Lanthanum(III) chloride

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Lanthanum(III) chloride
Lanthanum(III) chloride
Anhydrous
Names
Other names
Lanthanum trichloride
Identifiers
3D model (
JSmol
)
ChemSpider
ECHA InfoCard
 100.030.202 Edit this at Wikidata
EC Number
  • 233-237-5
UNII
  • InChI=1S/3ClH.La/h3*1H;/q;;;+3/p-3 checkY
    Key: ICAKDTKJOYSXGC-UHFFFAOYSA-K checkY
  • InChI=1/3ClH.La/h3*1H;/q;;;+3/p-3
    Key: ICAKDTKJOYSXGC-DFZHHIFOAJ
  • Cl[La](Cl)Cl
Properties
LaCl3
Molar mass 245.264 g/mol (anhydrous)
353.36 g/mol (hexahydrate)
371.37 g/mol (heptahydrate)
Appearance white odorless powder
hygroscopic
Density 3.84 g/cm3[1]
Melting point 858 °C (1,576 °F; 1,131 K) (anhydrous)[1]
Boiling point 1,000 °C (1,830 °F; 1,270 K) (anhydrous)
957 g/L (25 °C)[1]
Solubility soluble in ethanol (heptahydrate)
Structure[2]
UCl3 type), hP8
P63/m, No. 176
a = 0.74779 nm, b = 0.74779 nm, c = 0.43745 nm
2
Tricapped trigonal prismatic,(nine-coordinate)
Related compounds
Other anions
 Lanthanum oxide
Other cations
 Cerium(III) chloride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Lanthanum chloride is the inorganic compound with the formula LaCl3. It is a common salt of lanthanum which is mainly used in research. It is a white solid that is highly soluble in water and alcohols.

Preparation

Anhydrous lanthanum(III) chloride can be produced by the

ammonium chloride route.[3][4][5]
In the first step, lanthanum oxide is heated with ammonium chloride to produce the ammonium salt of the pentachloride:

La2O3 + 10 NH4Cl → 2 (NH4)2LaCl5 + 6 H2O + 6 NH3

In the second step, the ammonium chloride salt is converted to the trichlorides by heating in a vacuum at 350-400 °C:

(NH4)2LaCl5 → LaCl3 + 2 HCl + 2 NH3

Uses

Lanthanum chloride is also used in biochemical research to block the activity of divalent

calcium channels. Doped with cerium, it is used as a scintillator material.[6]

In

Lewis acid for converting aldehydes to acetals.[7]

The compound has been identified as a

catalyst for the high pressure oxidative chlorination of methane to chloromethane with hydrochloric acid and oxygen.[8]

Also used in the field of geology as a very dilute solution, which when combined with the proper acids can help identify small >1% Strontium content in powdered rock samples.

References

  1. ^
    ISBN 978-1439855119
    .
  2. doi:10.1063/1.1670543
    .
  3. ^ Brauer, G., ed. (1963). Handbook of Preparative Inorganic Chemistry (2nd ed.). New York: Academic Press.
  4. ^ Meyer, G. (1989). "The Ammonium Chloride Route to Anhydrous Rare Earth Chlorides—The Example of Ycl 3". The Ammonium Chloride Route to Anhydrous Rare Earth Chlorides-The Example of YCl3. Inorganic Syntheses. Vol. 25. pp. 146–150.
    ISBN 978-0-470-13256-2
    .
  5. ISBN 978-3-13-103021-4
    .
  6. doi:10.1063/1.2436269
    .
  7. doi:10.3998/ark.5550190.0008.d23
    .
  8. PMID 17295483
    .
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