How To Clean Plastic In Laboratory With Hcl

Strong mineral acid

This article is most the aqueous solution. For the gas, meet hydrogen chloride.

Hydrochloric acid

Names
IUPAC name Chlorane[3]
Other names Muriatic acid[1] Spirits of salt[2] Hydronium chloride Chlorhydric Acrid
Identifiers
CAS Number	7647-01-0 Y
ChEMBL	ChEMBL1231821 Due north
ChemSpider	307 Y
ECHA InfoCard	100.210.665
EC Number	231-595-7
Due east number	E507 (acerbity regulators, ...)
PubChem CID	313
UNII	QTT17582CB Y
United nations number	1789
Properties
Chemical formula	HCl(aq)
Appearance	Colorless, transparent liquid, fumes in air if concentrated
Odor	Pungent characteristic
Melting point	Concentration-dependent – see table
Humid point	Concentration-dependent – see table
log P	0.00[4]
Acerbity (pK a)	−5.9 (HCl gas)[five]
Pharmacology
ATC code	A09AB03 (WHO) B05XA13 (WHO)
Hazards
GHS labelling:
Pictograms
Signal word	Danger [6]
Hazard statements	H290, H314, H335 [6]
Precautionary statements	P260, P280, P303+P361+P353, P305+P351+P338 [6]
NFPA 704 (fire diamond)	3 0 1 Acrid
Related compounds
Related compounds	Hydrofluoric acid Hydrobromic acrid Hydroiodic acid
Supplementary data page
Hydrochloric acid (data page)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Nverify (what is Y N  ?)
Infobox references

Chemic compound

Hydrochloric acid [H⁺(aq) Cl⁻(aq) or H₃O⁺ Cl⁻], as well known equally muriatic acid, is an aqueous solution of hydrogen chloride (chemical formula: HCl). Information technology is a colorless solution with a distinctive pungent smell. It is classified as a strong acrid. Information technology is a component of the gastric acid in the digestive systems of about animate being species, including humans. Hydrochloric acid is an of import laboratory reagent and industrial chemical.^{[seven] [8]}

History [edit]

In the early on tenth century, the Persian physician and alchemist Abu Bakr al-Razi (c. 865–925, Latin: Rhazes) conducted experiments with sal ammoniac (ammonium chloride) and vitriol (hydrated sulfates of various metals), which he distilled together, thus producing the gas hydrogen chloride. In doing and then, al-Razi came very close to discovering hydrochloric acid, but it appears that he disregarded the gaseous products of his experiments, concentrating instead on the color changes that could be effected in the residue.^[ix] Cartoon on al-Razi's experiments, the De aluminibus et salibus ("On Alums and Salts", an eleventh- or twelfth century Arabic text falsely attributed to al-Razi and translated into Latin in the second half of the twelfth century by Gerard of Cremona, 1144-1187) described the heating of metals with diverse salts, which in the instance of mercury resulted in the production of mercury(Ii) chloride (corrosive sublimate).^[10] In this process, muriatic acid actually started to course, simply information technology immediately reacted with the mercury to produce corrosive sublimate. Thirteenth-century Latin alchemists, for whom the De aluminibus et salibus was one of the chief reference works, were fascinated past the chlorinating properties of corrosive sublimate, and they soon discovered that when the metals are eliminated from the procedure of heating vitriols, alums, and salts, strong mineral acids can direct be distilled.^[11] 1 important invention that resulted from the discovery of the mineral acids is aqua regia, a mixture of nitric acrid and muriatic acid in a 1:3 proportion, capable of dissolving gilt. This was commencement described in pseudo-Geber's De inventione veritatis ("On the Discovery of Truth", later c. 1300), where aqua regia was prepared by adding ammonium chloride to nitric acid.^[12] Still, the production of hydrochloric acid itself (i.e., every bit an isolated substance rather than as already mixed with nitric acid) depended on the use of more than efficient cooling apparatus, which would just develop in subsequent centuries.^[thirteen] Thus, recipes for the production of hydrochloric acid but appear in the late sixteenth century, the earliest being found in Giovanni Battista Della Porta'southward (1535–1615) Magiae naturalis ("Natural Magic") and in the works of other contemporary chemists similar Andreas Libavius (c. 1550–1616), Jean Beguin (1550–1620), and Oswald Croll (c. 1563– 1609).^[14] The knowledge of mineral acids such as hydrochloric acid would exist of fundamental importance to seventeenth-century chemists like Daniel Sennert (1572–1637) and Robert Boyle (1627–1691), who used their adequacy to rapidly dissolve metals in their demonstrations of the blended nature of bodies.^[15]

