TRICINE [N-(2-HYDROXY-1,1-BIS(HYDROXYMETHYL)ETHYL)GLYCINE]

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.

TRICINE
PRODUCT IDENTIFICATION
CAS NO.	5704-04-1
EINECS NO.	227-193-6
FORMULA	(HOCH₂)₃CNHCH₂COOH
MOL WT.	179.17
H.S. CODE
TOXICITY
SYNONYMS	N-(Tri(hydroxymethyl)methyl)glycine;
N-(2-Hydroxy-1,1-bis(hydroxymethyl)ethyl)glycine;
SMILES
CLASSIFICATION
PHYSICAL AND CHEMICAL PROPERTIES
PHYSICAL STATE	white crystalline powder
MELTING POINT	181 - 187 C
BOILING POINT
SPECIFIC GRAVITY
SOLUBILITY IN WATER	Soluble
AUTOIGNITION
pH
VAPOR DENSITY
NFPA RATINGS	Health: 1; Flammability: 0; Reactivity: 0
REFRACTIVE INDEX
FLASH POINT
STABILITY	Stable under ordinary conditions. Hygroscopic.
GENERAL DESCRIPTION & APPLICATIONS
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.
SALES SPECIFICATION
APPEARANCE	white crystalline powder
ASSAY	99.0% min
INSOLUBLES	0.01% max
LOSS ON DRYING	1.0% max
HEAVY METALS	5ppm max
CLARITY	clear (in 40% water)
pH	4.4 - 5.2
Fe	1ppm max
TRANSPORTATION
PACKING
HAZARD CLASS
UN NO.
OTHER INFORMATION
`Hazard Symbols: , Risk Phrases: , Safety Phrases: 22-24/25`