A study was made of the effect of P, N, T and pH on the solubilities of chlorine in concentrated sodium chloride solution.
The experimental range of P was from 0.1 to 1.0atm, N from 210 to 300g/L, T from 303 to 343°K (from 30 to 70°C), pH from 1 to 5. The results obtained of the solubilities which might be cosidered the sum of [Cl₂(aq)], [Cl₃-] and [HClO] were as follows:
The effect of pH on [HClO] is given by Eq. (5). In the range of pH less than 3, where [HClO] is found to be approximately negligible, the relation between solubilities and P is explained by Henry's law, [Eq. (10), ] and the effect of N by Eq. (11). Hence, calculation of the solubilities of unhydrolyzed chlorine in th pH range given above are made by means of the following empirical equation:
where P=0-1.0, N=200-300, and T=303-343.
This value can also be obtained graphically by employing the nomograph of Fig. 10 which is prepared from the above equation.

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Experimental studies were made on the limiting flow rate in a countercurrent liquid-1iquid extraction column equipped with stirrers.
Two types of operating regions were recognized to be caused by flow rates and stirrer speeds as shown in Fig. 3: the regular and the transition-region.
The regular-region was caused in direct proportion by higher stirrer speeds and higher flow rates of continuous phase. The maximum flow rate of dispersed phase was observed when flooding phenomena occurred.
The transition-region was caused in inverse proportion by lower stirrer speeds and lower flow rates of continuous phase. The maximum flow rate in this case was observed when inversion of two phases (from the state of oil in water to the state of water in oil) occurred.
Experimental data were correlated by plotting the dimensionless groups of (U_d/U_c) vs (U_cμ_c/σ) (NDND²ρ_c/μ_c)^0.94 (NDND²ρ_d/μ_d)^0.10 (NN²D³ρ_c/σ)^-0.53 (NN2D/g)^1.51 (Δρ/ρ_c)^-1.90 for flooding velocities, and (U_d /U_c) vs (U_cμ_c/σ) (NDND²ρ_c/μ_c)^0.97 (NN²D³ρ_c/σ)^-0.90 (NN²D/g)^0.76 (Δρ/ρ_c)^-0.60 for phase inversion velocities as shown in Fig. 9.

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In the earlier paper³⁾, the total reflux distillation by using a large-sized overflow vessel was introduced as a method of batch distillation. In the present paper, the sharpness of separation by the total reflux distllation stated above is compared with that by the usual batch reflux distillation having finite reflux ratio.
Figs. 6 & 7 thru Fig. 9 show experimental results of the total reflux distillation and those of the finite reflux ratio distillation. The results of experiments are summarized as shown in Fig. 12, where it is observed that the sharpness of separation by the total reflux distillation under the low hold up is equal to that by finite reflux ratio distillation operated under the high reflux ratio.

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Using a Rosanoff-type equilibrium still, we tried to determine the ternary equilibria of carbontetrachloride-benzene-solvent systems. The solvents used were phenol, aniline, nitrobenzene and furfural, which were chosen for the four reasons given below:
(1) They have relatively high boiling points.
(2) They are miscible with the original binary mixture.
(3) They do not make an azeotrope.
(4) Equilibrium data in connection with them and each component of the original mixture are available.
All the data obtained and the relative volatility calculated of ternary mixtures, αAB/C, are shown in Table 2. The values of αAB/C are compared with the relative volatility of the original binary mixture under the same mole fraction of the most volatile component in the ternary liquid as well as in the binary liquid. The results are shown in Fig. 1, which shows no regularity. A similar graphical representation was given of the data recalculated of those of some previous workers as shown in Fig. 2. From this figure, it may roughly be concluded that over the range of our experiments the larger the relative volatility of the original binary mixtures is, the larger that of the ternary mixtures will be, regardless of the kinds of solvents added. Similar relations were observed between αBC/A and αBC, as shown in Fig. 3.
A method for estimating ternary equilibria was obtained from the study of binary equilibria and from the two correlations of Figs. 2 & 3. The calculated values of vapor composition were compared with the observed ones as in Fig. 4, which shows a fairly good agreement.

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