SODIUM DIACETATE

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.

SODIUM DIACETATE
PRODUCT IDENTIFICATION
CAS NO.	126-96-5
EINECS NO.	204-814-9
FORMULA	C₄H₇O₄Na
MOL WT.	142.1
H.S. CODE	2915.22
TOXICITY
SYNONYMS	Acetic acid, sodium salt (2:1);
Natriumhydrogendi(acetat); Hidrogenodi(acetato) de sodio ; Hydrogénodi(acétate) de sodium; Sodium hydrogen diacetate; sodium hydrogen di(acetate);
SMILES
CLASSIFICATION
PHYSICAL AND CHEMICAL PROPERTIES
PHYSICAL STATE	white hygroscopic crystalline powder
MELTING POINT
BOILING POINT
SPECIFIC GRAVITY
SOLUBILITY IN WATER
pH	4.5-5.0 (10% sol.)
VAPOR DENSITY
AUTOIGNITION
NFPA RATINGS	Health: 1; Flammability: 1; Reactivity: 0
REFRACTIVE INDEX
FLASH POINT
STABILITY	Stable under ordinary conditions
APPLICATIONS
Anti-microbial agent in food industry. Technical grades are used as buffers in petroleum production and drillings.
SALES SPECIFICATION (FCC GRADE)
SODIUM DIACETATE	39.0-41.0%
SODIUM ACETATE	58.0-60.0%
pH	4.5-5.0 (10% sol.)
MOISTURE	2.0% max
FORMIC ACID	0.2% max
ARSENIC	3ppm max
HEAVY METAL	10ppm max
TRANSPORTATION
PACKING	25kgs in Bag
HAZARD CLASS
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.