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Properties of substance:

hydrogen bromide

Group of substances:

inorganic

Physical appearance:

colorless gas

Empirical formula (Hill's system for organic substances):

HBr

Structural formula as text:

HBr

Molar/atomic mass: 80.91

Melting point (°C):

-86.9

Boiling point (°C):

-66.8

Solubility (g/100 g of solvent):

ethanol: soluble [Ref.]
hydrogen fluoride : insoluble [Ref.]
water: 247.3 (-20°C) [Ref.]
water: 239 (-15°C) [Ref.]
water: 221.2 (0°C) [Ref.]
water: 210.3 (10°C) [Ref.]
water: 193 (25°C) [Ref.]
water: 171.5 (50°C) [Ref.]
water: 150.5 (75°C) [Ref.]
water: 130 (100°C) [Ref.]

Properties of solutions:

1% (wt.), solvent - water
  Density (g/cm3) = 1.0053 (20°)
2% (wt.), solvent - water
  Density (g/cm3) = 1.0124 (20°)
10% (wt.), solvent - water
  Density (g/cm3) = 1.0723 (20°)
  Electrical Conductivity (mS/cm) = 354.9 (15°)
15% (wt.), solvent - water
  Electrical Conductivity (mS/cm) = 494. (15°)
20% (wt.), solvent - water
  Density (g/cm3) = 1.1579 (20°)
30% (wt.), solvent - water
  Density (g/cm3) = 1.258 (20°)
39,4% (wt.), solvent - water
  Freezing point (°C) = -89.6
40% (wt.), solvent - water
  Density (g/cm3) = 1.3772 (20°)
45% (wt.), solvent - water
  Density (g/cm3) = 1.4446 (20°)
50% (wt.), solvent - water
  Density (g/cm3) = 1.5173 (20°)
60% (wt.), solvent - water
  Density (g/cm3) = 1.6787 (20°)
65% (wt.), solvent - water
  Density (g/cm3) = 1.7675 (20°)

Numerical data:

Polarizability of molecules (nm3): 0.0036

Density:

0.003645 (20°C, g/cm3)

Synthesis 1:

Reference: Wang, X., & Schlosser, M. A Convenient and Economic Way to Produce Anhydrous Hydrogen Bromide / Synthesis. - 1994. - No. 5 pp. 479 [doi: 10.1055/s-1994-25506]


(C6H5)3P + (CH3)3CBr → (C6H5)3PHBr + (CH3)2C=CH2
(C6H5)3PHBr → (C6H5)3P + HBr

A 0.5 L three-necked flask equipped with a reflux condenser and topped with a mercury seal was branched to a nitrogen/vacuum line and charged with triphenylphosphine (26 g, 0.10 mol), tert-butyl bromide (11 mL, 14 g, 0.10 mol) and tetrabutylammonium bromide (5.0 g, 16 mmol). The mixture was placed in an oil bath at 85 °C until the gentle reflux had completely ceased (ca. 3 h). Then, by means of a ground-glass joint, a glass tubing was fitted to the top of the condenser whose other end plunged in a Schlenk buret filled with anhydrous Et2O (0.10 L) and cooled with an ice-salt bath (see Figure). Xylene (50 mL) was added to the flask and the mixture was heated to reflux while a gentle stream of nitrogen was allowed to enter through a capillary into the flask and to escape through a mercury seal from the buret. After 2—3 h of heating the hydrogen bromide absorption was finished (no more warming or schlieren formation). The buret was stoppered and an aliquot of the ethereal solution was titrated; yield 70—75% (0.70—0.75 molarity). When stored at -25 °C (deep freeze), the decomposition of the ethereal solution of hydrogen bromide to ethyl bromide and ethanol is relatively slow (estimated half-time of 100 days).

