Low solubility of unconjugated bilirubin in dimethylsulfoxide – water systems: implications for pK a determinations
© Mukerjee et al; licensee BioMed Central Ltd. 2002
Received: 23 April 2002
Accepted: 17 June 2002
Published: 17 June 2002
Aqueous pK a values of unconjugated bilirubin are important determinants of its solubility and transport. Published pK a data on an analog, mesobilirubin-XIIIα, studied by 13C-NMR in buffered solutions containing 27 and 64 vol% (C2H3)2SO because of low aqueous solubility of mesobilirubin, were extrapolated to obtain pK a values in water of 4.2 and 4.9. Previous chloroform-water partition data on bilirubin diacid led to higher estimates of its pK a , 8.12 and 8.44, and its aqueous solubility. A thermodynamic analysis, using this solubility and a published solubility in DMSO, suggested that the systems used to measure 13C-NMR shifts were highly supersaturated. This expectation was assessed by measuring the residual concentrations of bilirubin in the supernatants of comparable DMSO-buffer systems, after mild centrifugation to remove microprecipitates.
Extensive sedimentation was observed from numerous systems, many of which appeared optically clear. The very low supernatant concentrations at the lowest pH values (4.1-5.9) were compatible with the above thermodynamic analysis. Extensive sedimentation and low supernatant concentrations occurred also at pH as high as 7.2.
The present study strongly supports the validity of the aqueous solubility of bilirubin diacid derived from partition data, and, therefore, the corresponding high pK a values. Many of the mesobilirubin systems in the 13C-NMR studies were probably supersaturated, contained microsuspensions, and were not true solutions. This, and previously documented errors in pH determinations that caused serious errors in pK a values of the many soluble reference acids and mesobilirubin, raise doubts regarding the low pK a estimates for mesobilirubin from the 13C-NMR studies.
The saturation status of unconjugated bilirubin (UCB) is relevant to understanding the pathophysiology of jaundice and to interpreting experiments with UCB . UCB, in its diacid form (H2B), has a low solubility (So) of 51 nM in water . The total solubility (S) at any pH is determined by So, pK a values, and pH :
S = [H2B] + [HB-] + [B=] = So·(1 + Ka 1/ [H+] + Ka 1·Ka 2/ [H+]2) (Eq. 1)
Self-association of UCB dianion, B=, can also increase S .
Beginning in 1995, a series of papers reported the use of 13C-NMR to study the ionization of a close analogue of bilirubin-IXα, mesobilirubin-XIIIα (MBR), along with several soluble reference acids, in buffered mixtures of (C2H3)2SO and water [3–7]. Due to the very low aqueous solubility of MBR, data were obtained only at two high concentrations of (C2H3)2SO (64 and 27 vol%). Its pK a values in "water" (actually in 1 vol% of ((C2H3)2SO), obtained by an extrapolation procedure based on the behavior of soluble reference acids, were 4.2 and 4.9, far lower than values of 8.12 and 8.44 obtained by solvent partition between chloroform and buffered aqueous solutions .
These serious discrepancies led us to reexamine several experimental aspects of the 13C-NMR studies and the implications of their purported low pK a values for the solubility of UCB. Inaccuracies in the measurements of buffer pH and of the pK a values of the reference 13C-carboxylic acids, related to failure to correct for the strong effects of DMSO on the pK a values of weak acids, have been previously noted  and acknowledged . In addition, as discussed later, a thermodynamic theory about solubility in mixed solvents, using the So values of 51 nM in water  and 10 mM in pure DMSO , suggested that So of UCB would be only about 0.15 μM in 27 vol% DMSO and 2.2 μM in 64 vol% DMSO, which are well below concentrations used in the MBR studies. This implies serious supersaturation effects. In fact, turbidity was reported for some of the systems used in the 13C-NMR papers , indicating the formation of coarse suspensions. By definition, as stressed in the Conclusions section, pK a determinations are valid only for monomeric species and require that solutions are below saturation at all pH values studied. Even reversible aggregation of monomers in undersaturated solutions is known to affect pK a estimates . If supersaturation leads to the formation of fine sols or coarse suspensions, the data are unacceptable for determination of the pK a values of monomers.
