8. The lattice energy of NaCl calculated using the Madelung
constant of the NaCl structure type is +788 kJ/mol. The
estimated enthalpy of hydration for sodium and chloride ions are
-406 and -363 kJ/mol respectively. Estimate the enthalpy of
solvation for NaCl.
10. The enthalpy of crystallization for KCl is -715 kJ/mol. The
enthalpies of hydration for potassium and chloride are -322 and
-363 kJ/mol respectively. From these values, estimate the
enthalpy of solution for KCl.
11. The lattice energy of NaCl calculated using the Madelung
constant of the NaCl structure type is +788 kJ/mol. The
estimated enthalpy of hydration for sodium and chloride ions
are -406 and -363 kJ/mol respectively. Estimate the enthalpy
of solvation for NaCl.
12. The hydration number
(solvation number)
The average number of molecules bound to the compound more
strongly than they are bound to other water molecules.
13. The hydration number
(solvation number)
The average number of molecules bound to the compound more
strongly than they are bound to other water molecules.
15. Electrophoreticeffect
Λc
m = Λ0
m – (A + B Λ0
m) √C
Λc
m = molar conductance of the electrolyte solution of
concentration C mol L-1.
Λ0
m = molar conductance of the electrolyte solution at infinite
dilution.
A and B = constant terms for a particular solvent at a given
temperature.
