塩酸

WordNet

the 8th letter of the Roman alphabet (同)h

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hydrogenの化学記号
鉛筆の硬度 / 《俗》heroin

Wikipedia preview

出典(authority):フリー百科事典『ウィキペディア（Wikipedia）』「2012/10/16 18:21:45」(JST)

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[Wiki ja表示]

塩化水素（えんかすいそ）は塩素と水素から成るハロゲン化水素。化学式 HCl。常温常圧で無色透明、刺激臭のある気体。有毒。塩化水素酸 (hydrochloric acid) あるいは塩酸ガスとも呼ばれる。

概要

塩化水素は常温常圧下では気体であり、塩化水素の水溶液を塩酸と呼ぶ。気体の塩化水素は、塩化水素分子として存在し、水溶液である塩酸中では、塩化水素はほぼ完全に正負のイオンに電離している。

常温常圧下で、濃度がほぼ25 ％以上の塩酸には発煙性がある。

日本では毒物及び劇物取締法により、原体および10 ％を超える製剤が劇物に指定されている。

ラットの吸入毒性ではLC₅₀が3124 ppm／1h。

発生方法

塩化水素は水素と塩素の反応で得る。

$\rm H_2 + Cl_2 \longrightarrow 2HCl$

もしくは塩化ナトリウムと濃硫酸の反応によって得ることができる。この反応では、濃硫酸が塩化水素より強酸であり且つ、硫酸が不揮発性で塩化水素が揮発性であることが重要である。

$\rm NaCl + H_2SO_4 \longrightarrow NaHSO_4 + HCl$

塩化ナトリウム + 濃硫酸 → 硫酸水素ナトリウム + 塩化水素

工業的には塩化ナトリウム水溶液の電気分解によって水酸化ナトリウムとともに水素と塩素を生成し、その後水素と塩素を混合して作る（イオン交換膜法）。近年では、以下の反応のように塩化ビニルや塩化ビニリデンなどの製造の副生成物として回収される塩化水素の生産量のほうが多い。

$\rm RH + Cl_2 \longrightarrow RCl + 2HCl$

(R:アルキル基、ビニル基など)

塩化水素ガス（塩酸分は除く）の2008年度日本国内生産量は 91,692 t、消費量は 88,078 t である^[1]。

自然には火山活動などで発生する。ルブラン法が炭酸ナトリウム（炭酸ソーダ）生成の主な方法であった頃はこのガスが問題となっていた。

他の物質との反応

塩酸とアンモニアの反応による白煙(ビーカーの中には塩酸、試験管の中にはアンモニア)

アンモニアと反応して白煙（塩化アンモニウム）を生成する。

$\rm NH_3 + HCl \longrightarrow NH_4Cl$

水によく溶け、水溶液は塩酸となる。塩酸は強酸で、水素よりもイオン化傾向の大きい金属と反応し水素を発する。
アルコール（主に三級アルコール）と置換してアルキル塩素化物を与える。
オレフィンなどに付加してアルキル塩素化物を与える。

脚注

^ 化学工業統計月報 - 経済産業省

Chemistry

Hydrochloric acid fumes turning pH paper red showing that the fumes are acidic

Hydrogen chloride is a diatomic molecule, consisting of a hydrogen atom H and a chlorine atom Cl connected by a covalent single bond. Since the chlorine atom is much more electronegative than the hydrogen atom, the covalent bond between the two atoms is quite polar. Consequently, the molecule has a large dipole moment with a negative partial charge δ^– at the chlorine atom and a positive partial charge δ⁺ at the hydrogen atom. In part because of its high polarity, HCl is very soluble in water (and in other polar solvents).

