Isothermal titration calorimetry (ITC) is now routinely used to directly characterize the thermodynamics of biopolymer binding interactions and the kinetics of enzyme-catalyzed reactions. This is the result of improvements in ITC instrumentation and data analysis software. Modern ITC instruments make it possible to measure heat effects as small as 0.1 microcal (0.4 microJ), allowing the determination of binding constants, K's, as large as 10(8) - 10(9)M(-1). Modern ITC instruments make it possible to measure heat rates as small as 0.1 microcal/sec, allowing for the precise determination of reaction rates in the range of 10(-12) mol/sec. Values for K(m) and k(cat), in the ranges of 10(-2) - 10(3) microM and 0.05 - 500 sec(-1), respectively, can be determined by ITC. This chapter reviews the planning of an optimal ITC experiment for either a binding or kinetic study, guides the reader through simulated sample experiments, and reviews analysis of the data and the interpretation of the results.

Isothermal Titration Calorimetry: Experimental Design, Data Analysis, and Probing Macromolecule/Ligand Binding and Kinetic Interactions

We have summarized results of many experimental investigations of the thermodynamics of ionization of H2O(liq.) from 0–300°C and from 1.0 atm to nearly 8000 atm. Results of these investigations (equilibrium constants, enthalpies of ionization, heat capacities, partial molal volumes, and compressibilities) have been used for a number of thermodynamic calculations. It is particularly noteworthy that it is possible to use thermal data from 0–145°C with an equilibrium constant for 25°C in calculating reasonably accurate equilibrium constants for temperatures as high as 300°C. Similarly, it is possible to use volumetric data that refer to 1.0 atm in calculating useful equilibrium constants that apply for pressures as high as 2000 atm.

Thermodynamics of ionization of water over wide ranges of temperature and pressure

Review of trace toxic elements (Pb, Cd, Hg, As, Sb, Bi, Se, Te) and their deportment in gold processing. Part 1: Mineralogy, aqueous chemistry and toxicity

Thermodynamics for ionization of water at temperatures from 278.15 K to 393.15 K and at the pressure 0.35 MPa: apparent molar volumes of aqueous KCl, KOH, and NaOH and apparent molar heat capacities of aqueous HCl, KCl, KOH, and NaOH☆

Cyanide does more to inhibit heme enzymes, than merely serving as an active-site ligand

Thermodynamics of metal cyanide coordination: Part IX. Log K, ΔHO, and ΔSO values for the Ni2+-, Zn2+-, Cd2+-, and Hg2+- CN− systems at 10, 25, and 40 °C☆

Calorimetric Determination of the Heat of Ionization of Water at 10° and 40°C*

Thermodynamik der metallcyanid-koordination 9. mitt. log k, h(0)- und s(0)-werte fuer die syst. ni(ii)-, zn(ii)-, cd(ii)- und hg(ii)-cn(-) bei 10, 15 und 40 grad

H.D. Johnston

Papers

Thermodynamics of metal cyanide coordination: Part IX. Log K, ΔHO, and ΔSO values for the Ni2+-, Zn2+-, Cd2+-, and Hg2+- CN− systems at 10, 25, and 40 °C☆

Calorimetric Determination of the Heat of Ionization of Water at 10° and 40°C*

Thermodynamik der metallcyanid-koordination 9. mitt. log k, h(0)- und s(0)-werte fuer die syst. ni(ii)-, zn(ii)-, cd(ii)- und hg(ii)-cn(-) bei 10, 15 und 40 grad