Calorimetric analysis of lisinopril binding to angiotensin I-converting enzyme

Isolation and Characterization of Angiotensin I-Converting Enzyme (ACE) Inhibitory Peptides from the Enzymatic Hydrolysate of Carapax Trionycis (the Shell of the Turtle Pelodiscus sinensis)

Carapax Trionycis (the shell of the turtle Pelodiscus sinensis) was hydrolyzed by six different commercial proteases. The hydrolysate prepared from papain showed stronger inhibitory activity against angiotensin I-converting enzyme (ACE) than other extracts. Two noncompetitive ACE inhibitory peptides were purified successively by ultrafiltration, gel filtration chromatography, ion exchange column chromatography, and high-performance liquid chromatography (HPLC). The amino acid sequences of them were identified as KRER and LHMFK, with IC₅₀ values of 324.1 and 75.6 μM, respectively, confirming that Carapax Trionycis is a potential source of active peptides possessing ACE inhibitory activities. Besides, both enzyme kinetics and isothermal titration calorimetry (ITC) assay showed that LHMFK could form more stable complex with ACE than KRER, which is in accordance with the better inhibitory activity of LHMFK.

Entropy-driven binding of opioid peptides induces a large domain motion in human dipeptidyl peptidase III

Opioid peptides are involved in various essential physiological processes, most notably nociception. Dipeptidyl peptidase III (DPP III) is one of the most important enkephalin-degrading enzymes associated with the mammalian pain modulatory system. Here we describe the X-ray structures of human DPP III and its complex with the opioid peptide tynorphin, which rationalize the enzyme's substrate specificity and reveal an exceptionally large domain motion upon ligand binding. Microcalorimetric analyses point at an entropy-dominated process, with the release of water molecules from the binding cleft ("entropy reservoir") as the major thermodynamic driving force. Our results provide the basis for the design of specific inhibitors that enable the elucidation of the exact role of DPP III and the exploration of its potential as a target of pain intervention strategies.

Binding dynamics and energetic insight into the molecular forces driving nucleotide binding by guanylate kinase

Plasmodium deoxyguanylate pathways are an attractive area of investigation for future metabolic and drug discovery studies due to their unique substrate specificities. We investigated the energetic contribution to guanylate kinase substrate binding and the forces underlying ligand recognition. In the range from 20 to 35°C, the thermodynamic profiles displayed marked decrease in binding enthalpy, while the free energy of binding showed little changes. GMP produced a large binding heat capacity change of -356 cal mol(-1) K(-1), indicating considerable conformational changes upon ligand binding. Interestingly, the calculated ΔCp was -32 cal mol(-1) K(-1), indicating that the accessible surface area is not the central change in substrate binding, and that other entropic forces, including conformational changes, are more predominant. The thermodynamic signature for GMP is inconsistent with rigid-body association, while dGMP showed more or less rigid-body association. These binding profiles explain the poor catalytic efficiency and low affinity for dGMP compared with GMP. At low temperature, the ligands bind to the receptor site under the effect of hydrophobic forces. Interestingly, by increasing the temperature, the entropic forces gradually vanish and proceed to a nonfavorable contribution, and the interaction occurs mainly through bonding, electrostatic forces, and van der Waals interactions.

Immobilization of arginase and its application in an enzymatic chromatographic column: Thermodynamic studies of nor-NOHA/arginase binding and role of the reactive histidine residue

