Table shows cryoscopic and ebullioscopic constant of selected substances.

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liquids#

Substance	Molecular formula	Cryoscopic constant [kg × K / mol]	Ebullioscopic constant [kg × K / mol]
water 25°C	H₂O	1.86	0.513
cyclohexane	C₆H₁₂	20.8	2.92
cyclohexanol	C₆H₁₁OH	42.2	-
ethylene glycol	C₂H₄(OH)₂	3.11	2.26
formic acid	HCOOH	2.38	-
acetate acid	CH₃COOH	3.63	3.22
phenylamine (aniline)	C₆H₅NH₂	5.23	3.82
benzene	C₆H₆	5.07	2.64
toluene	C₆H₅CH₃	3.55	3.4
orthoxylene	C₆H₄(CH₃)₂	5.92	-
metaxylene	C₆H₄(CH₃)₂	7.76	-
paraxylene	C₆H₄(CH₃)₂	7.2	-
chloroform	CHCl₃	4.9	3.8
tetrachloromethane	CCl₄	29.8	5.3
pyridine	C₅H₅N	4.26	2.83
diethyl ethere	(C₂H₅)₂O	1.79	2.02
nitrobenzene	C₆H₅NO₂	6.87	5.2

hydrocarbons#

Substance	Molecular formula	Cryoscopic constant [kg × K / mol]	Ebullioscopic constant [kg × K / mol]
cyclohexane	C₆H₁₂	20.8	2.92
benzene	C₆H₆	5.07	2.64
toluene	C₆H₅CH₃	3.55	3.4
orthoxylene	C₆H₄(CH₃)₂	5.92	-
metaxylene	C₆H₄(CH₃)₂	7.76	-
paraxylene	C₆H₄(CH₃)₂	7.2	-

alcohols#

Substance	Molecular formula	Cryoscopic constant [kg × K / mol]	Ebullioscopic constant [kg × K / mol]
cyclohexanol	C₆H₁₁OH	42.2	-
ethylene glycol	C₂H₄(OH)₂	3.11	2.26

carboxylic acids#

Substance	Molecular formula	Cryoscopic constant [kg × K / mol]	Ebullioscopic constant [kg × K / mol]
formic acid	HCOOH	2.38	-
acetate acid	CH₃COOH	3.63	3.22

amines#

Substance	Molecular formula	Cryoscopic constant [kg × K / mol]	Ebullioscopic constant [kg × K / mol]
phenylamine (aniline)	C₆H₅NH₂	5.23	3.82

other organic#

Substance	Molecular formula	Cryoscopic constant [kg × K / mol]	Ebullioscopic constant [kg × K / mol]
chloroform	CHCl₃	4.9	3.8
tetrachloromethane	CCl₄	29.8	5.3
pyridine	C₅H₅N	4.26	2.83
diethyl ethere	(C₂H₅)₂O	1.79	2.02
nitrobenzene	C₆H₅NO₂	6.87	5.2

inorganic acids#

Substance	Molecular formula	Cryoscopic constant [kg × K / mol]	Ebullioscopic constant [kg × K / mol]
sulfurous (VI) acid	H₂SO₄	6.17	5.33

Some facts#

The cryoscopic constant tells us how many degrees freezing temperature of 1 kilogram of pure solvent will drop after introducing 1 mole of substance into it.
Similarly, the ebullioscopic constant tells us how many degrees boiling point of 1 kilogram of pure solvent will raise after introducing 1 mole of substance into it.
Both constants (ebullioscopic and cryscopic) are specific for given solvent.
Basic unit for ebullioscopic and cryoscopic constants is kilogram times kelvin per mol:

$\dfrac{kg \times K}{mol}$
In case of so-called perfect solutuion the relationship between the changes of boiling point, the ebullioscopic constant and the composition of the solution is as follows:

$\Delta T_b = K_b \times \dfrac{m}{M \times m_s}$
where:
- $\Delta T_b$ - changes of boling temperature comparing to pure solvent,
- $K_b$ - ebullioscopic constant for given solvent,
- $m$ - mass of solute,
- $M$ - molar mass of solute,
- $m_s$ - mass of solvent.
Analogous, for cryoscopic and freezing point we can write below formula:

$\Delta T_f = K_f \times \dfrac{m}{M \times m_s}$
gdzie:
- $\Delta T_k$ - changes of freezing point comparing to pure solvent,
- $K_k$ - cryoscopic constant for given solvent,
- $m$ - mass of solute,
- $M$ - molar mass of solute,
- $m_s$ - mass of solvent.

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