Chemical Properties of Hydrochloric acid (CAS 7647-01-0)

InChI

InChI=1S/ClH/h1H

InChI Key

VEXZGXHMUGYJMC-UHFFFAOYSA-N

Formula

HCl

SMILES

Cl

Molecular Weight¹

36.46

CAS

7647-01-0

Other Names

• Acide chlorhydrique
• Acido cloridrico
• Anhydrous hydrochloric acid
• Anhydrous hydrogen chloride
• BASILIN
• Chloorwaterstof
• Chlorohydric acid
• Chlorowodor
• Chlorwasserstoff
• HCl
• Hydrochloric acid gas
• Hydrochloric acid, anhydrous
• Hydrochloric ccid
• Hydrochloride
• Hydrogen chloride (HCl)
• Hydrogen chloride (acid)
• Hydrogen-chloride-anhydrous-
• Marine acid
• Muriatic acid
• NA 1789
• NSC 77365
• Salzsaeure
• Soldering acid
• Spirit of salt
• Spirits of salt
• Spirits of salts
• UN 1050
• UN 1789
• UN 2186
• hydrogen chloride

• ω : Acentric Factor.
• PAff : Proton affinity (kJ/mol).
• BasG : Gas basicity (kJ/mol).
• C_p,gas : Ideal gas heat capacity (J/mol×K).
• μ : Dipole Moment (debye).
• η : Dynamic viscosity (Pa×s).
• Δ_fG° : Standard Gibbs free energy of formation (kJ/mol).
• R_g : Radius of Gyration.
• Δ_fH°_gas : Enthalpy of formation at standard conditions (kJ/mol).
• Δ_fusH° : Enthalpy of fusion at standard conditions (kJ/mol).
• Δ_subH : Enthalpy of sublimation at a given temperature (kJ/mol).
• Δ_vapH : Enthalpy of vaporization at a given temperature (kJ/mol).
• IE : Ionization energy (eV).
• logP_oct/wat : Octanol/Water partition coefficient.
• McVol : McGowan's characteristic volume (ml/mol).
• P_c : Critical Pressure (kPa).
• P_triple : Triple Point Pressure (kPa).
• P_vap : Vapor pressure (kPa).
• ρ_l : Liquid Density (kg/m³).
• S°_{gas,1 bar} : Molar entropy at standard conditions (1 bar) (J/mol×K).
• c_sound,fluid : Speed of sound in fluid (m/s).
• T_boil : Normal Boiling Point Temperature (K).
• T_c : Critical Temperature (K).
• T_fus : Normal melting (fusion) point (K).
• T_triple : Triple Point Temperature (K).
• V_c : Critical Volume (m³/kmol).
• Z_c : Critical Compressibility.
• Z_ra : Rackett Parameter.
• ¹: Molecular weight from the IUPAC atomic weights tables.

Physical Properties

Property	Value	Unit	Source
ω	0.1330		KDB
PAff	556.90	kJ/mol	NIST
BasG	530.10	kJ/mol	NIST
μ	1.10	debye	KDB
ΔfG°	95.30	kJ/mol	KDB
Rg	0.2990		KDB
ΔfH°gas	[-92.36; -92.31]	kJ/mol
ΔfH°gas	-92.36	kJ/mol	KDB
ΔfH°gas	-92.31 ± 0.10	kJ/mol	NIST
ΔfusH°	1.64	kJ/mol	Joback Calculated Property
IE	[12.72; 12.79]	eV
IE	12.74 ± 0.01	eV	NIST
IE	Outlier 12.79	eV	NIST
IE	12.75 ± 0.01	eV	NIST
IE	12.75	eV	NIST
IE	12.75 ± 0.00	eV	NIST
IE	12.75	eV	NIST
IE	12.72 ± 0.03	eV	NIST
IE	12.75	eV	NIST
IE	12.75 ± 0.01	eV	NIST
IE	12.74 ± 0.01	eV	NIST
IE	12.74 ± 0.01	eV	NIST
IE	12.74 ± 0.01	eV	NIST
logPoct/wat	0.422		Crippen Calculated Property
McVol	23.100	ml/mol	McGowan Calculated Property
Pc	[8256.00; 8310.00]	kPa
Pc	8310.00	kPa	KDB
Pc	8256.00 ± 8.24	kPa	NIST
Ptriple	13.80 ± 0.01	kPa	NIST
S°gas,1 bar	186.90 ± 0.01	J/mol×K	NIST
Tboil	188.00	K	KDB
Tc	[324.68; 324.70]	K
Tc	324.70	K	KDB
Tc	324.68 ± 0.03	K	NIST
Tfus	[158.97; 161.15]	K
Tfus	158.97	K	KDB
Tfus	161.15 ± 2.00	K	NIST
Ttriple	158.80	K	KDB
Vc	0.081	m3/kmol	KDB
Zc	0.2493260		KDB
Zra	0.27		KDB