Upon contact, H₂O and HCl combine to form hydronium cations H₃O⁺ and chloride anions Cl^– through a reversible chemical reaction:

HCl + H₂O → H₃O⁺ + Cl^–

The resulting solution is called hydrochloric acid and is a strong acid. The acid dissociation or ionization constant, K_a, is large, which means HCl dissociates or ionizes practically completely in water. Even in the absence of water, hydrogen chloride can still act as an acid. For example, hydrogen chloride can dissolve in certain other solvents such as methanol, protonate molecules or ions, and serve as an acid-catalyst for chemical reactions where anhydrous (water-free) conditions are desired.

HCl + CH₃OH → CH₃O⁺H₂ + Cl^–

Because of its acidic nature, hydrogen chloride is corrosive, particularly in the presence of moisture.

Structure and properties


The structure of DCl, as determined by neutron diffraction of DCl powder at 77 K. DCl was used instead of HCl because the deuterium nucleus is easier to detect than the hydrogen nucleus. The "infinite" chains of DCl are indicated by the dashed lines.

Solubility of HCl (g/L) in common solvents^[5]
Temperature (°C)	0	20	30	50
Water	823	720	673	596
Methanol	513	470	430
Ethanol	454	410	381
Ether	356	249	195

Frozen HCl undergoes a phase transition at 98.4 K. X-ray powder diffraction of the frozen material shows that the material changes from an orthorhombic structure to a cubic one during this transition. In both structures the chlorine atoms are in a face-centered array. However, the hydrogen atoms could not be located.^[6] Analysis of spectroscopic and dielectric data, and determination of the structure of DCl indicates that HCl forms zigzag chains in the solid, as does HF (see figure on right).^[7]

Infrared (IR) absorption spectrum

One doublet in the IR spectrum resulting from the isotopic composition of chlorine.

The infrared spectrum of gaseous hydrogen chloride, shown below, consists of a number of sharp absorption lines grouped around 2886 cm⁻¹ (wavelength ~3.47 µm). At room temperature, almost all molecules are in the ground vibrational state v = 0. To promote an HCl molecule to the v = 1 state, we would expect to see an infrared absorption about 2880 cm⁻¹. This absorption corresponding to the Q-branch is not observed due to it being forbidden by symmetry. Instead, two sets of signals (P- and R-branches) are seen owing to rotation of the molecules. Because of quantum mechanical rules, only certain rotational modes are permitted. They are characterized by the rotational quantum number J = 0, 1, 2, 3, ... ΔJ can only take values of ± 1.

E(J) = h·B·J(J+1)

The value of B is much smaller than ν e, such that a much smaller amount of energy is required to rotate the molecule; for a typical molecule, this lies within the microwave region. However, the vibrational energy of HCl molecule places its absorptions within the infrared region, allowing a spectrum showing the rovibrational modes of this molecule to be easily collected using an ordinary infrared spectrometer with a conventional gas cell.

Naturally abundant chlorine consists of two isotopes, ³⁵Cl and ³⁷Cl, in a ratio of approximately 3:1. While the spring constants are very similar, the reduced masses are different causing significant differences in the rotational energy, thus doublets are observed on close inspection of each absorption line, weighted in the same ratio of 3:1.

Production

Most hydrogen chloride produced on an industrial scale is used for hydrochloric acid production.

Direct synthesis

Flame inside HCl Oven.

In the chlor-alkali industry, brine (mixture of sodium chloride and water) solution is electrolyzed producing chlorine (Cl₂), sodium hydroxide, and hydrogen (H₂). The pure chlorine gas can be combined with hydrogen to produce hydrogen chloride.

Cl₂(g) + H₂(g) → 2 HCl(g)

As the reaction is exothermic, the installation is called an HCl oven or HCl burner. The resulting hydrogen chloride gas is absorbed in deionized water, resulting in chemically pure hydrochloric acid. This reaction can give a very pure product, e.g. for use in the food industry.

