Aluminum speciation studies in biological fluids. Part 7. A quantitative investigation of aluminum(III)-malate complex equilibria and their potential implications for aluminum metabolism and toxicity.

As a nonessential element, aluminum may be toxic at both environmental and therapeutic levels, depending on ligand interactions. Dietary acids that normally occur in fruits and vegetables and commonly serve as taste enhancers are good ligands of the Al(3+) ion. Malic acid is one of these and also one of the most predominant in food and beverages. The present paper reports an examination of its potential influence on aluminum bioavailability through speciation calculations based on Al(III)-malate complex formation constants especially determined for physiological conditions. According to the results obtained, malate appears to be extremely effective in maintaining Al(OH)(3) soluble over the whole pH range of the small intestine under normal dietary conditions. In addition, two neutral Al(III)--malate complexes are formed whose percentages are maximum from very low malate levels. When aluminum is administered therapeutically as its trihydroxide, the amount of metal neutralized by malate peaks as its solubility pH range regresses to its original limits in the absence of malate. The enhancing effect of malate towards aluminum absorption is therefore virtually independent of the aluminum level in the gastrointestinal tract. The presence of phosphate in the gastrointestinal juice is expected to limit the potential influence of malate on aluminum absorption. Under normal dietary conditions, phosphate effectively reduces the fraction of aluminum neutralized by malate but without nullifying it. Aluminum phosphate is predicted to precipitate when aluminum levels are raised as with the administration of aluminum hydroxide, but a significant amount of neutral aluminum malate still remains in solution. Even therapeutic aluminum phosphate is not totally safe in the presence of malate, even at low malate concentrations. As plasma simulations predict that no compensatory effect in favor of aluminum excretion may be expected from malate, simultaneous ingestion of malic acid with any therapeutic aluminum salt should preferably be avoided.

Aluminum speciation studies in biological fluids. Part 6. Quantitative investigation of aluminum(III)-tartrate complex equilibria and their potential implications for aluminum metabolism and toxicity.

Recent epidemiological studies have confirmed the existence of a correlation between aluminum level in low-silica drinking water and prevalence of Alzheimer's disease. Also, oral aluminum-based phosphate binders and antacids may induce acute aluminum toxicity. Whatever the source of the metal ingested, its bioavailability is a function of the chemical forms under which it occurs in the gastrointestinal tract, i.e. of the ligands with which the Al3+ ion may associate. Dietary acids in particular can favor the bioavailability of aluminum in different ways: by increasing its solubility, by complexing it into neutral species, and/or by acting indirectly on its absorption process. Among these, tartaric acid is commonly found in fruits and in industrial foods and drinks, and may therefore be ingested together with environmental or/and therapeutic aluminum. The present work examines its potential influence on aluminum bioavailability. Firstly, Al(III)-tartrate complex formation constants have been determined under physiological conditions (37 degrees C, 0.15 M NaCl). Then these constants have been used to simulate the influence of tartrate on aluminum speciation in different gastrointestinal situations in which phosphate was also taken into account. Under normal conditions of aluminum contamination, tartrate is expected to keep the metal soluble throughout the whole pH range of the small intestine, which is likely to enhance its bioavailability. Even at low concentrations, tartrate also gives rise to two neutral complexes that span over the 1.5-7.5 pH interval, a phenomenon that is aggravated by increased aluminum levels as may result from aluminum hydroxide therapy. The co-occurrence of dietary phosphate reduces the fraction of aluminum neutralized by tartrate under normal conditions, but this effect quickly decreases with increasing aluminum doses. Even the therapeutic use of aluminum phosphate is not expected to be totally safe in the presence of tartaric acid. As plasma simulations show that no aluminum mobilization can be expected from tartrate that could enhance aluminum excretion, avoiding ingestion of tartaric acid during any form of aluminum-based therapy appears advisable.

Does human betaA4 exert a protective function against oxidative stress in Alzheimer's disease?

