative, as in mammalian hemoglobins, above this temperature. Measurements with the isolated components show that the temperature dependence of oxygen binding for Components I and II and for Components III and IV is very similar. For both sets of components the apparent overall enthalpy of oxygenation at pH 7.5 is about -16.4 kcal/mol and -12.6 kcal/mol at pH 9.5. The measured enthalpies include contributions from the active Bohr groups, the buffer ions themselves, the hemoglobin groups contributing buffering, and any pH-dependent, oxygenation-dependent binding of ions such as chloride by the hemoglobin. The apportioning of the total enthalpy among these various processes remains to be determined. Between pH 8 and 10.5 tadpole oxyhemoglobin undergoes a pH-dependent dissociation from tetramer to dimer. The pH dependence of the apparent tetramer-dimer dissociation constant indicates that at pH 9.5 the dissociation of each tetramer is accompanied by the release of approximately 2 protons. In this pH range the oxygen equilibrium measurements indicate that about 0.5 proton is released for each oxygen molecule bound. The results are consistent with the conclusion that one acid group per alphabeta dimer changes its pK from about 10 to 8 or below upon dissociation of the tetramer.     

Thermodynamics of complex formation between nicotinamide adenine dinucleotide and pig skeletal muscle lactate dehydrogenase.

Formation of the binary complex between the reduced coenzyme nicotinamide adenine dinucleotide (NADH) and pig skeletal muscle lactate dehydrogenase (LDH, EC 1.1.1.27) has been investigated by calorimetric and equilibrium dialysis techniques in 0.2 M potassium phosphate buffer (pH 7.0) at various temperatures. Analysis of thermal titration curves at two temperatures (25 and 31.5 degrees) shows that the experimental enthalpy data can be rationalized assuming four independent and equivalent binding sites for the tetrameric enzyme. Binary complex formation is characterized by a negative temperature coefficient, delta cp, of the binding enthalpy, which amounts to -1300 plus or minus 53 cal/(deg mol of LDH) in the temperature range of 5-31.5 degrees. Despite the slightly smaller standard deviation resulting when polynomial regression analysis of the second degree is applied to the temperature dependence of the enthalpy values, binding enthalpies seem to be adequately represented in the temperature range studied by the equation delta H = -1.3T + 2.3, kcal/mol of LDH, T referring to the temperature in degrees C. By combination of the results obtained from equilibrium dialysis and calorimetric studies a set of apparent thermodynamic parameters for binding of NADH to LDH in 0.2 M potassium phosphate buffer at pH 7 has been established.     

An electrolytic method for determining oxygen dissociation curves using small blood samples: the effect of temperature on trout and human blood.

1. A detailed account is given of an electrolytic method for determining the oxygen dissociation curve of fish blood using a single sample of 50-100 mul for the whole curve. The accuracy and some of the problems arising from its uses are discussed. 2. Oxygen dissociation curves have been determined for trout blood and human blood at temperatures of 15 and 37 degrees C. The relationship between P50 and temperature is similar to that obtained using other methods. Absolute values of P50 are generally lower than those obtained by other methods, especially in the case of fish blood. 3. The effect of PCO2 and pH on the oxygen dissociation curve of trout blood is tested and it is shown that PCO2 has a more marked effect than pH when the other factor is maintained at a constant level. The Bohr factor (delta log P50/delta pH) appears to be approximately the same and independent of the PCO2. 4.The P50 of ray blood determined from fish during and after an operation showed an increased Bohr factor.     

Blood acid-base status, whole blood and whole body buffer values in sand rats (Psammomys obesus) exposed to hypercapnia

Arterial blood acid-base status of unanesthetized sand rats (Psammomys obesus) were studied under normocapnic and hypercapnic conditions, and compared to those obtained for the albino rat (Rattus norvegicus). The average control blood pH: 7.396 +/- 0.034; PaCO2: 30.5 +/- 2.9 mmHg; HCO-3: 18.8 +/- 2.5 mM/l; and HCO-3 std: 20.9 +/- 2.1 (N = 15) obtained here for the sand rat are in the lower range of values found in other mammals and indicate a status of partially compensated metabolic acidosis. The blood buffer values of the sand rat, delta log PCO2/delta pH = -2.32 +/- 0.35 (N = 25) are significantly higher than those found here for the rat, delta log PCO2/delta pH = -1.51 +/- 0.10 (N = 39), and those reported for other mammals. This high blood buffer value may be related to the natural high mineral diet of the sand rat. The in vivo (whole body) buffer value delta log PaCO2/delta pH = -1.41 and -1.65 for the sand rat and the rat found here are higher than those reported for the man and dog and may represent a physiological adaptation to the hypercapnic conditions prevailing in underground burrows.     

