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P 4 + 4 OH − + 4 H 2 O → 4 H 2 PO − 2 + 2 H 2. Any phosphites produced in this step can be selectively precipitated out by treatment with calcium salts. The purified material is then treated with a strong, non-oxidizing acid (often sulfuric acid) to give the free hypophosphorous acid: H 2 PO − 2 + H + → H 3 PO 2. HPA is usually ...
Solid HP(O)(OH) 2 has tetrahedral geometry about the central phosphorus atom, with a P−H bond of 132 pm, one P=O double bond of 148 pm and two longer P−OH single bonds of 154 pm. In common with other phosphorus oxides with P−H bonds (e.g. hypophosphorous acid and dialkyl phosphites ), [ 2 ] it exists in equilibrium with an extremely minor ...
The general formula of a phosphoric acid is H n+2−2x P n O 3n+1−x, where n is the number of phosphorus atoms and x is the number of fundamental cycles in the molecule's structure, between 0 and n + 2 / 2 . Pyrophosphate anion. Trimethyl orthophosphate.
These materials contain Ca 2+ combined with the polyphosphates, such as P 2 O 4− 7 and triphosphate P 3 O 5− 10: Dicalcium diphosphate (CAS#7790-76-3]: Ca 2 P 2 O 7; Calcium triphosphate (CAS# 26158-70-3): Ca 5 (P 3 O 10) 2
Hydrogen phosphate or monohydrogen phosphate (systematic name) is the inorganic ion with the formula [HPO 4] 2-. Its formula can also be written as [PO 3 (OH)] 2-. Together with dihydrogen phosphate, hydrogenphosphate occurs widely in natural systems. Their salts are used in fertilizers and in cooking. [1]
Phosphorus comprises 0.1% by mass of the average rock [11] (while, for perspective, its typical concentration in vegetation is 0.03% to 0.2%), [12] and consequently there are quadrillions of tons of phosphorus in Earth's 3×10 19-ton crust, [13] albeit at predominantly lower concentration than the deposits counted as reserves, which are ...
2 P –O– P(OH) –O– P(OH) 2), with five acidic hydrogens. Forms triphosphates or tripolyphosphates. Tetraphosphoric acid, H 6 P 4 O 13 (or (HO) 2 P (–O– P(OH)) 2 –O– P(OH) 2), with six acidic hydrogens. Forms tetraphosphates. The backbone may be branched, as in: Triphosphono phosphoric acid, H 6 P 4 O 13 or P(O)(– OP(O)(OH) 2) 3 ...
Pauling's second rule is that the value of the first pK a for acids of the formula XO m (OH) n depends primarily on the number of oxo groups m, and is approximately independent of the number of hydroxy groups n, and also of the central atom X. Approximate values of pK a are 8 for m = 0, 2 for m = 1, −3 for m = 2 and < −10 for m = 3. [28]