The hypothesis is advanced that human betaA4--as opposed to rodent betaA4--may exert a protective function against the iron-induced oxidative stress associated with neurological diseases (notably Alzheimer's disease). Subsequent to its release by the host in response to oxidative injury, human betaA4 would interact with Cu(2+)ions whose level is correlatively elevated, adopting the 'aggregated' structure recently characterized by Atwood et al.(15). Then, depending on the oxidative state--hence the pH--of the medium, it might either return to its original structure if physiological pH is restored, or undergo site-specific copper-mediated oxidation and, finally, degradation. In this context, betaA4 pathogenicity could be due to an interfering mechanism preventing the degradation of the oxidized peptide, making its aggregation irreversible and inducing its final deposition. Coordination of side group oxygen donors of the oxidized peptide with 'hard' metal ions occurring in the physiological medium (notably Al(3+)) might be at the origin of this interference.

Copper--ligand interactions and the physiological free radical processes. Part 3. Influence of histidine, salicylic acid and anthranilic acid on copper-driven Fenton chemistry in vitro.

With a view to the possible use of copper(II)-*OH inactivating ligand (OIL) complexes as regulators of inflammation, the reactivity of the copper(II)-ascorbate system with hydrogen peroxide has been investigated in the presence of three key substances: histidine (the main copper(II) low molecular mass ligand in extracellular fluid), salicylic acid (the well-known nonsteroidal antiinflammatory drug, previously shown to be potentiated by copper(II) in animal models of inflammation), and anthranilic acid (an inactive substance by itself, known to be activated by copper(II) in the same models) at physiological pH (7.4) and inflammatory pH (5.5). Such substances may affect the amount of TBARS detected in solution following copper-mediated Fenton-like reactions through three distinct mechanisms: (i) by decreasing the Cu(II)/Cu(I) redox potential, i.e. at the expense of *OH radical production, (ii) by scavenging *OH radicals in the body of the solution, and/or (iii) by acting as a true OIL, i.e. at the expense of *OH detection. Redox potential measurements of initial solutions have been performed in parallel to TBARS determinations to help discriminate between different ligand influences. Computer-aided speciation has been used to understand the role of copper(II) distribution on the ligand effects characterised. Contrary to previous interpretations, histidine has been found to mainly affect *OH production by lowering the redox potential of the Cu(II)/Cu(I) couple. Salicylate, which has no effect on *OH production, has been confirmed to mainly scavenge *OH radicals in the body of the solution. Anthranilate, which both increases *OH production and decreases *OH detection, behaves as a potential OIL. These results tend to confirm our previous hypothesis that copper potentiation of antiinflammatory substances is indirect, i.e. independent of any interaction between metal and drug, whereas copper activation of substances that are inactive by themselves results from specific metal-substance interactions taking place at inflammatory sites.

Aluminum speciation studies in biological fluids. Part 5. A quantitative investigation of A1(III) complex equilibria with desferrioxamine, 2,3-dihydroxybenzoic acid, Tiron, CP20 (L1), and CP94 under physiological conditions, and computer-aided assessment of the aluminum-mobilizing capacities of these ligands in vivo.

While the involvement of environmental aluminum toxicity in the advent of senile dementias is still debated, acute aluminum toxicity of iatrogenic origin is well documented. So far, the only treatment available against it has been desferrioxamine (DFO), which induces major side effects. New drugs are thus highly desirable, and possible DFO substitutes have already been considered through various techniques. An important test for such new drugs is to assess their A1-mobilizing capacity in vivo. This can be done by computer-aided speciation provided formation constants for the corresponding A1(III) complexes are known beforehand. The present work reports an investigation of A1(III) complex equilibria with five sequestering ligands including DFO, and predicts the respective capacities of these to mobilize aluminum in vivo under normal and inflammatory conditions.

Aluminum speciation studies in biological fluids. Part 4. A new investigation of aluminum-succinate complex formation under physiological conditions, and possible implications for aluminum metabolism and toxicity.