Blood osmolality in vitro: dependence on base addition, buffer value, and temperature

Blood osmolality (Osm) increases with PCO2 because of CO2 absorption. The influences of NaOH addition, equilibration temperature, and hemoglobin concentration on these respiratory changes of Osm were measured by freezing-point determination in true plasma. Addition of NaOH increases Osm by 2 mosmol X kg H2O-1 X mmol base-1 X l at constant PCO2 due to the osmotic effects of Na+ and produced bicarbonate. Respiratory compensation of the pH change further increases Osm. This contrasts to the respiratory compensation of the osmolar disturbance caused by fixed acid. Raising the equilibration temperature reduces Osm by 0.5 mosmol X kg H2O-1 X degrees C-1 at constant pH mainly caused by a lower absorption coefficient for CO2 and changed pK value for H2CO3. The slope of the linear regression lines between Osm and pH during CO2 equilibration increases with hemoglobin; the value of the quotient delta Osm/delta pH depends directly on the nonbicarbonate buffer value. The use of this quotient for the estimation of the mean nonbicarbonate buffer value of the whole body is suggested. The osmotic effects of therapeutic base infusion should be regarded with caution.     

Effects of magnesium and calcium on the oxygenation reaction of erythrocruorin from the marine polychaete Arenicola marina and the terrestrial oligochaete Lumbricus terrestris

Oxygenation function of annelid erythrocruorin (Er) is affected by Mg and Ca concentration in the blood. Four classes of responses may be encountered in different species: 1) Mg=Ca (equal effects), 2) Mg>Ca, 3) Mg相似文献   

Properties of ATP-driven reverse electron flow in chloroplasts.

1. The reverse reactions induced by coupled ATP hydrolysis were studied in spinach chloroplasts by measurements of the ATP-induced increase in chlorophyll fluorescence reflecting reverse electron flow, and of the ATP-induced decrease in 9-aminoacridine fluorescence, representing formation of the transthylakoidal proton gradient (deltapH). ATP-induced reverse electron flow was kinetically analysed into three phases, of which only the second and third one were paralleled by corresponding phases in deltapH formation. The rapid first phase and formation of a deltapH occur also in the absence of the electron transfer mediator phenazine methosulfate. 2. The rate and extent of the reverse reactions were measured at temperatures in the range from 0 to 30 degrees C. The rate of formation of delta pH and of reverse electron flow were faster at high temperatures, but the maximal extent of delta pH and chlorophyll fluorescence increase were observed at the lowest temperature. Considering rate and extent of the ATP-stimulated reactions, a temperature optimum around 15 degrees C was found. Light activation of the ATPase occurred throughout the range studied. At 0 degrees C and in the presence of inorganic phosphate the activated state for ATPase was maintained for more than 10 min. 3. The ATP-induced rise in chlorophyll fluorescence yield was found to be of similar magnitude as the rise induced by 3-(3,4-dichlorophenyl)-1,1-dimethyl-urea (DCMU), when both were measured with an extremely weak measuring beam. It is concluded, that both effects, although derived via distinctly different pathways, are limited by the same electron donating or electron accepting pool.     

Thermodynamics of phospholipid bilayer assembly

Thermodynamic properties of bilayer assembly have been obtained from measurements of the solubility of the sodium salt of dimyristoylphosphatidylglycerol (DMPG) in water. The standard free energy of bilayer assembly delta G degree a is shown to be RT 1n Xs + zF psi 0 where Xs is the mole fraction of dissolved lipid, F is the Faraday constant, z is the valence of the counterion (Na+), and psi 0 is the electrical double-layer potential of the ionized bilayer. The function d 1n Xs/dT was found to be discontinuous at 24 degrees C, the gel-liquid-crystal transition temperature (Tm) for DMPG. This function was unaffected when solubilities were measured in 0.001 M NaCl solutions; thus, psi 0 is constant in the experimental temperature interval (4-40 degrees C). Using a value of psi 0 = -180 mV [Eisenberg et al. (1979) Biochemistry 18, 5213-5223], and the temperature dependence of delta G degrees a, values for delta H degrees a and delta S degree a at 24 degrees C were calculated for the gel and liquid-crystal states of DMPG. For the gel, delta H degrees a and T delta S a are -26.2 and 12.7 kcal/mol, respectively; for the liquid-crystal, delta H degrees a and T delta S degrees a are -19.2 and -5.7 kcal/mol, respectively. The calculated value for the latent heat of the gel-liquid-crystal transition is 7 kcal/mol, in agreement with calorimetric measurements.     

