Chemistry and Physics. Ill 



solutions of borax and sal-ammoniac led to the suspicion that a new 

 borate of soda might be formed. 



One equivalent of chlorid of ammonium and two equivalents crystal- 

 lized borax were dissolved and boiled as long as ammonia was disen- 

 gaged. The filtered solution was evaporated very slowly — the first 

 crops of crystals were borax and the syrupy residue afforded no more 

 crystals — however by very slow evaporation and recrystallization, hard 

 milk-white shining but minute crystals were obtained. This salt con- 

 tains much water, but does not puff up so much as borax by heat. It is 

 soluble in 5 or 6 parts of water at common temperatures. The solu- 

 tion is nettral to tumeric and litmus paper. 



The formula furnished by analysis is 4B0 3 , NaO+lOHO. 



[The proportion of acid and base is the same as in the salt said 

 to be formed by combining borax with as much acid as it already 

 contains.] 



The reaction of chlorid of ammonium with borax furnishes the au- 

 thor with a very plausible theory for the formation of native boracic 

 acid. He has found that boracite and datholite have the same reaction 

 as borax. Tourmaline, axinite and other minerals however contain 

 boracic acid. In a volcanic region, sal-ammoniac is abundant, and in 

 contact with any of these minerals, free boracic acid will be produced. 

 An excess of sal-ammoniac will set free all the acid, as it does with 

 borax. The evaporation of the acid with the steam, &c, is well known ; 



hence we have all the conditions for the formation of the lagoons of 

 Tuscany. 



This theory is confirmed by the observations of Payen, that ammonia 

 was found by him in the vapors collected at Monte Rotundo in Tus- 

 cany. G. C. S. 



11. Solubility of Chlorid of Silver in Hydrochloric Acid. — M. J. 

 Pierrie states that hydrochloric acid dissolves ^foth of its weight of 

 chlorid of silver, and when diluted with twice its weight of water it 

 still retains ^th. G. C. S. 



12. Analysis of Phosphates of Manganese; by M. W. Heintz, 

 (Jour de Ph. et de Ch., Nov., 1848, in Phil. Mag.)— Phosphate of man- 

 ganese, a salt of manganese precipitated by phosphate of soda and 

 dissolved in phosphoric acid, yields, on evaporation, small prismatic 

 crystals, very soluble in water, insoluble in alcohol.— Formula P0 5 

 MnO+2H04-2HO. The water goes off between 230° and 248° F. 



Trisphosphate of manganese, obtained by precipitating sulphate of 

 manganese with phosphate of soda, is a white amorphous powder, very 

 •ittle soluble. Formula P0 5 3MnO+3HO+4HO. 4 equivs. of water 

 spelled between 230 and 248° F., the remainder by calcination. 



Ammonia-diphosphate of manganese obtained by adding gradually a 

 solution of sulphate of manganese with ammonia and sal-ammoniac, to 

 an ammoniacal solution of phosphate of soda; the viscid precipitate is 

 converted into crystalline scales. Formula P0 5 2MnO NH 3 3HO. 



Diphosphate of manganese— final permanent precipitate from acid 

 solution of sulphate— a reddish crystalline mass, but little soluble 

 ! » water, readily in acids. Formula PO,2MnOHO+HO+5HO. 

 . equivs. water expelled below 248° F., 1 at 392° and 1 by cal- 



5 



cination. 



G. 0. S. 



