DETERMINATION OF ION ASSOCIATION IN DILUTE AQUEOUS LITHIUM-CHLORIDE AND LITHIUM HYDROXIDE SOLUTIONS TO 600-DEGREES-C AND 300 MPA BY ELECTRICAL CONDUCTANCE MEASUREMENTS
Pc. Ho et Da. Palmer, DETERMINATION OF ION ASSOCIATION IN DILUTE AQUEOUS LITHIUM-CHLORIDE AND LITHIUM HYDROXIDE SOLUTIONS TO 600-DEGREES-C AND 300 MPA BY ELECTRICAL CONDUCTANCE MEASUREMENTS, Journal of chemical and engineering data, 43(2), 1998, pp. 162-170
The limiting molar conductances (Lambda(0)) and ion association consta
nts of dilute aqueous lithium chloride and lithium hydroxide solutions
(<0.01 mol.kg(-1)) were determined by electrical conductance measurem
ents at temperatures from 100 to 600 degrees C and pressures up to 300
MPa. The values of Lambda(0)(LiCl) and Lambda(0)(LiOH) obtained from
with Shedlovsky (at densities greater than or equal to 0.6 g.cm(-3)) a
nd Fuoss-Hsia-Fernandez-Prini (FHFP) equations (at densities <0.6 g.cm
(-8)) increase with increasing temperature up to 300 degrees C and dec
reasing density. Above 300 degrees C and densities between 0.8 and 0.5
g.cm(-3) for LiCl(aq) and 0.8 to 0.6 g.cm(-3) for LiOH(aq), Lambda(0)
is nearly temperature-independent but does increase linearly with dec
reasing density. The molal association constants, K-A(m) for both elec
trolytes were computed exclusively from the data greater than or equal
to 400 degrees C (at densities 0.8-0.3 for LiCl and 0.8-0.5 g.cm(-3)
for LiOH) by the Shedlovsky equation and can be represented as functio
ns of temperature (Kelvin) and the logarithm of water density (rho(w))
as follows: log K-A(m)(LiCl) = 0.724 - 8.980/(T/X) - (12.796 - 5431.2
/(T/K)) log rho(w)/g.cm(-3)) and log K-A(m)(LiOH) = 0.856 + 135.60/(T/
K) - (11.998 - 4226.3/(T/K)) log rho(w)/(g.cm(-3)). At corresponding c
onditions and within experimental error, the degree of ion association
of LiCl(aq) is comparable with NaCl(aq) and KCl(aq), whereas ion asso
ciation for LiOH(aq), is significantly stronger than for NaOH(aq) and
KOH(aq). Moreover, the same values of K-A(m) were obtained for each el
ectrolyte irrespective of the whether the Shedlovsky or FHFP equations
were employed. This point is exemplified by a comparison of the K-A(m
) value for LiCl obtained from the present study with those of a recen
t investigation that utilized an advanced design for moderately high t
emperature conductance measurements.