Temperature jump as a new technique to study the kinetics of fast transport of protons across membranes

Application of a temperature jump (2.5 degrees C) to a suspension of liposomes, having phosphate (delta pK/delta T approximately 0.005) as the internal buffer and tris(hydroxymethyl)aminomethane (delta pK/delta T approximately 0.031) as the external buffer, created a delta pH (pHin - pHout) of positive sign in ca. 5 microseconds. Decay of this delta pH was monitored by using the fluorescent pH indicator 8-hydroxy-1,3,6-pyrenetrisulfonic acid entrapped inside the liposome. This technique is useful to study transmembrane proton movement in the time range 5 microseconds-10 s at physiological pH values. The kinetics of proton transport aided by ion carriers such as nigericin, monensin, carbonyl cyanide m-chlorophenylhydrazone (CCCP), and valinomycin were studied by our method. The electrogenic nature of transport by CCCP and valinomycin and electroneutral ion transport by nigericin and monensin were shown. From the kinetics of proton transport aided by gramicidin, the time-averaged single-channel conductance of gramicidin channels was estimated to be (2.1 +/- 0.5) X 10(-16) S for H+ at pH 7.5.     

Stability mutants of staphylococcal nuclease: large compensating enthalpy-entropy changes for the reversible denaturation reaction

By use of intrinsic fluorescence to determine the apparent equilibrium constant Kapp as a function of temperature, the midpoint temperature Tm and apparent enthalpy change delta Happ on reversible thermal denaturation have been determined over a range of pH values for wild-type staphylococcal nuclease and six mutant forms. For wild-type nuclease at pH 7.0, a Tm of 53.3 +/- 0.2 degrees C and a delta Happ of 86.8 +/- 1.4 kcal/mol were obtained, in reasonable agreement with values determined calorimetrically, 52.8 degrees C and 96 +/- 2 kcal/mol. The heat capacity change on denaturation delta Cp was estimated at 1.8 kcal/(mol K) versus the calorimetric value of 2.2 kcal/(mol K). When values of delta Happ and delta Sapp for a series of mutant nucleases that exhibit markedly altered denaturation behavior with guanidine hydrochloride and urea were compared at the same temperature, compensating changes in enthalpy and entropy were observed that greatly reduce the overall effect of the mutations on the free energy of denaturation. In addition, a correlation was found between the estimated delta Cp for the mutant proteins and the d(delta Gapp)/dC for guanidine hydrochloride denaturation. It is proposed that both the enthalpy/entropy compensation and this correlation between two seemingly unrelated denaturation parameters are consequences of large changes in the solvation of the denatured state that result from the mutant amino acid substitutions.     

An investigation of the equilibria between aqueous ribose, ribulose, and arabinose

The thermodynamics of the equilibria between aqueous ribose, ribulose, and arabinose were investigated using high-pressure liquid chromatography and microcalorimetry. The reactions were carried out in aqueous phosphate buffer over the pH range 6.8-7.4 and over the temperature range 313.15-343.75 K using solubilized glucose isomerase with either Mg(NO3)2 or MgSO4 as cofactors. The equilibrium constants (K) and the standard state Gibbs energy (delta G degrees) and enthalpy (delta H degrees) changes at 298.15 K for the three equilibria investigated were found to be: ribose(aq) = ribulose(aq) K = 0.317, delta G degrees = 2.85 +/- 0.14 kJ mol-1, delta H degrees = 11.0 +/- 1.5 kJ mol-1; ribose(aq) = arabinose(aq) K = 4.00, delta G degrees = -3.44 +/- 0.30 kJ mol-1, delta H degrees = -9.8 +/- 3.0 kJ mol-1; ribulose(aq) = arabinose(aq) K = 12.6, delta G degrees = -6.29 +/- 0.34 kJ mol-1, delta H degrees = -20.75 +/- 3.4 kJ mol-1. Information on rates of the above reactions was also obtained. The temperature dependencies of the equilibrium constants are conveniently expressed as R in K = -delta G degrees 298.15/298.15 + delta H degrees 298.15[(1/298.15)-(1/T)] where R is the gas constant (8.31441 J mol-1 K-1) and T the thermodynamic temperature.     