Etymology [edit]

Because it was produced from rock table salt according to the methods of Johann Rudolph Glauber, muriatic acid was historically called by European alchemists spirits of table salt or acidum salis (common salt acid). Both names are still used, especially in other languages, such as German: Salzsäure, Dutch: Zoutzuur, Swedish: Saltsyra, Spanish: Salfumán, Turkish: Tuz Ruhu, Smooth: kwas solny, Hungarian: sósav and Czech: kyselina solná

Gaseous HCl was chosen marine acid air. The proper noun muriatic acid has the same origin (muriatic means "pertaining to alkali or salt", hence muriate ways hydrochloride), and this name is still sometimes used.^{[1] [16]} The name hydrochloric acid was coined by the French chemist Joseph Louis Gay-Lussac in 1814.^[17]

Industrial developments [edit]

During the Industrial Revolution in Europe, demand for alkali metal substances increased. A new industrial process adult past Nicolas Leblanc of Issoudun, France enabled cheap large-scale production of sodium carbonate (soda ash). In this Leblanc process, mutual common salt is converted to soda ash, using sulfuric acid, limestone, and coal, releasing hydrogen chloride as a by-product. Until the British Alkali Deed 1863 and similar legislation in other countries, the backlog HCl was oft vented into the air. An early on exception was the Bonnington Chemical Works where, in 1830, the HCl began to be captured and the hydrochloric acid produced was used in making sal ammoniac (ammonium chloride).^[18] After the passage of the act, soda ash producers were obliged to absorb the waste gas in water, producing hydrochloric acrid on an industrial calibration.^{[19] [20]}

In the 20th century, the Leblanc process was effectively replaced past the Solvay procedure without a hydrochloric acid past-product. Since hydrochloric acrid was already fully settled equally an important chemical in numerous applications, the commercial interest initiated other production methods, some of which are still used today. Afterward the year 2000, hydrochloric acid is mostly made by absorbing past-product hydrogen chloride from industrial organic compounds production.^{[19] [20] [seven]}

Structure and reactions [edit]

Hydrochloric acid is the salt of the protonated water and chloride. Its ions are frequently written as H₃O⁺ Cl⁻,^[21] although the cation is in fact frequently bonded to other water molecules. A combined IR, Raman, X-ray, and neutron diffraction written report of concentrated muriatic acid revealed that the primary form of H⁺ _(aq) in these solutions is H_fiveO_ii ⁺, which, forth with the chloride anion, is hydrogen-bonded to neighboring water molecules in several ways.^[22] (See Hydronium for farther word of this consequence.)

Acidity [edit]

As a strong acrid, hydrogen chloride has a large Yard _a. Theoretical estimates suggest that the pOne thousand _a of hydrogen chloride is −v.nine.^[5] However, it is important to distinguish between hydrogen chloride gas and hydrochloric acid. Due to the leveling issue, except when highly concentrated and behavior deviates from ideality, hydrochloric acid (aqueous HCl) is only as acidic equally the strongest proton donor bachelor in water, the aquated proton (popularly known every bit "hydronium ion"). When chloride salts such equally NaCl are added to aqueous HCl, they have merely a minor effect on pH, indicating that Cl⁻ is a very weak conjugate base and that HCl is fully dissociated. Dilute solutions of HCl have a pH close to that predicted by assuming full dissociation into hydrated H⁺ and Cl⁻.^[23]

Concrete backdrop [edit]

