Phosphoric acid

Phosphoric acid
Other names Orthophosphoric acid
Identifiers
CAS number	7664-38-2
Properties
Molecular formula	H3PO4
Molar mass	98.0 g/mol
Appearance	white solid or colourless, viscous liquid (>42°C)
Density	1.685 g/ml (liquid)
Melting point	42.35 °C, 316 K, 108 °F
Boiling point	158 °C, 431 K, 316 °F (decomp.)
Acidity (pKa)	2.12, 7.21, 12.67
Viscosity	85% aqueous solution  ? cP
Hazards
EU classification	Corrosive(C)
R-phrases	R34
S-phrases	(S1/2), S26, S45
Related compounds
Other anions	Nitric acid Arsenic acid
Other cations	Ammonium phosphate Trisodium phosphate
Related Phosphorus acid	Hypophosphorous acid Phosphorous acid Pyrophosphoric acid Tripolyphosphoric acid Hypophosphoric acid Perphosphoric acid Permonophosphoric acid
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references

Phosphoric acid, also known as orthophosphoric acid or phosphoric(V) acid, is a mineral (inorganic) acid having the chemical formula H₃PO₄. By contrast, orthophosphoric acid molecules can combine with themselves to form a variety of compounds referred to as phosphoric acids in a more general way. The term phosphoric acid can also refer to a chemical or reagent consisting of phosphoric acids, usually mostly orthophosphoric acid.

Orthophosphoric acid chemistry

Pure anhydrous phosphoric acid is a white solid that melts at 42.35 °C to form a colorless, viscous liquid.

Most people and even chemists refer to orthophosphoric acid as phosphoric acid, which is the IUPAC name for this compound. The prefix ortho is used to distinguish the acid from other phosphoric acids, called polyphosphoric acids. Orthophosphoric acid is a non- toxic, inorganic, rather weak triprotic acid, which, when pure, is a solid at room temperature and pressure. The chemical structure of orthophosphoric acid is shown above in the data table. Orthophosphoric acid is a very polar molecule; therefore it is highly soluble in water. The oxidation state of phosphorus (P) in ortho- and other phosphoric acids is +5; the oxidation state of all the oxygen atoms (O) is -2 and all the hydrogen atoms (H) is +1. Triprotic means that an orthophosphoric acid molecule can dissociate up to three times, giving up an H⁺ each time, which typically combines with a water molecule, H₂O, as shown in these reactions:

H₃PO_4(s)   + H₂O_(l) ⇌ H₃O⁺_(aq) + H₂PO₄^–_(aq)       K_a1= 7.5×10⁻³

H₂PO₄^–_(aq)+ H₂O_(l) ⇌ H₃O⁺_(aq) + HPO₄^2–_(aq)       K_a2= 6.2×10⁻⁸

HPO₄^2–_(aq)+ H₂O_(l) ⇌ H₃O⁺_(aq) +  PO₄^3–_(aq)        K_a3= 2.14×10⁻¹³

The anion after the first dissociation, H₂PO₄^–, is the dihydrogen phosphate anion. The anion after the second dissociation, HPO₄^2–, is the hydrogen phosphate anion. The anion after the third dissociation, PO₄^3–, is the phosphate or orthophosphate anion. For each of the dissociation reactions shown above, there is a separate acid dissociation constant, called K_a1, K_a2, and K_a3 given at 25°C. Associated with these three dissociation constants are corresponding pK_a1=2.12 , pK_a2=7.21 , and pK_a3=12.67 values at 25°C. Even though all three hydrogen (H ) atoms are equivalent on an orthophosphoric acid molecule, the successive K_a values differ since it is energetically less favorable to lose another H⁺ if one (or more) has already been lost and the molecule/ion is more negatively-charged.

