Hydrochloric acid
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Other names
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CAS Number |
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ChEMBL |
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ChemSpider |
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ECHA InfoCard | 100.210.665 | ||
EC Number | 231-595-7 | ||
E number | E507 (acidity regulators, ...) | ||
PubChem CID |
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UNII |
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UN number | 1789 | ||
| Properties | |||
Chemical formula | HCl(aq) | ||
| Appearance | Colorless, transparent liquid | ||
Melting point | Concentration dependent - see table | ||
Boiling point | Concentration dependent - see table | ||
log P | 0.00[3] | ||
Acidity (pKa) | −5.9 (HCl gas)[4] | ||
| Pharmacology | |||
ATC code | A09AB03 (WHO) B05XA13 (WHO) | ||
| Hazards | |||
Safety data sheet | See: data page | ||
GHS pictograms |   | ||
GHS signal word | Danger[5] | ||
GHS hazard statements | H290, H314, H335[5] | ||
GHS precautionary statements | P260, P280, P303+361+353, P305+351+338[5] | ||
NFPA 704 |  0 3 1 ACID | ||
| Related compounds | |||
Related compounds |
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Supplementary data page | |||
Structure and properties | Refractive index (n), Dielectric constant (εr), etc. | ||
Thermodynamic data | Phase behaviour solid–liquid–gas | ||
Spectral data | UV, IR, NMR, MS | ||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |||
 N verify (what is  Y N ?) | |||
Infobox references | |||
Hydrochloric acid is a colorless inorganic chemical system with the formula H
2O:HCl. Hydrochloric acid has a distinctive pungent smell. It is mainly produced as a precursor to vinyl chloride for PVC. It is classified as strongly acidic and can attack the skin over a wide composition range, since the hydrogen chloride practically dissociates completely in solution.
Hydrochloric acid is the simplest chlorine-based acid system containing water. It is a solution of hydrogen chloride and water, and a variety of other chemical species, including hydronium and chloride ions. It is an important chemical reagent and industrial chemical, used primarily in the production of polyvinyl chloride for plastic. In households, diluted hydrochloric acid is often used as a descaling agent. In the food industry, hydrochloric acid is used as a food additive and in the production of gelatin. Hydrochloric acid is also used in leather processing.
Hydrochloric acid was discovered by the alchemist Jabir ibn Hayyan around the year 800 AD.[6][7]
Hydrochloric acid was historically called acidum salis, muriatic acid, and spirits of salt because it was produced from rock salt and "green vitriol" (Iron(II) sulfate) (by Basilius Valentinus in the 15th century) and later from the chemically similar common salt and sulfuric acid (by Johann Rudolph Glauber in the 17th century). Free hydrochloric acid was first formally described in the 16th century by Libavius. Later, it was used by chemists such as Glauber, Priestley, and Davy in their scientific research. Unless pressurized or cooled, hydrochloric acid will turn into a gas if there is around 60% or less of water. Hydrochloric acid is also known as hydronium chloride.
Contents
1 Etymology
2 History
3 Structure and reactions
4 Physical properties
5 Production
5.1 Industrial market
6 Applications
6.1 Pickling of steel
6.2 Production of organic compounds
6.3 Production of inorganic compounds
6.4 pH control and neutralization
6.5 Regeneration of ion exchangers
6.6 Other
7 Presence in living organisms
8 Safety
9 See also
10 References
11 External links
Etymology
Hydrochloric acid was known to European alchemists as spirits of salt or acidum salis (salt acid). Both names are still used, especially in other languages, such as German: Salzsäure, Dutch: Zoutzuur, Swedish: Saltsyra, Turkish: Tuz Ruhu, Polish: kwas solny, Bulgarian: солна киселина, Russian: соляная кислота, Chinese: 鹽酸, Korean: 염산, and Taiwanese: iâm-sng. Gaseous HCl was called marine acid air.
