THE PHARMACEUTICAL JOURNAL AND TRANSACTIONS. [February 18,1871 
664 
DECOMPOSITION OF ACETATE OF 
MORPHIA IN SOLUTION.* * * § 
BY JOHN M. MAISCH. 
That aqueous solutions of the salts of most offici¬ 
nal alkaloids cannot be kept for indefinite periods is 
well known to all pharmacists. "Whether distilled 
water, or boiled and filtered hydrant water—the 
Litter containing but traces of foreign matter—be 
used for such solutions, whitish floccules usually 
make their appearance after some time, and gradually 
assume a soft gelatinous consistence, with the appear¬ 
ance of algaceous growth. In the few instances in 
which the writer assayed such altered solutions of 
the sulphates of quinia and of morphia, a diminution 
of the amount of alkaloid has not been observed, and 
the appearance of this foreign bodj r was therefore 
rather attributed to accidental organic impurities in 
1 lie water, and this belief was strengthened by the 
fact that the bulk of these fiocks varies in solutions 
made at different times, and after some time appa- 
rently does not increase, and that the presence of an 
excess of sulphuric acid prevents such a formation 
or at least diminishes its amount. 
It is also well known that a neutral solution of 
acetate of ammonia gradually deposits flocks, and 
that the liquid then assumes an alkaline reaction. 
This was first observed by Horst,f who attributes 
this decomposition of aqueous solutions of acetate 
and succinate of ammonia to the light, and recom¬ 
mends to keep them in a dark place; if ammonia 
was replaced by potash or soda, this decomposition 
did not take place. I am not aware that the amount 
of ammonia has ever been estimated in the fresh 
i ohition and after the decomposition has taken place. 
A solution of acetate of morphia is very prone to 
change; it soon acquires a brown-yellowish colour, 
and deposits a brown matter. A decomposition was 
already observed by E. Merck in 1837,'J when expe¬ 
rimenting about the best process for obtaining this 
salt dry, in a neutral condition; he states that the 
evaporation of its solution must be hastened at a 
low temperature by a current of air or other means, 
since it is decomposed at too slow an evaporation. 
But the nature of this decomposition is not stated. 
Some months ago, Dr. Wm. T. Taylor, of this city, 
informed me that lie prefers to use a solution of this 
salt for hypodermic injection, and that he had re¬ 
peatedly observed the separation in the liquid of one 
or more crystals, after keeping it on hand for some 
time.§ A careful examination of a crystal proved it 
to be pure morphia, entirely free from acetic or other 
acid; with nitric and iodic acids, and with sesqui- 
cliloride of iron, it showed the reactions characteristic 
for morphia; it had an alkaline reaction to test 
papers, and neither acetic, carbonic nor any mineral 
acid could be discovered by the appropriate tests; 
heated upon platinum foil it was consumed without 
leaving any residue. 
The liquid had deposited a considerable quantity 
ot a brown matter, and was of a pale brownish 
colour. It was neutral to test paper, but with pure 
* Read before the Philadelphia College of Pharmacy, Dec. 
20, 1870. J 
T Archiv d. Pharm. 1823. Buchner’s ‘ Repertorium,’ vol. 
xviii. p. 481. 
X Archiv d. Pharm. vol. xxiv. p. 46. Buchner’s Repert. 
vol. lxiv. p. 265. 
§ Mr. W. Martindale has already drawn attention to this 
in the Pharmaceutical Journal, 2nd series, vol. xi. p.480. 
•—Ed. Pharm. Journ. 
sesquicliloride of iron acquired a reddish tint, which 
disappeared on the addition of muriatic acid. Acidu¬ 
lated with nitric acid, iodoliydrargyrate of potassiimi 
occasioned a turbidity. Evidently a minute portion 
of acetate of morphia remained still in solution. 
To the kindness of Dr. Taylor I am indebted for 
the specimen upon the table, which was originally a 
solution of 8 grains acetate of morphia in half an 
ounce of distilled water. By accident, it had been 
set aside, and was lost sight of for several months. 
On examining it, the deposit and the change in colour 
of the solution, mentioned before, were observed, and 
a single crystal reaching from the surface of the 
liquid diagonally through the solution to the bottom 
of the vial on the opposite side. 
The gradual decomposition of acetic acid hi crude 
vinegar is well known, and it is possible that the 
changes noticed above are of the same or a similar 
nature. At any rate it is very evident that acetic 
acid, in contact with organic bodies, is very liable to 
undergo decomposition, and since an organic body 
in such a condition is apt to predispose others, with 
which it may be in direct contact, to similar changes, 
it is a question of great moment whether the addition 
of acetic acid to our officinal fluid extracts of ergot 
and of ipecacuanha may not lie more detrimental 
than useful .—American Journal of Pharmacy. 
©jajicrs fat 
CHEMICAL NOTES TO THE PHARMACOPOEIA. 
BY WILLIAM A. TILDEX, B.SC. LOND. 
DEMONSTRATOR OF PRACTICAL CHEMISTRY TO THE 
PHARMACEUTICAL SOCIETY. 
Greta Pileparata. —Chalk is a native carbonate 
of lime found in beds of considerable extent in the 
south of England. It consists almost exclusively of 
the remains of microscopic foraminiferous and other 
shells; it therefore contains numerous chemical im¬ 
purities, of which the most abundant is silica. Mag¬ 
nesia, alumina, iron and phosphates may also be 
present. Precipitated chalk, however, possesses a 
distinctly crystalline structure, and if carefully pre¬ 
pared, is chemically pure. 
Cupri Sulphas.— [§ CuS 0 4 5H 2 0. May be ob¬ 
tained by heating sulphuric acid and copper together, 
dissolving the soluble product in hot water, and 
evaporating the solution until crystallization, takes 
place on cooling.] In this process half of the sul¬ 
phuric acid is decomposed, with evolution of sul¬ 
phurous anhydride. 
Cu -f- 2H 2 S0 4 = CuS0 4 + S0 2 + 2H 2 0. 
A more economical plan, and one commonly adopted, 
consists in oxidizing the copper by heating it in a 
reverberatory furnace, before submitting it to the ac¬ 
tion of the sulphuric acid. The black oxide of copper 
thus formed dissolves easily without evolution of 
gas. 
CuO + H 2 S0 4 =: CuS0 4 + H 2 0. 
Like many other sulphates, this salt is strongly 
acid to test paper. Heated to about 390° F. it be¬ 
comes white and anhydrous; in this state it is em¬ 
ployed as a test for water in absolute alcohol. Con¬ 
tact with moisture causes it to reassume a blue colour. 
[§ The aqueous solution gives with chloride of 
barium a white precipitate (Ba S0 4 ) insoluble in by- 
