( 168 ) 
pyridine and benzolnitriel !) and also for solutions of CdJ,, Li Cl, 
NaJ, Hg Cl and NH, CNS in acetone’). It has further appeared, 
that KJ, NaJ, KbJ, NHJ and KCNS solved in liquid 50,5), 
conduct the electric current, notwithstanding their molecular weights 
are found to be abnormally great. 
4. Chiefly on account of what has been mentioned here, KAHLENBERG 
considers the dissociation theory of ARRHENIUS as untenable. Not 
sharing this opinion, I have mentioned his principal objections to 
the dissociation theory. 
KAHLENBERG has made experiments on non-diluted solutions, and 
this is a great impediment for the refutation of the correctness of 
the dissociation. 
For according to theory the degree of dissociation found from the 
conductivity, can agree with that calculated from the lowering of 
the freezing-point, the decrease of vapour-tension and the raising of 
the boiling-point, only in case of exceedingly diluted solutions, 
In what way a deviation from the diluted state will be felt in 
general, is not known, but what I have observed for NaCl, KCl 
and H,SQ,-solutions, where minima of the molecular decrease of 
vapour-tension and raising of the boiling-point are found at + 0.5 
gr. mol. and below it, gives the conviction, that already at these 
small concentrations the deviation from the diluted state brings about 
an influence, which is so great as to even reverse the direction of 
the course of the molecular decrease of vapour-tension and the 
raising of the boiling-point. 
That this influence is in very close connection with the nature 
of the salt, follows from the fact that for NaNos, KNOs ete. no 
minimum appears even at very great concentrations, which as I 
have already mentioned, may be due to the rapid decrease of the 
electric dissociation with increase of the concentration *). | 
It has been shortly mentioned that also non-aqueous solutions make 
us acquainted with facts, which seem at first sight in opposition to 
the theory of ARRHENIUS, but to state with certainty that they are 
really so, seems premature to me. 
If for aqueous solutions we should like to have a greater quan- 
1) Werner, Zeit. Anorg. Chem. 15, 1 (189%). 
*) Durorr, Frrprrtcn, Bull. Soc. Chim. Paris. (3), 19, 334 (1898). 
3) WarpeEN, Ber. Chem. Ges. Berlin 32, 2862. (1899). 
*) Proc. Royal Acad. at Amsterdam, Vol. ILL. p. 717. (1901), 
