Barium sulfite

Structural formula
General
Surname	Barium sulfite
Molecular formula	BaSO 3
Brief description	white odorless solid
External identifiers / databases
CAS number 7787-39-5 EC number 232-112-2 ECHA InfoCard 100.029.193 PubChem 6096951 Wikidata Q415543
properties
Molar mass	217.39 g mol −1
Physical state	firmly
density	4.43 g cm −3
solubility	very sparingly soluble in water (0.2 g l −1 )
safety instructions
GHS labeling of hazardous substances Caution H and P phrases H: 332-302 P: ?
As far as possible and customary, SI units are used. Unless otherwise noted, the data given apply to standard conditions .

Barium sulfite is a chemical compound from the group of barium compounds and sulfites .

Extraction and presentation

Barium sulfite can be obtained by reacting sodium sulfite with a solution of barium chloride or barium hydroxide .

${\displaystyle \mathrm {Na_{2}SO_{3}+BaCl_{2}\longrightarrow 2\ NaCl+BaSO_{3}} }$

${\displaystyle \mathrm {Na_{2}SO_{3}+Ba(OH)_{2}\longrightarrow 2\ NaOH+BaSO_{3}} }$

properties

Physical Properties

Barium sulfite is a white, odorless, non-flammable solid that is very sparingly soluble in water. It is easily soluble in acids. It has a monoclinic crystal system with a unit cell size of 664.7 × 548.3 × 464.5 A and an angle of 106.3 °. A triclinic shape is also known.

Chemical properties

Barium sulfite can be quantitatively oxidized to barium sulfate with hydrogen peroxide .

${\displaystyle \mathrm {BaSO_{3}+H_{2}O_{2}\longrightarrow BaSO_{4}+H_{2}O} }$

When a solution of barium sulphite is heated in sulphurous acid, it decomposes with the formation of barium sulphate and a polythionate.

When annealing in the absence of air, barium sulfite decomposes into barium sulfate and barium sulfide .

Web links

• IR spectrum (PDF; 3.0 MB)

Individual evidence

1. ↑ ^{a b c d} Entry for CAS no. 7787-39-5 in the GESTIS substance database of the IFA , accessed on January 22, 2012(JavaScript required) .
2. ^ ^{A b} Jean D'Ans, Ellen Lax: Paperback for chemists and physicists. 3. Elements, inorganic compounds and materials, minerals, Volume 3. 4. Edition, Springer, 1997, ISBN 978-3-540-60035-0 , p. 330. ( limited preview in the Google book search).
3. ↑ D. Van Nonstrant Company: Elementary General Chemistry . 1941 ( page 342 in the Google book search).
4. ↑ ^{a b} C. Saint-Pierre: "Sur la décomposition spontanée de divers bisulfites" in Compt. Rend. Hebd. 1872 , 74 , pp. 52-53. Full text
5. ↑ ^{a b c} R. Abegg, F. Auerbach: Handbuch der inorganic Chemie , Verlag S. Hirzel, Vol. 2, 1908. P. 270; Full text
6. ↑ RSW Braithwaite, AR Kampf, RG Pritchard, RPH Lamb: "The occurrence of thiosulfates and other unstable sulfur species as natural weathering products of old smelting slags" in Mineralogy and Petrology 1993 , 47 (2-4), pp. 255-261 . doi : 10.1007 / BF01161570
7. ^ A. Classen, O. Bauer: "About the applicability of hydrogen peroxide in analytical chemistry" in reports of the German chemical society 1883 , pp. 1061-1074. Full text