Cheméo can also estimate Enthalpy of vaporization at standard conditions, Log10 of Water solubility in mol/l for this compound, but they fall outside the models' validated range, so they are not shown here. Open the prediction tool to compute them on demand.

Temperature Dependent Properties

Property	Value	Unit	Temperature (K)	Source
Cp,gas	[12.24; 15.02]	J/mol×K	[236.13; 397.51]
Cp,gas	12.24	J/mol×K	236.13	Joback Calculated Property
Cp,gas	13.10	J/mol×K	263.03	Joback Calculated Property
Cp,gas	13.78	J/mol×K	289.92	Joback Calculated Property
Cp,gas	14.30	J/mol×K	316.82	Joback Calculated Property
Cp,gas	14.67	J/mol×K	343.72	Joback Calculated Property
Cp,gas	14.90	J/mol×K	370.61	Joback Calculated Property
Cp,gas	15.02	J/mol×K	397.51	Joback Calculated Property
η	[0.0000912; 0.0000994]	Pa×s	[136.05; 236.13]
η	0.0000994	Pa×s	136.05	Joback Calculated Property
η	0.0000972	Pa×s	152.73	Joback Calculated Property
η	0.0000955	Pa×s	169.41	Joback Calculated Property
η	0.0000941	Pa×s	186.09	Joback Calculated Property
η	0.0000929	Pa×s	202.77	Joback Calculated Property
η	0.0000920	Pa×s	219.45	Joback Calculated Property
η	0.0000912	Pa×s	236.13	Joback Calculated Property
ΔsubH	[19.60; 19.70]	kJ/mol	[127.00; 142.00]
ΔsubH	19.70	kJ/mol	127.00	NIST
ΔsubH	19.60	kJ/mol	142.00	NIST
ΔvapH	16.20	kJ/mol	188.00	NIST
ρl	1193.00	kg/m3	188.00	KDB
csound,fluid	[646.00; 940.00]	m/s	[218.30; 273.00]
csound,fluid	940.00	m/s	218.30	Speed of Sound Measurements and a Fundamental Equation of State for Hydrogen Chloride
csound,fluid	910.00	m/s	224.30	Speed of Sound Measurements and a Fundamental Equation of State for Hydrogen Chloride
csound,fluid	887.00	m/s	229.20	Speed of Sound Measurements and a Fundamental Equation of State for Hydrogen Chloride
csound,fluid	865.00	m/s	233.10	Speed of Sound Measurements and a Fundamental Equation of State for Hydrogen Chloride
csound,fluid	814.00	m/s	243.00	Speed of Sound Measurements and a Fundamental Equation of State for Hydrogen Chloride
csound,fluid	790.00	m/s	248.00	Speed of Sound Measurements and a Fundamental Equation of State for Hydrogen Chloride
csound,fluid	762.00	m/s	252.90	Speed of Sound Measurements and a Fundamental Equation of State for Hydrogen Chloride
csound,fluid	734.00	m/s	258.00	Speed of Sound Measurements and a Fundamental Equation of State for Hydrogen Chloride
csound,fluid	705.00	m/s	263.00	Speed of Sound Measurements and a Fundamental Equation of State for Hydrogen Chloride
csound,fluid	676.00	m/s	268.00	Speed of Sound Measurements and a Fundamental Equation of State for Hydrogen Chloride
csound,fluid	646.00	m/s	273.00	Speed of Sound Measurements and a Fundamental Equation of State for Hydrogen Chloride