The old (pre-systematic) name muriatic acid has the same origin (muriatic means "pertaining to brine or salt", hence muriate means hydrochloride), and this name is still sometimes used.[1][8] The name hydrochloric acid was coined by the French chemist Joseph Louis Gay-Lussac in 1814.[9]
History
Hydrochloric acid has been an important and frequently used chemical from early history and was discovered by the alchemist Jabir ibn Hayyan around the year 800 AD.[10][11]
Aqua regia, a mixture consisting of hydrochloric and nitric acids, prepared by dissolving sal ammoniac in nitric acid, was described in the works of Pseudo-Geber, a 13th-century European alchemist.[12][13][14][15][16] Other references suggest that the first mention of aqua regia is in Byzantine manuscripts dating to the end of the 13th century.[17][18][19][20]
Free hydrochloric acid was first formally described in the 16th century by Libavius, who prepared it by heating salt in clay crucibles.[21] Other authors claim that pure hydrochloric acid was first discovered by the German Benedictine monk Basil Valentine in the 15th century,[22] when he heated common salt and green vitriol,[23] whereas others argue that there is no clear reference to the preparation of pure hydrochloric acid until the end of the 16th century.[17]
In the 17th century, Johann Rudolf Glauber from Karlstadt am Main, Germany used sodium chloride salt and sulfuric acid for the preparation of sodium sulfate in the Mannheim process, releasing hydrogen chloride gas. Joseph Priestley of Leeds, England prepared pure hydrogen chloride in 1772,[24] and by 1808 Humphry Davy of Penzance, England had proved that the chemical composition included hydrogen and chlorine.[25]
During the Industrial Revolution in Europe, demand for alkaline substances increased. A new industrial process developed by Nicolas Leblanc of Issoudun, France enabled cheap large-scale production of sodium carbonate (soda ash). In this Leblanc process, common salt is converted to soda ash, using sulfuric acid, limestone, and coal, releasing hydrogen chloride as a by-product. Until the British Alkali Act 1863 and similar legislation in other countries, the excess HCl was vented into the air. After the passage of the act, soda ash producers were obliged to absorb the waste gas in water, producing hydrochloric acid on an industrial scale.[14][26]
In the 20th century, the Leblanc process was effectively replaced by the Solvay process without a hydrochloric acid by-product. Since hydrochloric acid was already fully settled as an important chemical in numerous applications, the commercial interest initiated other production methods, some of which are still used today. After the year 2000, hydrochloric acid is mostly made by absorbing by-product hydrogen chloride from industrial organic compounds production.[14][26][27]
Since 1988, hydrochloric acid has been listed as a Table II precursor under the 1988 United Nations Convention Against Illicit Traffic in Narcotic Drugs and Psychotropic Substances because of its use in the production of heroin, cocaine, and methamphetamine.[28]
Structure and reactions
Hydrochloric acid is the salt of hydronium ion, H3O+ and chloride. It is usually prepared by treating HCl with water.[29][30]
- HCl + H2O ⟶ H3O+ + Cl−{displaystyle mathrm {HCl + H_{2}O longrightarrow H_{3}O^{+} + Cl^{-}} }
- HCl + H2O ⟶ H3O+ + Cl−{displaystyle mathrm {HCl + H_{2}O longrightarrow H_{3}O^{+} + Cl^{-}} }
However, the speciation of hydrochloric acid is more complicated than this simple equation implies. The structure of bulk water is infamously complex, and likewise, the formula H3O+ is also a gross oversimplification of the true nature of the solvated proton, H+(aq), present in hydrochloric acid. A combined IR, Raman, X-ray and neutron diffraction study of concentrated solutions of hydrochloric acid revealed that the primary form of H+(aq) in these solutions is H5O2+, which, along with the chloride anion, is hydrogen-bonded to neighboring water molecules in several different ways. (In H5O2+, the proton is sandwiched midway between two water molecules at 180°). The author suggests that H3O+ may become more important in dilute HCl solutions.[31] (See hydronium ion for further discussion of this issue.)
Hydrochloric acid is a strong acid, since it is completely dissociated in water.[29][30] It can therefore be used to prepare salts containing the Cl– anion called chlorides.