Mass fraction	Concentration		Density	Molarity	pH	Viscosity	Specific rut	Vapour pressure	Boiling bespeak	Melting point
kg HCl/kg	kg HCl/m3	Baumé	kg/L	mol/L		mPa·south	kJ/(kg·G)	kPa	°C	°C
10%	104.fourscore	half dozen.vi	1.048	2.87	−0.v	1.16	3.47	1.95	103	−18
20%	219.60	13	1.098	6.02	−0.8	ane.37	2.99	ane.40	108	−59
thirty%	344.lxx	19	ane.149	9.45	−1.0	one.70	2.60	2.xiii	90	−52
32%	370.88	xx	1.159	ten.17	−1.0	ane.eighty	two.55	3.73	84	−43
34%	397.46	21	i.169	x.xc	−1.0	1.90	ii.50	7.24	71	−36
36%	424.44	22	ane.179	eleven.81	−1.1	ane.99	two.46	14.5	61	−xxx
38%	451.82	23	1.189	12.39	−1.1	two.10	ii.43	28.three	48	−26
The reference temperature and force per unit area 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^{[24] [25]}

Physical properties of hydrochloric acid, such as humid 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 muriatic acid at over forty% HCl.^{[26] [27] [28]}

Muriatic acid as the binary (ii-component) mixture of HCl and H₂O has a constant-humid 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 [H₃O]Cl (68% HCl), [H₅O₂]Cl (51% HCl), [H₇O₃]Cl (41% HCl), [H₃O]Cl·5H₂O (25% HCl), and ice (0% HCl). There is too a metastable eutectic bespeak at 24.viii% between water ice and the [H₇O_three]Cl crystallization.^[28] They are all Hydronium salts.

Production [edit]

Muriatic acid is usually prepared industrially by dissolving hydrogen chloride in water. Hydrogen chloride can be generated in many means, and thus several precursors to hydrochloric acid be. The large-scale product of hydrochloric acid is nigh always integrated with the industrial scale production of other chemicals, such equally in the chloralkali procedure which produces hydroxide, hydrogen, and chlorine, the latter of which can exist combined to produce HCl.^{[26] [27]}

Industrial market [edit]

Muriatic acid is produced in solutions up to 38% HCl (concentrated course). Higher concentrations up to simply over 40% are chemically possible, but the evaporation rate is then and then high that storage and handling require actress precautions, such as pressurization and cooling. Bulk industrial-course is therefore xxx% to 35%, optimized to balance transport efficiency and production loss through evaporation. In the Usa, solutions of betwixt 20% and 32% are sold as muriatic acrid. Solutions for household purposes in the US, mostly cleaning, are typically 10% to 12%, with strong recommendations to dilute before utilise. In the United Kingdom, where it is sold equally "Spirits of Salt" for domestic cleaning, the potency is the same equally the US industrial grade.^[19] In other countries, such as Italian republic, hydrochloric acid for domestic or industrial cleaning is sold as "Acido Muriatico", and its concentration ranges from v% to 32%.

Major producers worldwide include Dow Chemical at 2 million tonnes annually (Mt/twelvemonth), calculated as HCl gas, Georgia Gulf Corporation, Tosoh Corporation, Akzo Nobel, and Tessenderlo at 0.5 to one.5 Mt/year each. Total world production, for comparison purposes expressed as HCl, is estimated at 20 Mt/year, with 3 Mt/year from straight synthesis, and the remainder as secondary product from organic and similar syntheses. By far, well-nigh hydrochloric acid is consumed captively past the producer. The open world market size is estimated at v Mt/year.^[19]

Applications [edit]

Muriatic acid is a strong inorganic acid that is used in many industrial processes such equally refining metal. The awarding often determines the required product quality.^[nineteen] Hydrogen chloride, not muriatic acid, is used more widely in industrial organic chemistry, e.1000. for vinyl chloride and dichloroethane.^[8]

Pickling of steel [edit]

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.^{[19] [7]} Technical quality HCl at typically eighteen% concentration is the most commonly used pickling agent for the pickling of carbon steel grades.

${\displaystyle {\ce {Fe3O4 + Atomic number 26 + 8 HCl -> 4 FeCl2 + iv H2o}}}$

The spent acid has long been reused as iron(Two) chloride (also known as ferrous chloride) solutions, merely high heavy-metal levels in the pickling liquor accept decreased this exercise.

