98 
Solubility  of  Morphine  in  Water. 
f  Am.  Jour.  Pharm. 
t       Mar.,  1882. 
of  Roseiigarten  &  Sons,  of  this  city;  it  was  in  the  well-known  form 
of  light,  feathery  crystals,  and  was  taken  from  an  original  package, 
recently  opened. 
Experiment  I. — A  solution  was  prepared  by  digesting  sulphate  of 
morphine,  in  excess,  with  distilled  water  at  15°C.  (59°r.)  for  several 
days,  with  frequent  agitation. 
Experiment  II. — A  concentrated  hot  solution  of  the  morphine  salt 
in  water  was  allowed  to  cool  to  the  temperature  of  15°C.,  in  order  to 
ascertain  whether  under  these  circumstances  a  supersaturated  solution 
would  be  formed,  which,  hoAvever,  from  the  analytical  results,  appears 
to  be  not  the  case. 
From  the  two  solutions,  as  above  prepared,  and  filtered  from  the 
excess  of  the  salt,  with  the  proper  regulation  of  temperature,  the 
amounts  of  sulphate  of  morphine  contained  therein  was  determined 
by  the  application  of  the  method  suggested  a  few  years  ago  by  Victor 
Meyer,  by  precipitating  with  chloride  of  barium,  and,  from  the  amount 
of  ignited  sulphate  of  barium,  inversely  calculating  the  amount  of 
crystallized  sulphate  of  morphine,  (Ci7Hj9N03)2.H2S04+5H20. 
I.  10*9040  grams  of  the  cold  saturated  solution  gave  0"1396  gram 
of  sulphate  of  barium,  corresponding  to  0*4  545  gram  of  crystallized 
sulphate  of  morphine,  for 
232-8  :  758  =  0-1396  :  x.    x  =  0-4545. 
Or  expressed  in  percentage,  4*1682,  as 
10-904  :  0*4545      100  :  x.    x  =  4-1 682. 
II.  7*3250  grams  of  the  solution  of  the  salt  in  hot  water,  und  sub- 
sequently allowed  to  cool  to  15°C.,  gave  0*0946  gram  of  sulphate  of 
barium,  corresponding  to  0*3080  gram  of  crystallized  sulphate  of  mor- 
phine, for 
232*8  :  758  =  0*0946  :  x.    x  =  0*3080. 
Or  expressed  in  percentage,  4-2047,  as 
7*3250  :  0-3080  =  100  :  x.    x  =  4-2047. 
The  results  of  these  two  experiments  will  be  seen  to  agree  very 
closely,  and  if,  from  the  percentage  strength  of  the  solutions,  the 
amount  of  water  be  calculated  which  is  required  to  dissolve  one  part 
of  the  salt  at  15°C.,  the  relation  of  the  two  results,  disregarding  the 
slight  increase  of  volume  produced  by  solution,  will  be  as  follows : 
100  100 
I- »  =  23*99.    II.  4.-204-7  =  23*80. 
Another  experiment  was  made  by  preparing  a  saturated  solution  of 
