. 
} 
Vol. VII, No 4.] Action of Hydrazine Sulphate & Nitrites. 111 
[W.S.] 
tity of water to wash it down (about 2 c.c), the maximum 
amount of gas was obtained, and the proportion of nitrous 
oxide to nitrogen was found to be no longer 1:1, but approxi- 
mately 2: 1; in fact, on the assumption that the deficit in the 
amount of gas was due to nitrous oxide dissolved in the water 
employed, and applying the usual corrections for the solubility 
of nitrous oxide in water at the temperature of the experiment 
(32°C), the proportion of N,O: N, was found to be exactly 2: 1. 
The ordinary decomposition of the di-acid hydrazine 
nitrite, ecataing the hydrogen ree theory, would seem to 
proceed along the following lines :— 
NH, ON.OH N: N.OH 
oa > >——> | (hypothetical) 3% ——> N,+N.O 
NH, ON.OH N: N.OH 
This equation, though quite analogous to the equation 
representing the reaction between hydroxylamine and nitrous 
N--OH 
l 
acid giving rise to hyponitrous acid N—OH, fails to explain 
the gasometric relations between nitrous oxide and nitrogen 
actually observed. The fact should not be lost sight of, that 
the experiment was conducted with excess of the Hydrazine 
salt, and consequently, the formation of the monacid hydrazine 
nitrite is only too possible, which would decompose thus 
NH, 
| - +NO.OH = NH, + N,O + HO. 
NH 
2 
Taking the two equations together, we find that the pro- 
portion of nitrous oxide to nitrogen actually observed, exactly 
agrees with that demanded by the above equations conjointly. 
As, according to the above equations, ammonia e of 
products of reaction, it must have remained in solution as the 
sulphate. That ammonia is really formed, was demonstrated 
beyond doubt by treating the solution remaining after the 
reaction, with eaaes yee when a strong smell of ammonia 
was perceived. As will be shown subsequently, the quanti- 
tative determination or the ammonia formed is useless, in so far 
as the determination of the ratio of the nitrogen evolved to the 
total nitritic nitrogen of Barium nitrite, would be a better 
evidence and check as to the reactions actually occurring. It 
is important to note here, that the above statements have been 
found to be true not only of Barium nitrite, but also of the 
nitrites of the alkalis, the alkaline-earth metals, of those of the 
heavy metals, etc., and in fact of nitrites in general. In sup- 
port of what has preceded, the actual data of a few of the 
numerous experiments done are given below :-— 
