Ringer conducted a laboratory study of these processes. For his experiments he took water 

 with salinity 35. 05 o/oo and freezing point -1. 91°. Already at this temperature calcium carbonate 

 precipitated out from the sea water. 



With further cooling to a temperature of -8.2°, when glauber salt began to precipitate, only 

 pure ice was formed. With a further drop in temperature, the precipitation of glauber salt was so 

 rapid that at -20°, only 0. 1 of the initial amount of sulfates remained in the solution. At -23° table 

 salt began to precipitate, at -36° magnesium chloride and potassiimi chloride. At -55°, calcium 

 chloride began to precipitate, while at lower temperatures the whole mass hardened. 



TABLE 4. RESULTS OF THE SEA-WATER FREEZING (PRO MILLE BY WEIGHT) 



Table 4, according to Ringer, shows the behavior of the ice formation process and the pre- 

 cipitation of salts in grams per 1000 grams solution with cooling of sea water (initial salinity 

 35.05 o/oo) to -30°. 



Thus, in sea water at low temperatures (below the temperature at which ice formation begins), 

 the salt composition is a function of temperature; it is constant for each given temperature, but 

 differs from that at any other temperature. 



TABLE 5. FREEZING POINT OF HIGH-SALINITY SEA WATER 



I computed the freezing point of high-salinity sea water after Hansen's formula (for the freez- 

 ing point of sea water) and Ringer's experimental data. The results are given in table 5. * 



♦Computations for lower temperatures must be considered highly unreliable. 



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