D. G. Archer
Feb 4, 2005
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Journal
Journal of Chemical & Engineering Data
Abstract
An adiabatic calorimeter was used to measure the enthalpy of solution of potassium tetrafluoroborate (0.01 mol·kg-1 to 0.02 mol·kg-1) in water and in aqueous sodium fluoride of different ionic strengths (0.2 mol·kg-1 and 0.5 mol·kg-1) at 298 K and 313 K. The present results yield the standard-state enthalpy and heat capacity for the solution process and, when combined with literature values for solubilities, yield the standard-state entropy of the solution process. From these properties, and previous measurements involving potassium tetrafluoroborate, we provide a new analysis of thermodynamic properties of the aqueous tetrafluoroborate ion and compare these new properties to previous tabulations and explain the sources of discrepancies in the literature.