In the present paper, we assess whether some of the systems used in the 13C-NMR studies were supersaturated with MBR. Our experimental work on sedimentation was done with unconjugated bilirubin (UCB) and we used DMSO instead of its deuterated analogue, (C2H3)2SO. It is known that, when alkaline aqueous UCB is acidified to neutral or low pH's, "Usually a colloid suspension of bilirubin is formed and the solution remains clear, as observed by the naked eye, thus inviting an erroneous interpretation" . Such systems, which simulate true solutions, often show sedimentation on centrifugation [12–16]. We here report that sedimentation of UCB from apparently clear solutions can likewise be extensive when UCB in DMSO is diluted with aqueous buffers to final mole fractions (N) of DMSO = 0.025, 0.086 and 0.31, corresponding to 9, 27, and 64 vol% of DMSO. A thermodynamic theory is used to examine the effect of added DMSO on So. Our findings, consistent with our partition-derived So, S and pK a values of UCB in aqueous buffers , indicate that the recently reported low pK a values of MBR in comparable (C2H3)2SO -water systems [3–6], were determined above saturation.
Residual UCB in the supernatants after centrifugation
Many systems initially appeared optically clear, but well over 90% of initial UCB sedimented on centrifugation of most samples below pH 7.2. Overall recoveries (UCB in supernatant + UCB in redissolved precipitate) were between 90 and 100%. Only residual [UCB] in supernatants are reported.
Sedimentation of bilirubin-albumin complexes
The supernatant from the original supersaturated UCB-HSA system, when diluted with 1/8th vol. of buffer and centrifuged again, showed more sedimentation and a progressive rise in [UCB] as one moved down the column of fluid. By contrast, after dilution with 1/8th volume of DMSO to decrease UCB saturation, the supernatants produced no further sedimentation and there were no significant differences in [UCB] or protein concentrations along the axis of the fluid column. Thus, the UCB-HSA complex, which constitutes over 99.9% of the UCB in this system , did not sediment.
Findings and their relation to thermodynamic theory
Supersaturated aqueous systems of UCB, that are optically clear before centrifugation, may exhibit considerable variation in the extent of sedimentation [12–14, 18]. Although sedimentation is often extensive, it is generally incomplete and may not be observed at all. Our data in DMSO-water show the same features, which are expected from the complex kinetics of nucleation and growth of insoluble aggregates of UCB diacid (H2B), leading to the formation of a new solid phase [19, 20]. Our centrifugation, 5 min at 14,000 g, was quite mild, and the short 20-minute period between preparation of UCB-DMSO-water systems and centrifugation severely limited the time-dependent growth to large aggregates. Lack of sedimentation of the UCB-HSA complex (mol. wt. 68,000) indicates that fine colloids composed of 100 UCB molecules would be too small to sediment. Thus, supersaturated systems lacking coarse, insoluble aggregates may not show sedimentation, but any sedimentation observed indicates their presence.
To evaluate the important effect of pH on sedimentation efficiency, we calculated S in water using chloroform-water partition data on UCB and the best measure of So in chloroform, 0.88 mM . S at any pH, e.g. 62 nM at pH 7.4 and 0.32 μM at pH 8.5, can be calculated from the fitted partition data, or, equivalently, from Eq. 1, using the partition-derived So in water of 51 nM and pK a values of 8.12 and 8.44 . In aqueous systems , the lowest [UCB] in water, below which no sedimentation was observed at 100,000 × g for a few hours, was 100 nM at pH 7.4, modestly higher than our partition-derived S of 62 nM . Even under such vigorous centrifugation, the lowest [UCB] increased rapidly with increasing pH, to 17 μM (150 times S) at pH 8.05 and 34 μM (230 times S) at pH 8.2 . This indicates increasing charge-stabilization of fine, non-sedimenting colloids of H2B by adsorbed UCB anions [12, 19, 20]. In contrast, below pH 6.7, sedimentation of 10 μM UCB was nearly complete . This is compatible with a dearth of stabilizing UCB anions at this pH, as expected from the high pK a values of 8.12 and 8.44 .
