Abstract
The familiar “basic” solution of aqueous solution chemistry is produced by reacting the Lewis base Na2O with the Lewis acid H2O initially to produce the “neutral” compound NaOH and by then adding a large excess of the acid component (55.5 : 1 molar ratio for a one molar solution). In an exactly analogous fashion an ordinary silicate glass is produced by reacting the same Lewis base Na2O with the Lewis acid SiO2, initially to form the neutral Na4SiO6 compound, and by then adding a large excess of the acid component. It is not surprising then that the chemistry of the two types of acid-base systems should have common features: both are characterized by very low values of the mean oxide activity \(\,_{\text{a}}{\underset{\pm}{\text{N}}}\text{a}_2\text{O}\).
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© 1978 Plenum Press, New York
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Angell, C.A. (1978). Electron Free Energy Levels and Spectroscopic Character of Dilute Species in Oxidic Solvents: Relating Aqueous to Liquid (and Vitreous) Oxide Solutions. In: Mamantov, G. (eds) Characterization of Solutes in Nonaqueous Solvents. Springer, Boston, MA. https://doi.org/10.1007/978-1-4613-3982-3_13
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DOI: https://doi.org/10.1007/978-1-4613-3982-3_13
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