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Part 2. Cryoscopy

  • Chapter
Experimental Thermodynamics Volume II

Abstract

As a professor at the University of Grenoble, François-Marie Raoult formulated many of the basic laws of physical chemistry. One of these laws provides a definition for so-called ‘ideal solutions’; another one has a much broader content than was at first thought. It is the ‘cryoscopic’ law, which was so named by Raoult himself, from the Greek words χρνος (ice) and σκοπεω (I observe)64. Chemists, however, just saw in it one of the methods of determination of molar masses. It was only when van’t Hoff84 gave an expression for the solvent cryoscopic constant that Raoult’s experimental work gained universal acceptance.

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Abbreviations

A:

Coefficient of Debye-Höckel theory

a:

Ionic parameter of Debye-Höckel theory

a i :

Activity of particle i

a + :

Ideal activity of ionic substance

B:

Coefficient of Debye-Höckel theory

c:

Molarity (number of moles per liter of solvent)

d:

Density

E:

e.m.f. of one couple

f i :

Rational symmetric activity coefficient of component i

G:

Molar Gibbs function (free enthalpy)

g:

Gibbs function for n molecules or moles

I:

Ionic strength

i:

van’t Hoff coefficient

j:

Lewis cryoscopic variable

L i :

Heat of fusion, component i

l:

Length of wire

ln:

Natural or Napierian logarithm

log:

Decimal or common logarithm

m:

Molality (number of moles per kilogram of solvent)

N:

Number of junctions

R:

Universal ideal gas constant

R g :

Charging resistance

R j :

Resistance of wires

S or S' :

Cross-sectional area of a wire

S f :

Molar melting entropy

T:

Kelvin temperature

T 0i :

Melting point of pure component i

W:

Interaction parameter for regular solutions

X i :

Mole fraction, component i

Z i :

Ionic charge of ith ion

α:

Molecular dissociation coefficient

γ:

Practical dissymmetrical activity coefficient of solute

γ± :

Mean activity coefficient of ions

δ:

Hydrolysis ratio

Δc :

Difference of the molar specific heats of the liquid and the solid component

ΔS :

Entropy of mixing

θ:

Cry oscopic depression (T 01 − T)

λ:

Cryoscopic constant in molai scale

v:

Total number of ions in the molecule

v i :

Number of ions of type i

v i ' :

Number of ions of the solute common to the solvent of type i

π:

Osmotic pressure

π ' :

Osmotic pressure in milliosmols

ø:

Practical osmotic coefficient

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Authors and Affiliations

  1. Laboratoire de Thermodynamique, Université de Provence, Centre de St Jerome, 13013, Marseille, France

    Y. Doucet

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  1. Laboratoire des Interactions Moléculaires et des Hautes Pressions, CNRS, Meudon, France

    B. Le Neindre  & B. Vodar  & 

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Doucet, Y. (1968). Part 2. Cryoscopy. In: Le Neindre, B., Vodar, B. (eds) Experimental Thermodynamics Volume II. Springer, Boston, MA. https://doi.org/10.1007/978-1-4899-6569-1_25

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  • DOI: https://doi.org/10.1007/978-1-4899-6569-1_25

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