Previous in vivo studies devoted to the capacity of succinate to influence aluminum metabolism have led to apparent contradictory results. Understanding the mechanisms that lie behind such discrepancies requires a knowledge of aluminum-succinate interactions at the molecular level. In the absence of possible direct analysis of the ultrafiltrable fraction of aluminum in vivo, computer simulations can help quantify the mobilizing power of succinate towards aluminum in the main biofluids. Based on this technique, a first attempt to elucidate the above issue was made using especially determined aluminum-succinate formation constants. However, further investigations have led to reconsider the stoichiometry of the aluminum-succinate complexes characterized on that occasion. The present work deals with these new investigations. The results obtained confirm the great complexity of the aluminum-succinate system. No less than seven species, among which five polynuclear complexes, have been characterized in two series of independent experiments. New simulations indicate that succinate is expected to facilitate aluminum gastrointestinal absorption to a greater extent than initially predicted when the metal is administered as its trihydroxide, especially at high concentrations of the metal. In contrast, succinate is not able to significantly increase aluminum absorption when ingested concomitantly with aluminum phosphate. It is also confirmed that succinate cannot influence the fate of aluminum in blood plasma, which supports the view that the protective effect of succinate against aluminum toxicity in mice is not due to aluminum complexation.

Effect of aluminium ions on liposomal membranes as detected by Laurdan fluorescence.

We report here an investigation of the influence of aluminium on iron-induced peroxidation in brain model membranes. Laurdan fluorescence emission spectra and generalised polarisation measurements have been used to investigate how ferrous and aluminium ions can affect the phase components of phospholipid membranes. An increase in the generalised polarisation of oxidised liposomes with respect to controls has been observed, which reveals the presence of a less polar environment surrounding the probe that changes the properties of the bilayer. Aluminium has been shown to facilitate iron-mediated oxidation as detected from emission fluorescence spectra. However, no quantitative influence has been calculated relative to general polarisation and derived phase state determinations. The structural influence of aluminium on membranes may therefore be less significantly marked than initially expected.

Copper(II) interactions with nonsteroidal antiinflammatory agents. II. Anthranilic acid as a potential. OH-inactivating ligand.

It has long been established that copper complexes of inactive substances exert antiinflammatory activity and that copper complexes of nonsteroidal antiinflammatory drugs (NSAIDs) are more active than these drugs by themselves. Based on these observations, it was proposed that copper complexes of NAIDs are their active metabolites. This hypothesis was not confirmed for salicylic acid, however, as computer-aided speciation studies have shown that no copper-salicylate complex can reach significant levels in blood plasma. In view of this result, it was of interest to test with the same technique the influence on copper metabolism of an inactive substance known to be activated by copper. Anthranilic acid was chosen for this test in the present work. First, copper(II)-anthranilate interactions have been investigated by glass electrode potentiometry under physiological conditions. Given the key role of histidine as copper(II) ligand in blood plasma, copper(II)-histidine-anthranilate ternary equilibra have also been determined. Computer simulations of copper distribution have then been run relative to the two main biofluids in respect of global metabolism, i.e., gastrointestinal (g.i.) fluid and blood plasma. Like salicylic acid, anthranilic acid is expected to favor copper g.i. absorption, but cannot either exert any significant influence on plasma copper distribution. Clearly, the fact that anthranilate becomes antiinflammatory when administered with copper cannot originate in any effect of anthranilate on copper global metabolism. Speciation investigations have then been extended to the synovial fluid. Whereas salicylate does not appear to be a better ligand of copper in this medium than in blood plasma at any pH between 7.4 and 5.5, anthranilate on the contrary can mobilize increasing fractions of copper as the pH decreases, i.e., the more inflammation, the more copper is bound to anthranilate. This is in line with the recent observation that salicylate inactivates copper-induced .OH radicals through its bulk scavenging properties whereas .OH inactivation by anthranilate under the same conditions is a direct function of the copper-anthranilate binding. Anthranilate thus seems to correspond to the recently defined notion of .OH-inactivating ligand (OIL). More generally, these results provide a beginning of rationale for the antiinflammatory properties of copper complexes with substances that are active or inactive against inflammation by themselves. The extra antiinflammatory activity induced by copper on NSAIDs appears to be independent of any Cu(II)-NSAID association in vivo. On the contrary, the binding of inactive substances with copper(II) at inflammatory sites seems to be essential to their activation by copper.

