INDUSTRIAL AND ENGINEERING CHEMISTRY
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curve, concentration values are then taken which correspond to the measured optical densities: optical density where T = transmission, yo
5
log (loo/")
Vol. 37, No. 6
sorbed per 10 g r a m of cement and the equilibrium concentrations of calcium lignosulfonate (values in column 6 w. values in column 4). ACKNOWLEDGMENT
In eecuring the calibration curve, it is necesssary to measure the optical densities of a series of solutions of known calcium lignosulfonate content, which have been individually adjusted to approximately the same pH as the acidified equilibrium solutions. The calibration curve is then a graphic relation between observed o p t i d densitiea and known cdciumIignosulfonate concentrations. A typical set of Oement-calcium lignosulfonate adsorption data is shown in Table 11, where different concentrations of calcium lignosulfonate solutiona were used with a normal portland cement. The equilibrium solution concentration values in column 3 are plotted against the valuea in column 1, and the best curve is drawn through the points. Equilibrium concentration daluea are then taken from the curve and are shown in column 4. The adsorption in grams of lignosulfonate per 10 grams of cement ia calculated by subtracting the equilibrium solution concentration obtained from the curve from the initial concentration and multiplying by 1.5 (column 6). The adsorption isotherm (Figure 1) represents the relation between the grams of lignosulfonate ad-
The authora wish to express appreciation to the Master Buildem Company whom sponsorahip of an Ohio State University Research Foundation Fellowship made this work possible. The authore also wish to thank Donald R. MacPherson for his Bssistancc in securing the data in Table I. LITERATURE CITED
(1) DUUMM,W. M., Proe. Am. Soo. Tcsting Materiala, 39, 866-430
(1939).
Forbrich. L. R., J. Am. ConcrstoInat., 37, 181-84 (1940). (3) Mark,J. G.(to Dewey & Almy Chern. Co.), U. S. Patent 2,141,(2)
670 (Dec. 27, 1938). (4) Scripture, E. W., Jr., Eng. Nawa-Rscord, 127, 81-4 (1941). (6) Scripture, E. W., Jr., Master Builders Co., Rssurreh Papers, 35-40 (194142). (6) Scripture, E. W., Jr., U. 8.Patenta 2,081,642-3 (May 26, 1937); (to Mester Buildere Co.) 2,127,461 (Aug. 18, 1938) and 2,169,980 (Aug. IS, 1989); (to Dewey & Aimy Chem. Co.), 2,229,311 (Jan. 21,1941). (7) Wagner, L. A., Proo. Am. Soe. Tssting Materials., 33, 11, 6.53-70 (1933).
Molecular Refraction-Viscosity R. T. LAGEMANN Constant Nomograph S
Emory Univeraity, Emory University, Georgia
OUDEW (8)showed that for organic liquids there exists a viscosity-cmstitutiond constant Z which is defined as
Z = where
log^ loglo + 2.9) 9
-
= viscosity, millipoises; d density, grams per 00.; M = molecular weight 9
Values of 9 aud d are taken at thesametemperature. Recently (9) it was pointed out that Soudere' I is a linear function of the molecular refraction, R, which is defined aa ns-1 M R - -n * + 2 T where 9, the refractive index, and d must be measured under the same conditione. Thus it is possible to determine the viscosity of a liquid from ita refractive index which is easy to measure and for which a large amount of data is available. The nomograph ahown by Figure 1 providea a convenient way for estimating Souders' Z from the mole refraction. By aligning the mole refraction value with the series number of the compound, the corresponding value of I may be read from the right-hand scale. When values of the viscosity and the refractive index are to be connected with values of Z and R, respectively, use may be made of two nomographs designed by Davis (1). LITERATURE CITED
(1) Davis, D.S.,IND. ENQ.CREM.,33, 1537 (1941); 34,258(1942). (2) Lagemann, R. T.,J. An. Chem. Soc., 67, 498 (1945). (3) Seuders, M.,Zbid., 60,154 (1938).
IO - l
E
700
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I-Monohydric olcoholr 2-Monocarboxylic aclda, 3Estrro o f acetic acid 4-Ali hatlc ketone8
w&t
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6.Poraffinr 7-Alkyl iodide8
60
Figure 1. Molecular Refraction-Viscosity Constant Nomograph