Our present data on residual [UCB] in DMSO-water systems likewise show decreased sedimentation with increasing pH (Fig. 1A,1B,1C). At each NDMSO, the lowest [UCB] were at the lowest pH values: 0.1 μM (N = 0.025, pH 4.15); 0.3 μM (N = 0.086, pH 4.5); and 2.8 μM (N = 0.31, pH 5.9). As in water, these are likely to be closest to the So values at each N. Indeed, they are only moderately higher than the corresponding So values of 0.07 μM, 0.15 μM and 2.2 μM, respectively, calculated from Equation 2 using So values of 51 nM in water  and 10 mM in DMSO .
log So,mixed = log So,water + (log So,DMSO - log So,water) × N (Eq. 2)
Equation 2 is a thermodynamic relationship based on assumptions of complete ideality of mixing . In general, a roughly linear variation of log So with N at low N is expected. For example, data from 1-naphthoic acid in DMSO-water  show that log So is a linear function of N up to N = 0.35. Such a relationship leads to a relatively small effect of low N values on So. Thus, according to Equation 2, So increases by a factor of only 1.4 at N = 0.025 and 2.9 at N = 0.086, but by a relatively larger factor of 44 at N = 0.31. This would markedly reduce the supersaturation factor ([UCB]/ So), which is a measure of the tendency of UCB to come out of solution at N = 0.31. This explains in part the relatively high [UCB] at high pH at N = 0.31 (Fig. 1A).
The pH effects on [UCB] at each NDMSO are of interest also. The lowest [UCB] at each pH registered relatively small increases with significant increases in pH: for example from 0.1 μM (pH 4.14) to 0.2 μM (pH 7.0) at N = 0.025; from 0.3 μM (pH 4.5) to 1.4 μM (pH 7.1) at N = 0.086; and from 111 μM (pH 7.1) to 166 μM (pH 8.4) at N = 0.31. These increases are probably caused mainly by increasing charge-stabilization of colloidal aggregates, as in aqueous media [12, 19, 20]. If, instead, the relatively small increases are ascribed entirely to increases in true solubility (S) at the high pH (Eq. 1), the required pK a values are about 7 at N = 0.025 and 0.086, and 8.5 at N = 0.31. The true pK a s of UCB in DMSO-water are thus probably significantly higher.
We note that some variability in sedimentation results from our short-term experiments, most evident at the low residual [UCB] in Figs. 1B and 1C, in part magnified by the log-log scale used. Some variability is expected, however, because of the complexity of the kinetic processes of nucleation, growth and flocculation that precede sedimentation. In Fig. 1A, the difference between acetate and Tris buffers is quite small (note the linear scale), compatible with the 58% higher [H+] in the acetate buffer. In Fig. 1B, the markedly lower sedimentation from phosphate buffers at pH 7.6–7.7, as compared to Tris buffer at pH 7.1, can be ascribed mainly to the much higher pH values and ionic strength of the phosphate systems. Another significant factor may be the difference in charge between the buffer salts; phosphate is anionic whereas Tris is cationic and zwitterionic. The cationic species of Tris can, in principle, reduce the negative charges on the surface of the colloidal H2B sufficiently to facilitate the formation of coarser particles and, thus, increase sedimentation.
Implications for pK a values of mesobilirubin-XIIIα (MBR)
In the recent 13C-NMR studies of the ionization of the 13C-COOH groups of MBR [3–6], it was assumed that the relevant physical properties of UCB and MBR, and of (CH3)2SO (DMSO) and (C2H3)2SO, are similar. Actually, as expected from the replacement of two vinyl groups in UCB with two ethyl groups in MBR, MBR is slightly more soluble in organic solvents  and has a higher Rf on silica gel t.l.c. ; MBR is thus more hydrophobic and should be less soluble in water than is UCB. Our low [UCB] in DMSO-water systems at comparable N, therefore, indicate that many of the (C2H3)2SO/buffer systems used in the 13C-NMR studies [3–6] were likely supersaturated with MBR. In those studies, the MBR concentrations used were stated to be 1 to 100 μM at N = 0.086 , compared to our lowest [UCB] of 0.3 μM at pH 4.5 and 1.4 μM at pH 7.05. At this N, 9 of 11 MBR data points were obtained at pH below 7.05 and 5 below pH 4.5 , so that even 1 μM MBR was likely to be supersaturated. At N = 0.31, our lowest [UCB], 2.8 μM at pH 5.9, was close to the lower limit of the 2 to 800 μM range of [MBR] used [4, 5]. Thus, many data points, obtained at pH values down to 2 [4, 5], were probably from supersaturated systems, despite being optically clear. As noted here and elsewhere [12–16, 18], optical clarity gives no assurance of the absence of supersaturation.
