160 Report of Depaetmext of Axi:\ial Industry of the 



0.2907 gram substance gave 0.1052 gm. H2O and 0.1855 gm. CO2. 



0.1787 gram substance gave 0.0642 gm. H2O and 0.1144 gm. CO2. 



0.1816 gram substance gave 0.1331 gm, Mg2P207. 



Found I C 17.40, H 4.04, P 20.43 per ct. 

 II C 17.46, H 4.02 per ct. 



These results lead to the empirical formula Coo H56 O49 P9. 



Calculated for C20 H55 O49 P9=1358. 



C 17.67, H 4.05, P 20.54 per ct. 



This compound differs in composition from the barium salt from 

 which it was prepared by C5 Hio O5; in other words by the elements 

 of one pentose. This had probably been spHt off in the decomposition 

 of the barium salt with the dilute sulphuric acid or else by the copper 

 acetate, and if so should be found in the filtrate after the copper 

 salt of the acid had been removed. The filtrate was therefore 

 examined as follows: The copper was removed by hydrogen sul- 

 phide and the filtrate, after boiling off excess of H2S, was precipitated 

 with excess of barium hydroxide; filtered, and the barium precipi- 

 tated quantitatively with sulphuric acid and the resulting filtrate 

 evaporated to small bulk in vacuum. The solution was then found 

 to reduce Fehling's solution on boiling and ammoniacal silver nitrate 

 was also reduced. Unfortunately the substance obtained was too 

 small for any further examination. There is, however, absolutely 

 no doubt that a reducing body was present and this was most likely 

 the above mentioned pentose. 



properties of the free acid, 

 C20 H55 O49 P9. 



Dried in the desiccator it forms first a light-amber-colored thick 

 syrup which on continued drying forms a thick sticky mass. It is 

 very soluble in water and also readily soluble in alcohol from which 

 solution it is thrown out by the addition of ether as a white precipitate 

 which collects on the sides of the test tube in small oily drops. 



The aqueous solution has a strong acid reaction and a pleasant 

 sharp acid taste and it gives the following reactions: 



Magnesium acetate does not give a precipitate but the addition of 

 calcium acetate, barium chloride or alcohol causes in this solution 

 a white pr3cipitate. 



Silver nitrate does not produce any precipitate but the addition 

 of alcohol gives a white amorphous precipitate of the silver salt. 



It is not precipitated by barium or calcium chlorides but the 

 acetates of these metals and their hydroxides give white amorphous 

 precipitates which are soluble in acetic and mineral acids. 



Ferric chloride causes a white precipitate which is readily soluble 

 in dilute hydrochloric or nitric acids. 



The alkah salts are very soluble in water but in these solutions 

 salts of the alkaline earths or the heavy metals produce white 



