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coiiso(jiic;ntly uf icuctiuns wliich wuri peiiectly comparable to those 

 mentioned here; for they run on the equation: 



CHa J + Na CH^ = CH, CH3 + Na J, etc. 



Said investigators had proved that in tlie process of tlie aether- 

 formation the reactionconstant increases with the diluiion. To us 

 it is evident (whicli in 1890 could not yet be the case with H., 

 C. and Br.) that we must here think of the influence of the elec- 

 trolytic dissociation increasing in proportion to the dilution, that is 

 to the increase of tlie oxalkylious ') and to write the following 

 equation : 



Clla J + Na + Ü CII3 ^ CII, U CIIs + Na J- J 

 or, the iiatriumion not taking part in the reaction 



C1J;3 J + U CII, = ClI, CII3 + J. 



The reaction studied by Mr. Sti-xjer would then be represented by 

 Co H, (NO.)^ + CII3 = Cü H, NO,. CII3 + NOo. 



JJut then it came out, remarkably enough, that in opposition to 

 the process of actherformation the constant of the last nameil reac- 

 tion was not changed by the concentration. 



The question that now naturally offered itself as a consequence 

 of this result was this. If a regular influence of the dilution, as 

 required by the electrolytic dissociationtheory does exist in the aether- 

 formation and does not exist in the substitution of the dinitroben- 

 zenes, what is then in both reactions the influence of the addition 

 of a substance with the same ion? If a sodium salt is added, the 

 increase of the concentration of the natriumions will keep back that 

 of the oxalkylions and consequently cause the reactionconstant to 

 fall. By H., C. and Br. this question had been studied cursorily 

 and unsatisfiictorily only. 



When investigating the velocity of the actherformation while 

 adding increasing quantities of Na J, it was now shown, that the 

 reactionconstant, in accordance with the iontheory, decreases in re- 



') Neither CH3 J uor CcH4(NÜ2)- eoiidiu't the electric current in alcoholic solutions. 



