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Properties of substance:

nitric acid

Group of substances:

inorganic

Physical appearance:

colorless liquid

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

HNO3

Structural formula as text:

HONO2

Molar/atomic mass: 63.01

Melting point (°C):

-41.6

Boiling point (°C):

83

Solubility (g/100 g of solvent):

diethyl ether: soluble [Ref.]
iodine pentafluoride: miscible [Ref.]
methylene chloride: miscible [Ref.]
trinitroglycerol : miscible [Ref.]
water: miscible [Ref.]

Multicomponent solubility (in wt%):

water 98.44%, nitric acid 1.%, calcium sulfate 0.56%, 25 °C [Ref.]
water 94.904%, nitric acid 3.92%, calcium sulfate 1.176%, 25 °C [Ref.]
water 86.88%, nitric acid 11.26%, calcium sulfate 1.86%, 25 °C [Ref.]
water 97.1939%, nitric acid 2.796%, silver chloride 0.0101%, 0 °C [Ref.]
water 97.1807%, nitric acid 2.796%, silver chloride 0.0233%, 25 °C [Ref.]
water 97.178%, nitric acid 2.796%, silver chloride 0.026%, 30 °C [Ref.]
water 97.1477%, nitric acid 2.796%, silver chloride 0.0563%, 40 °C [Ref.]
water 97.095%, nitric acid 2.796%, silver chloride 0.109%, 50 °C [Ref.]
water 70.32%, nitric acid 4.93%, lead nitrate 24.75%, 26 °C, separating phase: Pb(NO3)2 [Ref.]
water 74.82%, nitric acid 12.96%, lead nitrate 12.22%, 26 °C, separating phase: Pb(NO3)2 [Ref.]
water 69.75%, nitric acid 25.99%, lead nitrate 4.26%, 26 °C, separating phase: Pb(NO3)2 [Ref.]
water 49.21%, nitric acid 50.26%, lead nitrate 0.53%, 26 °C, separating phase: Pb(NO3)2 [Ref.]
water 36.1%, nitric acid 63.84%, lead nitrate 0.06%, 26 °C, separating phase: Pb(NO3)2 [Ref.]
water 28.64%, nitric acid 71.35%, lead nitrate 0.008%, 26 °C, separating phase: Pb(NO3)2 [Ref.]
water 43.4%, nitric acid 3.5%, zinc nitrate 53.1%, 25 °C, separating phase: Zn(NO3)2 * 6H2O [Ref.]
water 34.5%, nitric acid 24.%, zinc nitrate 41.5%, 25 °C, separating phase: Zn(NO3)2 * 4H2O [Ref.]
water 21.3%, nitric acid 12.8%, zinc nitrate 65.9%, 25 °C, separating phase: Zn(NO3)2 * 2H2O [Ref.]
water 13.3%, nitric acid 42.1%, zinc nitrate 44.6%, 25 °C, separating phase: Zn(NO3)2 * 2H2O [Ref.]
water 10.5%, nitric acid 37.4%, zinc nitrate 52.1%, 25 °C, separating phase: Zn(NO3)2 * H2O [Ref.]
water 1.3%, nitric acid 88.8%, zinc nitrate 9.9%, 25 °C, separating phase: Zn(NO3)2 * H2O [Ref.]
water 41.86%, nitric acid 5.2%, potassium nitrate 17.68%, sodium nitrate 35.26%, 25 °C, separating phase: NaNO3 + KNO3 [Ref.]
water 37.13%, nitric acid 38.98%, potassium nitrate 16.74%, sodium nitrate 7.15%, 25 °C, separating phase: NaNO3 + KNO3 * 2HNO3 [Ref.]
water 33.07%, nitric acid 62.59%, potassium nitrate 1.02%, sodium nitrate 3.32%, 25 °C, separating phase: NaNO3 + KNO3 * 2HNO3 [Ref.]

Properties of solutions:

0,3296% (wt.), solvent - water
  Density (g/cm3) = 1. (20°)
1% (wt.), solvent - water
  Viscosity (mPa·s) = 1.005 (20°)
  Density (g/cm3) = 1.0037 (20°)
  Freezing point (°C) = -0.56
1,255% (wt.), solvent - water
  Density (g/cm3) = 1.005 (20°)
2,164% (wt.), solvent - water
  Density (g/cm3) = 1.01 (20°)
4% (wt.), solvent - water
  Viscosity (mPa·s) = 1.014 (20°)
  Density (g/cm3) = 1.0202 (20°)
  Freezing point (°C) = -2.32
5% (wt.), solvent - water
  Density (g/cm3) = 1.0256 (20°)
10% (wt.), solvent - water
  Dynamic viscosity (mPa·s) = 1.044 (20°)
  Density (g/cm3) = 1.0543 (20°)
  Index of refraction = 1.346 (20°)
  Freezing point (°C) = -6.6
10,12% (wt.), solvent - water
  Density (g/cm3) = 1.055 (20°)
12% (wt.), solvent - water
  Viscosity (mPa·s) = 1.058 (20°)
  Density (g/cm3) = 1.066 (20°)
  Freezing point (°C) = -8.27
13,9% (wt.), solvent - water
  Freezing point (°C) = -10.
15,9% (wt.), solvent - water

