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  2. Sodium nitrate - Wikipedia

    en.wikipedia.org/wiki/Sodium_nitrate

    Sodium nitrate is the chemical compound with the formula Na N O 3 . This alkali metal nitrate salt is also known as Chile saltpeter (large deposits of which were historically mined in Chile ) [ 4 ] [ 5 ] to distinguish it from ordinary saltpeter, potassium nitrate .

  3. Phosphoric acids and phosphates - Wikipedia

    en.wikipedia.org/.../Phosphoric_acids_and_phosphates

    Since the ends are condensed, its formula has one less H 2 O (water) than tripolyphosphoric acid. The general formula of a phosphoric acid is H n−2x+2 P n O 3n−x+1, where n is the number of phosphorus atoms and x is the number of fundamental cycles in the molecule's structure; that is, the minimum number of bonds that would have to be ...

  4. Sodium phosphate - Wikipedia

    en.wikipedia.org/wiki/Sodium_phosphate

    Sodium dihydrogen phosphate Sodium hydrogen phosphate Trisodium phosphate. 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 ...

  5. Alkali metal nitrate - Wikipedia

    en.wikipedia.org/wiki/Alkali_Metal_Nitrate

    The nitrate ion. Alkali metal nitrates are chemical compounds consisting of an alkali metal (lithium, sodium, potassium, rubidium and caesium) and the nitrate ion. Only two are of major commercial value, the sodium and potassium salts. [1] They are white, water-soluble salts with melting points ranging from 255 °C (LiNO 3) to 414 °C (CsNO

  6. Phosphate - Wikipedia

    en.wikipedia.org/wiki/Phosphate

    In chemistry, a phosphate is an anion, salt, functional group or ester derived from a phosphoric acid. It most commonly means orthophosphate, a derivative of orthophosphoric acid, a.k.a. phosphoric acid H 3 PO 4. The phosphate or orthophosphate ion [PO 4] 3− is derived from phosphoric acid by the removal of three protons H +.

  7. Sodium nitrite - Wikipedia

    en.wikipedia.org/wiki/Sodium_nitrite

    Above 330 °C sodium nitrite decomposes (in air) to sodium oxide, nitric oxide and nitrogen dioxide. [88] 2 NaNO 2 → Na 2 O + NO + NO 2. Sodium nitrite can also be used in the production of nitrous acid: 2 NaNO 2 + H 2 SO 4 → 2 HNO 2 + Na 2 SO 4. The nitrous acid then, under normal conditions, decomposes: 2 HNO 2 → NO 2 + NO + H 2 O

  8. Oxyanion - Wikipedia

    en.wikipedia.org/wiki/Oxyanion

    Although acids such as phosphoric acid are written as H 3 PO 4, the protons are attached to oxygen atoms forming hydroxyl groups, so the formula can also be written as OP(OH) 3 to better reflect the structure. Sulfuric acid may be written as O 2 S(OH) 2; this is the molecule observed in the gas phase.

  9. Nitrophosphate process - Wikipedia

    en.wikipedia.org/wiki/Nitrophosphate_process

    The process was an innovation for requiring neither the expensive sulfuric acid nor producing gypsum waste (known in the context of phosphate production as phosphogypsum). The calcium nitrate mentioned before, can as said be worked up as calcium nitrate fertilizer but often it is converted into ammonium nitrate and calcium carbonate using ...