Organic synthesis

The largest production of hydrochloric acid is integrated with the formation of chlorinated and fluorinated organic compounds, e.g., Teflon, Freon, and other CFCs, as well as chloroacetic acid, and PVC. Often this production of hydrochloric acid is integrated with captive use of it on-site. In the chemical reactions, hydrogen atoms on the hydrocarbon are replaced by chlorine atoms, whereupon the released hydrogen atom recombines with the spare atom from the chlorine molecule, forming hydrogen chloride. Fluorination is a subsequent chlorine-replacement reaction, producing again hydrogen chloride.

R-H + Cl₂ → R-Cl + HCl

R-Cl + HF → R-F + HCl

The resulting hydrogen chloride gas is either reused directly, or absorbed in water, resulting in hydrochloric acid of technical or industrial grade.

Laboratory methods

Small amounts of HCl gas for laboratory use can be generated in a HCl generator by dehydrating hydrochloric acid with either sulfuric acid or anhydrous calcium chloride. Alternatively, HCl can be generated by the reaction of sulfuric acid with sodium chloride:^[8]

NaCl + H₂SO₄ → NaHSO₄ + HCl

This reaction occurs at room temperature. Provided there is salt remaining in the generator and it is heated above 200 degrees Celsius, the reaction proceeds to;

NaCl + NaHSO₄ → HCl + Na₂SO₄

For such generators to function, the reagents should be dry.

HCl can also be prepared by the hydrolysis of certain reactive chloride compounds such as phosphorus chlorides, thionyl chloride (SOCl₂), and acyl chlorides. For example, cold water can be gradually dripped onto phosphorus pentachloride (PCl₅) to give HCl in this reaction:

PCl₅ + H₂O → POCl₃ + 2 HCl

High purity streams of the gas require lecture bottles or cylinders, both of which can be expensive. In comparison, the use of a generator requires only apparatus and materials commonly available in a laboratory.

Applications

Most hydrogen chloride is used in the production of hydrochloric acid. It is also an important reagent in other industrial chemical transformations, e.g.:

Hydrochlorination of rubber
Production of vinyl and alkyl chlorides

In the semiconductor industry, it is used to both etch semiconductor crystals and to purify silicon via trichlorosilane (SiHCl₃).

It may also be used to treat cotton to delint it, and to separate it from wool.^{[citation needed]}

In the laboratory, anhydrous forms of the gas are particularly useful for generating chloride-based Lewis acids, which must be absolutely dry for their Lewis sites to function. It can also be used to dry the corresponding hydrated forms of these materials by passing it over as they are heated; the materials would otherwise fume HCl(g) themselves and decompose. Neither can these hydrates be dried using standard desiccator methods.

History

Alchemists of the Middle Ages recognized that hydrochloric acid (then known as spirit of salt or acidum salis) released vaporous hydrogen chloride, which was called marine acid air. In the 17th century, Johann Rudolf Glauber used salt (sodium chloride) and sulfuric acid for the preparation of sodium sulfate, releasing hydrogen chloride gas (see production, below). In 1772, Carl Wilhelm Scheele also reported this reaction and is sometimes credited with its discovery. Joseph Priestley prepared hydrogen chloride in 1772, and in 1810 Humphry Davy established that it is composed of hydrogen and chlorine.^[9]

During the Industrial Revolution, demand for alkaline substances such as soda ash increased, and Nicolas Leblanc developed a new industrial-scale process for producing the soda ash. In the Leblanc process, salt was converted to soda ash, using sulfuric acid, limestone, and coal, giving hydrogen chloride as by-product. Initially, this gas was vented to air, but the Alkali Act of 1863 prohibited such release, so then soda ash producers absorbed the HCl waste gas in water, producing hydrochloric acid on an industrial scale. Later, the Hargreaves process was developed, which is similar to the Leblanc process except sulfur dioxide, water, and air are used instead of sulfuric acid in a reaction which is exothermic overall. In the early 20th century the Leblanc process was effectively replaced by the Solvay process, which did not produce HCl. However, hydrogen chloride production continued as a step in hydrochloric acid production.

