10049-21-5 Usage
Description
Sodium Phosphate Monobasic Monohydrate is a reagent with very high buffering capacity widely used in molecular biology, biochemistry and chromatography. it can be used as a buffer to adjust pH. In medicine, it is sometimes used as a stimulant laxative before certain operations and medical procedures. Sodium Phosphate Monobasic Monohydrate is often used in foods and in water treatment. It is used as sequestrant, emulsifier, mordant in dyeing, reagent and buffer in foods and analytical chemistry. It is applied as a fireproofing agent and for weighting silk in tanning. It is employed in manufacturing of enamels, ceramics, detergents, boiler compounds, in soldering and brazing instead of borax.
Monobasic sodium phosphate is used in baking powders, acid cleansers, electroplating, as a dry acidulant, and in treating boiler water.
Chemical Properties
Different sources of media describe the Chemical Properties of 10049-21-5 differently. You can refer to the following data:
1. Anhydrous salt: white crystalline powder; slightly hygroscopic; forms sodium acid pyrophosphate, Na2H2P2O7 on heating above 225°C and sodium metaphosphate (NaPO3)n at about 350 to 400°C; very soluble in water, aqueous solution acidic.
Monohydrate: white orthorhombic crystals or granules; density 2.04 g/cm3 ; loses its water of crystallization at 100°C; very soluble in water, pH of 1% solution 4.5; insoluble in alcohol.
Dihydrate: large transparent crystals; orthorhombic bisphenoidal structure; density 1.915 g/cm 3 ; decomposes at 60°C; very soluble in water; insoluble in alcohol.
2. The USP 32 states that monobasic sodium phosphate contains one
or two molecules of water of hydration or is anhydrous.
The hydrated forms of monobasic sodium phosphate occur as
odorless, colorless or white, slightly deliquescent crystals. The
anhydrous form occurs as a white crystalline powder or granules.
Uses
Different sources of media describe the Uses of 10049-21-5 differently. You can refer to the following data:
1. Excipient.
2. Sodium Phosphate Monobasic Monohydrate is often used in foods and in water treatment. it can be used as a buffer to adjust pH. In medicine, it is sometimes used as a stimulant laxative before certain operations and medical procedures.
3. Sodium phosphate monobasic monohydrate has been used for the preparation of cardioplegia solution. It has also been used as a component in McIlvaine′s buffer and MgCl2 buffer.
Preparation
Monobasic sodium phosphate can be prepared by partial neutralization of phosphoric acid with sodium hydroxide in equimolar amounts:
H3PO4+ NaOH →NaH2PO4+ H2O
It also can be made by treating disodium hydrogen phosphate with phosphoric acid in proper stoichiometric amount:
Na2HPO4+ H3PO4→2NaH2PO4
Production Methods
Monobasic sodium phosphate is prepared by adding phosphoric
acid to a hot, concentrated solution of disodium phosphate until the
liquid ceases to form a precipitate with barium chloride. This solution is then concentrated and the monobasic sodium phosphate
is crystallized.
General Description
Useful in conjuction with sodium phosphate, dibasic (Cat. No. 567550) in the preparation of biological buffers(absorbance: ≤0.01 at 260 nm and 280 nm).
Pharmaceutical Applications
Monobasic sodium phosphate is used in a wide variety of
pharmaceutical formulations as a buffering agent and as a
sequestering agent. Therapeutically, monobasic sodium phosphate
is used as a mild saline laxative and in the treatment of hypophosphatemia.
Monobasic sodium phosphate is also used in food products, for
example, in baking powders, and as a dry acidulant and
sequestrant.
Safety
Monobasic sodium phosphate is widely used as an excipient in
parenteral, oral, and topical pharmaceutical formulations.
Phosphate occurs extensively in the body and is involved in
many physiological processes since it is the principal anion of
intracellular fluid. Most foods contain adequate amounts of
phosphate, making hypophosphatemia virtually unknown except
in certain disease states or in patients receiving total parenteral
nutrition. Treatment is usually by the oral administration of up to
100 mmol of phosphate daily.
Approximately two-thirds of ingested phosphate is absorbed
from the gastrointestinal tract, virtually all of it being excreted in the
urine, and the remainder is excreted in the feces.
Excessive administration of phosphate, particularly intravenously,
rectally, or in patients with renal failure, can cause
hyperphosphatemia that may lead to hypocalcemia or other severe
electrolyte imbalances. Adverse effects occur less frequently
following oral consumption, although phosphates act as mild saline
laxatives when administered orally or rectally (2–4 g of monobasic
sodium phosphate in an aqueous solution is used as a laxative).
Consequently, gastrointestinal disturbances including diarrhea,
nausea, and vomiting may occur following the use of monobasic
sodium phosphate as an excipient in oral formulations. However,
the level of monobasic sodium phosphate used as an excipient in a pharmaceutical formulation is not usually associated with adverse
effects.
