On Ice and Brines 



139 



its zero-point was verified almost daily. Along with the 

 thermometer, a pipette of suitable capacity was immersed in 

 the beaker, and used with the thermometer for keeping the 

 mass well mixed. Its upper aperture was closed with a small 

 cork, which was removed from time to time to permit of 

 some of the brine being sucked up and allowed to run back 

 again. The inside of the pipette was thus kept constantly 

 moistened with the slowly altering solution in the beaker. 

 The temperature was read after very thorough mixing, and 

 the sample thereupon immediately removed and preserved 

 for analysis. 



TABLE IV. Giving the percentage of Chlorine in Sohitions of 

 various Chlorides in which Ice melts at given Temperatures. 



As a rule, samples were taken for analysis at intervals of 

 o'4 C. The results for three classes of salt in dilute solutions 

 are arranged in Tables IV, V, and VI. 



On considering them, it was at once evident that the 

 lowering of the melting-point of ice followed the concentra- 

 tion of the solution, but the law deviated in all cases from 

 that of strict proportionality to the amount of salt dissolved, 

 in some cases to a greater extent than in others. In comparing 

 the effects of different salts in solution on the melting-point 