Historical uses of hydrogen chloride in the 20th century include hydrochlorinations of alkynes in producing the chlorinated monomers chloroprene and vinyl chloride, which are subsequently polymerized to make polychloroprene (Neoprene) and polyvinyl chloride (PVC), respectively. In the production of vinyl chloride, acetylene (C₂H₂) is hydrochlorinated by adding the HCl across the triple bond of the C₂H₂ molecule, turning the triple into a double bond, yielding vinyl chloride.

The "acetylene process", used until the 1960s for making chloroprene, starts out by joining two acetylene molecules, and then adds HCl to the joined intermediate across the triple bond to convert it to chloroprene as shown here:

This "acetylene process" has been replaced by a process which adds Cl₂ to one of the double bonds in 1,3-butadiene instead, and subsequent elimination produces HCl instead, as well as chloroprene.

Safety

Hydrogen chloride forms corrosive hydrochloric acid on contact with water found in body tissue. Inhalation of the fumes can cause coughing, choking, inflammation of the nose, throat, and upper respiratory tract, and in severe cases, pulmonary edema, circulatory system failure, and death. Skin contact can cause redness, pain, and severe skin burns. Hydrogen chloride may cause severe burns to the eye and permanent eye damage.

The gas, being strongly hydrophilic, can be easily scrubbed from the exhaust gases of a reaction by bubbling it through water, producing useful hydrochloric acid as a byproduct.

Any equipment handling hydrogen chloride gas must be checked on a routine basis; particularly valve stems and regulators. The gas requires the use of specialized materials on all wetted parts of the flow path, as it will interact with or corrode numerous materials hydrochloric acid alone will not; such as stainless and regular polymers.

References

^ "hydrogen chloride (CHEBI:17883)". Chemical Entities of Biological Interest (ChEBI). UK: European Bioinformatics Institute. https://www.ebi.ac.uk/chebi/searchId.do?chebiId=17883.
^ Haynes, William M. (2010). Handbook of Chemistry and Physics (91 ed.). Boca Raton, Florida: CRC Press. p. 4–67. ISBN 978-1439820773.
^ Hydrogen Chloride. Gas Encyclopaedia. Air Liquide
^ Perrin, D. D. Dissociation constants of inorganic acids and bases in aqueous solution. Butterworths, London, 1969.
^ Hydrochloric Acid - Compound Summary. Pubchem
^ Natta, G. (1933). "Struttura e polimorfismo degli acidi alogenidrici" (in Italian). Gazzetta Chimica Italiana 63: 425–439.
^ Sándor, E.; Farrow, R. F. C. (1967). "Crystal Structure of Solid Hydrogen Chloride and Deuterium Chloride". Nature 213 (5072): 171–172. Bibcode 1967Natur.213..171S. doi:10.1038/213171a0.
^ Francisco J. Arnsliz (1995). "A Convenient Way To Generate Hydrogen Chloride in the Freshman Lab". J. Chem. Ed. 72 (12): 1139. Bibcode 1995JChEd..72.1139A. doi:10.1021/ed072p1139. http://jchemed.chem.wisc.edu/journal/Issues/1995/Dec/abs1139.html.
^ Hartley, Harold (1960). "The Wilkins Lecture. Sir Humphry Davy, Bt., P.R.S. 1778–1829". Proceedings of the Royal Society of London (A) 255 (1281): 153–180. Bibcode 1960RSPSA.255..153H. doi:10.1098/rspa.1960.0060.

External links

Wikimedia Commons has media related to: Hydrogen chloride

International Chemical Safety Card 0163
Thames & Kosmos Chem C2000 Experiment Manual

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English Journal

Formulation of ciprofloxacin hydrochloride loaded biodegradable nanoparticles: optimization of technique and process variables.

