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IUPAC-NIST Solubility Database
NIST Standard Reference Database 106
Solubility System:
1-Proponal with Decane and Water
Components:
(1) Water; H2O; [7732-18-5]
NIST Chemistry WebBook
for detail
(2) 1-Proponal (n-propanol, propyl alcohol, n-propyl alcohol); C3H8O; [71-23-8]
NIST Chemistry WebBook
for detail
(3) Decane (n-decane); C10H22; [124-18-5]
NIST Chemistry WebBook
for detail
Evaluator:
A. Skrzecz, Institute of Physical Chemistry, Polish Academy of Sciences, Warsaw, Poland (1996.01)
Critical Evaluation:
A survey of reported compositions along the saturation curve (sat), and compositions of coexisting phases in equilibrium (eq.) for the system 1-propanol-decane-water is given in Table 54.
Saturation curve
Compositions along the saturation curve of the 1-propanol-decane-water system were obtained at 293.2 K by titration method, Refs. 1 and 2. All experimental solubility data at 293.2 K are presented in
Figure 1
. Only one binary pair of components, decane-water, is partially miscible. Experimental values of mutual solubilities in this binary system were compiled and critically evaluated in previously published SDS Volume, Ref. 3. At 293 K the tentative value for solubility of decane in water was reported to be
x
"
2
=2.5·10
–9
while for solubility of water in decane reasonable data were not accessible; they are expected by the evaluator to be about
x
'
3
=6·10
–4
mole fraction. Mutual solubilities of decane and water were not reported in the papers evaluated in Ref. 3. Compositions of four points in the water-rich phase at the lowest 1-propanol concentration were reported to be decane free,
2
which suggests that 1-propanol is only partially soluble in water. These numerical results are the consequence of the limited sensitivity of experimental measurements (reading the equilibrium phase composition from previously obtained curves of refractive index and density along the saturation curve). The concentration of the decane-rich phase (Ref. 2) in the range of
x
2
>0.83 appears to contain errors since it is inconsistent with the expected concentration of the binary mixture. The other experimental points of both types are consistent with one another and were fitted to the equation:
x
1
=1.009 02+0.133 81 ln(
x
2
)–1.031 32
x
2
–0.010 20
x
2
2
.
The parameters were calculated by the least-squares method and the standard error of estimate was 0.0153. (The parameters describe experimental data which are in the region of 0.01-0.92 mole fraction of decane.) Points on the saturation curve calculated in the range of experimental data by the proposed equation are presented in Table 55 and in
Fig. 28
.
Phases in equilibrium
Compositions of coexisting phases in equilibrium of the ternary system 1-propanol-decane-water were reported in two references. Similar experimental procedures were used in both references; when the equilibrium was reached then the phases were separated and the densities
1,2
and refractive indexes
2
of each phase were measured. The tie lines in each reference cover the whole area of the miscibility gap, but they are inconsistent with one another, the directions of the tie lines are quite different although the compositions of phases in equilibrium are located on the saturation curve. On the basis of tie lines consistency in a series 1-propanol-alkane-water systems,
4
the equilibrium data of Mahers and Dawe
2
appear to be more reasonable because they are similar to other systems. The equilibrium data of Dubovskaya and Karapetyants
1
are rejected.
The plait point estimated by Mahers and Dawe, Ref. 2, is
x
1
=0.529,
x
2
=0.299.
Experimental Data:
(Notes on the Nomenclature)
TABLE 54. Summary of experimental data for the system 1-propanol-decane-water
Author
T/K
DataType
Reference
Dubovskaya and Karapetyants, 1968
293
sat. (17), eq. (4)
1
Mahers and Dawe, 1986
293
sat. (78), eq. (12)
2
TABLE 55. Calculated composition along the saturation curve at 293.2 K
T/K
Mole Fraction x
1
10
0
* Mole Fraction x
2
293.2
0.0000
2.5 Ref. 3
293.2
0.3825
0.0100
293.2
0.4649
0.0200
293.2
0.5371
0.0400
293.2
0.5707
0.0600
293.2
0.5886
0.0800
293.2
0.5979
0.1000
293.2
0.6017
0.1200
293.2
0.6017
0.1400
293.2
0.5990
0.1600
293.2
0.5942
0.1800
293.2
0.5878
0.2000
293.2
0.5800
0.2200
293.2
0.5711
0.2400
293.2
0.5613
0.2600
293.2
0.5507
0.2800
293.2
0.5394
0.3000
293.2
0.5276
0.3200
293.2
0.5152
0.3400
293.2
0.5024
0.3600
293.2
0.4891
0.3800
293.2
0.4755
0.4000
293.2
0.4616
0.4200
293.2
0.4474
0.4400
293.2
0.4329
0.4600
293.2
0.4181
0.4800
293.2
0.4032
0.5000
293.2
0.3880
0.5200
293.2
0.3726
0.5400
293.2
0.3571
0.5600
293.2
0.3414
0.5800
293.2
0.3255
0.6000
293.2
0.3096
0.6200
293.2
0.2934
0.6400
293.2
0.2772
0.6600
293.2
0.2608
0.6800
293.2
0.2444
0.7000
293.2
0.2278
0.7200
293.2
0.2111
0.7400
293.2
0.1944
0.7600
293.2
0.1775
0.7800
293.2
0.1606
0.8000
293.2
0.1436
0.8200
293.2
0.1266
0.8400
293.2
0.1094
0.8600
293.2
0.9222
0.8800
293.2
0.0750
0.9000
293.2
0.0577
0.9200
View Figure 1 for this Evaluation
Notes:
Table 54
Number of experimental points in parentheses.
References: (Click a link to see its experimental data associated with the reference)
1
Dubovskaya, A.S.; Karapetyants, M.Kh., Tr. Inst.-Mosk., Khim.-Tekhnol. Inst. Im. D. I. Mendeleeva 58, 92 (1968).
2
Mahers, E.G.; Dawe, R.A., J. Chem. Eng. Data 31, 28 (1986).
3 Shaw, D.G., ed., Solubility Data Series, Vol. 37, Hydrocarbons with Water and Seawater, Part I: Hydrocarbons C8 to C36 (Pergamon, New York, 1989).
4 Vorobeva, A.I.; Karapetyants, M., Kh., Zh. Fiz. Khim. 41, 1144 (1967).