As a strong acid, hydrogen chloride has a large Ka. Theoretical attempts to assign the pKa of hydrogen chloride have been made, with the most recent estimate being −5.9.[32] However, it is important to distinguish between hydrogen chloride gas and hydrochloric acid. Due to the leveling effect, except when highly concentrated and behavior deviates from ideality, hydrochloric acid (aqueous HCl) is only as acidic as the strongest proton donor available in water, the aquated proton (popularly known as "hydronium ion"). When chloride salts such as NaCl are added to aqueous HCl, they have only a minor effect on pH, indicating that Cl− is a very weak conjugate base and that HCl is fully dissociated in aqueous solution. Dilute solutions of HCl have a pH close to that predicted by assuming full dissociation into hydrated H+ and Cl−.[33]
Of the six common strong mineral acids in chemistry, hydrochloric acid is the monoprotic acid least likely to undergo an interfering oxidation-reduction reaction. It is one of the least hazardous strong acids to handle; despite its acidity, it consists of the non-reactive and non-toxic chloride ion. Intermediate-strength hydrochloric acid solutions are quite stable upon storage, maintaining their concentrations over time. These attributes, plus the fact that it is available as a pure reagent, make hydrochloric acid an excellent acidifying reagent.
Hydrochloric acid is the preferred acid in titration for determining the amount of bases. Strong acid titrants give more precise results due to a more distinct endpoint. Azeotropic, or "constant-boiling", hydrochloric acid (roughly 20.2%) can be used as a primary standard in quantitative analysis, although its exact concentration depends on the atmospheric pressure when it is prepared.[34]
Hydrochloric acid is frequently used in chemical analysis to prepare ("digest") samples for analysis. Concentrated hydrochloric acid dissolves many metals and forms oxidized metal chlorides and hydrogen gas. It also reacts with basic compounds such as calcium carbonate or copper(II) oxide, forming the dissolved chlorides that can be analyzed.[29][30]
Physical properties
Concentration | Density | Molarity | pH | Viscosity | Specific heat | Vapour pressure | Boiling point | Melting point | ||
|---|---|---|---|---|---|---|---|---|---|---|
| kg HCl/kg | kg HCl/m3 | Baumé | kg/L | mol/L | mPa·s | kJ/(kg·K) | kPa | °C | °C | |
| 10% | 104.80 | 6.6 | 1.048 | 2.87 | −0.5 | 1.16 | 3.47 | 1.95 | 103 | −18 |
| 20% | 219.60 | 13 | 1.098 | 6.02 | −0.8 | 1.37 | 2.99 | 1.40 | 108 | −59 |
| 30% | 344.70 | 19 | 1.149 | 9.45 | −1.0 | 1.70 | 2.60 | 2.13 | 90 | −52 |
| 32% | 370.88 | 20 | 1.159 | 10.17 | −1.0 | 1.80 | 2.55 | 3.73 | 84 | −43 |
| 34% | 397.46 | 21 | 1.169 | 10.90 | −1.0 | 1.90 | 2.50 | 7.24 | 71 | −36 |
| 36% | 424.44 | 22 | 1.179 | 11.64 | −1.1 | 1.99 | 2.46 | 14.5 | 61 | −30 |
| 38% | 451.82 | 23 | 1.189 | 12.39 | −1.1 | 2.10 | 2.43 | 28.3 | 48 | −26 |
| The reference temperature and pressure for the above table are 20 °C and 1 atmosphere (101.325 kPa). Vapour pressure values are taken from the International Critical Tables and refer to the total vapour pressure of the solution. | ||||||||||
Melting temperature as a function of HCl concentration in water[35][36]
Physical properties of hydrochloric acid, such as boiling and melting points, density, and pH, depend on the concentration or molarity of HCl in the aqueous solution. They range from those of water at very low concentrations approaching 0% HCl to values for fuming hydrochloric acid at over 40% HCl.[29][30][37]
Hydrochloric acid as the binary (two-component) mixture of HCl and H2O has a constant-boiling azeotrope at 20.2% HCl and 108.6 °C (227 °F). There are four constant-crystallization eutectic points for hydrochloric acid, between the crystal form of HCl·H2O (68% HCl), HCl·2H2O (51% HCl), HCl·3H2O (41% HCl), HCl·6H2O (25% HCl), and ice (0% HCl). There is also a metastable eutectic point at 24.8% between ice and the HCl·3H2O crystallization.[37]
Production
Hydrochloric acid is prepared by dissolving hydrogen chloride in water. Hydrogen chloride can be generated in many ways, and thus several precursors to hydrochloric acid exist. The large-scale production of hydrochloric acid is almost always integrated with the industrial scale production of other chemicals.