Because the triprotic dissociation of orthophosphoric acid, the fact that its conjugate bases (the phosphates mentioned above) cover a wide pH range, and, because phosphoric acid/phosphate solutions are, in general, non-toxic, mixtures of these types of phosphates are often used as buffering agents or to make buffer solutions, where the desired pH depends on the proportions of the phosphates in the mixtures. Similarly, the non-toxic, anion salts of triprotic organic citric acid are also often used to make buffers. Phosphates are found pervasively in biology, especially in the compounds derived from phosphorylated sugars, such as DNA, RNA, and adenosine triphosphate (ATP). There is a separate article on phosphate as an anion or its salts.

Upon heating orthophosphoric acid, condensation of the phosphoric units can be induced by driving off the water formed from condensation. When one molecule of water has been removed for each two molecules of phosphoric acid, the result is pyrophosphoric acid (H₄P₂O₇). When an average of one molecule of water per phosphoric unit has been driven off, the resulting substance is a glassy solid having an empirical formula of HPO₃ and is called metaphosphoric acid. Metaphosphoric acid is a singly anhydrous version of orthophosphoic acid and is sometimes used as a water- or moisture-absorbing reagent. Further dehydrating is very difficult, and can be accomplished only by means of an extremely strong desiccant (and not by heating alone). It produces phosphoric anhydride, which has an empirical formula P₂O₅, although an actual molecule has a chemical formula of P₄O₁₀. Phosphoric anhydride is a solid, which is very strongly moisture-aborbing and is used as a desiccant.

pH and composition of a phosphoric acid solution

For a given total acid concentration [A] = [H₃PO₄] + [H₂PO₄⁻] + [HPO₄²⁻] + [PO₄³⁻] ([A] is the total number of moles of pure H₃PO₄ which have been used to prepare 1 liter of solution) , the composition of an aqueous solution of phosphoric acid can be calculated using the equilibrium equations associated with the three reactions described above together with the [H⁺][OH⁻] = 10⁻¹⁴ relation and the electrical neutrality equation. The system may be reduced to a fifth degree equation for [H⁺] which can be solved numerically, yielding:

[A] (mol/L)	pH	[H3PO4]/[A] (%)	[H2PO4−]/[A] (%)	[HPO42−]/[A] (%)	[PO43−]/[A] (%)
1	1.08	91.7	8.29	6.20×10−6	1.60×10−17
10−1	1.62	76.1	23.9	6.20×10−5	5.55×10−16
10−2	2.25	43.1	56.9	6.20×10−4	2.33×10−14
10−3	3.05	10.6	89.3	6.20×10−3	1.48×10−12
10−4	4.01	1.30	98.6	6.19×10−2	1.34×10−10
10−5	5.00	0.133	99.3	0.612	1.30×10−8
10−6	5.97	1.34×10−2	94.5	5.50	1.11×10−6
10−7	6.74	1.80×10−3	74.5	25.5	3.02×10−5
10−10	7.00	8.24×10−4	61.7	38.3	8.18×10−5

For large acid concentrations, the solution is mainly composed of H₃PO₄. For [A] = 10⁻², the pH is closed to pK_a1, giving an equimolar mixture of H₃PO₄ and H₂PO₄⁻. For [A] below 10⁻³, the solution is mainly composed of H₂PO₄⁻ with [HPO₄²⁻] becoming non negligible for very dilute solutions. [PO₄³⁻] is always negligible.

Phosphoric acid as a chemical reagent

Pure 75-85% aqueous solutions (the most common) are clear, colourless, odourless, non- volatile, rather viscous, syrupy liquids, but still pourable. Phosphoric acid is very commonly used as an aqueous solution of 85% phosphoric acid or H₃PO₄. Because it is a concentrated acid, an 85% solution can be corrosive, although nontoxic when diluted. Because of the high percentage of phosphoric acid in this reagent, at least some of the orthophosphoric acid is condensed into polyphosphoric acids in a temperature-dependent equilibrium, but, for the sake of labeling and simplicity, the 85% represents H₃PO₄ as if it were all orthophosphoric acid. Other percentages are possible too, even above 100%, where the phosphoric acids and water would be in an unspecified equilibrium, but the overall elemental mole content would be considered specified. When aqueous solutions of phosphoric acid and/or phosphate are dilute, they are in or will reach an equilibrium after a while where practically all the phosphoric/phosphate units are in the ortho- form.