Mobarak DH, Salah S, Elkheshen SA.Author information Department of Pharmaceutics and Industrial Pharmacy, Faculty of Pharmacy, Cairo University , Cairo , Egypt and.AbstractAbstract Poly lactic-co-glycolic acid (PLGA 502 H) nanoparticles incorporating ciprofloxacin HCl (CP) were prepared by double emulsion solvent diffusion technique. Methods: The influence of the application of probe sonication besides the high pressure homogenization in the preparation of the secondary emulsion and its application during the solidification step were studied. Their effect on the particle size, Zeta potential and the percent encapsulation efficiency of the drug (EE %) were investigated. The effect of the addition of polyvinyl alcohol (PVA) during the preparation of the primary emulsion was studied. Moreover, the effect of the addition of 0.1 M sodium chloride and/or adjusting the external and extracting phases to pH 7.4 were investigated. The selected formula was examined using IR, X-ray, DSC and SEM and in vitro drug release. Results: These formulations showed an appropriate particle size ranges between 135.7-187.85 nm, a mean zeta potential ranging from -0.839 to -6.81 mV and a mean EE% which ranged from 35% to 69%. Conclusion: The presented data revealed the superiority of using probe sonication besides high pressure homogenization during the formation of secondary emulsion. Moreover, the results indicated that the tested factors had a pronounced significant effect on the EE%.
Pharmaceutical development and technology.Pharm Dev Technol.2014 Nov;19(7):891-900. doi: 10.3109/10837450.2013.836293. Epub 2013 Sep 13.
Abstract Poly lactic-co-glycolic acid (PLGA 502 H) nanoparticles incorporating ciprofloxacin HCl (CP) were prepared by double emulsion solvent diffusion technique. Methods: The influence of the application of probe sonication besides the high pressure homogenization in the preparation of the seconda
PMID 24032531

Development and characterization of lutein-loaded SNEDDS for enhanced absorption in Caco-2 cells.

Niamprem P, Rujivipat S, Tiyaboonchai W.Author information Department of Pharmaceutical Technology, Faculty of Pharmaceutical Sciences, Naresuan University , Phitsanulok 65000 , Thailand.AbstractAbstract A self-nanoemulsifying drug delivery system (SNEDDS) has been developed for enhanced oral bioavailability of lutein. Its permeation enhancement has been evaluated using monolayers of Caco-2 cells. SNEDDS is composed of a mixture of Lexol® and Emulmetik® 900, Labrasol®, and Tween 80 as oil, surfactant and co-surfactant, respectively. Upon dilution of lutein-loaded SNEDDS with water, a nanoemulsion was obtained in <10 s with spherical droplets of 40-150 nm in diameter. The zeta potential was in the range of -19 to -32 mV. Increasing the ratio of surfactant to co-surfactant decreased the mean droplet size. Dissolution studies showed that lutein was released rapidly (<5 min) from SNEDDS into 0.1 N HCl and pH 6.8 phosphate buffer solution without any aggregation. In vitro studies using Caco-2 cells revealed that lutein-loaded SNEDDS showed shorter lag time and greater (2-fold) cellular accumulation compared with the lutein dispersion.
Pharmaceutical development and technology.Pharm Dev Technol.2014 Sep;19(6):735-42. doi: 10.3109/10837450.2013.829092. Epub 2013 Aug 28.
Abstract A self-nanoemulsifying drug delivery system (SNEDDS) has been developed for enhanced oral bioavailability of lutein. Its permeation enhancement has been evaluated using monolayers of Caco-2 cells. SNEDDS is composed of a mixture of Lexol® and Emulmetik® 900, Labrasol®, and Tween 80 as oi
PMID 23985012

Sediments in concentrated green tea during low-temperature storage.