Industrial market
Hydrochloric acid is produced in solutions up to 38% HCl (concentrated grade). Higher concentrations up to just over 40% are chemically possible, but the evaporation rate is then so high that storage and handling require extra precautions, such as pressurization and cooling. Bulk industrial-grade is therefore 30% to 35%, optimized to balance transport efficiency and product loss through evaporation. In the United States, solutions of between 20% and 32% are sold as muriatic acid. Solutions for household purposes in the US, mostly cleaning, are typically 10% to 12%, with strong recommendations to dilute before use. In the United Kingdom, where it is sold as "Spirits of Salt" for domestic cleaning, the potency is the same as the US industrial grade.[14] In other countries, such as Italy, hydrochloric acid for domestic or industrial cleaning is sold as "Acido Muriatico", and its concentration ranges from 5% to 32%.
Major producers worldwide include Dow Chemical at 2 million metric tons annually (2 Mt/year), calculated as HCl gas, Georgia Gulf Corporation, Tosoh Corporation, Akzo Nobel, and Tessenderlo at 0.5 to 1.5 Mt/year each. Total world production, for comparison purposes expressed as HCl, is estimated at 20 Mt/year, with 3 Mt/year from direct synthesis, and the rest as secondary product from organic and similar syntheses. By far, most hydrochloric acid is consumed captively by the producer. The open world market size is estimated at 5 Mt/year.[14]
Applications
Hydrochloric acid is a strong inorganic acid that is used in many industrial processes such as refining metal. The application often determines the required product quality.[14]
Pickling of steel
One of the most important applications of hydrochloric acid is in the pickling of steel, to remove rust or iron oxide scale from iron or steel before subsequent processing, such as extrusion, rolling, galvanizing, and other techniques.[14][27] Technical quality HCl at typically 18% concentration is the most commonly used pickling agent for the pickling of carbon steel grades.
- Fe2O3 + Fe + 6 HCl ⟶ 3 FeCl2 +3 H2O{displaystyle mathrm {Fe_{2}O_{3} + Fe + 6 HCl longrightarrow 3 FeCl_{2} +3 H_{2}O} }
- Fe2O3 + Fe + 6 HCl ⟶ 3 FeCl2 +3 H2O{displaystyle mathrm {Fe_{2}O_{3} + Fe + 6 HCl longrightarrow 3 FeCl_{2} +3 H_{2}O} }
The spent acid has long been reused as iron(II) chloride (also known as ferrous chloride) solutions, but high heavy-metal levels in the pickling liquor have decreased this practice.
The steel pickling industry has developed hydrochloric acid regeneration processes, such as the spray roaster or the fluidized bed HCl regeneration process, which allow the recovery of HCl from spent pickling liquor. The most common regeneration process is the pyrohydrolysis process, applying the following formula:[14]
- 4 FeCl2 + 4 H2O + O2 ⟶ 8 HCl +2 Fe2O3{displaystyle mathrm {4 FeCl_{2} + 4 H_{2}O + O_{2} longrightarrow 8 HCl +2 Fe_{2}O_{3}} }
- 4 FeCl2 + 4 H2O + O2 ⟶ 8 HCl +2 Fe2O3{displaystyle mathrm {4 FeCl_{2} + 4 H_{2}O + O_{2} longrightarrow 8 HCl +2 Fe_{2}O_{3}} }
By recuperation of the spent acid, a closed acid loop is established.[27] The iron(III) oxide by-product of the regeneration process is valuable, used in a variety of secondary industries.[14]
Production of organic compounds
Another major use of hydrochloric acid is in the production of organic compounds, such as vinyl chloride and dichloroethane for PVC. This is often captive use, consuming locally produced hydrochloric acid that never actually reaches the open market. Other organic compounds produced with hydrochloric acid include bisphenol A for polycarbonate, activated carbon, and ascorbic acid, as well as numerous pharmaceutical products.[27]
2 H2C=CH2 + 4 HCl + O2 ⟶ 2 ClCH2CH2Cl + 2 H2O{displaystyle mathrm {2 H_{2}C=CH_{2} + 4 HCl + O_{2} longrightarrow 2 ClCH_{2}CH_{2}Cl + 2 H_{2}O} }(dichloroethane by oxychlorination)
Production of inorganic compounds
Numerous products can be produced with hydrochloric acid in normal acid-base reactions, resulting in inorganic compounds. These include water treatment chemicals such as iron(III) chloride and polyaluminium chloride (PAC).