Preparation of hydrogen halides

Phosphoric acid reacts with halides to form the corresponding hydrogen halide gas (steamy fumes are observed on warming the reaction mixture). This is a common practice for the laboratory preparation of hydrogen halides.

3NaCl(s) + H₃PO₄(l) → NaH₂PO₄(s) + HCl(g)

3NaBr(s) + H₃PO₄(l) → NaH₂PO₄(s) + HBr(g)

3NaI(s) + H₃PO₄(l) → NaH₂PO₄(s) + HI(g)

Rust removal

Phosphoric acid may be used by direct application to rusted iron, steel tools, or surfaces to convert iron(III) oxide ( rust) to a water-soluble phosphate compound. It is usually available as a greenish liquid, suitable for dipping (acid bath), but is more generally used as a component in a gel, commonly called naval jelly. As a thick gel, it may be applied to sloping, vertical, or even overhead surfaces. Care must be taken to avoid acid burns of the skin and especially the eyes, but the residue is easily diluted with water. When sufficiently diluted, it can even be nutritious to plant life, containing the essential nutrients phosphorus and iron. It is sometimes sold under other names, such as "rust remover" or "rust killer." It should not be directly introduced into surface water such as creeks or into drains, however. After treatment, the reddish-brown iron oxide will be converted to a black iron phosphate compound coating that may be scrubbed off. Multiple applications of phosphoric acid may be required to remove all rust. The resultant black compound can provide further corrosion resistance (such protection is somewhat provided by the superficially similar Parkerizing and blued electrochemical conversion coating processes.) After application and removal of rust using phosphoric acid compounds, the metal should be oiled (if to be used bare, as in a tool) or appropriately painted, by using a multiple coat process of primer, intermediate, and finish coats.

Processed food use

Food-grade phosphoric acid is used to acidify foods and beverages such as various colas, but not without controversy regarding its health effects. It provides a tangy taste, and, being a mass-produced chemical, is available cheaply and in large quantities. The low cost and bulk availability is unlike more expensive natural seasonings that give comparable flavours, such as ginger for tangyness, or citric acid for sourness, obtainable from lemons and limes. (However most citric acid in the food industry is not extracted from citrus fruit, but fermented by Aspergillus niger mold from scrap molasses, waste starch hydrolysates and phosphoric acid.) It is labeled as E number E338.

Biological effects on bone calcium and kidney health

Phosphoric acid, used in many soft drinks (primarily cola), has been linked to lower bone density in epidemiological studies. For example, a study using dual-energy X-ray absorptiometry rather than a questionnaire about breakage, provides reasonable evidence to support the theory that drinking cola results in lower bone density. This study was published in the American Journal of Clinical Nutrition. A total of 1672 women and 1148 men were studied between 1996 and 2001. Dietary information was collected using a food frequency questionnaire that had specific questions about the number of servings of cola and other carbonated beverages and that also made a differentiation between regular, caffeine-free, and diet drinks. The paper cites significant statistical evidence to show that women who consume cola daily have lower bone density. Total phosphorus intake was not significantly higher in daily cola consumers than in nonconsumers; however, the calcium-to-phosphorus ratios were lower. The study also suggests that further research is needed to confirm the findings.

On the other hand, a study funded by Pepsi suggests that low intake of phosphorus leads to lower bone density. The study does not examine the effect of phosphoric acid, which binds with magnesium and calcium in the digestive tract to form salts that are not absorbed, but, rather, it studies general phosphorus intake.