Actually, turbidity was reported in some of the 13C-NMR samples , indicating that coarse, insoluble aggregates of MBR were present. The claim that such turbidity did not affect 13C-NMR measurements [3, 5, 6] contrasts with evidence that even small multimers can change NMR chemical shifts [25, 26]. It should be noted also that, at high concentrations of B=, extensive, reversible self-association of B= can lead to apparently stable supersaturation with no separation of an insoluble phase . For example, at pH 8.5 and a UCB concentration of 20 μM (63 times S), the weight-average aggregation number of UCB has been found to be 7.17 , corresponding to a molecular weight of 4,195. The aggregation number remained fairly high, 4.2, in 60% (w/v) ethanol . The successful application of equilibrium ultracentrifugation for that study  suggests a complete absence of even small colloidal species of UCB. Self-association of MBR dianions in (C2H3)2SO-water mixtures cannot be ruled out on a priori grounds. It has been shown that neglect of self-association of B= leads to an artefactually low estimate of pK a values for UCB .
In addition to the problems of insolubility, supersaturation and self-aggregation of the MBR systems in (C2H3)2SO-water [3–6], we had shown previously that inaccuracies in the pH measurements affected both the magnitude of ΔpK a (the change in pK a on adding (C2H3)2SO to water), as well as the degree of the variation of ΔpK a with N . This is important for extrapolating pK a values in (C2H3)2SO-water to pure water (N = 0). Indeed, remeasurement of one soluble acid raised its pK a by as much as 3 units at N = 0.31 . Thus, the inaccuracies in pH measurement produced serious errors in reported pK a values of more than fifteen soluble acids used as models for MBR, as well as for MBR itself [3–7].
Many methods, using appropriate pH measurements, have been applied in the past to determine thermodynamic pK a values of soluble acids in non-aqueous or partially aqueous media, including DMSO-water systems [27, 28]. Many other relevant references were given in our prior paper . In that paper, our pK a measurements on acetic acid in DMSO-water systems were based on the potentiometric method, using properly calibrated glass electrodes, which determine the activity of H+, and on estimates of the activity coefficients of the acetate ion. This method, which is well established for aqueous solutions, yielded results in good agreement with data from the literature that was based on a very different method, measurements of electrical conductivity . In the 13C-NMR papers, therefore, it was not justified, to assume that pH values do not change on adding DMSO [3–7], or to use uncalibrated pH measurements for determination of the pK a values of soluble acids .
Our sedimentation data and their interpretation indicate that significant additional uncertainties, not important for the soluble acids investigated, exist for the reported pK a values of the relatively insoluble MBR in (CD3)2SO-water (4.2 and 4.9 at N = 0.086 and 4.3 and 5.0 at N = 0.31), as well as their extrapolation to obtain pK a values of 4.2 and 4.9 in water . Indeed, if these low aqueous pK a values, along with the experimental S values at pH 8.5 of 0.32 μM , or 0.6 μM , are applied to Eq. 1, the calculated extremely low So values of UCB diacid of 4 or 8 × 10-15 M are seven orders of magnitude lower than the experimental So, 5.1 × 10–8 M . Applying the So of 4 or 8 × 10-15 M to Eq. 2, moreover, would indicate massive supersaturation (up to 8 to 10 orders of magnitude) of MBR at the concentrations (1–800 μM) used in the 13C-NMR studies [3–6].
The present sedimentation data for UCB in DMSO-water demonstrate that the true solubilities of UCB, even at fairly high pH values, are low at DMSO mole fractions up to 0.31. The results and related considerations are compatible with similar results in purely aqueous solutions [12–14], and support both the estimated solubility (So) of 5.1 × 10–8 M for uncharged UCB (H2B) in water, and the corresponding high aqueous pK a values of 8.12 and 8.44, derived from our partition studies . These were performed in undersaturated systems and took into account the self-association of B=. Our experimental data indicate problems of insolubility, supersaturation and self-aggregation of UCB in DMSO-water mixtures with compositions similar to the MBR systems in (C2H3)2SO -water [3–6]. In (C2H3)2SO-water, DMSO-water  or any other medium , properly determined pK a values for the dissociation equilibria of a diacid H2A (H2A <--> HA- + H+ and HA- <--> A= + H+) must pertain to monomeric H2A, HA- and A=, the solute species involved in the stated equilibria, and require unambiguous determination of [H+] or pH. Unless pK a values are determined for monomeric systems, relative concentrations of H2A, HA- and A= cannot be determined from the pK a values and the pH. The 13C-NMR data, suggesting low pK a values for MBR in (C2H3)2SO -water and water [3–6, 9], did not meet these essential requirements of proper pH measurements  nor provide assurance that the MBR in every system was below saturation and not self-associated . The issues raised are not trivial, since the pK a and So values of UCB are clinically relevant to the effects of pH on the precipitation of calcium bilirubinates in pigment gallstones and the neurotoxicity caused by UCB diacid in severely jaundiced neonates .