Fe2O3 + 6 HCl ⟶ 2 FeCl3 + 3 H2O{displaystyle mathrm {Fe_{2}O_{3} + 6 HCl longrightarrow 2 FeCl_{3} + 3 H_{2}O} }(iron(III) chloride from magnetite)
Both iron(III) chloride and PAC are used as flocculation and coagulation agents in sewage treatment, drinking water production, and paper production.
Other inorganic compounds produced with hydrochloric acid include road application salt calcium chloride, nickel(II) chloride for electroplating, and zinc chloride for the galvanizing industry and battery production.[27]
CaCO3 + 2 HCl ⟶ CaCl2 + CO2 + H2O{displaystyle mathrm {CaCO_{3} + 2 HCl longrightarrow CaCl_{2} + CO_{2} + H_{2}O} }(calcium chloride from limestone)
pH control and neutralization
Hydrochloric acid can be used to regulate the acidity (pH) of solutions.
- OH− + HCl ⟶ H2O + Cl−{displaystyle mathrm {OH^{-} + HCl longrightarrow H_{2}O + Cl^{-}} }
- OH− + HCl ⟶ H2O + Cl−{displaystyle mathrm {OH^{-} + HCl longrightarrow H_{2}O + Cl^{-}} }
In industry demanding purity (food, pharmaceutical, drinking water), high-quality hydrochloric acid is used to control the pH of process water streams. In less-demanding industry, technical quality hydrochloric acid suffices for neutralizing waste streams and swimming pool pH control.[27]
Regeneration of ion exchangers
High-quality hydrochloric acid is used in the regeneration of ion exchange resins. Cation exchange is widely used to remove ions such as Na+ and Ca2+ from aqueous solutions, producing demineralized water. The acid is used to rinse the cations from the resins.[14] Na+ is replaced with H+ and Ca2+ with 2 H+.
Ion exchangers and demineralized water are used in all chemical industries, drinking water production, and many food industries.[14]
Other
Hydrochloric acid is used for a large number of small-scale applications, such as leather processing, purification of common salt, household cleaning,[38] and building construction.[27]Oil production may be stimulated by injecting hydrochloric acid into the rock formation of an oil well, dissolving a portion of the rock, and creating a large-pore structure. Oil well acidizing is a common process in the North Sea oil production industry.[14]
Hydrochloric acid has been used for dissolving calcium carbonate, i.e. such things as de-scaling kettles and for cleaning mortar off brickwork, but it is a hazardous liquid which must be used with care. When used on brickwork the reaction with the mortar only continues until the acid has all been converted, producing calcium chloride, carbon dioxide, and water:
- CaCO3 + 2 HCl ⟶ CaCl2 + CO2 + H2O{displaystyle mathrm {CaCO_{3} + 2 HCl longrightarrow CaCl_{2} + CO_{2} + H_{2}O} }
- CaCO3 + 2 HCl ⟶ CaCl2 + CO2 + H2O{displaystyle mathrm {CaCO_{3} + 2 HCl longrightarrow CaCl_{2} + CO_{2} + H_{2}O} }
Many chemical reactions involving hydrochloric acid are applied in the production of food, food ingredients, and food additives. Typical products include aspartame, fructose, citric acid, lysine, hydrolyzed vegetable protein as food enhancer, and in gelatin production. Food-grade (extra-pure) hydrochloric acid can be applied when needed for the final product.[14][27]
Presence in living organisms
Diagram of alkaline mucous layer in stomach with mucosal defense mechanisms
Gastric acid is one of the main secretions of the stomach. It consists mainly of hydrochloric acid and acidifies the stomach content to a pH of 1 to 2.[39][40]
Chloride (Cl−) and hydrogen (H+) ions are secreted separately in the stomach fundus region at the top of the stomach by parietal cells of the gastric mucosa into a secretory network called canaliculi before it enters the stomach lumen.[41]
