SODIUM ACETATE

PRODUCT IDENTIFICATION
CAS NO. 127-09-3

SODIUM ACETATE
EINECS NO. 204-823-8
FORMULA CH3COONa
MOL WT. 82.03
H.S. CODE 2915.22

TOXICITY

 Oral rat LD50: 3530 mg/kg
SYNONYMS Acetic acid, sodium salt; Acetic acid, sodium salt (1:1);
Sodium Ethanoate; Acetate De Sodium; Natrium Aceticum; Natriumacetat (German); Sodii Acetas; Acetato de sodio (Spanish); Acétate de sodium (French);

SMILES

 

CLASSIFICATION

 

PHYSICAL AND CHEMICAL PROPERTIES
PHYSICAL STATE white hygroscopic crystalline powder
MELTING POINT 324 C
BOILING POINT  
SPECIFIC GRAVITY 1.45
SOLUBILITY IN WATER

 
pH

8.9
VAPOR DENSITY 2.83
AUTOIGNITION

611 C
NFPA RATINGS Health: 1; Flammability: 1; Reactivity: 0

REFRACTIVE INDEX

  
FLASH POINT

 
STABILITY Stable under ordinary conditions

APPLICATIONS

Sodium Acetate, sodium salt of acetic acid, is a white or colourless crystalline compound, prepared by the reaction of acetic acid with sodium carbonate or with sodium hydroxide. There are commercially anhydrous salt or trihydrate form losing water at 58 C. Both are soluble in water and in ethoxyethane, and slightly soluble in ethanol. Sodium Acetate is a salt of a strong base and a weak acid providing the application to be used as buffers in petroleum production and drilling muds, in food preservations, and in electroplating. It is used as a retardant in elastomer industry. It is used in tanning to effect a more even and rapid penetration of the tan in the leather industry. It is also used as a mordant in dyeing processes. Sodium Acetate is an intermediate to manufacture organic compounds like dyes, pigments, pharmaceuticals, cinnamic acid. It is also used in soap industry and purification of glucose.

SALES SPECIFICATION
ANHYDROUS TECHNICAL GRADE

APPEARANCE

 white odourless powder
PURITY 99.0% min
INSOLUBLE MATTERS

0.01% max
CHLORIDE

0.01% max
CALCIUM

0.1% max
POTASSIUM

0.1% max
SULFATE

0.1% max

IRON

5ppm max
HEAVY METAL(as Pb)

5ppm max
TRIHYDRATE TECHNICAL GRADE

APPEARANCE

 white pr colorless crystals
PURITY 58.0 - 60.0%

FREE ALKALI

0.03% max
INSOLUBLE MATTERS

0.03% max
CHLORIDE

0.04% max
PHOSPHATE

0.1% max
SULFATE

0.02% max

IRON

5ppm max
HEAVY METAL(as Pb)

5ppm max

TRANSPORTATION
PACKING 25kgs, 50kgs in bag
HAZARD CLASS Not regulated
UN NO.  
OTHER INFORMATION

Hazard Symbols: , Risk Phrases: , Safety Phrases: 24/25

GENERAL DESCRIPTION OF BUFFER
Buffer is a substance, generally a solution, that can keep its pH constant, despite the addition of strong acids or strong bases and external influences of temperature, pressure, volume, redox potential. Buffer prevents change in the concentration of another chemical substance, e.g., proton donor and acceptor systems that prevent marked changes in hydrogen ion concentration (pH). Many acid-base reactions take place in living organisms. However, for organisms to perform certain vital functions, the body fluids associated with these functions must maintain a constant pH. For example, blood must maintain a pH of close to 7.4 in order to carry oxygen from the lungs to cells; blood is therefore a powerful buffer. The commonest buffer in chemical solution systems is the acid-base buffer.
  • Bicarbonate buffer; a buffer system composed of bicarbonate ions and dissolved carbon dioxide; in the body, this system is an important factor in determining the pH of the blood as the concentration of bicarbonate ions is regulated by the kidneys and of carbon dioxide by the respiratory system.
  • Cacodylate buffer; one containing an organic arsenical salt, used in preparing fixatives for electron microscopy.
  • Phosphate buffer,   a buffer system composed of KH2PO4 and Na2HPO4; in the body, it is important in regulating the pH of the renal tubular fluids; when 0.025 molal (equimolal of the potassium and sodium salts), the pH is 6.865 at 25 C.
  • Protein buffer,   a buffer system involving proton donor and proton acceptor groups of the amino acid residues of proteins.
  • TRIS buffer (tromethamine): an amine base used intravenously as an alkalizer for the correction of metabolic acidosis. The pH values of all buffers are temperature- and concentration-dependent. For Tris buffers, pH increases about 0.03 unit per C temperature decrease, and decreases 0.03-0.05 unit per ten-fold dilution.
  • Veronal buffer; a barbital buffer commonly used in the preparation of fixatives for electron microscopy.