كلوريد هيدروجين

المركب الكيميائي كلوريد الهيدروجين إنگليزية: Hydrogen chloridecode: en is deprecated بالصيغة HCl هو غاز أكال عديم اللون ، يكوُن أدخنة بيضاء من حمض الهيدروكلوريك عندما يتلامس مع الرطوبة في الهواء. حمض الهيدروكلوريك، المحلول المائي لكلوريد الهيدروجين، يُطلق عليه أيضاً الصيغة HCl.

كلوريد هيدروجين

الأسماء
اسم أيوپاك Hydrogen chloride
أسماء أخرى غاز حمض الهيدروكلوريك حمض الهيدروكلوريك هيدروكلوريد
Identifiers
رقم CAS
3D model (JSmol)	Interactive image
مرجع بايلستاين	1098214
ChEBI	CHEBI:17883 Y
ChEMBL	ChEMBL1231821 N
ChemSpider	307 Y
ECHA InfoCard	100.028.723
رقم EC	231-595-7
مرجع Gmelin	322
KEGG	D02057 Y
عناوين مواضيع طبية MeSH	{{{value}}}
رقم RTECS	MW4025000
UNII	QTT17582CB Y
UN number	1050
CompTox Dashboard (EPA)	DTXSID2020711
InChI	InChI={{{value}}}
SMILES
الخصائص
الصيغة الجزيئية	HCl
كتلة مولية	36.46 g/mol
المظهر	غاز عديم اللون
الرائحة	كريهة؛ حادة وحراقة
الكثافة	1.49 g L−1
نقطة الانصهار
نقطة الغليان
قابلية الذوبان في الماء	823 g/L (0 °C) 720 g/L (20 °س) 561 g/L (60 °C)
قابلية الذوبان	يذوب في ميثانول، إيثانول، إيثر
ضغط البخار	4352 kPa (at 21.1 °C)
الحموضة (pKa)	-3.0; -5.9 (±0.4)
القاعدية (pKb)	17.0
معامل الانكسار (nD)	1.0004456 (غاز) 1.254 (سائل)
اللزوجة	0.311 cP (−100 °س)
البنية
الشكل الجزيئي	linear
Dipole moment	1.05 D
الكيمياء الحرارية
الإنتالپية المعيارية للتشكل ΔfHo298	–92.31 kJ mol−1
الانتالبية المعيارية للاحتراق ΔcHo298	–95.31 kJ mol−1
Standard molar entropy So298	186.902 J K−1 mol−1
سعة الحرارة النوعية، C	0.7981 J K−1 g−1
المخاطر
صفحة بيانات السلامة	JT Baker MSDS
ن.م.ع. مخطط تصويري
ن.م.ع. كلمة الاشارة	Danger
ن.م.ع. عبارات المخاطر	H280, H314, H331
ن.م.ع. العبارات الاحتياطية	P261, P280, P305+P351+P338, P310, P410+P403
NFPA 704 (معيـَّن النار)	0 3 1 ACID
الجرعة أو التركيز القاتل (LD, LC):
LD50 (الجرعة الوسطى)	238 mg/kg (rat, oral)
LC50 (التركيز الأوسط)	3124 ppm (الجرذ، 1 ساعة) 1108 ppm (الفأر، 1 ساعة)
LCLo (المنشورة الأقل)	1300 ppm (البشر، 30 دق.) 4416 ppm (أرنب، 30 دق.) 4416 ppm (فأر التجارب، 30 دق.) 3000 ppm (البشر، 5 دق.)
حدود التعرض الصحية بالولايات المتحدة (NIOSH):
PEL (المسموح)	C 5 ppm (7 mg/m3)
REL (الموصى به)	C 5 ppm (7 mg/m3)
IDLH (خطر عاجل)	50 ppm
مركبات ذا علاقة
مركـّبات ذات علاقة	فلوريد الهيدروجين بروميد الهيدروجين يوديد الهيدروجين أستاتيد الهيدروجين
ما لم يُذكر غير ذلك، البيانات المعطاة للمواد في حالاتهم العيارية (عند 25 °س [77 °ف]، 100 kPa).
N verify (what is YN ?)
مراجع الجدول

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 الكيمياء

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 polar covalent bond. The chlorine atom is much more electronegative than the hydrogen atom, which makes this bond 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 and protonate molecules or ions, and can also 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 a corrosive substance, particularly in the presence of moisture.