Xu YQ, Chen GS, Du QZ, Que F, Yuan HB, Yin JF.Author information Institute of Food Chemistry, Zhejiang Gongshang University, 149 Jiaogong Road, Hangzhou, Zhejiang 310012, China; Tea Research Institute, Chinese Academy of Agricultural Sciences, 9 South Meiling Road, Hangzhou 310008, China.AbstractThe formation and the main chemical components of sediments, including reversible tea sediments (RTS) and irreversible tea sediments (IRS), in concentrated green tea during low-temperature storage were studied. RTS was mainly formed in the first 10days, and IRS was mainly formed between 20 and 40days of storage. The RTS were the primary sediment, contributing more than 90% of the total sediment. The RTS comprised of polyphenols, total sugar, caffeine, flavones and proteins, while the IRS mainly comprised of oxalates of Ca, Mg, Ga and Mn. The total mineral content in the IRS (17.1%) was much higher than that in the RTS (2.6%) after 80days of storage. The Ca, Mg, Mn and Ga contents in IRS were over 1.0% (w/w) each. About 75% of the IRS was soluble in 0.1M aqueous HCl, with the oxalate accounting for 68%. Minerals and oxalic acid were the crucial factors in the IRS formation.
Food chemistry.Food Chem.2014 Apr 15;149:137-43. doi: 10.1016/j.foodchem.2013.10.084. Epub 2013 Oct 30.
The formation and the main chemical components of sediments, including reversible tea sediments (RTS) and irreversible tea sediments (IRS), in concentrated green tea during low-temperature storage were studied. RTS was mainly formed in the first 10days, and IRS was mainly formed between 20 and 40day
PMID 24295687

Japanese Journal

花崗岩墓石の風化に及ぼす表面研磨の影響 : 室内実験による予察

高屋康彦,八反地剛,松倉公憲
地形 34(4), 293-302, 2013-10-25
… Two tablet-type specimens (3.5-cm diameter, 1.0-cm height) polished by three types of processes (#1000, buff, and Sanwa final} were set in a bottle where HCl aqueous solution of pH 4.5 flows at a rate of ca. …
NAID 110009661938

Selective recovery of indium from the etching waste solution of the flat-panel display fabrication process

Hasegawa Hiroshi,Rahman Ismail M. M.,Umehara Yoshihiro,Sawai Hikaru,Maki Teruya,Furusho Yoshiaki,Mizutani Satoshi
Microchemical Journal 110, 133-139, 2013-09
… A three-step elution with 0.3molL-1 HNO3, 6molL-1 HCl and 1molL-1 HCl/10mmolL-1 EDTA was required to accomplish the sequential selectivity in the process. …
NAID 120005254064

Effects of Chemical Treatments and Ultrathin Al

Akazawa Masamichi,Nakano Takuma
Jpn J Appl Phys 52(8), 08JN23-08JN23-3, 2013-08-25
… Independent of the extent of native oxide removal, the In 4d core-level binding energy was the same for untreated, HCl-treated, and HF-treated InAlN. …
NAID 150000107628

