DIVISION I.
EXPERIMENTS and OBSERVATIONS on the COMBINATIONS of NITROUS OXIDE.
I. Combination of Water with Nitrous Oxide.
a. The discoverer of nitrous oxide first observed its solubility in water; and it has since been noticed by different experimentalists.
Dr. Priestley found that water dissolved about one half of its bulk of nitrous oxide, and that at the temperature of ebullition, this substance was incapable of remaining in combination with it.[153]
b. I introduced to 9 cubic inches of pure water, i. e. water distilled under mercury, 7 cubic inches of nitrous oxide, which had been obtained over mercury, from the decomposition of nitrate of ammoniac, and in consequence was perfectly pure. After they had remained together for 11 hours, temperature being 46°, during which time they were frequently agitated, the gas remaining was 2,3; consequently 4,7 cubic inches had been absorbed. And then, 100 cubic inches, = 25300 grains of water, will absorb 54 cubic inches, = 27 grains, of nitrous oxide.
c. The taste of water impregnated with nitrous oxide, is distinctly sweetish; it is softer than common water, and, in my opinion, much more agreeable to the palate. It produces no alteration in vegetable blues, and effects no change of color in metallic solutions.
d. Thinking that water impregnated with nitrous oxide might probably produce some effects when taken into the stomach, by giving out its gas, I drank, in June, 1799, about 3 ounces of it, but without perceiving any effects.
A few days ago, considering this quantity as inadequate, I took at two draughts nearly a pint, fully saturated; and at this time Mr. Joseph Priestley drank the same quantity.
We neither of us perceived any remarkable effects.
Since that time I have drank near three pints of it in the course of a day. In this instance it appeared to act as a diuretic, and I imagined that it expedited digestion. As a matter of taste, I should always prefer it to common water.
e. Two cubic inches of pure water, that had been made to absorb about 1,1 cubic inches of nitrous oxide; when kept for some time in ebullition, and then rapidly cooled, produced nearly 1 of gas. Sulphur burnt in this gas with a vivid rose-colored flame.
In another experiment, in which the gas was expelled by heat from impregnated water, and absorbed again after much agitation on cooling; the residuum was hardly perceptible, and most likely depended upon some gas which had adhered to the mercury, and was liberated during the ebullition. Hence it appears that nitrous oxide is expelled unaltered from its aqueous solution by heat.
f. I have before mentioned, [Division III], that nitrous oxide, during its combination with spring water, expels the common air dissolved in it. This common air generally amounts to one sixteenth, the volume of the water being unity. A correction on account of this circumstance must be made for the apparent deficiency of diminution, and for the common air mingled in consequence, with nitrous oxide during its absorption by common water.
g. Water impregnated with nitrous gas absorbed nitrous oxide; but the residual gas was much greater than that of common water, and gave red fumes with atmospheric air. Nitrous gas agitated for a long while over water highly impregnated with nitrous oxide, was not in the slightest degree diminished, in one experiment indeed it was rather increased; doubtless from the liberation of some nitrous oxide from the water by the agitation.
h. Nitrous oxide kept in contact with aqueous solution of sulphurated hydrogene and often agitated, was not in the slightest degree diminished.
Sulphurated hydrogene, introduced into a solution of nitrous oxide, was rapidly absorbed, and as the process advanced, the nitrous oxide was given out.
i. Water impregnated with carbonic acid, possessed no action upon nitrous oxide, and did not in the slightest degree absorb it. When carbonic acid was introduced to an aqueous solution of nitrous oxide; the aëriform acid was absorbed, and the nitrous oxide liberated.
k. From these observations it appears that nitrous oxide has less affinity for water, than even the weaker acids, sulphurated hydrogene and carbonic acid; as indeed one might have conjectured a priori from its degree of solubility: likewise that it has a stronger attraction for water than the gases not possessed of acid or alkaline properties; it expelling from water nitrous gas, oxygene, and common air; probably hydrocarbonate, hydrogene, and nitrogene.
II. Combinations of Nitrous Oxide with
Fluid Inflammable Bodies.
a. Vitriolic ether absorbs nitrous oxide in much larger quantities than water.
A cubic inch of ether, at temperature 52°, combined with a cubic inch and seven tenths of nitrous oxide.
Ether thus impregnated was not at all altered in its appearance; its smell was precisely the same, but the taste appeared less pungent, and more agreeable. Nitrous oxide is liberated unaltered from ether at a very low temperature, that is, at about the boiling point of this fluid.
For expelling nitrous oxide from impregnated ether, and for ascertaining in general the quantity of gases combined with fluids, I have lately made use of a very simple method, which it may not be amiss to describe.
The impregnated fluid is introduced into a small thin tube, graduated to,05 cubic inches, through mercury. The quantity of fluid should never equal more than a fifth or sixth of the capacity of the tube.
The lower part of the tube is adapted to an orifice in the shelf of the mercurial apparatus, so as to make an angle of about 40° with the surface of the mercury.
The flame of a small spirit lamp is then applied to that part of the tube containing the fluid; and after the expulsion of the gas from it, the heat is raised so as to drive out the fluid through the orifice of the tube. Thus the liberated gas is preserved in a state proper for accurate examination.
Impregnated ether, during its combination with water, gives out the greater part of its nitrous oxide. During the liberation of nitrous oxide from ether, by its combination with water, a very curious phænomenon takes place.
If the water employed is colored, so that it may be seen in a stratum distinct from the impregnated ether, at the point of contact a number of small spherules of fluid will be perceived, apparently repulsive both to water and ether; these spherules become gradually covered with minute globules of gas, and as this gas is liberated from their surfaces, they gradually disappear.
b. Alcohol dissolves considerable quantities of nitrous oxide.