 البنية والخصائص

The structure of solid 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.

Frozen HCl undergoes 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. Analysis of spectroscopic and dielectric data, and determination of the structure of DCl (deuterium chloride) indicates that HCl forms zigzag chains in the solid, as does HF (انظر الشكل إلى اليمين).

قابلية ذوبان HCl (g/L) في المذيبات الشائعة

درجة الحرارة (°س)	0	20	30	50
ماء	823	720	673	596
ميثانول	513	470	430
إيثانول	454	410	381
إيثر	356	249	195

طيف امتصاص الآشعة تحت الحمراء (IR).

ثنائي واحد في طيف الآشعة تحت الحمراء يَنتـُج عن التركيب النظير للكلور.

infrared spectrum of gaseous hydrogen chloride, shown on the left, 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. Including anharmonicity the vibrational energy can be written as.

$E_{\mathrm {vib} }=h\nu _{e}\cdot \left(v+{\tfrac {1}{2}}\right)+hx_{e}\nu _{e}\cdot \left(v+{\tfrac {1}{2}}\right)^{2}$

To promote an HCl molecule from the v = 0 to the v = 1 state, we would expect to see an infrared absorption about ν_o = ν_e + 2x_eν_e = 2880 cm⁻¹. However, 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 a simultaneous change in the rotational state of the molecules. Because of quantum mechanical selection rules, only certain rotational transitions are permitted. The states are characterized by the rotational quantum number J = 0, 1, 2, 3, ... selection rules state that ΔJ is only able to take values of ±1.

$E(J)_{\mathrm {rot} }=h\cdot B\cdot J(J+1)$

The value of the rotational constant B is much smaller than the vibrational one ν_o, 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 transitions of this molecule to be easily collected using an infrared spectrometer with a gas cell. The latter can even be made of quartz as the HCl absorption lies in a window of transparency for this material.

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

 الانتاج

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

 التخليق المباشر

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):

2 NaCl + 2 H₂O → Cl₂ + 2 NaOH + H₂

The pure chlorine gas can be combined with hydrogen to produce hydrogen chloride in the presence of UV light:

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.

 التخليق العضوي

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.

 الطرق المعملية

Small amounts of HCl gas for laboratory use can be generated in an 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:

NaCl + H₂SO₄ → NaHSO₄ + HCl

This reaction occurs at room temperature. Provided there is NaCl remaining in the generator and it is heated above 200 °C, the reaction proceeds further:

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:

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.

 الاستخدامات

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).

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 gas themselves and decompose. Neither of these hydrates can be dried using standard desiccator methods.

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 التاريخ

تعرف خيميائيو العصور الوسطى على أن حمض الهيدروكلوريك (المعروف آنذاك بإسم روح الملح أو acidum salis) يطلق أبخرة كلوريد الهيدروجين، الذي كان يُسمى الهواء الحامضي البحري. وفي القرن 17، استخدم يوهان رودلف گلاوبر الملح (كلوريد الصوديوم) و حمض الكبريتيك لتحضير كبريتات الصوديوم، مطلقاً غاز كلوريد الهيدروجين (انظر "الانتاج"، أدناه). وفي 1772، أفاد أيضاً كارل ڤيلهلم شيله هذا التفاعل وأحياناً يُنسب له فضل اكتشافه. حضـّر جوسف پريستلي كلوريد الهيدروجين في 1772، وفي 1810 أرسى همفري ديڤي أنه يتكون من هيدروجين وكلور.

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 كلوريد الڤينيل.

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.

 السلامة

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.

The U.S. Occupational Safety and Health Administration and the National Institute for Occupational Safety and Health have established occupational exposure limits for hydrogen chloride at a ceiling of 5 ppm (7 mg/m³), and compiled extensive information on hydrogen chloride workplace safety concerns.

 انظر أيضاً

• Chloride, inorganic salts of hydrochloric acid
• Gastric acid, hydrochloric acid secreted into the stomach to aid digestion of proteins
• Hydrochloride, organic salts of hydrochloric acid

 وصلات خارجية

• بطاقة السلامة الكيميائية العالمية 0163
• Thames & Kosmos Chem C2000 Experiment Manual