Speciation of aluminum in biological systems.

As a "hard", trivalent metal ion, Al3- binds strongly to oxygen-donor ligands such as citrate and phosphate. The aqueous coordination chemistry of Al is complicated by the tendency of many Al complexes to hydrolyze and form polynuclear species, many of which are sparingly soluble. Thus there is considerable variation among the Al stability constants reported for several important ligands. The complexity in the aqueous chemistry of Al has also affected Al toxicity studies, which have often utilized poorly characterized Al stock solutions. Serum fractionation studies show that most Al is protein bound, primarily to the serum iron transport protein transferrin. Albumin appears to play little, if any, role in serum transport. There is little agreement as to the speciation of the remaining low-molecular mass fraction of serum Al. The lability of the Al3+ion precludes the simple separation and identification of individual Al complexes. Computational methods are available for detailed computer calculations of the Al speciation in serum, but efforts in this area have been severely hampered by the uncertainties regarding the stability constants of the low molecular mass Al complexes with citrate, phosphate, and hydroxide. Specific recommendations for further research on Al speciation include: (1) Determine more accurate Al stability constants with critical low molecular mass ligands such as citrate and phosphate; (2) supplement traditional potentiometric studies on Al complexes with data from other techniques such as 27Al-NMR and accelerator mass spectrometry with 26Al; (3) develop new methods for generating reliable linear free energy relationships for Al complexation; (4) determine equilibrium and rate constants for Al binding to transferrin at 37 degrees C; (5) confirm the possible formation of low-molecular-mass Al-protein complexes following desferrioxamine therapy; (6) continue research efforts to incorporate kinetic considerations into the present equilibrium speciation calculations; (7) improve methods for preparing chemically well-defined stock solutions for toxicological studies; (8) incorporate more detailed speciation data into studies on Al toxicity and pharmacokinetics; and (9) incorporate more detailed speciation data into future epidemiological studies on the relationship between Al toxicity and various water quality parameters.

Aluminum-succinate complex equilibria and their potential implications for aluminum metabolism.

Apparent contradictory results have been reported about the effect of succinate on aluminum toxicity, distribution and excretion in mice. Investigating the influence of this ligand on aluminum speciation in the main biofluids may help understand the above observations at the molecular level. In the absence of experimental access to ultrafiltrable aluminum speciation, computer simulations have been used in the gastrointestinal fluid and blood plasma, based on Al-succinate complex formation constants determined under physiological conditions. Calculations run for gastrointestinal conditions show that Al-succinate soluble complexes are formed in the 2 to 6 pH range--especially the neutral M2L(OH)4--which may enhance aluminum absorption. This influence, however, should be limited by dietary phosphate. In blood plasma, there is no possibility for succinate to mobilize a significant aluminum fraction, which confirms a recent suggestion that the possible protective effect of succinate against aluminum toxicity in mice may not be due to aluminum complexation.

Copper(II) interactions with nonsteroidal antiinflammatory agents. I. Salicylic acid and acetylsalicylic acid.