A biochromatographic approach is developed to measure for the first time changes in enthalpy, heat capacity change and protonation for the binding of nor-NOHA to arginase in a wide temperature range. For this, the arginase enzyme was immobilized on a chromatographic support. It was established that this novel arginase column was stable during an extended period of time. The affinity of nor-NOHA to arginase is high and changes slightly with the pH, because the number of protons linked to binding is low. The determination of the enthalpy change at different pH values suggested that the protonated group in the nor-NOHA-arginase complex exhibits a heat protonation of approximately -33 kJ/mol. This value agrees with the protonation of an imidazole group. Our result confirmed that active-site residue Hist 141 is protonated as imidazolium cation. Hist 141 can function as a general acid to protonate the leaving amino group of L-ornithine during catalysis. The thermodynamic data showed that nor-NOHA-arginase binding, for low temperature (<15 degrees C), is enthalpically unfavourable and being dominated by a positive entropy change. This result suggests that dehydration at the binding interface and charge-charge interactions contribute to the nor-NOHA-arginase complex formation. The temperature dependence of the free energy of binding is weak because of the enthalpy-entropy compensation caused by a large heat capacity change, DeltaC(p)=-2.43 kJ/mol/K, of arginase. Above 15 degrees C, the thermodynamic data DeltaH and DeltaS became negative due to van der Waals interactions and hydrogen bonding which are engaged at the complex interface confirming strong enzyme-inhibitor hydrogen bond networks. As well, by the use of these thermodynamic data and known correlations it was clearly demonstrated that the binding of nor-NOHA to arginase produces slight conformational changes in the vicinity of the active site. Our work indicated that our biochromatographic approach could soon become very attractive for studying other enzyme-ligand binding.

Spontaneous Formation of Core/Shell Bimetallic Nanoparticles: A Calorimetric Study

We showed recently that low entropy core/shell structured nanoparticles form spontaneously from the physical mixture of a dispersion of Ag nanoparticles and that of another noble metal (Rh, Pd, or Pt) at room temperature. Here we use isothermal titration calorimetry (ITC) and show that the initial step of such a spontaneous process is strongly exothermic. When the alcohol dispersion of poly(N-vinyl-2-pyrrolidone) (PVP)-protected Rh nanoparticles (average diameter 2.3 nm) was titrated into the alcoholic dispersion of PVP-protected Ag nanoparticles, a strong exothermic enthalpy change, DeltaH, was observed: DeltaH = -908 kJ/mol for Ag(S) nanoparticle (average diameter 10.8 nm) and -963 kJ/mol for Ag(L) nanoparticles (average diameter 22.5 nm). The strength of interaction increases in the order of Rh/Ag > Pd/Ag > Pt/Ag. This strong exothermic interaction is considered as a driving force to from low entropy bimetallic nanoparticles by simple mixing of two kinds of monometallic nanoparticles. We show also that exothermic interactions occur between a pair of noble metal nanoparticles themselves by using ITC.

Future challenges facing the development of specific active-site-directed synthetic inhibitors of MMPs

Despite a deep knowledge on the 3D-structure of several catalytic domains of MMPs, the development of highly specific synthetic active-site-directed inhibitors of MMPs, able to differentiate the different members of this protease family, remains a strong challenge. Due to the flexible nature of MMP active-site, the development of specific MMP inhibitors will need to combine sophisticated theoretical and experimental approaches to decipher in each MMP the specific structural and dynamic features that can be exploited to obtain the desired selectivity.

Calorimetric determination of thermodynamic parameters of 2'-dUMP binding to Leishmania major dUTPase

We have investigated the binding of 2'-deoxyuridine 5'-monophosphate (2'-dUMP) to Leishmania major deoxyuridine 5'-triphosphate nucleotide hydrolase (dUTPase) by isothermal titration microcalorimetry under different experimental conditions. Binding to dimeric L. major dUTPase is a non-cooperative process, with a stoichiometry of 1 molecule of 2'-dUMP per subunit. The utilization of buffers with different ionization enthalpies has allowed us to conclude that the formation of the 2'-dUMP-dUTPase complex, at pH 7.5 and 30 degrees C, is accompanied by the uptake of 0.33 +/- 0.05 protons per dUTPase subunit from the buffer media. Moreover, 2'-dUMP shows a moderate affinity for the enzyme, and binding is enthalpically driven across the temperature range studied. Besides, whereas DeltaG degrees remains practically invariant as a function of temperature, both DeltaH and DeltaS degrees decrease with increasing temperature. The TS and TH were 23.4 and 13.6 degrees C, respectively. The temperature dependence of the enthalpy change yields a heat capacity change of DeltaCp degrees = -618.1 +/- 126.4 cal x mol(-1) x K(-1), a value low enough to discard major conformational changes, in agreement with the fitting model. An interpretation of this value in terms of solvent-accessible surface areas is provided.