The steel pickling industry has developed hydrochloric acid regeneration processes, such as the spray roaster or the fluidized bed HCl regeneration procedure, which let the recovery of HCl from spent pickling liquor. The most common regeneration process is the pyrohydrolysis process, applying the following formula:^[xix]

${\displaystyle {\ce {4 FeCl2 + four Water + O2 -> eight HCl + ii Fe2O3}}}$

By recuperation of the spent acid, a closed acid loop is established.^[7] The iron(III) oxide by-production of the regeneration process is valuable, used in a diversity of secondary industries.^[19]

Production of inorganic compounds [edit]

Alike to its employ for pickling, hydrochloric acid is used to deliquesce many metals, metal oxides and metallic carbonates. The conversion are often depicted in simplified equations:

Zn + ii HCl → ZnCl₂ + H₂

NiO + 2 HCl → NiCl₂ + H_twoO

CaCO₃ + 2 HCl → CaCl_two + CO_two + H₂O

These processes are used to produce metal chlorides for assay or farther production.^{[26] [27] [7]}

pH command and neutralization [edit]

Hydrochloric acrid tin be used to regulate the acidity (pH) of solutions.

${\displaystyle {\ce {OH^- + HCl -> H2o + Cl^-}}}$

In industry demanding purity (food, pharmaceutical, drinking water), high-quality hydrochloric acrid is used to control the pH of process water streams. In less-demanding industry, technical quality hydrochloric acid suffices for neutralizing waste material streams and pond pool pH control.^[7]

Regeneration of ion exchangers [edit]

High-quality hydrochloric acid is used in the regeneration of ion exchange resins. Cation commutation is widely used to remove ions such every bit Na⁺ and Ca²⁺ from aqueous solutions, producing demineralized water. The acid is used to rinse the cations from the resins.^[19] Na⁺ is replaced with H⁺ and Ca²⁺ with 2 H⁺.

Ion exchangers and demineralized water are used in all chemic industries, drinking water production, and many food industries.^[19]

Laboratory use [edit]

Of the six mutual strong mineral acids in chemistry, hydrochloric acid is the monoprotic acid least likely to undergo an interfering oxidation-reduction reaction. Information technology is 1 of the to the lowest degree hazardous stiff acids to handle; despite its acidity, it contains the non-reactive and not-toxic chloride ion. Intermediate-force muriatic acid solutions are quite stable upon storage, maintaining their concentrations over time. These attributes, plus the fact that information technology is available equally a pure reagent, make muriatic acid an excellent acidifying reagent. It is also inexpensive.

Hydrochloric acid is the preferred acrid in titration for determining the amount of bases. Potent acid titrants requite more precise results due to a more distinct endpoint. Azeotropic, or "abiding-boiling", muriatic acid (roughly 20.2%) can exist used as a primary standard in quantitative analysis, although its verbal concentration depends on the atmospheric pressure when information technology is prepared.^[29]

Other [edit]

Hydrochloric acid is used for a big number of small-calibration applications, such as leather processing, household cleaning,^[30] and edifice structure.^[7] Oil production may be stimulated past injecting hydrochloric acrid into the stone 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 Bounding main oil production industry.^[19]

Muriatic acid has been used for dissolving calcium carbonate, e.g. such things as de-scaling kettles and for cleaning mortar off brickwork. When used on brickwork the reaction with the mortar only continues until the acrid has all been converted, producing calcium chloride, carbon dioxide, and h2o:

${\displaystyle {\ce {CaCO3 + 2 HCl -> CaCl2 + CO2 + H2o}}}$

Many chemical reactions involving muriatic acid are applied in the production of food, food ingredients, and food additives. Typical products include aspartame, fructose, citric acid, lysine, hydrolyzed vegetable poly peptide as food enhancer, and in gelatin production. Nutrient-grade (extra-pure) muriatic acid can be applied when needed for the final production.^{[19] [7]}

Presence in living organisms [edit]

Diagram of alkaline mucous layer in stomach with mucosal defense mechanisms

Gastric acrid is one of the main secretions of the stomach. It consists mainly of hydrochloric acid and acidifies the tum content to a pH of ane to 2.^{[31] [32]} Chloride (Cl⁻) and hydrogen (H⁺) ions are secreted separately in the tum fundus region at the top of the stomach past parietal cells of the gastric mucosa into a secretory network called canaliculi before it enters the breadbasket lumen.^[33]

Gastric acrid acts as a barrier against microorganisms to forestall infections and is important for the digestion of food. Its depression pH denatures proteins and thereby makes them susceptible to deposition 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 bicarbonate.^[31]

The stomach itself is protected from the potent 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 neglect. 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 acrid.^{[31] [34]}

Safety [edit]

