34 MORRIS LOEB 



one substance from one-fourth normal solution up to the 

 very highest dilution amenable to experiment. For different 

 acids, this constant assumes different values which have 

 proved to be closely connected with the chemical activity of 



these acids. Putting m=^ and K=-, we can note for refer- 



fr C 



ence the equation to which Ostwald now reduces his results : 



^ =K (III) 

 (l-m)F 



4. If the solution of an electrolyte really contains free 

 ions, how is it that this does not at once become apparent, 

 either by the decomposition of water, or by some physical 

 heterogeneity of the system? The answer lies in the further 

 definition that these free ions bear equal and opposite electro- 

 static charges, which do not permit any local preponderance 

 of one sort of ions over another, as this would mean a local 

 accumulation of electricity in a system which is in equi- 

 librium. Consequently although the ions travel with dif- 

 ferent velocities if they are traveling in the same direction 

 as in diffusion, the attraction of their electrostatic charges 

 compels them to accommodate their rates one to another, so 

 that the slower ion is accelerated while the faster is retarded; 

 the rate of diffusion of the salt is therefore intermediate be- 

 tween the velocities of the two ions. These conditions have 

 received a rigorous mathematical formulation, and the close 

 agreement between the theoretical and experimental results 

 affords a beautiful confirmation of the fundamental hypoth- 

 esis. (Nernst.) 



5. Any cause, on the other hand, which produces a rela- 

 tive dislocation of the positive and negative ions must occa- 

 sion electrical heterogeneity, showing itself by differences 

 of potential at different points. Upon this idea a plausible 