LD50 (rat, IM): 0.25 g/kg(10)
LD50 (rat, oral): 8.29 g/kg
storage
Monobasic sodium phosphate is chemically stable, although it is
slightly deliquescent. On heating at 100°C, the dihydrate loses all of
its water of crystallization. On further heating, it melts with
decomposition at 205℃, forming sodium hydrogen pyrophosphate,
Na2H2P2O7. At 250℃ it leaves a final residue of sodium
metaphosphate, NaPO3.
Aqueous solutions are stable and may be sterilized by autoclaving.
Monobasic sodium phosphate should be stored in an airtight
container in a cool, dry place.
Incompatibilities
Monobasic sodium phosphate is an acid salt and is therefore
generally incompatible with alkaline materials and carbonates;
aqueous solutions of monobasic sodium phosphate are acidic and
will cause carbonates to effervesce.
Monobasic sodium phosphate should not be administered
concomitantly with aluminum, calcium, or magnesium salts since
they bind phosphate and could impair its absorption from the
gastrointestinal tract. Interaction between calcium and phosphate,
leading to the formation of insoluble calcium phosphate precipitates,
is possible in parenteral admixtures.
Regulatory Status
GRAS listed. Accepted for use as a food additive in Europe.
Included in the FDA Inactive Ingredients Database (injections;
infusions; ophthalmic, oral, topical, and vaginal preparations).
Included in nonparenteral and parenteral medicines licensed in the
UK. Included in the Canadian List of Acceptable Non-medicinal
Ingredients.
Check Digit Verification of cas no
The CAS Registry Mumber 10049-21-5 includes 8 digits separated into 3 groups by hyphens. The first part of the number,starting from the left, has 5 digits, 1,0,0,4 and 9 respectively; the second part has 2 digits, 2 and 1 respectively.
Calculate Digit Verification of CAS Registry Number 10049-21:
(7*1)+(6*0)+(5*0)+(4*4)+(3*9)+(2*2)+(1*1)=55
55 % 10 = 5
So 10049-21-5 is a valid CAS Registry Number.
InChI:InChI=1/Na.H3O4P.H2O/c;1-5(2,3)4;/h;(H3,1,2,3,4);1H2/q+1;;/p-3
10049-21-5Relevant articles and documents
Structure, phase transition and vibrational spectra of the NaH5(PO4)2 and NaD5(PO4)2 crystals
Baran,Lis,Drozd,Ratajczak
, p. 185 - 202 (2000)
The crystals of sodium pentahydrogenbis(phosphate), NaH5(PO4)2 [NaH2PO4·H3PO4] and its deuterated analogue, NaD5(PO4)2 [NaD2PO4 D3PO4], were obtained for the first time. They exhibit the second-order phase transition at ca. 200 K slightly sensitive on deuteration (ca. 6-8 K) as determined by the DSC experiments. Their structures were solved by the X- ray method at 150 K (for NaH5(PO4)2) and at 240 K (for deuterated) crystals. Both these crystals belong to the P21/c space group of the monoclinic system (a = 8.464(4), b = 7.817(5), c = 10.337(5) A?, β = 90.58(4)° for NaH5(PO4)2 and a= 8.495(3), b = 7.854(3), c = 10.352(3) A?, β = 90.67(3)°for deuterated one) and their structures are similar, although determined in different phases. The crystals are built of the layers of orthophosphoric acid molecules and of the layers of dihydrogenphosphate anions. The layers are built of the centrosymmetric dimers of the orthophosphoric acid molecules and of the dihydrogenphosphate anions, respectively. Two corresponding moieties are joined into dimers by two equivalent hydrogen bonds. The structures of title crystals differ from that of KH5 (PO4)2. The powder IR and Raman spectra were measured at room temperature. The IR spectra of the NaHs (PO4)2 crystal were also measured at low temperatures. It is suggested that the phase transition is related to the changes in the motions of the protons in weak hydrogen bonds.
Beans, H. T.,Kiehl, S. J.
, p. 1878 - 1891 (1927)
Kohl, W.,Klemenc, A.
, (1954)
Zettlemoyer, A. C.,Schneider, C. H.,Anderson, H. V.,Fuchs, R. J.
, p. 991 - 994 (1957)
Optimization of dissolution of ulexite in phosphate acid solutions
Doan, Tuba Hatice,Yartai, Ahmet
, p. 601 - 605 (2015/01/16)
The Taguchi optimization method was used to determine optimum conditions for the dissolution of ulexite in phosphate acid solutions. Reaction temperature, solid-to-liquid ratio, phosphate acid concentration, reaction time, particle size and stirring speed
RECOMBINANT HCV E2 GLYCOPROTEIN
-
, (2011/02/18)
The invention provides modified hepatitis C virus (HCV) E2 glycoproteins comprising the HCV-E2 receptor-binding domain (RBD) including the HVR1, HVR2 and igVR variable regions wherein in at least one of said variable regions at least a part of the variabl