A calorimetric study of the binding of lisinopril, enalaprilat and captopril to angiotensin-converting enzyme

The angiotensin I-converting enzyme (ACE; EC.3.4.15.1) is a dipeptidyl carboxypeptidase that plays a central role in blood pressure regulation. The somatic form of the enzyme is composed of two highly similar domains, usually referred to as N and C domains, each containing one active site. Nevertheless, a 1:1 stoichiometry for the binding of lisinopril, captopril or enalaprilat to somatic pig lung ACE is shown by isothermal titration calorimetry (ITC) and enzymatic assays. The binding of the three inhibitors at neutral pH is very tight and the enthalpy changes are positive, indicating that the binding is entropically driven. The origin of this thermodynamic signature is discussed under the new structural information available.

Structure of human ACE gives new insights into inhibitor binding and design

Angiotensin-converting enzyme (ACE) is a primary target of drugs used for controlling hypertension. A new X-ray crystallographic structure of the key catalytic domain of ACE provides detailed information about the structure of its active site, located in a deep channel, and its interactions with an inhibitor. Such information might facilitate the rational design of ACE inhibitors that are more potent and more selective and therefore of clinical use.

Isothermal titration calorimetry in drug discovery

Isothermal titration calorimetry (ITC) follows the heat change when a test compound binds to a target protein. It allows precise measurement of affinity. The method is direct, making interpretation facile, because there is no requirement for competing molecules. Titration in the presence of other ligands rapidly provides information on the mechanism of action of the test compound, identifying the intermolecular complexes that are relevant for structure-based design. Calorimetry allows measurement of stoichiometry and so evaluation of the proportion of the sample that is functional. ITC can characterize protein fragments and catalytically inactive mutant enzymes. It is the only technique which directly measures the enthalpy of binding (delta H degree). Interpretation of delta H degree and its temperature dependence (delta Cp) is usually qualitative, not quantitative. This is because of complicated contributions from linked equilibria and a single change in structure giving modification of several physicochemical properties. Measured delta H degree values allow characterization of proton movement linked to the association of protein and ligand, giving information on the ionization of groups involved in binding. Biochemical systems characteristically exhibit enthalpy-entropy compensation where increased bonding is offset by an entropic penalty, reducing the magnitude of change in affinity. This also causes a lack of correlation between the free energy of binding (delta G degree) and delta H degree. When characterizing structure-activity relationships (SAR), most groups involved in binding can be detected as contributing to delta H degree, but not to affinity. Large enthalpy changes may reflect a modified binding mode, or protein conformation changes. Thus, delta H degree values may highlight a potential discontinuity in SAR, so that experimental structural data are likely to be particularly valuable in molecular design.

Thermodynamic analysis of the binding of glutathione to glutathione S-transferase over a range of temperatures

The binding properties of a glutathione S-transferase (EC 2.5.1.18) from Schistosoma japonicum to substrate glutathione (GSH) has been investigated by intrinsic fluorescence and isothermal titration calorimetry (ITC) at pH 6.5 over a temperature range of 15-30 degrees C. Calorimetric measurements in various buffer systems with different ionization heats suggest that protons are released during the binding of GSH at pH 6.5. We have also studied the effect of pH on the thermodynamics of GSH-GST interaction. The behaviour shown at different pHs indicates that at least three groups must participate in the exchange of protons. Fluorimetric and calorimetric measurements indicate that GSH binds to two sites in the dimer of 26-kDa glutathione S-transferase from Schistosoma japonicum (SjGST). On the other hand, noncooperativity for substrate binding to SjGST was detected over a temperature range of 15-30 degrees C. Among thermodynamic parameters, whereas DeltaG degrees remains practically invariant as a function of temperature, DeltaH and DeltaS degrees both decrease with an increase in temperature. While the binding is enthalpically favorable at all temperatures studied, at temperatures below 25 degrees C, DeltaG degrees is also favoured by entropic contributions. As the temperature increases, the entropic contributions progressively decrease, attaining a value of zero at 24.3 degrees C, and then becoming unfavorable. During this transition, the enthalpic contributions become progressively favorable, resulting in an enthalpy-entropy compensation. The temperature dependence of the enthalpy change yields the heat capacity change (DeltaCp degrees ) of -0.238 +/- 0.04 kcal per K per mol of GSH bound.

