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Element Index
Samarium
Scandium
Seaborgium
Selenium
Silicon
Sodium
Strontium
Sulfur
Chemical's truth
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Combinatorial chemistry is the study of techniques capable of rapidly synthesizing and generating millions of related compounds. |
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Sodium carbonate, decahydrate
(sal soda, washing soda)
CAS no: 6132-02-1 Formula: Na2CO3.10H2O Molecular weight: 286.142
Physical Data
Appearance: Colorless crystalline solids
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Melting point: 34°C (decompose)
Boiling point: -
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Density: 1.46 g/cm3
Solubility: 30.7 g/100 g H2O
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Thermodynamic Data
Enthalpy of formation: -
Gibbs energy of formation: -
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Entropy: -
Heat capacity: -
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Production and preparation
Previously, sodium carbonate was obtained from seaweed ashes, which the name 'soda ash' was derived.
The substance can now be obtained from several mineral sources such as trona, Na2CO3.NaHCO3.nH2O, and natron,
Na2CO3.
Natron, a powdery mass, encased in a plastic cover, to prevent adsorption of moisture. It is obtained from British Columbia.
Alternatively, it can be obtained from the ammonia-soda (Solvay) process. It was first carried out successfully in Belgium in the 1860s to
produce sodium carbonate. It was patented in 1861 by the Belgian chemist Ernest Solvay (1838-1922). In this process, a concentrated brine is treated with ammonia and carbon
dioxide (from calcium carbonate) to give sodium bicarbonate and ammonium chloride. Sodium carbonate is produced by simply
heating sodium bicarbonate. The decahydrate crystals can be obtained by crystallization from solutions. Ammonia is recovered when ammonium chloride is heated with lime.
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Behavior and Chemical Properties
Sodium carbonate decahydrate readily effloresces on exposure to air. It decomposes at about 34°C to give the monohydrate compound.
It behaves as a weak alkali when dissolves in water. For example, in 19% aqueous solution the pH ~11.5. It reacts with acids to release carbon dioxide.
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When carbon dioxide is bubbled into a carbonate solution, sodium bicarbonate (hydrogen carbonate) is formed:
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History and Uses
Sodium carbonate is one of the most important starting materials in chemical manufacturing. The decahydrate compound was once used extensively as washing powders and household cleansing agent. However,
the market was eroded due to the increase domestic use of detergents. It is also used as a bleach for cotton and linen.
In the laboratory, sodium carbonate is used in volumetric analysis to standardize acids, and in qualitatively way, for testing cations. This is because sodium carbonate solution gives
precipitates for salts of many metals as the metal carbonate or basic carbonate. In the case of insoluble salts (such as barium sulfate), it is
fused with solid sodium carbonate. Potassium carbonate is usually added to lower the melting point (fusion mixture).
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Hazard, Storage and Handling
Keep in a tightly closed container and isolate from incompatible substances, such as strong acids and aluminium. Dust is dry and fine and ensure the container is stored in a cool, dry and well-ventilated area.
Cause eye irritation and upon prolonged exposure may result skin irritation. It is only slightly toxic but harmful when ingested in large doses. The symptons may include abdominal
pain, vomiting, diarrhea and even death. Inhalation of dust may aggravate asthma and other chronic pulmonary diseases. The oral LD50 for rats is 3160 mg/kg.
Upon spillage, splash the affected area with plenty of water. If swallowed, give plenty of water or milk to drink and seek medical advice. Do not induce vomiting. Do not give acidic fluids such as carbonated drinks or vinegar.
Avoid breathing dust.
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(Last update: March 2006) |
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