20% (wt.), solvent - water
  Density (g/cm3) = 1.115 (20°)
24,8% (wt.), solvent - water
  Electrical Conductivity (mS/cm) = 767.6 (18°)
25,48% (wt.), solvent - water
  Density (g/cm3) = 1.15 (20°)
30% (wt.), solvent - water
  Density (g/cm3) = 1.18 (20°)
31% (wt.), solvent - water
  Electrical Conductivity (mS/cm) = 781.9 (18°)
31,5% (wt.), solvent - water
  Freezing point (°C) = -40.
32,7% (wt.), solvent - water
  Freezing point (°C) = -43.
32,94% (wt.), solvent - water
  Density (g/cm3) = 1.2 (20°)
40% (wt.), solvent - water
  Molality (moles of solute per kg of solvent) = 10.58
  Molarity (moles of solute per liter of solution) = 7.913
  Density (g/cm3) = 1.2463 (20°)
  Freezing point (°C) = -30.
48,42% (wt.), solvent - water
  Density (g/cm3) = 1.3 (20°)
50% (wt.), solvent - water
  Density (g/cm3) = 1.31 (20°)
53,8% (wt.), solvent - water
  Freezing point (°C) = -18.5
60% (wt.), solvent - water
  Density (g/cm3) = 1.3667 (20°)
64,74% (wt.), solvent - water
  Density (g/cm3) = 1.39 (20°)
65% (wt.), solvent - water
  Density (g/cm3) = 1.3913 (20°)
68,1% (wt.), solvent - water
  Density (g/cm3) = 1.405 (20°)
69,7% (wt.), solvent - water
  Freezing point (°C) = -40.
70% (wt.), solvent - water
  Density (g/cm3) = 1.4134 (20°)
70,5% (wt.), solvent - water
  Freezing point (°C) = -42.
71,63% (wt.), solvent - water
  Density (g/cm3) = 1.42 (20°)
72,5% (wt.), solvent - water
  Freezing point (°C) = -40.
75% (wt.), solvent - water
  Density (g/cm3) = 1.4337 (20°)
77,75% (wt.), solvent - water
  Freezing point (°C) = -38.
80% (wt.), solvent - water
  Density (g/cm3) = 1.4521 (20°)
82,4% (wt.), solvent - water
  Freezing point (°C) = -40.
85% (wt.), solvent - water
  Density (g/cm3) = 1.4686 (20°)
89,95% (wt.), solvent - water
  Freezing point (°C) = -66.3
90% (wt.), solvent - water
  Density (g/cm3) = 1.4826 (20°)
91,9% (wt.), solvent - water
  Freezing point (°C) = -60.
94,8% (wt.), solvent - water
  Freezing point (°C) = -50.
95,46% (wt.), solvent - water
  Density (g/cm3) = 1.495 (20°)
99,01% (wt.), solvent - water
  Density (g/cm3) = 1.509 (20°)

Density:

1.513 (20°C, g/cm3)

Reactions:

