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Phosphoric acid

Dissociation reaction: 3H+ + PO4-3 H2O↔ 2H+ + PO4-2 + H+

Dissociation constant K value: 6.9 × 10-8; this is the ionization constant of water where the mathematical product hydronium and hydroxide remains constant in water and dilute aqueous solutions at constant temperature.

Example reaction with a strong base: 3Ca(OH)2 + 2H3PO4 ↔ Ca3(PO4)2 + 6H2O

Example reaction with a weak: H3PO4 + NH3 ↔ 3(NH4)3PO4

Formula: H3PO4

Phase at room temperature: Solid

Conjugate base from the reaction: Dihydrogen phospate ion

Molar Mass: 98.00 g/mol

Density: 1.88 g/cm3

How is it made: It is produced from fluorapatite, known as phosphate rock, 3Ca3(PO4)2.CaF2.

Safety Hazards: Uses:
 * Health Hazards: Burns on mouth and lips, sour acrid taste, severe gastrointestinal irritation, nausea, vomiting, bloody diarrhea, difficult swallowing, severe abdominal pains, thirst, acidemia, difficult breathing, convulsions, collapse, shock, death (all from the acidity of Phosphoric acid)
 * Fire Hazards: 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
 * fertilizers
 * soaps and detergents
 * inorganic phosphates
 * pickling and rust-proofing of metals
 * sugar refining
 * gelatin manufacturing
 * water treatment
 * animal feeds
 * in foods and carbonated beverages