( 99 ) 
a glass scale divided into m.m. was adjusted behind the legs of the 
manometer. The error of reading amounted to less than 0,1 mm, so 
1 
to less than mm. Hg. 
4000 
The results of the research with NaCl solutions follow. 
Na Cl 
Concentration in gr. | Pu—ps | Pm …__ Pw—ps N 
mol. per 1000 gr. 11,0. in mm. He. | in m.m. He. dar Pu n 
0.05185 0.00675 0.130 Wee 
0.10735 0.01476 0.138 1.65 
0.25770 0.03650 0.141 | 170 
1. 0307 0.14626 | 0.112 1.706 
1.6075 0.23082 0.144 1.726 
From this table follows that the changed method of experimenting 
has had no influence on the course of the molecular depression of the 
vapour tension. The differences of the absolute values are due to 
the use of a new manometer, the sensibility of which was to be 
determined anew. 
As to the results obtained by another method, we have to mention, 
that Loomis and Ponsor have found that in general the molecular 
lowering of the freezing point of greater concentration to the con- 
centration of 0,1 gr. mol. decreases in case of rarefaction as well 
for electrolytes as for non-electrolytes, whereas below these concen- 
trations both investigators observed an increase of the molecular 
lowering of the freezing point, when the rarefaction increased. Mr. 
Loomis expresses his astonishment, that other investigators have not 
discovered this minimum, as this is so evident for binary chlorides, 
that it may be easily shown with an ordinary thermometer divided 
into 1/10° and with a beaker. 
Mr. R. ABeaG, who points out some inaccuracies in his criticism 
on the researches of Mr. Loomis, doubts of the results of Mr. Loomis 
and also of those of Ponsor. 
Mr. ABgeGcG@ finds for KCl between the concentrations 0.009 or. 
mol. and 0.4007 gr. mol. per 1000 gr. water a mol. lowering of the 
freezing point, increasing with the rarefaction. He has not observed 
a minimum. 