Recently a growing body of evidence has accumulated on the beneficial effects of copper compounds toward various models of inflammation, and copper complexes of nonsteroidal antiinflammatory drugs (NSAIDs) have been shown to be more effective in this respect than the parent agents. However, the origin of this activity remains unclear: The ability of NSAIDs to influence copper metabolism is still questionable, and apart from the claimed SOD-like activity of copper salts in vivo, relatively little is known about how copper-NSAID interactions may help regulate the inflammatory process. Before the potential role of copper-NSAID complexes versus inflammation can be elucidated, speciation studies are necessary (i) to analyze the overall influence of these drugs on copper metabolism and (ii) to discriminate the individual complexes likely to represent the active form of the drug in vivo. In this paper, copper(II) complex equilibria with salicylic and acetylsalicylic acids--and benzoic acid used as a reference--as well as the mixed-ligand complex equilibria generated by these binary systems and L-histidine [main low-molar-mass ligand of copper(II) in blood plasma] have been investigated under physiological conditions (37 degrees C; 0.15-M NaCl). Confirming previous observations by others, resulting simulated plasma copper distributions virtually rule out any quantitative influence of salicylate on copper tissue diffusion at therapeutic levels. Even though, as is presently shown, both salicylate and acetylsalicylate may favor the gastrointestinal absorption of copper, it seems unlikely that salicylate can exert its antinflammatory activity predominantly through copper complexation. The assertion that copper-NSAID complexes represent the active forms of NSAIDs therefore seems to be of limited significance for salicylate.

Copper-ligand interactions and physiological free radical processes. Part 2. Influence of Cu2+ ions on Cu(+)-driven .OH generation and comparison with their effects on Fe(2+)-driven .OH production.

In our search to establish a reference .OH production system with respect to which the reactivity of copper(II) complexes could then be tested, the influence of free Cu2+ ions on the Cu+/H2O2 reaction has been investigated. This influence depends on the CCu2+/CCu+ ratio. At low Cu2+ concentrations, .OH damage to various detector molecules decreases with increasing Cu2+ concentrations until CCu2+/CCu+ reaches unity. Above this value, .OH damage increases sharply until CCu2+/CCu+ becomes equal to 5 with salicylate and 2 with deoxyribose, ratios for which the protective effect of Cu2+ cancels. Finally, at higher concentrations, Cu2+ ions logically add their own .OH production to that normally expected from Cu+ ions. The possible origin of this unprecedented alternate effect has been discussed. The possible influence of Cu+ ions on the generation of .OH radicals by water gamma radiolysis has also been tested and, as already established for Cu2+ in a previous work, shown to be nonexistent. This definitely confirms that either form of ionised copper cannot scavenge .OH radicals in the absence of a ligand.

A new investigation of copper(II)-serine, copper(II)-histidine-serine, copper(II)-asparagine, and copper(II)-histidine-asparagine equilibria under physiological conditions, and implications for simulation models relative to blood plasma.

Some years ago, the application of computer modeling to metal speciation in biofluids was questioned based on the discrepancy between the simulated distribution of copper(II) in blood plasma and related experimental results obtained by Neumann and Sass-Kortsak in reconstituted serum. A recent investigation of the relevant copper(II)-amino acid equilibria reconciled these conflicting data, confirming that the reliability of computer models crucially depends on the data on which they are based. Since then, however, some of the constants of the copper-serine system used in that study have been suspected to be overestimated. This work thus reports the redetermination of copper-serine and copper-histidine-serine formation constants under physiological conditions. In addition, serine being close to asparagine in Neumann and Sass-Kortsak's classification, copper-asparagine and copper-histidine-asparagine equilibria have also been reinvestigated. For asparagine complexes, former constants have been basically confirmed. In contrast, all constants relative to serine have effectively been found lower than the previous ones. The effects of these new data on the stimulated distribution of plasma copper are only minor, but a better agreement is observed relative to Neumann and Sass-Kortsak's models in reconstituted serum.

Is copper pro- or anti-inflammatory? A reconciling view and a novel approach for the use of copper in the control of inflammation.