Inhibition of lactate and malate dehydrogenase by dyes containing vinylsulfone and chlorotriazine groups

The difference spectra of lactate and malate dehydrogenase complexes with four native dyes containing vinylsulfonic and triazinic groups (light-resistant yellow 2KT, red-violet 2KT, etc.) were monitored in 0.1 M phosphate buffer pH 8.2 at 20 degrees C. The dissociation constants were calculated from the spectral data. The most stable complexes were lactate dehydrogenase--light-resistant yellow 2KT and malate dehydrogenase--light-resistant yellow 2KT ones. The values of delta H degree = 5.75 kcal/mole and standard thermodynamic parameters, delta G degree = -6.5 kcal/mole and delta S degree = 41.2 e. u., were calculated from the values of association constants for temperature dependence. The thermodynamic characteristics confirmed the key role of hydrophobic interactions in lactate dehydrogenase--reactive dye complex formation. All the dyes under study competitively inhibit lactate and malate oxidation by the corresponding dehydrogenases. The inhibition constants of both enzymes by the four dyes were determined at 20 degrees C in 0.1 M phosphate buffer pH 8.2. Light-resistant yellow 2KT appeared to be the most effective inhibitor of the enzymes.     

Counteracting osmolyte trimethylamine N-oxide destabilizes proteins at pH below its pKa. Measurements of thermodynamic parameters of proteins in the presence and absence of trimethylamine N-oxide

Earlier studies have reported that trimethylamine N-oxide (TMAO), a naturally occurring osmolyte, is a universal stabilizer of proteins because it folds unstructured proteins and counteracts the deleterious effects of urea and salts on the structure and function of proteins. This conclusion has been reached from the studies of the effect of TMAO on proteins in the pH range 6.0-8.0. In this pH range TMAO is almost neutral (zwitterionic form), for it has a pK(a) of 4.66 +/- 0.10. We have asked the question of whether the effect of TMAO on protein stability is pH-dependent. To answer this question we have carried out thermal denaturation studies of lysozyme, ribonuclease-A, and apo-alpha-lactalbumin in the presence of various TMAO concentrations at different pH values above and below the pK(a) of TMAO. The main conclusion of this study is that near room temperature TMAO destabilizes proteins at pH values below its pK(a), whereas it stabilizes proteins at pH values above its pK(a). This conclusion was reached by determining the T(m) (midpoint of denaturation), delta H(m) (denaturational enthalpy change at T(m)), delta C(p) (constant pressure heat capacity change), and delta G(D) degrees (denaturational Gibbs energy change at 25 degrees C) of proteins in the presence of different TMAO concentrations. Other conclusions of this study are that T(m) and delta G(D) degrees depend on TMAO concentration at each pH value and that delta H(m) and the delta C(p) are not significantly changed in presence of TMAO.     

The electrochemical proton gradient in Escherichia coli membrane vesicles.

Membrane vesicles isolated from Escherichia coli grown under various conditions generate a transmembrane pH gradient (delta pH) of about 2 pH units (interior alkaline) under appropriate conditions when assayed by flow dialysis. Using the distribution of weak acids to measure delta pH and the distribution of the lipophilic cation triphenylmethylphosphonium to measure the electrical potential (delta psi) across the membrane, the vesicles are demonstrated to develop an electrochemical proton gradient (delta-muH+) of almost - 200 mV (interior negative and alkaline) at pH 5.5 in the presence of reduced phenazine methosulfate or D-lactate, the major component of which is a deltapH of about - 120 mV. As external pH is increased, deltapH decreases, reaching 0 at about pH 7.5 and above, while delta psi remains at about - 75 mV and internal pH remains at pH 7.5-7.8. The variations in deltapH correlate with changes in the oxidation of reduced phenazine methosulfate or D-lactate, both of which vary with external pH in a manner similar to that described for deltapH. Finally, deltapH and delta psi can be varied reciprocally in the presence of valinomycin and nigericin with little change in delta-muH+ and no change in respiratory activity. These data and those presented in the following paper (Ramos and Kaback 1976) provide strong support for the role of chemiosmotic phenomena in active transport and extend certain aspects of the chemiosmotic hypothesis.     