Reactions of synthesis:

  1. Yeild 94%. [Ref.1aster]
    C10H12 + 4Br2 → C10H8Br4 + 4HBr
  2. [Ref.1aster]
    H2 + Br2 → 2HBr
  3. [Ref.1aster]
    2KBr + H2SO4 → 2HBr + K2SO4

Reactions:

  1. Yeild 89%. [Ref.1]
    CH3(CH2)3C≡CH + HBr → CH3(CH2)3CBr=CH2
  2. Yeild 91%. [Ref.1]
    HOCH2C≡CH + HBr → HOCH2CBr=CH2
  3. [Ref.1aster]
    Si + 3HBr → SiHBr3 + H2
  4. [Ref.1aster]
    SOCl2 + 2HBr → SOBr2 + 2HCl
  5. [Ref.1aster]
    CrO2Cl2 + 2HBr → CrO2Br2 + 2HCl

Dissociation:

H0 (1) = -10 (25°C)
H0 (1) = -4.85 (25°C, water)
pKa (1) = -9 (25°C, water)
pKa (1) = 5.6 (25°C, acetic acid)

Permittivity (dielectric constant):

6.3 (-80°C)
1.0028 (21°C)

Dipole moment (D):

0.79 (20°C)

Speed sound (m/s):

200 (0°C, aggregative state - gas)

Standard molar enthalpy (heat) of formation ΔfH0 (298.15 K, kJ/mol):

-34.1 (g)

Standard molar Gibbs energy of formation ΔfG0 (298.15 K, kJ/mol):

-51.2 (g)

Standard molar entropy S0 (298.15 K, J/(mol·K)):

198.6 (g)

Molar heat capacity at constant pressure Cp (298.15 K, J/(mol·K)):

28.01 (g)

Molar enthalpy (heat) of fusion ΔfusH (kJ/mol):

2.41

Enthalpy (heat) of vaporization ΔvapH (kJ/mol):

17.61

Enthalpy (heat) of vaporization ΔvapH (kJ/mol)

12.69 (l) [25°C] [Ref.]

Critical temperature (°C):

89.8

Critical pressure (MPa):

8.51

Critical density (g/cm3):

0.807

References:

  1. Comey A. M., Hahn D. A. A dictionary of Chemical Solubilities Inorganic. - 2 ed. - New York, The MacMillan Company, 1921. - pp. 114-115
  2. Inorganic Syntheses. - Vol. 1. - New York and London, 1939. - pp. 149-157
  3. Olah G.A., Prakash G.K.S., Molnar A., Sommer J. Superacid chemistry. - 2ed. - Wiley, 2009. - pp. 62
  4. Seidell A. Solubilities of inorganic and metal organic compounds. - 3ed., vol.1. - New York: D. Van Nostrand Company, 1940. - pp. 568-569
  5. Девятых Г.Г., Зорин А.Д. Летучие неорганические гидриды особой чистоты. - М.: Наука, 1974. - pp. 179-190 [Russian]
  6. Неводные растворители. - М.: Химия, 1971. - pp. 81 [Russian]
  7. Рабинович В.А., Хавин З.Я. Краткий химический справочник. - Л.: Химия, 1977. - pp. 57 [Russian]
  8. Справочник по растворимости. - Т.1, Кн.1. - М.-Л.: ИАН СССР, 1961. - pp. 345 [Russian]
  9. Справочник по растворимости. - Т.1, Кн.2. - М.-Л.: ИАН СССР, 1962. - pp. 996-998 [Russian]
  10. Справочник химика. - Т. 3. - М.-Л.: Химия, 1965. - pp. 78 [Russian]
  11. Справочник химика. - Т. 3. - М.-Л.: Химия, 1965. - pp. 367, 452-453 [Russian]
  12. Успехи химии. - 1966. - Т.35, №11. - pp. 1937 [Russian]
  13. Химическая энциклопедия. - Т. 1. - М.: Советская энциклопедия, 1988. - pp. 320 [Russian]

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    © Collected Ruslan Anatolievich Kiper, burewestnik@mail.ru