The anti-inflammatory role of copper is well-known although still largely unexplained. On the other hand, the capacity of copper to induce the formation of damaging .OH radicals in vivo is no longer debated. These two aspects of the physiological activity of copper have been considered to be paradoxical. Arguments developed here show that they may actually derive from a single chemical process, the type of physiological effect observed depending on the ligand bound to the copper ions involved in Fenton chemistry. Both iron and copper are Fenton catalysts. Given its intrinsic coordination properties, however, copper induces more site-specific .OH damage to the ligands bound to it. It, therefore, appears that copper complexes with specific .OH-inactivating ligands (OILs) can be used as "lures" for the Fenton reaction, .OH radicals preferentially formed on these being immediately inactivated. The hypothesis is thus put forward here that copper-OIL complexes acting as effective Fenton catalysts are potential "catalase-like" anti-inflammatory drugs.

Can N-acetyl-L-cysteine affect zinc metabolism when used as a paracetamol antidote?

N-Acetyl-L-cysteine (NAC) has long been used in the treatment of chronic lung diseases. Inhalation and oral administration of the drug are both effective in reducing mucus viscosity. In addition, NAC oral therapy allows to restore normal mucoprotein secretion in the long term. Although displaying heavy metal-complexing potential, NAC exerts no detectable influence on the metabolism of essential trace metals when used in the above context (i.e. at doses near 600 mg day-1). However, this may no longer be the case when NAC is used as an oxygen radical scavenger, like in the treatment of paracetamol poisoning. In the latter case, intravenous doses as high as 20 g day-1 are administered, which may induce excessive zinc urinary excretion. In order to allow a better appreciation of the risk of zinc depletion during NAC therapy, the present work addresses the role of this drug towards zinc metabolism at the molecular level. First, formation constants for zinc-NAC complexes have been determined under physiological conditions. Then, computer simulations for blood plasma and gastrointestinal fluid have been run to assess the influence of NAC and its metabolites (e.g. cysteine and glutathione) on zinc excretion and absorption. Blood plasma simulations reveal that NAC can effectively mobilise an important fraction of zinc into urinary excretable complexes as from concentrations of 10(-3) mol dm-3 (which corresponds to a dose of about 800 mg). This effect can still be enhanced by the action of NAC metabolites, among which cysteine is the most powerful zinc sequestering agent. In contrast, simulations relative to gastrointestinal conditions suggest that NAC should tend to increase zinc absorption, regardless of its dose.

Why aluminum phosphate is less toxic than aluminum hydroxide.

Initially characterized in uremic patients undergoing hemodialysis, toxic effects due to high aluminum (Al) body loads were subsequently observed in a number of conditions, in particular following ingestion of Al-containing antacids. Among compounds of this class, aluminum phosphate (AlPO4) was recognized as safer than aluminum hydroxide (Al(OH)3), which was thought to result from its lower solubility and thus absorption in the gastrointestinal (gi) tract. However, while virtually insoluble at acid pH, AlPO4 is more soluble than Al(OH)3 under alkaline conditions, leading to the hypothesis that Al is predominantly absorbed in the acidic region of the gi tract. Our present results suggest otherwise. Al bioavailability depends on the solubility of the salt ingested as well as on the physicochemical properties of the Al soluble complexes formed in the gi fluid. Anions of dietary acids may indeed dissolve significant fractions of Al salts and form absorbable Al complexes. It is in these terms that the well documented increase of Al gi absorption by citrate has been interpreted from computer-based speciation studies. Using similar calculations, we now demonstrate that a series of dietary acids (namely malic, oxalic, tartaric, succinic, aspartic and glutamic acids) can also dissolve significant amounts of Al(OH)3 and form Al neutral complexes available to the gi membrane. In contrast, both effects are far less apparent when Al is administered as AlPO4. We conclude from this observation that the lower toxicity of AlPO4 vs Al(OH)3 stems from its better capacity to resist dissolution and neutral complex formation in the presence of acids commonly present in food.

A quantitative investigation of proton- and lead(II)-dithioerythritol complex equilibria under physiological conditions.