Materials and Methods
UCB (Calbiochem) was purified by alkaline extraction of a chloroform solution, recrystallized twice from chloroform-methanol , dried under Argon, stored invacuo in the dark and used within 6 weeks. DMSO was spectroscopic grade, 99.8% pure (UVASol, Merck). Human serum albumin (HSA, lot 903635) was from Calbiochem-Boehringer. All other chemicals were reagent grade (Merck). Water used was deionized and distilled. All flasks and tubes were Kimax glass, washed with 0.1 N HCl and rinsed 4X with water and then dried before use. Stock buffers, 1.0 M, were: Tris-HCl, pH 7.01; Na- phosphate, pH 6.85, or 6.99; and Na-acetate, pH 4.01. Stock UCB in DMSO (4 to 6 mM) and stock HSA, 613 μM in 0.1 M Tris-HCl buffer, pH 7.01, were prepared freshly for each experiment.
Preparation of UCB-DMSO-buffer systems
Test systems (4.0 mL) of UCB were prepared in duplicate: to 0.4 mL of the stock buffer were added successively the appropriate volumes of water, DMSO and, finally, up to 150 μL of stock UCB/DMSO solution. To minimize UCB oxidation, all tubes and solutions were deoxygenated with Argon and kept in the dark . To determine the [UCB] in the UCB/DMSO stock, 6.0 μL, was added to 3.0 mL of the HSA stock. The absorbance, A, at 460 nm was read against a blank containing 2.0 mL of HSA stock plus 4.0 μL DMSO, and the [UCB] calculated using the extinction coefficient, ε, 47,000 M-1.cm-1. The pH measurement of each final DMSO/aqueous buffer system included an electrode calibration using the strong acid, HClO4. The 0.1 M phosphate buffer in N = 0.31 DMSO was centrifuged because of partial insolubility  and only the supernatant was used.
Centrifugation and analysis of residual UCB in supernatants
Fifteen min after mixing, samples were assessed visually for turbidity or precipitation. After Vortex-mixing, duplicate 1.8 mL aliquots were transferred to polypropylene tubes and centrifuged for 5 min at 25°C and 14,000 g (Mikroliter centrifuge, Hettich, Tuttlingen, Germany). The supernatants were assayed spectrophotometrically within 20 min. The precipitates were washed once with 1.8 mL of water, again centrifuged, the water aspirated, and the packed precipitate dissolved in DMSO for spectrophotometry. Absorbance (A) was measured in triplicate at 458 nm on each sample, diluted, when necessary, with DMSO or DMSO/buffer mixture to A of 0.2 to 0.8; a comparable medium without UCB was used as a blank. In all systems, including the redissolved UCB sediments, we applied the extinction coefficient of 0.0634 μM-1cm-1 at the peak wavelength of 458 nm for UCB in pure DMSO . Preliminary calibration studies. of the effects of DMSO concentration and buffer composition on A had confirmed this value for pure UCB in pure DMSO and in DMSO/buffer systems containing 64 vol% DMSO. In the systems containing 27 and 9 vol% DMSO, the spectrum developed a plateau between 458 and 450 nm, but A at 458 nm remained within ± 10% of the value expected from applying the extinction coefficient of 0.0634 μM-1cm-1 to the measured quantity of UCB dissolved in each system. The variability is in part due to degradation, discussed above, and in part due to the low absorbances at [UCB] below the saturation limit in some buffer/DMSO systems. For these reasons, no corrections were made for these minor differences in A.
