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
Phosphorous acid is a white crystalline 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. Phosphorus acid is used to prepare phosphite salts. It is usually sold as a 20% aqueous solution.
Physical properties
White crystalline mass; deliquescent; garlic-like odor; density 1.651 g/cm
3 at 21°C; melts at 73.6°C; decomposes at 200°C to phosphine and phosphoric acid; soluble in water, about 310 g/100mL; K
1 5.1x10
-2 and K
2 1.8x10
-7; soluble in alcohol.
Uses
Phosphorous acid is used to produce the fertilizer phosphate salt like potassium phosphite, ammonium phosphite and calcium phosphite. It is actively involved in the preparation of phosphites like aminotris(methylenephosphonic acid) (ATMP), 1-hydroxyethane 1,1-diphosphonic acid (HEDP) and 2-phosphonobutane-1,2,4-tricarboxylic Acid (PBTC), which find application in water treatment as a scale or corrosive inhibitor. It is also used in chemical reactions as a reducing agent. Its salt, lead phosphite is used as PVC stabilizer. It is also used as a precursor in the preparation of phosphine and as an intermediate in the preparation of other phosphorus compounds.
Definition
ChEBI: Phosphorous acid is a phosphorus oxoacid. It is a conjugate acid of a dihydrogenphosphite. It is a tautomer of a phosphonic acid.
Application
Phosphorous acid (H3PO3, orthophosphorous acid) may be used as one of the reaction components for the synthesis of the following:
α-aminomethylphosphonic acids via Mannich-Type Multicomponent Reaction
1-aminoalkanephosphonic acids via amidoalkylation followed by hydrolysis
N-protected α-aminophosphonic acids (phospho-isosteres of natural amino acids) via amidoalkylation reaction
Preparation
Phosphorus acid can be prepared by the reaction of phosphorus trichloride with water: PCl
3 + 3H
2O → H
3PO
4 + 3HClThe reaction is violent. Addition of PCl
3 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 PCl
3 vapor is passed into icecold water and solid crystals of H
3PO
4 form. Alternatively, phosphorus acid can be prepared by adding phosphorus trichloride to anhydrous oxalic acid: PCl
3 + 3(COOH）
2 → H
3PO
3 + 3CO + 3CO
2 + 3HCl In this reaction, all products except H
3PO
3 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 . P
4O
6 + 6H
2O → 4H
3PO
3 However, in hot water part of the phosphorus acid disproportionates to phosphoric acid and phosphorus or phosphine.
General Description
Phosphorous acid appears as a white or yellow crystalline solid (melting point 70.1°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.
Flammability and Explosibility
Non flammable
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.
