Phosphoric acids and phosphates
There are various kinds of phosphoric acids and phosphates. Of the many phosphorus oxoacids, the phosphoric acids constitute the largest and most diverse group. The simplest phosphoric acid series begins with monophosphoric (orthophosphoric) acid, continues with many oligophosphoric acids such as diphosphoric (pyrophosphoric) acid and concludes in the polyphosphoric acids. But, phosphoric acid units can bind together into rings or cyclic structures, chains (catenas), or branched structures, with various combinations possible. Each of these can form phosphates (salts or esters of phosphoric acids).
- 1 Orthophosphoric acid
- 2 Orthophosphate
- 3 Polyphosphoric acids
- 4 Polyphosphates
- 5 Phosphate and phosphite esters
- 6 See also
- 7 References
- 8 Further reading
- 9 External links
The simplest compound of a series of phosphoric acids is sometimes called by its common name, orthophosphoric acid, but more often called by its IUPAC name, simply phosphoric acid, by both non-technical people and even many chemists. It has also been called monophosphoric acid. The chemical formula of orthophosphoric acid is H3PO4 and its chemical structure is shown in the illustration below. Two or more orthophosphoric acid molecules can be joined by condensation into larger molecules by elimination of water. This way, a series of polyphosphoric acids can be obtained.
Orthophosphoric acid has three hydrogen atoms bonded to oxygen atoms in its structure. All three hydrogens are acidic to varying degrees and can be lost from the molecule as H+ ions (alternatively referred to as protons). When all three H+ ions are lost from orthophosphoric acid, an orthophosphate ion (PO43−) is formed. Orthophosphate is the simplest in a series of phosphates, and is usually just called phosphate by both non-technical people and many chemists alike; see a separate article on phosphate for details.
Because orthophosphoric acid can undergo as many as three dissociations or ionizations (losses of H+ ions), it has three acid dissociation constants called Ka1, Ka2, and Ka3. Another way to provide acid dissociation constant data is to list pKa1, pKa2, and pKa3 instead. Orthophosphate is in a sense the triple conjugate base of phosphoric acid and has three related basicity constants, Kb1, Kb2, and Kb3, which likewise have corresponding pKb1, pKb2, and pKb3 values.
When two orthophosphoric acid molecules are condensed into one molecule, pyrophosphoric acid (H4P2O7) is obtained as follows:
- 2 H3PO4 → H4P2O7 + H2O
The chemical structure of pyrophosphoric acid is also shown in the illustration. Three orthophosphoric acid molecules can condense in a row to obtain tripolyphosphoric acid (H5P3O10), which is also shown in the illustration. This condensation process can continue with additional orthophosphoric acid units to obtain tetrapolyphosphoric acid (H6P4O13, pictured) and so on. Note that each extra phosphoric unit adds 1 extra H (hydrogen) atom, 1 extra P (phosphorus) atom, and 3 extra O (oxygen) atoms. The "backbone" chain of these types of molecules consists of alternating P and O atoms covalently bonded together. Polyphosphoric acid molecules can have dozens of such phosphoric units bonded in a row. A general formula for such poly-acid compounds is HO(PO2OH)xH, where x = number of phosphoric units in the molecule. The four oxygen atoms bonded to each phosphorus atom are in a tetrahedral configuration with the phosphorus in the center of the tetrahedron and the oxygens in each of the four corners.
In a pyrophosphoric acid molecule, there are four hydrogens bonded to oxygens, and one, two, three, or all four can be lost as H+ ions. When all four are lost from pyrophosphoric acid, a pyrophosphate ion is formed. Because pyrophosphoric acids can undergo four dissociations, there are four Ka values for it, as well as four corresponding pKa values. Similarly, pyrophosphate is a base with four Kb and, of course, four pKb values for regaining the H+ ions in reverse order.
