E.m.f. studies of electrolytic dissociation. Part 7.—Some alkali and alkaline earth metal hydroxides in water

Abstract

The dissociation constants of the ion-pairs LiOH, NaOH, CaOHf, SrOHf and BaOH+ in water at several temperatures, and of CsCl at 25" C, have been calculated from e.m.f. measurements of the cell Pt, H2/M, OH-, X-/AgX/Ag.Although the alkali metal hydroxides are generally regarded as completely strong electrolytes, there are indications that the first two members do not fully dissociate in aqueous solution. Thus Kolthoff,l using an indicator method, concluded that LiOH has a dissociation constant K of about 0.5, while Darken and Meier 2 obtained 1.2 from conductivity data. The latter authors also estimated that K -5 for NaOH, but they did not regard the evidence for this as very conclusive. However, Bell and Prue 3 also report K -5 for NaOH from their kinetic studies, and point out that activity coefficients also suggest that NaOH does not dissociate completely since its value is about 8 % lower at 0.5 M than

IUPAC-NIST Solubility Data Series. 95. Alkaline Earth Carbonates in Aqueous Systems. Part 1. Introduction, Be and Mg

“…For Sr and Ba, the same values as for Ca were used. 91 Bell and Prue, 92 Bell and George, 93 Gimblett and Monk, 94 Bates et al, 95 Martynova et al, 68 McGee and Hostetler, 96 Seewald and Seyfried, 97 and a compilation of Baes and Mesmer. 98 These are summarized in Table 11.…”

“…75 Hence, it is much easier to determine the temperature dependence of the equilibrium constant of reaction (94). Based on this idea, and the data of Table 8, an equation of the form A þ B=T was fitted to the data, transformed to Eq.…”

Fluxes of dissolved carbon dioxide and inorganic carbon from an upland peat catchment: implications for soil respiration

“…(K 4 ),Gimblett and Monk (1954) (K 5 ),Covington et al (1977) (K 6 ), and Stumm and Morgan (1995) (K H ).…”

Electrokinetic properties of calcium aluminate hydrates

“…Activity coefficients at x = 0 were calculated from the Debye-Hiickel equation as given by Gimblett and Monk (15); the ionic strength I used in this calculation was taken proportional to the concentration of univalent ions of opposite charge:…”