Related Pictures

★リンクテーブル★

リンク元	「塩化水素」「hydrochloric」
拡張検索	「dil. HCl」「HClO」「conc. HCl」「CHCl3」
関連記事	「HCL」「H」

「塩化水素」

Hydrogen chloride
	IUPAC name Hydrogen chloride
	Other names Hydrochloric acid gas; Hydrochloride
Identifiers
CAS number	7647-01-0
PubChem	313
ChemSpider	307
UNII	QTT17582CB
EC number	231-595-7
UN number	1050
KEGG	D02057
MeSH	Hydrochloric+acid
ChEBI	CHEBI:17883
ChEMBL	CHEMBL1231821
RTECS number	MW4025000
ATC code	A09AB03,B05XA13
Beilstein Reference	1098214
Gmelin Reference	322
Jmol-3D images	Image 1
	SMILES Cl ;
	InChI InChI=1S/ClH/h1H ; Key: VEXZGXHMUGYJMC-UHFFFAOYSA-N InChI=1/ClH/h1H; Key: VEXZGXHMUGYJMC-UHFFFAOYAT ;
Properties
Molecular formula	HCl
Molar mass	36.46 g mol−1
Appearance	Colorless gas
Odor	pungent
Density	1.490 g L−1
Melting point	-114.22 °C, 159 K, -174 °F
Boiling point	-85.05 °C, 188 K, -121 °F
Vapor pressure	4352 kPa (at 21.1 °C)
Acidity (pKa)	-7.0
Basicity (pKb)	21.0
Refractive index (nD)	1.0004456 (gas)
Structure
Molecular shape	linear
Dipole moment	1.05 D
Thermochemistry
Std enthalpy of; formation ΔfHo298	–92.31 kJ mol−1
Std enthalpy of; combustion ΔcHo298	–95.31 kJ mol−1
Standard molar; entropy So298	186.902 J K−1 mol−1
Specific heat capacity, C	0.7981 J K−1 g−1
Hazards
MSDS	JT Baker MSDS
GHS pictograms
GHS signal word	Danger
GHS hazard statements	H280, H314, H331
GHS precautionary statements	P261, P280, P305+351+338, P310, P410+403
EU Index	017-002-00-2
EU classification	T C
R-phrases	R23, R35
S-phrases	(S1/2), S9, S26, S36/37/39, S45
NFPA 704	0 3 1 ACID
LD50	238 mg/kg (rat, oral)
Related compounds
Related compounds	Hydrogen fluoride; Hydrogen bromide; Hydrogen iodide
	(verify) (what is: /?); Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
	Infobox references

塩化水素
	IUPAC名塩化水素
	別称塩酸（水溶液）
識別情報
CAS登録番号	7647-01-0
RTECS番号	MW4025000
特性
化学式	HCl
モル質量	36.46 g/mol
外観	無色気体または液体
密度	1.00045 m g/cm3
融点	−114 °C
沸点	−85 °C
水への溶解度	67 g/100 mL (30 ℃)
酸解離定数 pKa	−4
危険性
MSDS	厚生労働省モデルMSDS
主な危険性	T C
Rフレーズ	R23, R35
Sフレーズ	（S1/2）, S9, S26, S36/37/39, S45
関連する物質
その他の陰イオン	フッ化水素; 臭化水素; ヨウ化水素
	特記なき場合、データは常温（25 °C）・常圧（100 kPa）におけるものである。

　　[★]

英: hydrochloric acid、HCl
関: 塩酸

「hydrochloric」

　　[★]

塩酸の

関: HCl、hydrochloric acid

「dil. HCl」

　　[★]

希塩酸

関: dilute hydrochloric acid、diluted hydrochloric acid

「HClO」

　　[★]

過塩素酸

関: perchlorate、perchloric acid

「conc. HCl」

　　[★]

濃塩酸

関: concentrated hydrochloric acid

「CHCl3」

　　[★] クロロホルム, chloroform

「HCL」

　　[★]

「H」

　　[★]

[0] 化学工業統計月報 - 経済産業省

[0] "hydrogen chloride (CHEBI:17883)". Chemical Entities of Biological Interest (ChEBI). UK: European Bioinformatics Institute. https://www.ebi.ac.uk/chebi/searchId.do?chebiId=17883.

[1] Haynes, William M. (2010). Handbook of Chemistry and Physics (91 ed.). Boca Raton, Florida: CRC Press. p. 4–67. ISBN 978-1439820773.

[2] Hydrogen Chloride. Gas Encyclopaedia. Air Liquide

[3] Perrin, D. D. Dissociation constants of inorganic acids and bases in aqueous solution. Butterworths, London, 1969.

[4] Hydrochloric Acid - Compound Summary. Pubchem

[5] Natta, G. (1933). "Struttura e polimorfismo degli acidi alogenidrici" (in Italian). Gazzetta Chimica Italiana 63: 425–439.

[6] Sándor, E.; Farrow, R. F. C. (1967). "Crystal Structure of Solid Hydrogen Chloride and Deuterium Chloride". Nature 213 (5072): 171–172. Bibcode 1967Natur.213..171S. doi:10.1038/213171a0.

