Phosphorous acidCAS NO.: 13598-36-2

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1 Kilogram	FOB Price:USD 0.2000 -1.0000

1 Kilogram

FOB Price:USD 0.2000 -1.0000

Min.Order :1 Kilogram
Purity: 99%
Payment Terms : L/C,D/A,D/P,T/T,Other

Keywords

Phosphorous acid PHOSPHOROUS ACIDPHOSPHOROUS ACIDPHOSPHOROUS ACIDPHOSPHOROUS ACID high purity Phosphorous acid

Quick Details

Appearance:Colorless to yellow liquid
Application:Synthetic fragrances
PackAge:drum
ProductionCapacity:11000|Metric Ton|Month
Storage:Room temperature
Transportation:By sea or by air

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Details:

Hazard Codes	C
Risk Statements	22-35
Safety Statements	26-36/37/39-45
RIDADR	UN 2834 8/PG 3
WGK Germany	1
RTECS	SZ6400000
F	3
TSCA	Yes
HazardClass	8
PackingGroup	III
HS Code	28092019

MSDS Information

Provider	Language
ACROS	English
SigmaAldrich	English
ALFA	English

Phosphorous acid Usage And Synthesis

Description	Phosphorous acid is an intermediate in the preparation of other phosphorous compounds. It is a raw material to prepare phosphonates for water treatment such as iron and manganese control, scale inhibition and removal, corrosion control and chlorine stabilization. The alkali metal salts (phosphites) of phosphorous acid are being widely marketed either as an agricultural fungicide (e.g. Downy Mildew) or as a superior source of plant phosphorous nutrition. Phosphorous acid is used in stabilizing mixtures for plastic materials. Phosphorous acid is used for inhibiting high-temperature of corrosion-prone metal surfaces and to produce lubricants and lubricant additives.
References	[1] Allison E. McDonald, Bruce R. Grant and William C. Plaxton, Phosphite (Phosphorous Acid): Its Relevance in The Environment and Agriculture and Influence on Plant Phosphate Starvation Response, Journal of Plant Nutrition, 2001, vol. 24, 1505-1519 [2] Sai-Shek Young, Stabilizers for plastic materials, Patent, 1993 [3] Guido Sartori, Method for inhibiting corrosion using phosphorous acid, Patent,2004 [4] John R Morris, Lubricant containing a phosphorous acid ester-aldehyde condensation product, Patent, 1956
Description	Phosphorous acid, H3PO3, is diprotic (readily ionizes two protons), not triprotic as might be suggested by this formula. Phosphorous acid is as an intermediate in the preparation of other phosphorous compounds. Because preparation and uses of “phosphorous acid” actually pertain more to the major tautomer, phosphonic acid, it is more often referred to as “phosphorous acid”. Phosphorous acid has the chemical formula H3PO3, which is best expressed as HPO(OH)2 to show its diprotic character. P(OH)3 (IUPAC: phosphorous acid) has CAS number 10294-56-1. It has been shown to be a stable tautomer.
Chemical Properties	white crystalline solid
Physical properties	White crystalline mass; deliquescent; garlic-like odor; density 1.651 g/cm³ at 21°C; melts at 73.6°C; decomposes at 200°C to phosphine and phosphoric acid; soluble in water, about 310 g/100mL; K₁ 5.1x10^-2 and K₂ 1.8x10^-7; soluble in alcohol.
Uses	Phosphorus acid is used to prepare phosphite salts. It is usually sold as a 20% aqueous solution.
Definition	A colorless deliquescent solid that can be prepared by the action of water on phosphorus( III) oxide or phosphorus(III) chloride. It is a dibasic acid producing the anions H₂PO₃^- and HPO₃ ^2- in water. The acid and its salts are slow reducing agents. On warming, phosphonic acid decomposes to phosphine and phosphoric(V) acid.
Preparation	Phosphorus acid can be prepared by the reaction of phosphorus trichloride with water: PCl₃ + 3H₂O → H₃PO₄ + 3HCl The reaction is violent. Addition of PCl₃ should be extremely cautious and slow. The addition can be carried out safely in the presence of concentrated HCl. Alternatively, a stream of air containing PCl₃ vapor is passed into icecold water and solid crystals of H₃PO₄ form. Alternatively, phosphorus acid can be prepared by adding phosphorus trichloride to anhydrous oxalic acid: PCl₃ + 3(COOH）₂ → H₃PO₃ + 3CO + 3CO₂ + 3HCl In this reaction, all products except H₃PO₃ escape as gases leaving the liquid acid. Dissolution of phosphorus sesquioxide in water also forms phosphorus acid. When shaken with ice water, phosphorus acid is the only product . P₄O₆ + 6H₂O → 4H₃PO₃ However, in hot water part of the phosphorus acid disproportionates to phosphoric acid and phosphorus or phosphine.
General Description	A white or yellow crystalline solid (melting point 70.1 deg C) or a solution of the solid. Density 1.651 g /cm3 . Contact may severely irritate skin, eyes, and mucous membranes. Toxic by ingestion, inhalation and skin absorption.
Air & Water Reactions	Deliquescent. Absorbs oxygen from the air very readily to form phosphoric acid [Hawley]. Soluble in water.
Reactivity Profile	Phosphorous acid decomposes when heated to form phosphine, a gas that usually ignites spontaneously in air. Absorbs oxygen from the air to form phosphoric acid [Hawley]. Forms yellow deposits in aqueous solution that are spontaneously flammable upon drying. Reacts exothermically with chemical bases (for example: amines and inorganic hydroxides) to form salts. These reactions can generate dangerously large amounts of heat in small spaces. Dissolution in water or dilution of a concentrated solution with additional water may generate significant heat. Reacts in the presence of moisture with active metals, including such structural metals as aluminum and iron, to release hydrogen, a flammable gas. Can initiate the polymerization of certain alkenes. Reacts with cyanide compounds to release gaseous hydrogen cyanide. May generate flammable and/or toxic gases in contact with dithiocarbamates, isocyanates, mercaptans, nitrides, nitriles, sulfides, and strong reducing agents. Additional gas-generating reactions occur with sulfites, nitrites, thiosulfates (to give H2S and SO3), dithionites (to give SO2), and carbonates (to give CO2).
Health Hazard	TOXIC; inhalation, ingestion or skin contact with material may cause severe injury or death. Contact with molten substance may cause severe burns to skin and eyes. Avoid any skin contact. Effects of contact or inhalation may be delayed. Fire may produce irritating, corrosive and/or toxic gases. Runoff from fire control or dilution water may be corrosive and/or toxic and cause pollution.
Fire Hazard	Non-combustible, substance itself does not burn but may decompose upon heating to produce corrosive and/or toxic fumes. Some are oxidizers and may ignite combustibles (wood, paper, oil, clothing, etc.). Contact with metals may evolve flammable hydrogen gas. Containers may explode when heated.
Industrial uses	This collector was developed recently and was used primarily as specific collector for cassiterite from ores with complex gangue composition.On the basis of the phosphonic acid, Albright and Wilson had developed a range of collectors mainly for flotation of oxidic minerals (i.e. cassiterite, ilmenite and pyrochlore). Very little is known about the performance of these collectors. Limited studies conducted with cassiterite and rutile ores showed that some of these collectors produce voluminous froth but were very selective.
Safety Profile	Moderately toxic by ingestion. When heated to decomposition at 200℃ it emits toxic fumes of POx and phosphme whch may ignite. See also PHOSPHINE.