Dithioerythritol (DTE) is frequently employed as a reducing agent or a protective reagent for thiol groups in biological assays. Owing to its known inhibiting properties in enzyme catalysis reactions, lead is also commonly used in such experiments, and often simultaneously with DTE. Given the potential affinity of these two reactants, their measured individual effects may well depend on their interactions in the medium used. Any quantitative assessment of these interactions necessitates, however, that the complex equilibria between lead and DTE be investigated beforehand. To test this hypothesis, the formation constants of lead(II) complexes with DTE under physiological conditions (37 degrees, NaCl 0.15M) have been calculated from the results of glass electrode potentiometry, with the help of the MINIQUAD and ESTA computer programs. The pK values for dissociation of DTE have been found equal to 8.926 +/- 0.003 and 9.840 +/- 0.003. The following lead-DTE species have been characterized: ML (12.774 +/- 0.037), MLH(-1) (2.858 +/- 0.037), M(2)LH(-1) (13.349 +/- 0.025) and M(6)L(5) (86.586 +/- 0.099); the log *beta-values are given in the parentheses. Appropriate computer simulations effectively show that the interactions of the two reactants are indeed quite significant within the concentration ranges commonly used in in vitro biological assays. They should thus be taken into account in interpretation of the effects observed.

Copper-ligand interactions and physiological free radical processes. pH-dependent influence of Cu2+ ions on Fe2(+)-driven OH. generation.

Prior to comparative studies on the reactivity of various copper complexes with respect to OH. radicals, the influence of free Cu2+ ions on the superoxide-independent generation of OH. radicals through Fenton assays and water gamma radiolysis has been tested in the present work. Cu2+ ions have been shown to behave in a distinct manner towards each of these two production systems. As was logically expected from the noninvolvement of copper in OH. radical production through gamma radiolysis, no influence of Cu2+ ions has been observed on the amount of radicals detected in that case. In contrast, Cu2+ ions do influence OH. radical generation through iron-driven Fenton reactions, but differently depending on copper concentration. When present in high concentrations, Cu2+ ions significantly contribute to OH. radical production, which confirms previous observations on the reactivity of these in the presence of hydrogen peroxide. At lower levels corresponding to copper/iron ratios below unity on the contrary, Cu2+ ions behave as inhibitors of the OH. production in a pH-dependent manner over the 1-6 range investigated: the lower the pH, the greater the inhibition. The possible origin of this previously unreported inhibitory effect is discussed.

Lead (II)-dithiothreitol equilibria and their potential influence on lead inhibition of 5-aminolevulinic acid dehydratase in in vitro assays.

Dithiothreitol (threo-2,3-dihydroxy-1,4-dithiobutane = DTT) has recently been used to activate 5-aminolevulinic acid dehydratase in kinetic studies for the inhibition of this zinc enzyme by lead. Since the DTT molecule contains donor groups capable of forming metal ion complexes, its presence in the experimental medium used for this kind of assay may largely influence the concentration of lead available for the active sites of the enzyme. Before any quantitative investigation of this phenomenon can be contemplated, all possible complexes formed by lead with DTT must first be identified and their stabilities determined. Accordingly, formation equilibria of DTT complexes with lead(II) have been investigated under physiological conditions (37 degrees C, NaCl, 0.15 mol. dm-3 using glass electrode potentiometry. Corresponding stability constants were refined with MINIQUAD and ESTA computer programs. DTT log protonation constants have been found equal to 9.811 +/- 0.002 and 18.672 +/- 0.002. The following lead-dithiothreitol complexes have been characterized: ML (12.243 +/- 0.063), MLH-1 (2.391 +/- 0.061), M2LH-1 (13.285 +/- 0.059), and M4L3 (51.668 +/- 0.157). Appropriate computer simulations show that the interactions of the two reactants are indeed most significant under the pH and concentration conditions used in the above mentioned biological investigations. In particular, the influence of lead(II)-DTT equilibria on the free concentration of lead available for the active sites of the enzyme is described.