Isopropyl alcohol (data page)

Last updated November 21, 2022

This page provides supplementary chemical data on isopropanol.

Material Safety Data Sheet

The handling of this chemical may incur notable safety precautions. It is highly recommend that you seek the Material Safety Datasheet (MSDS) for this chemical from a reliable source such as eChemPortal, and follow its directions.

Structure and properties

Structure and properties
Index of refraction, n_D	1.3776 at 20°C
Abbe number	?
Dielectric constant, ε_r	18.23 ε₀ at 25 °C
Bond strength	?
Bond length	?
Bond angle	?
Magnetic susceptibility	?
Surface tension	21.7 dyn/cm at 20°C
Viscosity ^[1]	4.5646 mPa·s at 0°C 2.3703 mPa·s at 20°C 1.3311 mPa·s at 40°C

Thermodynamic properties

Phase behavior
Triple point	184.9 K (−88.2 °C), ? Pa
Critical point	508.7 K (235.6 °C), 5370 kPa
Std enthalpy change of fusion, Δ_fusH^o	5.28 kJ/mol
Std entropy change of fusion, Δ_fusS^o	28.6 J/(mol·K)
Std enthalpy change of vaporization, Δ_vapH^o	44.0 kJ/mol
Std entropy change of vaporization, Δ_vapS^o	124 J/(mol·K)
Solid properties
Std enthalpy change of formation, Δ_fH^o_solid	? kJ/mol
Standard molar entropy, S^o_solid	? J/(mol K)
Heat capacity, c_p	0.212 J/(mol K) at −200°C
Liquid properties
Std enthalpy change of formation, Δ_fH^o_liquid	−318.2 kJ/mol
Standard molar entropy, S^o_liquid	180 J/(mol K)
Heat capacity, c_p	2.68 J/(gK) at 20°C-25°C
Gas properties
Std enthalpy change of formation, Δ_fH^o_gas	−261.1 kJ/mol
Standard molar entropy, S^o_gas	333 J/(mol K)
Heat capacity, c_p	1.54 J/(gK) at 25°C

Vapor pressure of liquid

P in mm Hg		1	10	40	100	400	760	1520	3800	7600	15200	30400	45600
T in °C		−26.1	2.4	23.8	39.5	67.8	82.5	101.3	130.2	155.7	186.0	220.2	—

Table data obtained from CRC Handbook of Chemistry and Physics 44th ed.

Distillation data

BP temp. °C	% by mole isopropanol
Vapor-liquid equilibrium for isopropanol/water^[4] P = 760 mm Hg
BP temp. °C	liquid	vapor
82.2	100.00	100.00
81.48	95.35	93.25
80.70	87.25	83.40
80.37	80.90	77.45
80.23	76.50	73.70
80.11	69.55	69.15
80.16	66.05	67.15
80.15	64.60	66.45
80.31	55.90	62.55
80.38	51.45	60.75
80.67	44.60	59.20
80.90	38.35	57.00
81.28	29.80	55.10
81.29	29.75	55.40
81.23	28.35	55.30
81.62	24.50	53.90
81.75	19.35	53.20
81.58	18.95	53.75
81.99	16.65	52.15
82.32	12.15	51.20
82.70	10.00	50.15
84.57	5.70	45.65
88.05	3.65	36.55
93.40	1.60	21.15
95.17	1.15	16.30
100.0	0.00	0.00

BP temp. °C	% by mole methanol
Vapor-liquid equilibrium for isopropanol/methanol ^[4] P = 101.325 kPa
BP temp. °C	liquid	vapor
64.37	100.0	100.0
67.34	81.26	90.32
67.64	79.45	89.10
69.54	68.64	81.73
70.77	61.72	76.52
71.88	55.96	71.76
72.78	51.03	67.78
73.80	46.34	63.08
74.85	39.75	56.21
75.65	35.50	51.62
76.36	31.71	46.91
77.93	23.79	35.98
78.67	19.49	30.22
79.45	15.45	24.40
80.04	12.30	19.56
80.57	9.30	14.66
80.82	8.43	12.43
82.20	0.0	0.0