Being a strong acid, hydrochloric acid is corrosive to living tissue and to many materials, merely not to safe. Typically, condom protective gloves and related protective gear are used when handling concentrated solutions.^[8]

Mass fraction	Classification[35]	Listing of H-phrases
10% ≤ C < 25%	Causes skin irritation, Causes serious eye irritation,	H315, H319
C ≥ 10%	May cause respiratory irritation	H335
C ≥ 25%	Causes astringent skin burns and eye damage	H314

Muriatic acid has been listed as a Table II forerunner under the 1988 United Nations Convention Against Illicit Traffic in Narcotic Drugs and Psychotropic Substances because of its apply in the production of heroin, cocaine, and methamphetamine.^[36]

See also [edit]

• Chloride, inorganic salts of muriatic acid
• Hydrochloride, organic salts of hydrochloric acrid
• Aqua regia

References [edit]

1. ^ ^{a b} "Muriatic acid". Archived from the original on 15 Oct 2022. Retrieved sixteen September 2022.
2. ^ "spirits of salt". Retrieved 29 May 2022.
3. ^ Favre HA, Powell WH, eds. (2014). Nomenclature of Organic Chemistry: IUPAC Recommendations and Preferred Names 2022. Cambridge: The Royal Society of Chemistry. p. 131.
4. ^ "Hydrochloric acid". www.chemsrc.com.
5. ^ ^{a b} Trummal A, Lipping L, Kaljurand I, Koppel IA, Leito I (May 2022). "Acidity of Strong Acids in Water and Dimethyl Sulfoxide". The Periodical of Concrete Chemistry A. 120 (twenty): 3663–ix. Bibcode:2016JPCA..120.3663T. doi:x.1021/acs.jpca.6b02253. PMID 27115918.
6. ^ ^{a b c} Sigma-Aldrich Co., Hydrochloric acid.
7. ^ ^{a b c d e f m h} Greenwood, Norman Northward.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. pp. 946–48. ISBN978-0-08-037941-8.
8. ^ ^{a b c} Austin, Severin; Glowacki, Arndt (2000). Hydrochloric Acid. doi:10.1002/14356007.a13_283. ISBN3527306730.
9. ^ Multhauf, Robert P. (1966). The Origins of Chemical science. London: Oldbourne. OCLC 977570829. pp. 141-142.
10. ^ Multhauf 1966, pp. 160–162.
11. ^ Multhauf 1966, pp. 162–163.
12. ^ Karpenko, Vladimír; Norris, John A. (2002). "Vitriol in the History of Chemistry". Chemické listy. 96 (12): 997–1005. p. 1002.
13. ^ Multhauf 1966, p. 204.
14. ^ Multhauf 1966, p. 208, note 29; cf. p. 142, note 79.
15. ^ Newman, William R. (2006). Atoms and Abracadabra: Chymistry and the Experimental Origins of the Scientific Revolution. Chicago: Academy of Chicago Press. p. 98.
16. ^ "Hydrochloric acid" (PDF). PPG Industries. 2005. Archived from the original (PDF) on 2 July 2022. Retrieved 10 September 2022.
17. ^ Gay-Lussac (1814) "Mémoire sur l'iode" (Memoir on iodine), Annales de Chemie, 91 : v–160. From page 9: " ... mais cascade les distinguer, je propose d'ajouter au mot spécifique de fifty'acide que l'on considère, le mot générique de hydro; de sorte que le combinaisons acide de hydrogène avec le chlore, 50'iode, et le soufre porteraient le nom d'acide hydrochlorique, d'acide hydroiodique, et d'acide hydrosulfurique; ... " (... but in society to distinguish them, I suggest to add to the specific suffix of the acid beingness considered, the general prefix hydro, and so that the acidic combinations of hydrogen with chlorine, iodine, and sulfur will bear the proper name muriatic acid, hydroiodic acid, and hydrosulfuric acrid; ...)
18. ^ Ronalds BF (2019). "Bonnington Chemic Works (1822-1878): Pioneer Coal Tar Company". International Journal for the History of Engineering & Applied science. 89 (one–2): 73–91. doi:10.1080/17581206.2020.1787807. S2CID 221115202.
19. ^ ^{a b c d east f g h i j k l} "Hydrochloric Acrid". Chemicals Economics Handbook. SRI International. 2001. pp. 733.4000A–733.3003F.