  1. [Ref.1]
    Au + HNO3 + 4HCl → H[AuCl4] + NO + 2H2O
  2. [Ref.1]
    3Ag + 4HNO3 → 3AgNO3 + NO + 2H2O
  3. [Ref.1]
    Ag + 2HNO3 → AgNO3 + NO2 + H2O
  4. Yeild 85-95%. [Ref.1aster]
    ClF + HNO3 → ClNO3 + HF
  5. [Ref.1aster]
    Se + 4HNO3 → H2SeO3 + 4NO2 + H2O
    H2SeO3 → SeO2 + H2O
  6. Yeild 50%. [Ref.1]
    (CH3)3C6H3 + HNO3 → (CH3)3C6H2NO2 + H2O
  7. [Ref.1]
    V + 6HNO3 → VO2NO3 + 5NO2 + 3H2O
  8. [Ref.1]
    3Ni + 8HNO3 → 3Ni(NO3)2 + 2NO + 4H2O
  9. [Ref.1, Ref.2, Ref.3, Ref.4]
    Fe + 4HNO3 + 7H2O → Fe(NO3)3 * 9H2O + NO
  10. [Ref.1]
    4Zn + 10HNO3 (0,5%) → 4Zn(NO3)2 + NH4NO3 + 3H2O
  11. [Ref.1, Ref.2]
    5Zn + 12HNO3 (6-10%) → 5Zn(NO3)2 + N2 + 6H2O
  12. [Ref.1]
    4Zn + 10HNO3 (20%) → 4Zn(NO3)2 + N2O + 5H2O
  13. [Ref.1, Ref.2]
    Zn + 4HNO3 (68%) → Zn(NO3)2 + 2NO2 + 2H2O
  14. [Ref.1]
    Mg + 4HNO3 (68%) → Mg(NO3)2 + 2NO2 + 2H2O
  15. [Ref.1]
    3Cu + 8HNO3(30%) + 14H2O → 3Cu(NO3)2 * 6H2O + 2NO
  16. [Ref.1aster]
    C6H5ClO3 + HNO3 → O2NC6H4ClO3 + H2O
  17. [Ref.1, Ref.2aster, Ref.3aster]
    2P + 4HNO3 + H2O → 2H3PO4 + 3NO + NO2
  18. [Ref.1]
    HNO3 + 2HClO4 → NO2ClO4 + H3OClO4
  19. [Ref.1aster]
    BaCrO4 + 2HNO3 → CrO3 + Ba(NO3)2 + H2O
  20. [Ref.1]
    Hg + 4HNO3 → Hg(NO3)2 + 2NO2 + 2H2O
  21. [Ref.1]
    3Hg + 8HNO3 (30%) → 3Hg(NO3)2 + 2NO + 4H2O
  22. Yeild 90%. [Ref.1, Ref.2]
    4CH2=C=O + 4HNO3 → C(NO2)4 + CO2 + 3CH3COOH
  23. [Ref.1]
    CH2=C=O + HNO3 → CH3COONO2

Refractive index (nD):

1.397 (10.4°C)

Vapour pressure (Torr):

10 (-4.4°C)
47 (22°C)
60 (26°C)
100 (34.2°C)

Dissociation:

H0 (1) = -6 (25°C, water)
H0 (1) = -3.78 (20°C, water)
pKa (1) = -1.64 (25°C, water)
pKa (1) = 9.38 (25°C, acetic acid)
pKa (1) = 3.17 (25°C, methanol)
pKa (1) = 3.57 (25°C, ethanol)

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

-174.1 (l)

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

-80.8 (l)

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

155.6 (l)

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

109.9 (l)

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

10.47

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

-133.9 (g)

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

-73.5 (g)

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

266.9 (g)

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

54.1 (g)

References:

  1. Armarego W. L. F. Purification of Laboratory Chemicals. - 5ed. - 2003. - pp. 445
  2. CRC Handbook of Chemistry and Physics. - 90ed. - CRC Press, 2010. - pp. 5-13
  3. Holleman A.F., Wiberg E., Wiberg N. Lehrbuch der Anorganischen Chemie. - Berlin: Walter de Gruyter, 1995. - pp. 244
  4. Seidell A. Solubilities of inorganic and metal organic compounds. - 3ed., vol.1. - New York: D. Van Nostrand Company, 1940. - pp. 582-583
  5. Вредные вещества в промышленности: Справочник для химиков, инженеров и врачей. - 7-е изд., Т.3. - Л.: Химия, 1976. - pp. 117-118 [Russian]
  6. Мельников Е.Я., Салтанова В.П., Наумова А.М., Блинова Ж.С. Технология неорганических веществ и минеральных удобрений. - М.: Химия, 1983. - pp. 138-139 [Russian]
  7. Некрасов Б.В. Основы общей химии. - Т.1. - М.: Химия, 1973. - pp. 416-418, 427-430 [Russian]
  8. Неорганическая химия. - Под ред. Третьякова Ю.Д., Т.2. - М.: Academa, 2004. - pp. 196-201 [Russian]
  9. Рабинович В.А., Хавин З.Я. Краткий химический справочник. - Л.: Химия, 1977. - pp. 51 [Russian]
  10. Реми Г. Курс неорганической химии. - Т.1. - М., 1963. - pp. 642-647 [Russian]
  11. Справочник азотчика. - М.: Химия, 1987. - pp. 18-141 [Russian]
  12. Справочник химика. - 2 изд., Т.1. - Л.-М.: Химия, 1966. - pp. 607 [Russian]
  13. Справочник химика. - Т. 2. - Л.-М.: Химия, 1964. - pp. 12-13 [Russian]
  14. Химическая технология неорганических веществ. - Кн.1, под ред. Ахметова Т.Г. - М.: Высшая школа, 2002. - pp. 490-549 [Russian]
  15. Химическая энциклопедия. - Т. 1. - М.: Советская энциклопедия, 1988. - pp. 61-63 [Russian]

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    © Collected Ruslan Anatolievich Kiper, burewestnik@mail.ru