Gastric acid acts as a barrier against microorganisms to prevent infections and is important for the digestion of food. Its low pH denatures proteins and thereby makes them susceptible to degradation by digestive enzymes such as pepsin. The low pH also activates the enzyme precursor pepsinogen into the active enzyme pepsin by self-cleavage. After leaving the stomach, the hydrochloric acid of the chyme is neutralized in the duodenum by sodium bicarbonate.[39]
The stomach itself is protected from the strong acid by the secretion of a thick mucus layer, and by secretin induced buffering with sodium bicarbonate. Heartburn or peptic ulcers can develop when these mechanisms fail. Drugs of the antihistaminic and proton pump inhibitor classes can inhibit the production of acid in the stomach, and antacids are used to neutralize excessive existing acid.[39][42]
Safety
| Concentration by weight | Classification[43] | R-Phrases |
|---|---|---|
| 10–25% | Irritant (Xi) | R36/37/38 |
| > 25% | Corrosive (C) | R34 R37 |
Concentrated hydrochloric acid (fuming hydrochloric acid) forms acidic mists. Both the mist and the solution have a corrosive effect on human tissue, with the potential to damage respiratory organs, eyes, skin, and intestines irreversibly. Upon mixing hydrochloric acid with common oxidizing chemicals, such as sodium hypochlorite (bleach, NaClO) or potassium permanganate (KMnO4), the toxic gas chlorine is produced.
- NaClO +2 HCl ⟶ H2O + NaCl + Cl2{displaystyle mathrm {NaClO +2 HCl longrightarrow H_{2}O + NaCl + Cl_{2}} }
- NaClO +2 HCl ⟶ H2O + NaCl + Cl2{displaystyle mathrm {NaClO +2 HCl longrightarrow H_{2}O + NaCl + Cl_{2}} }
- 2 KMnO4 + 16 HCl ⟶ 2 MnCl2 + 8 H2O + 2 KCl + 5 Cl2{displaystyle mathrm {2 KMnO_{4} + 16 HCl longrightarrow 2 MnCl_{2} + 8 H_{2}O + 2 KCl + 5 Cl_{2}} }
- 2 KMnO4 + 16 HCl ⟶ 2 MnCl2 + 8 H2O + 2 KCl + 5 Cl2{displaystyle mathrm {2 KMnO_{4} + 16 HCl longrightarrow 2 MnCl_{2} + 8 H_{2}O + 2 KCl + 5 Cl_{2}} }
- PbO2 + 4 HCl ⟶ PbCl2 + Cl2 + 2 H2O{displaystyle mathrm {PbO_{2} + 4 HCl longrightarrow PbCl_{2} + Cl_{2} + 2 H_{2}O} }
- PbO2 + 4 HCl ⟶ PbCl2 + Cl2 + 2 H2O{displaystyle mathrm {PbO_{2} + 4 HCl longrightarrow PbCl_{2} + Cl_{2} + 2 H_{2}O} }
Personal protective equipment such as latex gloves, protective eye goggles, and chemical-resistant clothing and shoes will minimize risks when handling hydrochloric acid. The United States Environmental Protection Agency rates and regulates hydrochloric acid as a toxic substance.[44]
The UN number or DOT number is 1789. This number will be displayed on a placard on the container.
See also
Chloride, inorganic salts of hydrochloric acid
Hydrochloride, organic salts of hydrochloric acid- Aqua regia
References
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External links
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Hydrogen chloride (chemical compound) at Encyclopædia Britannica
- NIST WebBook, general link
Hydrochloric Acid – Part One and Hydrochloric Acid – Part Two at The Periodic Table of Videos (University of Nottingham)- Calculators: surface tensions, and densities, molarities and molalities of aqueous HCl
- General safety information
- EPA Hazard Summary
- Hydrochloric acid MSDS by Georgia Institute of Technology
- NIOSH Pocket Guide to Chemical Hazards
- Pollution information
- National Pollutant Inventory – Hydrochloric Acid Fact Sheet
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