Correlations

Property	Value	Unit	Temperature (K)	Source
Pvap	[13.50; 8356.93]	kPa	[158.97; 324.65]	The Yaws Handbook of Vapor Pressure
Equation			ln(Pvp) = A + B/(T + C)
Coefficient A			1.46857e+01
Coefficient B			-1.76110e+03
Coefficient C			-1.32200e+01
Temperature range, min.			158.97
Temperature range, max.			324.65
Pvap	13.50	kPa	158.97	Calculated Property
Pvap	52.34	kPa	177.38	Calculated Property
Pvap	154.38	kPa	195.79	Calculated Property
Pvap	373.54	kPa	214.20	Calculated Property
Pvap	779.23	kPa	232.61	Calculated Property
Pvap	1450.63	kPa	251.01	Calculated Property
Pvap	2469.80	kPa	269.42	Calculated Property
Pvap	3915.45	kPa	287.83	Calculated Property
Pvap	5858.10	kPa	306.24	Calculated Property
Pvap	8356.93	kPa	324.65	Calculated Property

Similar Compounds

Find more compounds similar to Hydrochloric acid.

Mixtures

• caesium chloride + Hydrochloric acid + Water
• Hydrochloric acid + Glycine + Water
• Acetaminophen + Hydrochloric acid + Water
• Hydrochloric acid + Methyldiethanolamine + Water
• D-Serine + Hydrochloric acid + Water
• Hydrochloric acid + Water
• Hydrochloric acid + Vitamin C + Water
• Nitrous oxide + Hydrochloric acid
• Nitrous oxide + Methyl fluoride + Hydrochloric acid
• D-Aspartic acid + Hydrochloric acid + Water
• D-Glutamic acid + Hydrochloric acid + Water
• xylose + Hydrochloric acid + Water
• D-Alanine + Hydrochloric acid + Water
• potassium chloride + Hydrochloric acid + Water
• Diisopropyl ether + Hydrochloric acid + Water
• Hydrochloric acid + Water + 5-methyl-N-(4-(trifluoromethyl)phenyl)-4-isoxazolecarboxamide
• Hydrochloric acid + Chloromethane
• Hydrochloric acid + allo-L-isoleucine + Water
• D-Methionine + Hydrochloric acid + Water

