Free Ions in Aqueous Solutions of Eleotrolytes. 245 



galvanometer was closed only while taking a deflection, and 

 this was never done while the circuit of the Daniell was closed. 



The connections were generally made as follows (fig. 2) : 



If a of the galvanometer circuit was found to be negative 

 and a' positive when beginning the observations, then A was 

 connected to the positive pole and A^ to the negative pole of 

 a Daniell. After the Daniell had been connected thus for a 

 few minutes, it was disconnected and the sign of a and a' 

 tested by closing the galvanometer circuit, a might still be 

 negative and a' positive, but by connecting up the Daniell the 

 same way and repeating this, a could always be made of the 

 same sign as A. Then keeping the circuit of the Daniell 

 open and leaving everything else as before except turning the 

 electrodes a and a' through an arc of 180°, so that they ex- 

 changed places, and after a few minutes closing the galva- 

 nometer circuit, it was found that the direction of the deflection 

 was reversed. Turning back to the first position would reverse 

 it again. This could be repeated several times without connect- 

 ing up the Daniell again. 



This woLild show that the liquid in the neighborhood of a 

 positive pole connected to a Daniell is charged with positive 

 ions, or around the negative pole is charged with negative 

 ions, or both. 



The electrodes connected to the Daniell became polarized 

 and remained so for some time. The same results were 

 obtained, however, if after disconnecting the Daniell, the 

 electrodes were discharged by short circuiting them. In this 

 case the Daniell had to be connected for a longer period to 

 obtain the same result, but this was all. 



By connecting the Daniell to the inner electrodes and the 

 galvanometer to the outer electrodes, the results were the same 

 but it took a longer time. 



This would show that tlie ions diffuse in all directions, but 

 that they are more numerous between the electrodes. 



Richarz and Lonnis* have shown, by means of the reaction 

 with titanic acid, the presence of hydrogen peroxide at the 

 cathode in dilute sulpliuric acid at electromotive forces too 

 small to produce an evolution of gas. But no hydrogen peroxide 

 was discovered at voltages below one Daniell. 



The same results as those above mentioned with one Daniell 

 were obtained in my experiments by using J, J or f the voltage 

 of a Daniell, but it took a correspondingly longer time. When 

 the electrolytic limit of decomposition was reached, the deflec- 

 tions became very large and the solution responded more 

 quickly to the influence of an electrostatic charge, but the 



*Zeitsclir. Phys. Chem., xx, 



