Determination of Equilibrium Constants by Titration Calorimetry

  • Lee D. Hansen
  • Mark K. Transtrum
  • Colette F. Quinn
Chapter
Part of the SpringerBriefs in Molecular Science book series (BRIEFSMOLECULAR)

Abstract

The equilibrium constant for a reaction is defined as

References

  1. Broecker J, Vargas C, Keller S (2011) Revisiting the optimal c value for isothermal titration calorimetry. Anal Biochem 418:307–309CrossRefGoogle Scholar
  2. Christensen JJ, Izatt RM, Hansen LD (1967) Thermodynamics of proton ionization in dilute aqueous solution. VII. ΔH0 and ΔS0 values for proton ionization from carboxylic acids at 25°C. J Am Chem Soc 89:213–222CrossRefGoogle Scholar
  3. Christensen JJ, Izatt RM, Wrathall DP, Hansen LD (1969) Thermodynamics of proton ionization in dilute aqueous solution. Part XI. pK, ΔH° and ΔS° values for proton ionization from protonated amines at 25°C. J Chem Soc A:1212–1223Google Scholar
  4. Hansen CW, Hansen LD, Nicholson AD, Chilton MC, Thomas N, Clark J, Hansen JC (2011a) Correction for instrument time constant and baseline in determination of chemical kinetics. Int J Chem Kinetics 43(2):53–61CrossRefGoogle Scholar
  5. Hansen LD, Fellingham GW, Russell DJ (2011b) Simultaneous determination of equilibrium constants and enthalpy changes by titration calorimetry: methods, instruments, and uncertainties. Anal Biochem 409:220–229CrossRefGoogle Scholar
  6. Wiseman T, Williston S, Brandts JF, Lin LN (1989) Rapid measurement of binding constants and heats of binding using a new titration calorimeter. Anal Biochem 179(1):131–137CrossRefGoogle Scholar

Copyright information

© The Author(s) 2018

Authors and Affiliations

  • Lee D. Hansen
    • 1
  • Mark K. Transtrum
    • 2
  • Colette F. Quinn
    • 3
  1. 1.Department of Chemistry and BiochemistryBrigham Young UniversityProvoUSA
  2. 2.Department of Physics and AstronomyBrigham Young UniversityProvoUSA
  3. 3.TA InstrumentsLindonUSA

Personalised recommendations