Sedimentation of bilirubin-albumin complexes
To determine if UCB bound to HSA would sediment, we prepared a system containing HSA, 300 μM, and UCB 170 μM, in 0.1 M Tris-HCl buffer, pH 7.01. Microcentrifugation for 5 min yielded a small amount of precipitated UCB. Three aliquots of the clear supernatant were diluted with 1/8th volume of DMSO and a fourth aliquot diluted with 1/8th volume of buffer. The diluted samples (in duplicate) were then microcentrifuged for another 10 min and 25 μL samples taken from the top, middle and bottom of the fluid column in each tube, using a Hamilton syringe. Protein concentrations were determined with the Bio-Rad bicinchonic acid method, which is unaffected by bilirubin. After dilution with 1.8 mL DMSO, triplicate A readings were taken at 458 nm.
An abstract of this work has been published (Gastroenterology 2000; 118:A1477)
- N =:
mole fraction of DMSO in DMSO-aqueous buffer systems
nuclear magnetic resonance
solubility of UCB or MBR at a given pH
solubility of UCB diacid.
- Ostrow JD, Pascolo L, Tiribelli C: Editorial: Mechanisms of bilirubin neurotoxicity. Hepatology. 2002, 35: 1277-1280.PubMedView ArticleGoogle Scholar
- Hahm JS, Ostrow JD, Mukerjee P, Celic L: Ionization and self-association of unconjugated bilirubin, determined by rapid solvent partition from chloroform, with further studies of bilirubin solubility. J Lipid Res. 1992, 33: 1123-1137.PubMedGoogle Scholar
- Holmes DL, Lightner DA: Synthesis and acidity constants of 13CO2H-labelled dicarboxylic acids. p K a s from 13C-NMR. Tetrahedron. 1996, 52: 5319-5338. 10.1016/0040-4020(96)00153-6.View ArticleGoogle Scholar
- Lightner DA, Holmes DL, McDonagh AF: On the acid dissociation constants of bilirubin and biliverdin. pK a values from 13C NMR spectroscopy. J Biol Chem. 1996, 271: 2397-2405. 10.1074/jbc.271.5.2397.PubMedView ArticleGoogle Scholar
- Lightner DA, Holmes DL, McDonagh AF: Dissociation constants of water-insoluble carboxylic acids by 13C-NMR. p K a s of mesobiliverdin-XIIIα and mesobilirubin-XIIIα. Experientia. 1996, 51: 639-642.View ArticleGoogle Scholar
- Trull FR, Boiadjiev SE, Lightner DA, McDonagh AF: Aqueous dissociation constants of bile pigments and sparingly soluble carboxylic acids by 13C NMR in aqueous dimethyl sulfoxide: effects of hydrogen bonding. J Lipid Res. 1997, 38: 1178-1188.PubMedGoogle Scholar
- Holmes DL, Lightner DA: Synthesis and acidity constants of 13CO2H-labelled mono- and dipyrrole carboxylic acids. pK a from 13C-NMR. Tetrahedron. 1995, 51: 1607-1622. 10.1016/0040-4020(94)01052-2.View ArticleGoogle Scholar
- Mukerjee P, Ostrow JD: Effects of added dimethylsulfoxide on pKa values of uncharged organic acids and pH values of aqueous buffers. Tetrahedron Letters. 1998, 39: 423-426. 10.1016/S0040-4039(97)10537-8.View ArticleGoogle Scholar
- McDonagh AF, Phimster A, Boiadjiev SE, Lightner DA: Dissociation constants of carboxylic acids by 13C-NMR in DMSO/water. Tetrahedron Letters. 1999, 40: 8515-8518. 10.1016/S0040-4039(99)01841-9.View ArticleGoogle Scholar
- Brodersen R: Bilirubin: solubility and interaction with albumin and phospholipid. J Biol Chem. 1979, 254: 2364-2369.PubMedGoogle Scholar
- Brodersen R: Binding of bilirubin to albumin. CRC Crit Rev Clin Lab Sci. 1980, 11: 305-399.PubMedView ArticleGoogle Scholar
- Brodersen R, Thielgaard J: Bilirubin colloid formation in neutral aqueous solution. Scand J Clin Lab Invest. 1969, 24: 395-398.PubMedView ArticleGoogle Scholar
- Wennberg RP, Cowger ML: Spectral characteristics of bilirubin-bovine albumin complexes. Clin Chim Acta. 1973, 43: 55-64. 10.1016/0009-8981(73)90117-4.PubMedView ArticleGoogle Scholar