BP temp. °C	% by mole acetone
Vapor-liquid equilibrium for isopropanol/acetone ^[4] P = 101.325 kPa
BP temp. °C	liquid	vapor
77.92	6.12	19.90
76.71	8.28	25.52
71.50	19.59	47.03
70.99	20.91	48.90
69.20	26.01	55.29
68.85	27.10	56.50
65.91	37.55	66.12
63.55	48.12	73.37
63.42	48.74	73.75
62.46	53.77	76.63
62.37	54.27	76.91
61.85	57.22	78.49
61.86	57.12	78.43

Spectral data

UV-Vis
λ_max	205 nm
Extinction coefficient, ε	100.2 m²/mol
IR
Major absorption bands	3334, 2970, 1466, 1378, 1160, 1128, 951, 817, 639 cm⁻¹
NMR
Proton NMR
Carbon-13 NMR
Other NMR data
MS
Masses of main fragments	m/z (% of relative intensity): 45 (100), 43 (19.1), 27 (16.8), 29 (12.5), 19 (9.9), 15 (9.5), 41 (8.2), 31 (6.8), 39 (6.6), 42 (4.4)

This box:

Except where noted otherwise, data relate to Standard temperature and pressure.
Reliability of data general note.

Related Research Articles

Distillation, or classical distillation, is the process of separating the components or substances from a liquid mixture by using selective boiling and condensation. Dry distillation is the heating of solid materials to produce gaseous products. Dry distillation may involve chemical changes such as destructive distillation or cracking and is not discussed under this article. Distillation may result in essentially complete separation, or it may be a partial separation that increases the concentration of selected components in the mixture. In either case, the process exploits differences in the relative volatility of the mixture's components. In industrial applications, distillation is a unit operation of practically universal importance, but it is a physical separation process, not a chemical reaction.

Vapor pressure or equilibrium vapor pressure is defined as the pressure exerted by a vapor in thermodynamic equilibrium with its condensed phases at a given temperature in a closed system. The equilibrium vapor pressure is an indication of a liquid's evaporation rate. It relates to the tendency of particles to escape from the liquid. A substance with a high vapor pressure at normal temperatures is often referred to as volatile. The pressure exhibited by vapor present above a liquid surface is known as vapor pressure. As the temperature of a liquid increases, the kinetic energy of its molecules also increases. As the kinetic energy of the molecules increases, the number of molecules transitioning into a vapor also increases, thereby increasing the vapor pressure.

Freezing-point depression is a drop in the temperature at which a substance freezes, caused when a smaller amount of another, non-volatile substance is added. Examples include adding salt into water, alcohol in water, ethylene or propylene glycol in water, adding copper to molten silver, or the mixing of two solids such as impurities into a finely powdered drug.

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References

↑ Lange's Handbook of Chemistry, 10th ed. pp 1669–1674
↑ Parks, J. S.; B. Barton (1928). "Vapor pressure data for isopropyl alcohol and tertiary butyl alcohol". Journal of the American Chemical Society. 50: 24–26. doi:10.1021/ja01388a004.
↑ Barr-David, F; B. F. Dodge (1959). "Vapor-Liquid Equilibrium at High Pressures. The Systems Ethanol-Water and 2-Propanol-Water". Journal of Chemical and Engineering Data. 4: 107–121. doi:10.1021/je60002a003.
1 2 3 "Binary Vapor-Liquid Equilibrium Data" (Queriable database). Chemical Engineering Research Information Center. Retrieved 5 May 2007.

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[lange1669-1] Lange's Handbook of Chemistry, 10th ed. pp 1669–1674

[2] Parks, J. S.; B. Barton (1928). "Vapor pressure data for isopropyl alcohol and tertiary butyl alcohol". Journal of the American Chemical Society. 50: 24–26. doi:10.1021/ja01388a004.

[3] Barr-David, F; B. F. Dodge (1959). "Vapor-Liquid Equilibrium at High Pressures. The Systems Ethanol-Water and 2-Propanol-Water". Journal of Chemical and Engineering Data. 4: 107–121. doi:10.1021/je60002a003.

[cheric_p-4] 1 2 3 "Binary Vapor-Liquid Equilibrium Data" (Queriable database). Chemical Engineering Research Information Center. Retrieved 5 May 2007.

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