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Sodium sulfate decahydrate
(Glauber's salt)
CAS no: 7727-73-3 Formula: Na2SO4.10H2O Molecular weight: 322.197
Physical Data
Appearance: Colorless monoclinic, efflorescent or granules crystals.
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Melting point: 32°C (decompose)
Boiling point: -
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Density: 1.46 g/cm3
Solubility: 28.1 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
Sodium sulfate decahydrate can be obtained from the treatment of sodium chloride with sulfuric acid:
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It is also produce industrially by the reaction of magnesium sulfate and sodium chloride in solution followed by crystallization. In both cases,
sodium sulfate is subsequently crystallised.
In the laboratory it can be prepared by the neutralization reaction by mixing sodium hydroxide and sulfuric acid.
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Behavior and Chemical Properties
The decahydrate crystals decompose at around 33°C to give the anhydrous salt. The solubility of sodium sulfate increases sharply with temperature and achieve maximum solubility at around 33°C and decreases slowly beyond this temperature.
The anhydrous salt readily adsorbs moisture in air to give the efflorescence decahydrate crystals.
If, say a solution of barium chloride, is added to a solution of sodium sulfate, an insoluble white precipitate of barium sulfate is formed.
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This is an important reaction which is used both as a qualitative and quantitative test for the barium and sulfate ions.
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History and Uses
The preparation of sodium sulfate from sodium chloride (common salt) and sulfuric acid
was discovered by Johann R Glauber (1604-1668), a German-Dutch chemist. The white efflorescense residue is called sal mirabile, or Glauber's salt.
The decahydrate crystals are used in printing textiles, standardizing dyes and freezing mixture.
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Hazard, Storage and Handling
Keep in a tightly closed container and isolate from incompatible substances such as aluminium, magnesium and strong acids and bases.
Not expected to be a health hazard when sodium sulfate is inhaled or come into skin contact. It may be mildly toxic by ingestion. Because of its
osmosis activity, it will draw water into the lumen of the bowel and may cause purging, fluid loss, fall of blood pressure and
blood in stools.
No adverse effects is expected upon eye contact, although this should be avoided as it may couse mild irritation.
Use usual emergency measures upon skin contacts: wash with soap and water. Upon eye contact splash with running water. Get medical attention if
irritation develops. If swallowed, give several glasses of water to drink.
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(Last update: February 2006) |
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