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Sodium hypophosphite (NaPO 2 H 2, also known as sodium phosphinate) is the sodium salt of hypophosphorous acid and is often encountered as the monohydrate, NaPO 2 H 2 ·H 2 O. It is a solid at room temperature, appearing as odorless white crystals. It is soluble in water, and easily absorbs moisture from the air.
An amphiprotic molecule (or ion) can either donate or accept a proton, thus acting either as an acid or a base. Water, amino acids, hydrogencarbonate ion (or bicarbonate ion) HCO − 3, dihydrogen phosphate ion H 2 PO − 4, and hydrogensulfate ion (or bisulfate ion) HSO − 4 are common examples of amphiprotic species. Since they can donate a ...
The salt is obtained by partial neutralization of phosphoric acid. The pK a of monosodium phosphate is 6.8-7.2 (depending on the physicochemical characteristics during pK a determination). [2] Heating this salt above 169 °C gives disodium pyrophosphate: 2 NaH 2 PO 4 → Na 2 H 2 P 2 O 7 + H 2 O. When heated at 550 °C, anhydrous trisodium ...
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.
Pyrophosphoric acid. In chemistry, a phosphoric acid, in the general sense, is a phosphorus oxoacid in which each phosphorus (P) atom is in the oxidation state +5, and is bonded to four oxygen (O) atoms, one of them through a double bond, arranged as the corners of a tetrahedron.
Sodium atoms have 11 electrons, one more than the stable configuration of the noble gas neon. As a result, sodium usually forms ionic compounds involving the Na + cation. [1] Sodium is a reactive alkali metal and is much more stable in ionic compounds. It can also form intermetallic compounds and organosodium compounds.
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. The hydrates are more common than the anhydrous forms. [1]
Each layer forms by positioning their lypophilic chains to the same side of the layer. The two layers then stack such that their lyphphilic chains touch on the inside and their polar groups are outside facing the surrounding aqueous media. Thus the inside of the bilayer sheet is a non-polar region sandwiched between the two polar sheets. [2]