- Burnstine RC, Schmid R: Solubility of bilirubin in aqueous solutions. Proc Soc Exp Biol Med. 1962, 109: 356-358.PubMedView ArticleGoogle Scholar
- Siam M, Blaha G, Lehner H: Maximum binding capacity of serum albumin for bilirubin is one, as revealed by circular dichroism. J Chem Soc Perkin Trans II. 1998, 853-856. 10.1039/a708192h.Google Scholar
- Mukerjee P, Mysels KJ: A re-evaluation of the spectral change method of determining critical micelle concentration. J Am Chem Soc. 1955, 77: 2937-2943.View ArticleGoogle Scholar
- Brodersen R: Physical chemistry of bilirubin: Binding to macromolecules and membranes. In Bilirubin. Vol. 1: Chemistry. Edited by: Heirwegh KPM, Brown SB. 1982, Boca Raton, FL: CRC Press, 75-123.Google Scholar
- Lightner DA: Structure, photochemistry and organic chemistry of bilirubin. In Bilirubin. Vol. 1: Chemistry. Edited by: Heirwegh KPM, Brown SB. 1982, Boca Raton, FL: CRC Press, 1-58.Google Scholar
- Overbeek JTG: Stability of hydrophobic colloids and emulsions. In Colloid Science. Edited by: Kruyt HR. 1952, New York: Elsevier, 302-341.Google Scholar
- Vold RD, Vold MJ: Colloid and Interface Chemistry. Edited by: Reading MA. 1983, Addison-WesleyGoogle Scholar
- Hildebrand JH, Prausnitz JM, Scott RL: Regular and Related Solutions. 1970, New York: van NostrandGoogle Scholar
- Perez-Camino MC, Sanchez E, Balon M, Maestre A: Thermodynamic function for the transfer of 1-naphthoic acid from water to mixed aqueous solvents at 298 K. J Chem Soc Faraday Trans I. 1985, 81: 1555-1561.View ArticleGoogle Scholar
- Becker W, Sheldrick WS: Bile pigment structures II. The crystal structure of mesobilirubin-IXα-bis(chloroform). Acta Crystallogr B. 1978, 34: 1298-1304. 10.1107/S0567740878005397.View ArticleGoogle Scholar
- Rege RV, Webster CC, Ostrow JD, Carr SH, Ohkubo H: Validation of infrared spectroscopy for assessment of vinyl polymers of bile-pigment gallstones. Biochem J. 1984, 224: 871-876.PubMed CentralPubMedView ArticleGoogle Scholar
- Persson BO, Drakenberg T, Lindman B: 13C NMR of micellar solutions: micellar aggregation number from the concentration dependence of the 13C chemical shifts. J Phys Chem. 1979, 83: 3011-3015.View ArticleGoogle Scholar
- Müller N, Birkhahn RH: Micellar structure by fluoride magnetic resonance. 1. Sodium 10-10-10-trifluorocaproate and related compounds. J Phys Chem. 1967, 71: 957-962.View ArticleGoogle Scholar
- DeMaria P, Fini A, Guarnieri A, Varoli L: Thermodynamic dissociation constants of 3-substituted 3-(4 biphenylyl)-3-hydroxypropionic acids in aqueous DMSO. Arch Pharm (Weinheim). 1983, 316: 559-563.View ArticleGoogle Scholar
- Morel JP: Conductivités de quelque électrolytes, dissociation de l'acide acétique et potentiels normaux de l'électrode Ag-AgCl dans les mélanges eau-dimethylsulfoxyde. Bull Soc Chim de France. 1967, 1405-1411.Google Scholar
- Ostrow JD, Mukerjee P, Tiribelli C: Structure and binding of unconjugated bilirubin: relevance for physiological and pathophysiological function. J Lipid Res. 1994, 35: 1715-1737.PubMedGoogle Scholar
- McDonagh AF, Assisi F: The ready isomerization of bilirubin-IXα in aqueous solution. Biochem J. 1972, 129: 797-800.PubMed CentralPubMedView ArticleGoogle Scholar
- Blanckaert N, Heirwegh KPM: Analysis and preparation of bilirubins and biliverdins. In Bile Pigments and Jaundice; Molecular, Metabolic and Medical Aspects. Edited by: Ostrow JD. 1986, New York: Marcel Dekker, 31-79.Google Scholar
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