However, a well-controlled clinical study by Heaney and Rafferty using calcium-balance methods found no impact of carbonated soft drinks containing phoshporic acid on calcium excretion. The study compared the impact of water, milk, and various soft drinks (two with caffeine and two without; two with phosphoric acid and two with citric acid) on the calcium balance of 20- to 40-year-old women who customarily consumed ~3 or more cups (680 ml) of a carbonated soft drink per day. They found that, relative to water, only milk and the two caffeine-containing soft drinks increased urinary calcium, and that the calcium loss associated with the caffeinated soft drink consumption was about equal to that previously found for caffeine alone. Phosphoric acid without caffeine had no impact on urine calcium, nor did it augment the urinary calcium loss related to caffeine. Because studies have shown that the effect of caffeine is compensated for by reduced calcium losses later in the day, Heaney and Rafferty concluded that the net effect of carbonated beverages – including those with caffeine and phosphoric acid - is negligible, and that the skeletal effects of carbonated soft drink consumption are likely due primarily to milk displacement.

Other chemicals such as caffeine (also a significant component of popular common cola drinks) were also suspected as possible contributors to low bone density, due to the known effect of caffeine on calciuria. One other study, comprised of 30 women over the course of a week, suggests that phosphoric acid in colas has no such effect, and postulates that caffeine has only a temporary effect, which is later reversed. The authors of this study conclude that the skeletal effects of carbonated beverage consumption are likely due primarily to milk displacement. (Another possible confounding factor may be an association between high soft drink consumption and sedentary lifestyle.)

Cola consumption has also been linked to chronic kidney disease and kidney stones through medical research. This study differentiated between the effects of cola (generally contains phosphoric acid), non-cola carbonated beverages (substitute citric acid) and coffee (control for caffeine), and found that drinking 2 or more colas per day more than doubled the incidence of kidney disease.

Medical use

Phosphoric acid is used in dentistry and orthodontics as an etching solution, to clean and roughen the surfaces of teeth where dental appliances or fillings will be placed. Phosphoric acid is also an ingredient in over-the-counter anti-nausea medications that also contain high levels of sugar (glucose and fructose). It should not be used by diabetics without consultation with a doctor. This acid is also used in teeth whiteners to eliminate any plaque that may be on your teeth.

Preparation of phosphoric acid

Phosphoric acid can be prepared by two routes - the Thermal Process and the Wet Process.

Thermal phosphoric acid: This very pure phosphoric acid is obtained by burning elemental phosphorus to produce phosphorus pentoxide and dissolving the product in dilute phosphoric acid. This produces a very pure phosphoric acid, since most impurities present in the rock have been removed when extracting phosphorus from the rock in a furnace. The end result is food-grade, thermal phosphoric acid; however, for critical applications, additional processing to remove arsenic compounds may be needed.

Wet phosphoric acid: Wet process phosphoric acid is prepared by adding sulfuric acid to calcium phosphate rock.

The simplified reaction is:

3 H₂SO₄ + Ca₃(PO₄)₂ + 6 H₂O ↔ 2 H₃PO₄ + 3 CaSO₄.2H₂O

Wet-process acid can be purified by removing fluorine to produce animal-grade phosphoric acid, or by solvent extraction and arsenic removal to produce food-grade phosphoric acid.

Other applications

Phosphoric acid is used as the electrolyte in phosphoric-acid fuel cells. It is also used as an external standard for phosphorus-31 nuclear magnetic resonance (NMR).

Phosphoric acid is used as a cleaner by construction trades to remove mineral deposits, cementitious smears, and hard water stains. It is also used as an ingredient in some household cleaners aimed at similar cleaning tasks.

Hot phosphoric acid is used in microfabrication to etch silicon nitride (Si₃N₄). It is highly selective in etching Si₃N₄ instead of SiO₂, silicon dioxide.

Phosphoric acid is used as a flux by hobbyists (such as model railroaders) as an aid to soldering.

Phosphoric acid is also used in hydroponics pH solutions to lower the pH of nutrient solutions. While other types of acids can be used, phosphorus is a nutrient used by plants, especially during flowering, making phosphoric acid particularly desirable. General Hydroponics pH Down liquid solution contains phosphoric acid in addition to citric acid and ammonium bisulfate with buffers to maintain a stable pH in the nutrient reservoir.

Phosphoric acid is used as a pH adjuster in cosmetics and skin-care products.

Phosphoric acid is used as a chemical oxidizing agent for activated carbon production.