Barium acetate
| Names | |
|---|---|
| IUPAC name
Barium acetate
| |
| Other names
Barium diacetate
| |
| Properties | |
| BaC4H6O4 Ba(CH3COO)2 | |
| Molar mass | 255.415 g/mol |
| Appearance | Colorless crystalline solid |
| Odor | Odorless |
| Density | 2.468 g/cm3 (anhydrous) 2.19 g/cm3 (monohydrate) |
| Melting point | 450 °C (842 °F; 723 K) (decomposition) |
| Boiling point | Decomposes |
| 55.8 g/100 ml (0 °C) 71 g/100ml (20 °C) 75 g/100ml (30 °C) 79 g/100ml (40 °C)[1] | |
| Solubility | Soluble in acetic acid Slightly soluble in ethanol, methanol Insoluble in acetone |
| Solubility in acetic acid | 13.9 g/100 ml (22.5 °C) 75.4 g/100 ml (88 °C)[2] |
| Solubility in ethanol | 0.092 g/100 ml (25 °C)[3] |
| Solubility in methanol | 0.55 g/100 ml (18 °C) 0.23 g/100 ml (66 °C)[4] |
| Vapor pressure | ~0 mmHg |
| Thermochemistry | |
| Std enthalpy of
formation (ΔfH |
-1,485.7 kJ/mol[5] |
| Hazards | |
| Safety data sheet | Sigma-Aldrich |
| Flash point | Non-flammable |
| Lethal dose or concentration (LD, LC): | |
| LD50 (Median dose)
|
921 mg/kg (rat, oral) |
| Related compounds | |
| Related compounds
|
Barium formate |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Barium acetate is the acetic acid salt of barium. It has the formula Ba(CH3COO)2.
Contents
Properties
Chemical
Barium acetate will react with a soluble sulfate salt, like sodium sulfate, to yield the very insoluble barium sulfate. This is a good way of neutralizing any barium acetate that may have been ingested.
- Ba(CH3COO)2 + Na2SO4 → BaSO4 + 2 CH3COONa
If concentrated sulfuric acid is used, pure acetic acid is obtained (also known as glacial acetic acid).
Thermal decomposition of barium acetate yields barium carbonate and acetone, as well as traces of organic side products from the decomposition reaction:
- Ba(CH3COO)2 → BaCO3 + (CH3)2CO
Physical
Barium acetate is a hygroscopic white solid, soluble in water and acetic acid, while slightly soluble in alcohol.
Availability
Barium acetate is sold by chemical suppliers.
Since it's a soluble barium salt, in some countries its sale may be regulated.
Preparation
Barium acetate is generally produced by the reaction of acetic acid with barium carbonate, hydroxide or oxide:
- BaCO3 + 2 CH3COOH → Ba(CH3COO)2 + H2O + CO2
- Ba(OH)2 + 2 CH3COOH → Ba(CH3COO)2 + 2 H2O
- BaO + 2 CH3COOH → Ba(CH3COO)2 + H2O
Projects
- Compound collecting
- Make acetone
- Make glacial acetic acid
Handling
Safety
Barium acetate is soluble in water, which makes it toxic. Solutions of soluble sulfate salts, such as Epsom salt (magnesium sulfate) or sodium sulfate may be given as first aid for barium poisoning, as they precipitate the soluble barium to the insoluble (and non-toxic) barium sulfate.
Storage
In closed plastic or glass bottles, away from acidic vapors.
Disposal
Barium acetate can be precipitated to the non-toxic barium sulfate by adding sodium or magnesium sulfate to its solution. The resulting barium sulfate doesn't require special disposal and can be dumped in trash.
References
- ↑ Краткий справочник химика. - Под ред. Перельмана В.И. - М.-Л.: Химия, 1964 (A quick reference book of a chemist. - Ed. Perelman V.I. - M.-L .: Chemistry, 1964)
- ↑ Справочник экспериментальных данных по растворимости солевых систем. - Т. 4. - Л.: ГНТИХЛ, 1963 pp. 2630 (Handbook of experimental data on the solubility of salt systems. - T. 4. - L .: GNTIHL, 1963 pp. 2630)
- ↑ Справочник по растворимости. - Т.1, Кн.1. - М.-Л.: ИАН СССР, 1961 (Solubility Handbook. - Vol. 1, Book 1. - M.-L .: IAN USSR, 1961)
- ↑ H. Henstock, J. Chem. Soc., 1934, 1340-1343
- ↑ Franzosini P., Sanesi M. Thermodynamic and transport properties of organic salts. - IUPAC Chemical Data Series, No. 28. - Pergamon Press, 1980 pp. 104