A calorimetric study of the binding of S-alkylglutathiones to glutathione S-transferase

The binding of three competitive glutathione analogue inhibitors (S-alkylglutathione derivatives) to glutathione S-transferase from Schistosoma japonicum, SjGST, has been investigated by isothermal titration microcalorimetry at pH 6.5 over a temperature range of 15--30 degrees C. Calorimetric measurements in various buffer systems with different ionization heats suggest that no protons are exchanged during the binding of S-alkylglutathione derivatives. Thus, at pH 6.5, the protons released during the binding of substrate may be from its thiol group. Calorimetric analyses show that S-methyl-, S-butyl-, and S-octylglutathione bind to two equal and independent sites in the dimer of SjGST. The affinity of these inhibitors to SjGST is greater as the number of methylene groups in the hydrocarbon side chain increases. In all cases studied, Delta G(0) remains invariant as a function of temperature, while Delta H(b) and Delta S(0) both decrease as the temperature increases. The binding of three S-alkylglutathione derivatives to the enzyme is enthalpically favourable at all temperatures studied. The temperature dependence of the enthalpy change yields negative heat capacity changes, which become less negative as the length of the side chain increases.

Influence of dynamic power compensation in an isothermal titration microcalorimeter

A theoretical analysis in Laplace's transformed domain based on a power balance represents a suitable model for an isothermal titration calorimeter with dynamic power compensation, designed and implemented in our laboratory. A rigorous calibration of the injection system and the calorimetric response was also made. Using electrically generated heat pulses, two different time constants have been determined from the calorimetric transfer function and assigned to the physical parts of the calorimeter. The same was done for a protein-ligand interaction. The binding of 2'-CMP to ribonuclease A at low and high ionic strengths was used to check the apparatus and the results were compared with those obtained by other authors (Wiseman, T.; Williston, S.; Brandts, J.F.; Lung-Nan, L. Anal. Biochem. 1989, 179, 131-137). In this case, the analysis showed a different time constant for the heat source. Independently of the nature of the heat source, the calorimetric time constants obtained while working under compensation are always smaller than those corresponding to a noncompensated system. The improvement of the calorimetric response introduced by dynamic power compensation is thus explained in terms of the reduction of the time constants characteristic of the calorimeter. This theoretical model can be used to predict the shape of the thermogram for any given reaction of either known or supposed thermodynamic parameters. Therefore, the calorimetric study is extended to the other nucleotides, 2'-UMP and 5'-dUMP, which have not hitherto been reported in the literature.

Enthalpy of captopril-angiotensin I-converting enzyme binding

High-sensitivity titration calorimetry is used to measure changes in enthalpy, heat capacity and protonation for the binding of captopril to the angiotensin I-converting enzyme (ACE; EC 3.4.15.1). The affinity of ACE to captopril is high and changes slightly with the pH, because the number of protons linked to binding is low. The determination of the enthalpy change at different pH values suggests that the protonated group in the captopril-ACE complex exhibits a heat protonation of approximately -30 kJ/mol. This value agrees with the protonation of an imidazole group. The residues which may become protonated in the complex could be two histidines existing in two active sites, which are joined to the amino acids coordinated to Zn2+. Calorimetric measurements indicate that captopril binds to two sites in the monomer of ACE, this binding being enthalpically unfavorable and being dominated by a large positive entropy change. Thus, binding is favored by both electrostatic and hydrophobic interactions. The temperature dependence of the free energy of binding deltaG degrees is weak because of the enthalpy-entropy compensation caused by a large heat capacity change, deltaCp =-4.3+/-0.1 kJ/K/mol of monomeric ACE. The strong favorable binding entropy and the negative deltaCp indicate both a large contribution to binding due to hydrophobic effects, which seem to originate from dehydration of the ligand-protein interface, and slight conformational changes in the vicinity of the active sites.