Sources

• Crippen Method
• Crippen Method
• Low-Temperature Heat Capacities and Standard Molar Enthalpy of Formation of Dichloro Bis(2-aminopyridine) Zinc (II), ZnCl2(C5H6N2)2(s)
• Solubility of silybin in aqueous hydrochloric acid solution
• Prediction of CO2 and H2S solubility and enthalpy of absorption in reacting N-methyldiethanolamine /water systems with ePC-SAFT
• Thermochemical study of chloropyrazines and chloroquinoxalines
• (Vapour + liquid) equilibria of {xCH3Cl + (1-x)HCl} at temperatures (159.01 and 182.33) K
• Partial molar volume of paracetamol in water, 0.1 M HCl and 0.154 M NaCl at T = (298.15, 303.15, 308.15 and 310.65) K and at 101.325 kPa
• Standard molar enthalpies of formation of 2-chloroquinoline, 4-chloroquinoline, 6-chloroquinoline and 4,7-dichloroquinoline by rotating-bomb calorimetry
• Densities, molar volumes, and isobaric expansivities of (D-xylose + hydrochloric acid + water) systems
• Thermodynamics of proton dissociations from aqueous glycine at temperatures from 278.15 to 393.15 K, molalities from 0 to 1.0 mol.kg-1, and at the pressure 0.35 MPa: Apparent molar heat capacities and apparent molar volumes of glycine, glycinium chloride, and sodium glycinate
• Thermodynamics of proton dissociations from aqueous serine at temperatures from (278.15 to 393.15) K, molalities from (0.01 up to 1.0) mol Ae kg-1, and at the pressure 0.35 MPa: Apparent molar heat capacities and apparent molar volumes of serine, serinium chloride, and sodium serinate
• Thermodynamics of proton dissociations from aqueous alanine at temperatures from (278.15 to 393.15) K, molalities from (0.0075 to 1.0) mol*kg-1, and at the pressure 0.35 MPa: Apparent molar heat capacities and apparent molar volumes of alanine, alaninium chloride, and sodium alaninate
• Thermodynamics of aqueous methyldiethanolamine (MDEA) and methyldiethanolammonium chloride (MDEAH+Cl-) over a wide range of temperature and pressure: Apparent molar volumes, heat capacities, and isothermal compressibilities
• Vapour pressure and excess Gibbs free energy of the ternary system {x1CH3F + x2HCl + x3N2O} at temperature of 182.33 K
• Thermodynamics of proton dissociations from aqueous threonine and isoleucine at temperatures from (278.15 to 393.15) K, molalities from (0.01 to 1.0) mol * kg-1, and at the pressure 0.35 MPa: Apparent molar heat capacities and apparent molar volumes of zwitterionic, protonated cationic, and deprotonated anionic forms
• Thermodynamics of proton dissociations from aqueous L-methionine at temperatures from (278.15 to 393.15) K, molalities from (0.0125 to 1.0) mol Ae kg 1, and at the pressure 0.35 MPa: Apparent molar heat capacities and apparent molar volumes of L-methionine, methioninium chloride, and sodium methioninate
• Thermodynamics of the first and second proton dissociations from aqueous L-aspartic acid and L-glutamic acid at temperatures from (278.15 to 393.15) K and at the pressure 0.35 MPa: Apparent molar heat capacities and apparent molar volumes of zwitterionic, protonated cationic, and deprotonated anionic forms at molalities from (0.002 to 1.0) mol Ae kg 1
• Thermochemical study of some chloro and bromo alkyl substituted phthalimides: Structural energetic correlations
• Volumetric properties of ascorbic acid (vitamin C) and thiamine hydrochloride (vitamin B1) in dilute HCl and in aqueous NaCl solutions at (283.15, 293.15, 298.15, 303.15, 308.15, and 313.15) K
• Combined experimental and computational thermochemistry of isomers of chloronitroanilines
• Thermochemistry of phenylacetic and monochlorophenylacetic acids
• Standard molar enthalpies of formation of the three isomers of chloroanisole
• Thermochemical study of four isomers of dichloroanisole
• Experimental thermochemical study of the monochloronitrobenzene isomers
• Experimental and computational thermochemical study of the dichloronitrobenzene isomers
• Experimental and computational thermochemical study of the tri-, tetra-, and pentachloronitrobenzene isomers
• Experimental thermochemical study of 2,5- and 2,6-dichloro-4-nitroanilines
• Experimental thermochemical study of 4,5-dichloro-2-nitroaniline
• Experimental thermochemical study of two chlorodinitroaniline isomers
• Energetic studies of urea derivatives: Standard molar enthalpy of formation of 3,4,40-trichlorocarbanilide
• Experimental and computational energetic study of two halogenated 2-acetylpyrrole derivatives: 2-trichloroacetylpyrrole and 2-trifluoroacetylpyrrole
• A calorimetric and computational study of the thermochemistry of halogenated 1-phenylpyrrole derivatives
• Standard molar enthalpies of formation of monochloroacetophenone isomers
• Thermochemical study of some dichloroacetophenone isomers
• Enthalpy of formation of zinc acetate dihydrate