[7] Francisco J. Arnsliz (1995). "A Convenient Way To Generate Hydrogen Chloride in the Freshman Lab". J. Chem. Ed. 72 (12): 1139. Bibcode 1995JChEd..72.1139A. doi:10.1021/ed072p1139. http://jchemed.chem.wisc.edu/journal/Issues/1995/Dec/abs1139.html.

[8] Hartley, Harold (1960). "The Wilkins Lecture. Sir Humphry Davy, Bt., P.R.S. 1778–1829". Proceedings of the Royal Society of London (A) 255 (1281): 153–180. Bibcode 1960RSPSA.255..153H. doi:10.1098/rspa.1960.0060.

塩化水素

IUPAC名塩化水素
別称塩酸（水溶液）
識別情報
CAS登録番号	7647-01-0
RTECS番号	MW4025000
特性
化学式	HCl
モル質量	36.46 g/mol
外観	無色気体または液体
密度	1.00045 m g/cm3
融点	−114 °C
沸点	−85 °C
水への溶解度	67 g/100 mL (30 ℃)
酸解離定数 pK_a	−4
危険性
MSDS	厚生労働省モデルMSDS
主な危険性	T C
Rフレーズ	R23, R35
Sフレーズ	（S1/2）, S9, S26, S36/37/39, S45
関連する物質
その他の陰イオン	フッ化水素臭化水素ヨウ化水素
特記なき場合、データは常温（25 °C）・常圧（100 kPa）におけるものである。

Hydrogen chloride

IUPAC name Hydrogen chloride^[1]
Other names Hydrochloric acid gas Hydrochloride
Identifiers
CAS number	7647-01-0^Y
PubChem	313
ChemSpider	307^Y
UNII	QTT17582CB^Y
EC number	231-595-7
UN number	1050
KEGG	D02057^Y
MeSH	Hydrochloric+acid
ChEBI	CHEBI:17883^Y
ChEMBL	CHEMBL1231821^N
RTECS number	MW4025000
ATC code	A09AB03,B05XA13
Beilstein Reference	1098214
Gmelin Reference	322
Jmol-3D images	Image 1
SMILES Cl
InChI InChI=1S/ClH/h1H^Y Key: VEXZGXHMUGYJMC-UHFFFAOYSA-N^Y InChI=1/ClH/h1H Key: VEXZGXHMUGYJMC-UHFFFAOYAT
Properties
Molecular formula	HCl
Molar mass	36.46 g mol⁻¹
Appearance	Colorless gas
Odor	pungent
Density	1.490 g L⁻¹^[2]
Melting point	-114.22 °C, 159 K, -174 °F
Boiling point	-85.05 °C, 188 K, -121 °F
Vapor pressure	4352 kPa (at 21.1 °C)^[3]
Acidity (pK_a)	-7.0^[4]
Basicity (pK_b)	21.0
Refractive index (n_D)	1.0004456 (gas)
Structure
Molecular shape	linear
Dipole moment	1.05 D
Thermochemistry
Std enthalpy of formation Δ_fH^o₂₉₈	–92.31 kJ mol⁻¹
Std enthalpy of combustion Δ_cH^o₂₉₈	–95.31 kJ mol⁻¹
Standard molar entropy S^o₂₉₈	186.902 J K⁻¹ mol⁻¹
Specific heat capacity, C	0.7981 J K⁻¹ g⁻¹
Hazards
MSDS	JT Baker MSDS
GHS pictograms
GHS signal word	Danger
GHS hazard statements	H280, H314, H331
GHS precautionary statements	P261, P280, P305+351+338, P310, P410+403
EU Index	017-002-00-2
EU classification	T C
R-phrases	R23, R35
S-phrases	(S1/2), S9, S26, S36/37/39, S45
NFPA 704	0 3 1 ACID
LD₅₀	238 mg/kg (rat, oral)
Related compounds
Related compounds	Hydrogen fluoride Hydrogen bromide Hydrogen iodide
N (verify) (what is: Y/N?) Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references

匿名

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案内

HCl