Thermodynamics of the conversion of fumarate to L-(-)-malate

The thermodynamics of the conversion of aqueous fumarate to L-(-)-malate has been investigated using both heat conduction microcalorimetry and a gas chromatographic method for determining equilibrium constants. The reaction was carried out in aqueous Tris-HCl buffer over the pH range 6.3-8.0, the temperature range 25-47 degrees C, and at ionic strengths varying from 0.0005 to 0.62 mol kg-1. Measured enthalpies and equilibrium ratios have been adjusted to zero ionic strength and corrected for ionization effects to obtain the following standard state values for the conversion of aqueous fumarate 2- to malate 2- at 25 degrees C: K = 4.20 +/- 0.05, delta G degrees = -3557 +/- 30 J mol-1, delta H degrees = -15670 +/- 150 J mol-1, and delta C degrees p = -36 +/- J mol-1 K-1. Equations are given which allow one to calculate the combined effects of pH and temperature on equilibrium constants and enthalpies of this reaction.     

Binding of the bovine and porcine pancreatic secretory trypsin inhibitor (Kazal) to human leukocyte elastase: a thermodynamic study.

The effect of pH and temperature on the apparent association equilibrium constant (Ka) for the binding of the bovine and porcine pancreatic secretory trypsin inhibitor (Kazal-type inhibitor, PSTI) to human leukocyte elastase has been investigated. At pH 8.0, values of the apparent thermodynamic parameters for human leukocyte elastase: Kazal-type inhibitor complex formation are: bovine PSTI--Ka = 6.3 x 10(4) M-1, delta G degree = -26.9 kJ/mol, delta H degree = +11.7 kJ/mol, and delta S degree = +1.3 x 10(2) entropy units; porcine PSTI--Ka = 7.0 x 10(3) M-1, delta G degree = -21.5 kJ/mol, delta H degree = +13.0 kJ/mol, and delta S degree = +1.2 x 10(2) entropy units (values of Ka, delta G degree and delta S degree were obtained at 21.0 degrees C; values of delta H degree were temperature independent over the range (between 5.0 degrees C and 45.0 degrees C) explored). On increasing the pH from 4.5 to 9.5, values of Ka for bovine and porcine PSTI binding to human leukocyte elastase increase thus reflecting the acidic pK-shift of the His57 catalytic residue from congruent to 7.0, in the free enzyme, to congruent to 5.1, in the serine proteinase: inhibitor complexes. Thermodynamics of bovine and porcine PSTI binding to human leukocyte elastase has been analyzed in parallel with that of related serine (pro)enzyme/Kazal-type inhibitor systems. Considering the known molecular models, the observed binding behaviour of bovine and porcine PSTI to human leukocyte elastase was related to the inferred stereochemistry of the serine proteinase/inhibitor contact region(s).     

Blood osmolality during in vivo changes of CO2 pressure

In 16 experiments male subjects, age 22.4 +/- 0.5 (SE) yr, inspired CO2 for 15 min (8% end-tidal CO2) or hyperventilated for 30 min (2.5% end-tidal CO2). Osmolality (Osm) and acid-base status of arterialized venous blood were determined at short intervals until 30 min after hypo- and hypercapnia, respectively. During hypocapnia [CO2 partial pressure (PCO2) -2.31 +/- 0.32 kPa (-17.4 Torr), pH + 0.19 units], Osm decreased by 3.9 +/- 0.3 mosmol/kg H2O; during hypercapnia [PCO2 + 2.10 +/- 0.28 kPa (+15.8 Torr), pH -0.12 units], Osm increased by 5.8 +/- 0.7 mosmol/kg H2O. Presentation of the data in Osm-PCO2 or Osm-pH diagrams yields hysteresis loops probably caused by exchange between blood and tissues. The dependence of Osm on PCO2 must result mainly from CO2 buffering and therefore from the formation of bicarbonate. In spite of the different buffer capacities in various body compartments, water exchange allows rapid restoration of osmotic equilibrium throughout the organism. Thus delta Osm/delta pH during a PCO2 jump largely depends on the mean buffer capacity of the whole body. The high estimated buffer value during hypercapnia (38 mmol/kg H2O) compared with hypocapnia (19 mmol/kg H2O) seems to result from very strong muscle buffering during moderate acidosis.