• Experimental thermochemical study of fluoro-, chloro- and bromo- derivatives of uracil
• Experimental and computational thermochemical studies of benzoxazole and two chlorobenzoxadole derivatives
• Structure and energetics correlations in some chlorohydroxypyridines
• Thermodynamic modeling of ternary and quaternary (liquid + liquid) systems containing water, FeCl3, HCl and diisopropyl ether
• Experimental thermochemical study of 2-chloroacetophenone and 2,4'-dichloroacetophenone
• Phase equilibria of the systems of CsCl + ErCl3 + H2O and CsCl + ErCl3 + HCl (~10.7%, ~14.4%) + H2O at T = 298.15 K and the standard molar enthalpies of formation of solid phase compounds
• Thermochemical properties of two mixed alkali-alkaline earth metal borates as non-linear optical materials: NaSrBO3 and KSr4B3O9
• Diffusion of levodopa in aqueous solutions of hydrochloric acid at 25 C
• Enthalpies of formation of europium alkoxides: What lessons can be drawn from them
• Heat capacities and thermodynamics of formation of flat-Al13 nitrate - [Al13(OH)24(H2O)24](NO3)15.11H2O
• Phase equilibria of the systems of CsCl + HoCl3 + H2O and CsCl + HoCl3 + HCl (~10%) + H2O at T = 298.15 K and the thermodynamic and fluorescent properties of the new solid-phase compounds
• Thermochemical study of dichloromethylpyrimidine isomers
• Thermodynamics of aqueous adenine: Standard partial molar volumes and heat capacities of adenine, adeninium chloride, and sodium adeninate from T = 283.15 K to 363.15 K
• Solubility and distribution of bicycle derivatives of 1,3-selenazine in pharmaceutically relevant media by saturation shake-flask method
• Determination of the temperature dependence of Titanium(IV) hydrolysis and complexation constants in aqueous sulfuric or chlorhydric solutions
• Solid-liquid equilibria for the systems of (CsCl + DyCl3 + H2O) and {CsCl + DyCl3 + HCl (~10.7%) + H2O} at T = 298.15 K and the thermodynamic properties of the new solid compounds
• Thermochemistry of hydrated ammonium borates
• Enthalpies of formation and lattice enthalpies of alkaline metal acetates
• Synthesis, characterization and standard molar enthalpy of formation of La(C7H5O3)2*(C9H6NO)
• Thermochemistry of NaRb[B4O5(OH)4]*4H2O
• Thermochemistry of dicesium calcium tetraborate octahydrate
• Synthesis, characterization and thermochemistry of K2B5O8(OH)*2H2O
• Thermodynamic properties of K2Sr[B4O5(OH)4]2*10H2O
• Thermochemistry of Potassium Strontium Tetraborate Decahydrated
• Synthesis, Characterization and Standard Molar Enthalpy of Formation of Sm (C7H5O3)2 * (C9H6NO)
• Thermodynamics of the Pt-Cl system
• Synthesis, characterization and thermodynamic properties of NaCs[B4O5(OH)4]*4H2O
• Standard Molar Enthalpies of Formation for the Two Mixed Alkali-Alkaline Earth Metal Borates of LiBaB9O15 and NaBaB9O15
• Effect of different excipients on aqueous solubility of leflunomide.Thermodynamic study
• Thermodynamics and kinetics analysis of thermal dissociation of tri-n-octylamine hydrochloride in open system: A DFT and TGA study
• Determination of standard molar enthalpies of formation of Bi2Mo3O12 (s), Bi2MoO6 (s), Bi6Mo2O15 (s) and Bi6MoO12 (s) by solution calorimetry
• Solubility of FeSO4*7H2O in the H2SO4 Ti(SO4)2 H2O, H2SO4 MgSO4 H2O, and HCl H2O Systems from 278 to 313 K
• Thermodynamics of the Antiviral and Antiparkinsonian Drug Amantadine Hydrochloride: Condensed State Properties and Decomposition
• Speed of Sound Measurements and a Fundamental Equation of State for Hydrogen Chloride
• Phase Diagram of AlCl3-FeCl3-H2O(-HCl) Salt Water System at 298.15 K and Its Application in the Crystallization of AlCl3*6H2O
• Solubilities of Triethanolamine Hydrochloride Ionic Liquid in Aqueous Hydrochloric Acid Solutions with Concentrations from (0 to 8.37) mol*kg-1
• Electrical Conductivity of Electrolytes Found In Natural Waters from (5 to 90) deg C
• Solubility of Hydrogen Chloride in Three 1-Alkyl-3-methylimidazolium Chloride Ionic Liquids in the Pressure Range (0 to 100) kPa and Temperature Range (298.15 to 363.15) K
• Thermochemical Parameters of the Chloronitrophenol Isomers: A Combined Experimental and Theoretical Investigation
• Solution Enthalpies of Ionic Liquid I-Hexyl-3-methylimidazolium Chloride
• Solubilities of LaCl3 in HCl Aqueous Solution at (25, 35, and 45) deg C
• Low-Temperature Heat Capacities and Standard Molar Enthalpy of Formation of Chromium Nicotinate Cr(C6H4NO2)3(s)
• Synthesis, Characterization, and Thermodynamic Study of the Coordination Compound Cd(HNic)2Cl2(s)
• Joback Method
• KDB
• McGowan Method
• NIST Webbook
• The Yaws Handbook of Vapor Pressure

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Outlier This icon means that the value is more than 2 standard deviations away from the property mean.