Abstract
The concentration of free water molecules at the surface of a strong sulfuric acid solution is found to be very low, mainly as a consequence of the formation of acid hydrates. Values of equilibrium constants and enthalpy changes for successive hydration reactions of H2SO4 have been calculated from the variation of water vapour pressure with acid strength and temperature. The results support the conclusion of Fried et al. that the rate of reaction of a molecule such as N2O5 with a sulfuric acid aerosol is controlled by the rate at which the molecule can penetrate into the bulk of the liquid.
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