The situation with higher order polyphosphoric acids and polyphosphates continues in a similar way. Tripolyphosphoric acid can lose up to five H+ ions to form a tripolyphosphate ion, tetrapolyphosphoric acid can lose up to six H+ ions to form tetrapolyphosphate, etc. As more dissociations per molecule are possible, the intervals between individual pKa and pKb values now start becoming smaller on the pH scale.
As the polyphosphoric molecules grow increasingly larger and more complex, practically any number of the somewhat acidic -OH groups in them can dissociate to become negatively charged oxygens, forming numerous combinations of multiple-charged polyphosphoric/polyphosphate anions. Generally in an aqueous solution, the degree or percentage of dissociation depends on the pH of the solution.
Ortho-, pyro-, and tripolyphosphate compounds have been commonly used in detergents (i. e. cleaners) formulations. For example, see Sodium tripolyphosphate. Sometimes pyrophosphate, tripolyphosphate, tetrapolyphosphate, etc. are called diphosphate, triphosphate, tetraphosphate, etc., especially when they are part of phosphate esters in biochemistry. They are also used for scale and corrosion control by potable water providers. As a corrosion inhibitor, polyphosphates work by forming a protective film on the interior surface of pipes.
Metaphosphoric acids and metaphosphates
The phosphoric acid units can be bonded together in rings (cyclic structures) forming metaphosphoric acid molecules. The simplest such compound is trimetaphosphoric acid or cyclo-triphosphoric acid having the formula H3P3O9. Its structure is shown in the illustration. Since the ends are condensed, its formula has one less H2O (water) than tripolyphosphoric acid. What are commonly called trimetaphosphates actually have a mixture of ring sizes. A general formula for such cyclic compounds is (HPO3)x where x = number of phosphoric units in the molecule. The hypothetical monomer monometaphosphoric acid (HPO3), which would be valence isoelectronic with nitric acid, is not known to exist.
When these metaphosphoric acids lose their hydrogens as H+, cyclic anions called metaphosphates are formed. An example of a compound with such an anion is sodium hexametaphosphate (Na6P6O18), used as a sequestrant and a food additive.
The third -OH group on an orthophosphoric acid unit can also be used for condensation with other phosphoric groups to form branches in the polyphosphoric/polyphosphate chains. The simplest example of this is triphosphono phosphate, a branched isomer of tetrapolyphosphoric acid. The ultimate example of cyclic and branching condensation would be the cyclic four-phosphate unit double-branched to form the phosphoric anhydride P4O10; see illustration.
Hydrolysis of polyphosphoric/polyphosphates
These phosphoric acids series are generally water-soluble considering the polarity of the molecules. Ammonium and alkali phosphates are also quite soluble in water. The alkaline earth salts start becoming less soluble and phosphate salts of various other metals are even less soluble. 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.
Conversely, polyphosphoric acids or polyphosphates are often formed by dehydrating a phosphoric acid solution; in other words, removing water from it often by heating and evaporating the water off.
Phosphate and phosphite esters
The -OH groups in phosphoric acids can also condense with the hydroxyl groups of alcohols to form phosphate esters. Since orthophosphoric acid has three -OH groups, it can esterify with one, two, or three alcohol molecules to form a mono-, di-, or triester. See the general structure image of an ortho- (or mono-) phosphate ester below on the left, where any of the R groups can be a hydrogen or an organic radical. Pyro- (or di-) phosphate esters and tripoly- (or tri-) phosphate esters, etc. are also possible. Any -OH groups on the phosphates in these ester molecules may lose H+ ions to form anions, again depending on the pH in a solution. In the biochemistry of living organisms, there are many kinds of (mono)phosphate, diphosphate, and triphosphate compounds (essentially esters), many of which play a significant role in metabolism such as adenosine diphosphate (ADP) and triphosphate (ATP).
Similarly, phosphorous acid can bond with alcohol molecules to form a phosphite ester. See the general structure image below on the right. The two dots on the P represent the lone electron pair of the phosphorus atom.
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