Mean distance of closest approach of ions: Sodium salts in aqueous solutions

Ribeiro, Ana C.F.; Esteso, Miguel A.; Lobo, Victor M.M.; Amado, Ana M.; Costa, A. M. Amorim da; Sobral, Abílio J.F.N.; Azevedo, Eduarda F. G.; Ribeiro, Maria Aparecida

doi:10.1016/j.molliq.2005.12.004

Cited by 14 publications

(7 citation statements)

References 29 publications

Supporting

Mentioning

Contrasting

Order By: Relevance

“…[46]. That is, the ab initio values and the values calculated from MM2-0 and Marcus data (a = R 1 + R 2 ) are similar, whereas those found from MM2-1 and the other Marcus data (a = d cation-water + d anion-water ), i.e., by considering one water molecule placed in between both ions, are larger.…”

Section: Molecular Mechanics Studies (Mm2)supporting

confidence: 59%

“…By looking at Table 1, some other analogies with the sodium results [46] are observed. Thus, it can be seen that, in general, the values of a obtained by fitting experimental activity coefficients data are greater than the sum of ionic radii in solution (or crystal-lattice spacing) or the interatomic distances, d ion-ion , what could be explained in terms of the presence of the hydration shell for both cations and anions.…”

Section: Resultsmentioning

confidence: 52%

See 1 more Smart Citation

Mean distance of closest approach of ions: Lithium salts in aqueous solutions

Ribeiro

Lobo

Valente

et al. 2008

Journal of Molecular Liquids

Self Cite

View full text Add to dashboard Cite

show abstract

Section: Molecular Mechanics Studies (Mm2)supporting

confidence: 59%

Section: Resultsmentioning

confidence: 52%

Mean distance of closest approach of ions: Lithium salts in aqueous solutions

Ribeiro

Lobo

Valente

et al. 2008

Journal of Molecular Liquids

Self Cite

View full text Add to dashboard Cite

show abstract

“…Because there is no any direct method for measuring this value, it must be estimated [17]. Three different estimations were done: a) Two of them came from Marcus data (Table XIII in [18]) by using two approximations.…”

Section: Resultsmentioning

confidence: 99%

Diffusion coefficients and electrical conductivities for calcium chloride aqueous solutions at 298.15K and 310.15K

Ribeiro¹,

Barros²,

Teles³

et al. 2008

Electrochimica Acta

Self Cite

View full text Add to dashboard Cite

a b s t r a c tExperimental values for mutual diffusion coefficients (interdiffusion coefficients) for CaCl 2 aqueous solutions at 298.15 K and 310.15 K, not available in the literature, were experimentally determined between 0.005 mol dm −3 and 0.1 mol dm −3 . The measurements were performed by using a conductimetric openended capillary cell. Values at infinitesimal concentration, D 0 , were also obtained. These data were analysed using the Onsager-Fuoss and Gordon models. In addition, molar conductance data were measured at 310.15 K for CaCl 2 aqueous solutions at the same concentration range and the value at infinitesimal concentration determined. Afterwards, it was split into the ionic limiting values. By replacing them into the Nernst equation, diffusion coefficients at infinitesimal concentration were derived (1.335 × 10 −9 m 2 s −1 and 1.659 × 10 −9 m 2 s −1 ) at both temperatures (298.15 K and 310.15 K, respectively). They agree well with the extrapolated experimental ones (1.312 × 10 −9 m 2 s −1 and 1.613 × 10 −9 m 2 s −1 ).

show abstract

“…There is no direct method for measuring the ion size parameter a, the ''mean distance of closest approach'' from the Debye-Huckel theory, but it may be estimated from the data of Marcus (table XIII in [17]), considering two approximations [18][19][20][21][22][23]. The first one considers the a-value as the sum of the ionic radii (R ion ) reported by Marcus [17] (i.e., a = 2.7Á10 À10 m).…”

Section: Resultsmentioning

confidence: 99%