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Many phosphates are soluble in water at standard temperature and pressure. The sodium, potassium, rubidium, caesium, and ammonium phosphates are all water-soluble. Most other phosphates are only slightly soluble or are insoluble in water. As a rule, the hydrogen and dihydrogen phosphates are slightly more soluble than the corresponding phosphates.
The tables below provides information on the variation of solubility of different substances (mostly inorganic compounds) in water with temperature, at one atmosphere pressure. Units of solubility are given in grams of substance per 100 millilitres of water (g/100 ml), unless shown otherwise. The substances are listed in alphabetical order.
The following chart shows the solubility of various ionic compounds in water at 1 atm pressure and room temperature (approx. 25 °C, 298.15 K). "Soluble" means the ionic compound doesn't precipitate, while "slightly soluble" and "insoluble" mean that a solid will precipitate; "slightly soluble" compounds like calcium sulfate may require heat to precipitate.
In aqueous solutions (solutions of water), water gradually (over the course of hours) hydrolyzes polyphosphates into smaller phosphates and finally into ortho-phosphate, given enough water. Higher temperature or acidic conditions can speed up the hydrolysis reactions considerably.
A sodium phosphate is a generic variety of salts of sodium (Na +) and phosphate (PO 3− 4). Phosphate also forms families or condensed anions including di-, tri-, tetra-, and polyphosphates . Most of these salts are known in both anhydrous (water-free) and hydrated forms.
Trisodium phosphate (TSP) is an inorganic compound with the chemical formula Na 3 P O 4.It is a white, granular or crystalline solid, highly soluble in water, producing an alkaline solution.
Triammonium phosphate can be prepared in the laboratory by treating 85% phosphoric acid with 30% ammonia solution: [citation needed] H 3 PO 4 + 3 NH 3 → (NH 4) 3 PO 4 (NH 4) 3 PO 4 is a colorless, crystalline solid. The solid, which has the odor of ammonia, is readily soluble in water. The salt converts to diammonium hydrogen phosphate (NH 4 ...
In the 1960s scientists recognized that phosphates in water caused eutrophication. [23] There was disagreement at that time about whether water with high phosphate came to have the chemical because of somehow being polluted with it. [23] By the 1970s it was established that high phosphate levels in water were a consequence of pollution. [23]