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François-Marie Raoult

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François-Marie Raoult
François-Marie Raoult
Born10 May 1830
Fournes
Died1 April 1901 (1901-05) (aged 70)
Grenoble
NationalityFrench
Known forRaoult's law
AwardsDavy Medal (1892)
Scientific career
FieldsChemistry

François-Marie Raoult (/rɑːˈuːl/; 10 May 1830 – 1 April 1901) was a French chemist who conducted research into the behavior of solutions, especially their physical properties.

Life and work

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Raoult was born at Fournes, in the département of Nord. He became aspirant répétiteur at the Lycée of Reims in 1853, and after holding several intermediate positions was appointed in 1862 to the professorship of chemistry in Sens lycée. There he prepared a thesis on electromotive force which gained him a doctor's degree in Paris the following year.[1]

In 1867 Raoult was put in charge of chemistry classes at the University of Grenoble, and three years later he succeeded to the chair of chemistry, which he held until his death in 1901. Raoult's earliest researches were physical in character, being largely concerned with the phenomena of the voltaic cell; later there was a period when more purely chemical questions engaged his attention.[1]

Raoult's name is best known in connection with work on solutions, to which he devoted the last two decades of his life. His first paper describing how solutes depressed the freezing points of solutions was published in 1878.[2] Further experiments with various solvents, such as benzene and acetic acid, in addition to water, led him to believe in a simple relation between the molecular weights of a solute and the freezing-point of a solution. He expressed the relationship as the loi générale de la congélation (general law of freezing), that if one molecule of a substance be dissolved in 100 molecules of any given solvent, the temperature of solidification of the latter will be lowered by 0.63 °C.[1] Another relation on which Raoult worked was that concerning the depression of a solvent's vapor pressure, due to a solute, showing that the decrease is proportional to the solute's molecular weight. This relationships holds best in the limiting case of a dilute solution.[3] These two generalizations afforded a new method of determining the molecular weights of dissolved substances, and were utilized by Jacobus van 't Hoff and Wilhelm Ostwald, among other chemists, in support of the hypothesis of electrolytic dissociation in solutions. Raoult's freezing-point depression method became even more useful after it was improved by Ernst Otto Beckmann and became a standard technique for determining molecular weights of organic substances.[4]

An account of Raoult's life and work was given by van 't Hoff in a memorial lecture delivered before the London Chemical Society on 26 March 1902.[5]

Activities and honors

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References

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  1. ^ a b c Chisholm 1911.
  2. ^ F.-M. Raoult (1878) "Sur la tension de vapeur et sur le point de congélation des solutions salines" (On vapor pressure and on the freezing point of saline solutions), Comptes rendus, 87 : 167-169.
  3. ^ Note:
    • Raoult first stated his law in terms of the reduction of the freezing points of solutions:
    1. F.-M. Raoult (1882) "Loi de congélation des solutions benzéniques des substances neutres" (Law of freezing of solutions of neutral substances in benzene), Comptes rendus, 95 : 187-189. From p. 189: "Il est donc permis de dire, dès à présent: Dans une multitude de cas, l'abaissement du point de congélation d'un dissolvant ne dépend que du rapport entre le nombres de molécules du corps dissous et du dissolvant; il est indépendant de la nature, du nombre, de l'arrangement des atomes qui composent les molécules dissoutes." (It is thus allowable to say, as of now: In the multitude of cases, the lowering of the freezing point of a solvent depends only on the relation between the number of molecules of the dissolved substance and of the solvent; it is independent of the nature, number, [or] arrangement of the atoms composing the dissolved molecules.)
    2. In his next paper, Raoult specified (p. 1033) that in a solution containing one mole of solute per 100 moles of solvent, the freezing point is reduced by 0.62 °C, regardless of the nature of solute or solvent. See: F.-M. Raoult (1882) "Loi générale de congélation des dissolvants" (General law of the freezing of solvents), Comptes rendus, 95 : 1030-1033. English translation available on-line at: Le Moyne College
    • Raoult later stated his law in terms of the reduction of the vapor pressures of solutions:
    1. F.-M. Raoult (1887) Loi générale des tensions de vapeur des dissolvants" (General law of vapor pressures of solvents), Comptes rendus, 104 : 1430-1433.
    2. This reduction in vapor pressure had been predicted, via thermodynamic calculations, by two investigators:
  4. ^ By 1889, Beckmann had developed a convenient apparatus for measuring the increase in the boiling points of solutions. See:
  5. ^ Jacobus Henricus van 't Hoff (1902). "Raoult Memorial Lecture". Journal of the Chemical Society, Transactions. 81: 969–981. doi:10.1039/CT9028100969.

Further reading

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  • Morachevskii, A. G. (2005). "Francois Marie Raoult (To 175th Anniversary of His Birthday)". Russian Journal of Applied Chemistry. 78 (5): 856–858. doi:10.1007/s11167-005-0409-6. S2CID 94880672.
  • Wisniak, Jaime (2001). "François-Marie Raoult: Past and Modern Look". The Chemical Educator. 6 (1): 41–49. doi:10.1007/s00897000432a. S2CID 120321275.
  • Getman, Frederick H. (1936). "Francois-Marie Raoult, Master Cryoscopist". Journal of Chemical Education. 13 (4): 153–155. doi:10.1021/ed013p153.
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