20. ^ ^{a b} Aftalion F (1991). A History of the International Chemical Industry. Philadelphia: University of Pennsylvania Press. ISBN978-0-8122-1297-half dozen.
21. ^ Petrucci, Ralph H.; Harwood, William S.; Herring, F. Geoffrey (2002). General chemistry: principles and modern applications. Prentice Hall. pp. 668–669. ISBN978-0-xiii-014329-seven.
22. ^ Agmon N (January 1998). "Structure of Concentrated HCl Solutions". The Periodical of Physical Chemistry A. 102 (1): 192–199. Bibcode:1998JPCA..102..192A. CiteSeerX10.1.i.78.3695. doi:x.1021/jp970836x. ISSN 1089-5639.
23. ^ McCarty CG, Vitz E (May 2006). "pH Paradoxes: Demonstrating That It Is Not Truthful That pH ≡ −log[H⁺]". Journal of Chemic Education. 83 (v): 752. Bibcode:2006JChEd..83..752M. doi:10.1021/ed083p752. ISSN 0021-9584.
24. ^ "Systemnummer vi Chlor". Gmelins Handbuch der Anorganischen Chemie. Chemie Berlin. 1927.
25. ^ "Systemnummer 6 Chlor, Ergänzungsband Teil B – Lieferung 1". Gmelins Handbuch der Anorganischen Chemie. Chemie Weinheim. 1968.
26. ^ ^{a b c} Lide D (2000). CRC Handbook of Chemistry and Physics (81st ed.). CRC Press. ISBN978-0-8493-0481-one.
27. ^ ^{a b c} Perry R, Greenish D, Maloney J (1984). Perry's Chemical Engineers' Handbook (6th ed.). McGraw-Hill Volume Company. ISBN978-0-07-049479-iv.
28. ^ ^{a b} Aspen Backdrop. binary mixtures modeling software (calculations by Akzo Nobel Engineering ed.). Aspen Applied science. 2002–2003.
29. ^ Mendham J, Denney RC, Barnes JD, Thomas MJ, Denney RC, Thomas MJ (2000). Vogel's Quantitative Chemical Assay (6th ed.). New York: Prentice Hall. ISBN978-0-582-22628-9.
30. ^ Simhon R (xiii September 2003). "Household plc: actually filthy bathroom". The Daily Telegraph. London. Archived from the original on 23 Feb 2009. Retrieved 31 March 2022.
31. ^ ^{a b c} Maton A, Hopkins J, McLaughlin CW, Johnson S, Warner MQ, LaHart D, Wright JD (1993). Human Biology and Health . Englewood Cliffs, New Jersey, U.s.: Prentice Hall. ISBN978-0-13-981176-0.
32. ^ Haas Eastward (6 December 2000). "Digestive Aids: Hydrochloric acid". salubrious.net.
33. ^ Arthur C, Guyton MD, Hall JE (2000). Textbook of Medical Physiology (10th ed.). W.B. Saunders Company. ISBN978-0-7216-8677-6.
34. ^ Bowen R (xviii March 2003). "Control and Physiologic Effects of Secretin". Colorado State Academy. Retrieved 16 March 2009.
35. ^ "Regulation (EC) No 1272/2008 of the European Parliament and of Council of 16 December 2008 on classification, labelling and packaging of substances and mixtures, amending and repealing Directives 67/548/EEC and 1999/45/EC, and amending Regulation (EC) No 1907/2006". EUR-lex. Retrieved 16 December 2008.
36. ^ List of precursors and chemicals frequently used in the illicit manufacture of narcotic drugs and psychotropic substances under international control (PDF) (Eleventh ed.). International Narcotics Control Board. January 2007. Archived from the original (PDF) on 2008-02-27.

External links [edit]

This audio file was created from a revision of this article dated 23 April 2005 (2005-04-23), and does not reverberate subsequent edits.

• NIST WebBook, general link
• Hydrochloric Acid – Part Ane 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 data

• EPA Take chances Summary
• Hydrochloric acid MSDS by Georgia Found of Technology
• NIOSH Pocket Guide to Chemical Hazards

Pollution information

• National Pollutant Inventory – Hydrochloric acid Fact Sheet

Source: https://en.wikipedia.org/wiki/Hydrochloric_acid

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