( 039 ) 



3. Tlio niiiiiiumn iii / may l)o Itroii.ulil al»oul 1)y llio roruialion 

 of livdnxles in solulioii. 1 showed already ludore '), how <ii'eat the 

 inthience can he, which tiie fornialioii of hy(h-ales in solntion can 

 exert on the course of the factor /, specially with regard to not 

 very dilule solutions. 



For vei-y small concent ratious, however, the number of water 

 molecules is so predominant, that the number of molecules withdrawn 

 from the solution, ])ractically does not bring about any change in 

 the molecular concentration. Towards higher concentrations the in- 

 crease of the molecular concentration in consequence of the forma- 

 tion of hydrates augments continually, and so it may be assumed, 

 that for a certain concentration it has increased so much, that it has 

 become equal to the dimimition of the molecular concentration in 

 consequence of the retrogression of the electrolytic dissociation. If this 

 is the case, / has reached its smallest value, and will increase 

 towards higher concentration, because the intluence of the formation 

 of hydrates prevails more and more over the retrogression of the 

 electrolytic dissociation. 



Besides the abo\e mentioned formation of hydrates, we may gene- 

 rally assume auto-comi)lex-formation and hydrolysis, so that probably 

 many electrolytes form a system so intricate, that some time will 

 probably elapse before the desired insight into it will be acquired. 

 Referring here to salts of strong bases and acids I could leave hydrolysis 

 out of account. The auto-complex-formation has not been discussed, 

 because it brings about a diminution of the molecular concentration, 

 and was therefore of no use for the explanation of the phenomenon. 



4. Finally I will call attention to the very remarkable fact, that 

 solutions of Na NOg, which qualitatively behave in a very normal 

 way, do not follow the dilution law of Ostwaj.d, whereas solutions 

 of KNOg follow this law according to my measurements, and as the 

 deviations for KaN(J, solutions lie in this directi(^n that K increases 

 with the concentration as is seen in the following table, this points 

 to an intluence as e. g. occurs for NaCl solutions, but in a much 

 smaller degree ^). 



1) Archiv. Need. (2) 1 (1897). 



2) That KNO:5-solulions harmonize better with the theory than NaNO:;-solutions 

 is in accordance -willi the results of experiments made by Abegg and Bodl.'vnuer 

 (Zeitschr. f. anorg. Chem. 20, 453 (1899)), from which could be derived, that the 

 tendency to complex-formation depends on the degree of the tendency to ionisafion, 

 which latter tendency is indicated by the tendency of dissociation. The greater 

 the tendency to ionisalion the smaller the tendency to complex-formation. According 

 to WiLSMORE (Zeitschr. f. physik. Chem. 35, 318 (1900)) the tension of disso- 

 ciation is for K = 8. •20 and for Na = 2.82, from wliicli would follow, that kalium 

 salts have a slighter tendency to complex-formation than natrium salts. 