2 cubic inches of alcohol, at 52°, combined with 2,4 cubic inches of nitrous oxide. The alcohol thus impregnated had a taste rather sweeter than before, but in other physical properties was not perceptibly altered.
Nitrous oxide is incapable of remaining in combination with this fluid at the temperature of ebullition; it is liberated from it unaltered by heat.
Impregnated alcohol, during its combination with water, gives out the greater part of its combined nitrous oxide: on mingling the two fluids together, at the point of contact the alcohol becomes covered with an infinite number of small globules of gas, which continue to be generated during the whole of the combination, and in passing through the fluid render it almost opaque.
c. The essential oils absorb nitrous oxide to a greater extent than either alcohol or ether.
,5 cubic inches of oil of carui combined with 1,2 cubic inches of nitrous oxide at 51°. The color of the oil thus impregnated was rather paler than before.
Nitrous oxide is expelled unaltered from impregnated oil of carui, by heat.
1 of oil of turpentine absorbed nearly 2 of nitrous oxide, at 57°. Its properties were not sensibly altered from this combination, and the gas was expelled from it undecompounded, by heat.
d. As well as the essential oils, the fixed oils dissolve nitrous oxide at low temperatures, whilst at high temperatures they do not remain in combination.
1 of olive oil absorbed, at 61°, 1,2 of nitrous oxide, but without undergoing any apparent physical change.
III. Action of Fluid Acids on Nitrous Oxide.
a. Nitrous oxide exposed to concentrated sulphuric acid, undergoes no change, and suffers no diminution, that may not be accounted for from the abstraction of a portion of its water by the acid.
b. Nitrous oxide is scarcely at all soluble in nitrous acid, and exposed to that substance, undergoes no alteration.
c. Muriatic acid, of specific gravity 1,14 absorbs about a third of its bulk of nitrous oxide. It suffers no apparent change in its properties from being thus impregnated, and the gas is again given out from it on the application of heat.
d. Acetic acid absorbs nearly one third of its bulk of nitrous oxide.
e. Aqua regia, that is, the nitro-muriatic acid, absorbs a very minute portion of nitrous oxide.
f. Nitrous oxide was exposed to a new compound acid, consisting of oxygenated muriatic acid, and sulphuric acid, which I discovered in July, 1799, and of which an account will be shortly published; but it was neither absorbed or altered.
I have before mentioned that the aqueous solutions of sulphurated hydrogene and carbonic acid, neither dissolve or alter nitrous oxide.
IV. Action of Saline Solutions, and other Substances,
on Nitrous Oxide.
a. Nitrous oxide exposed to concentrated solution of green sulphate of iron, at 58°, underwent no perceptible diminution; not even after it had been suffered to remain in contact with it for half an hour.
b. It underwent diminution of nearly,2 when agitated in contact with a solution of red sulphate of iron, the volume of the solution being unity.
c. Solution of green sulphate of iron, fully impregnated with nitrous gas, did not in the slightest degree absorb nitrous oxide, and appeared to have no action upon it.
d. Solution of green muriate of iron, whether impregnated with nitrous gas, or unimpregnated, has no affinity for, or action upon, nitrous oxide.
e. Solution of red muriate of iron in alcohol, absorbed nearly one fifth of its bulk, of nitrous oxide.
f. Solution of prussiate of potash absorbed nearly one third of its volume, of nitrous oxide, which was again expelled from it by heat.
g. Solution of nitrate of copper appeared to have no affinity for nitrous oxide.
h. Concentrated solution of nitrate of ammoniac, at 58°, absorbed one eighth of its bulk of nitrous oxide.
i. Solutions of alkaline sulphures absorb nitrous oxide in quantities proportionable to the water they contain; it is expelled from them unaltered by heat. None of the hydro-sulphures dissolve more than half their bulk of nitrous oxide.
k. Concentrated solutions of the sulphites possess little or no action on nitrous oxide; diluted solutions absorb it in small quantities.
l. Concentrated solution of muriate of tin absorbs about one eighth of nitrous oxide; more dilute solutions absorb larger quantities.
From these observations we learn, that neutro-saline solutions in general, have very feeble attractions for nitrous oxide; and as solutions of green muriate, and sulphate of iron, whether free from nitrous gas, or impregnated with it, possess no action upon nitrous oxide, nitrous gas may be separated from this substance by those solutions with greater facility than nitrous oxide can be separated from nitrous gas, by water or alcohol.
Charcoal absorbs nitrous oxide as well as all other gases; and it is disengaged from it by heat.
I have as yet found no other solid body, not possessed of alkaline properties, capable of absorbing nitrous oxide in any state of existence.
The bodies possessing the strongest affinity for oxygene, the dry sulphites, muriate of tin, the common sulphures, white prussiate of potash, and green oxide of iron, do not in the slightest degree act on nitrous oxide at common temperatures.
V. Action of different Gases on Nitrous Oxide.
a. 12 measures of muriatic acid gas were mingled with 7 measures of nitrous oxide at 56°. After remaining together for a minute, they filled a space equal to 19½ measures. When water was introduced to them, the muriatic acid was absorbed much more slowly than if it had been unmingled.
In another experiment, when the gases were saturated with water, 9 measures of each of them, when mingled and suffered to remain in contact for a quarter of an hour, filled a space nearly equal to 19; and after the muriatic acid had been absorbed by potash, the nitrous oxide remained unaltered in its properties.
From the expansion, it appears most probable that aëriform muriatic acid, and nitrous oxide, have a certain affinity for each other, and that they combine when mingled together; for in the last experiment, the increase of volume cannot be accounted for by supposing that nitrous oxide undergoes less change of volume than muriatic acid, by aëriform combination with water, and that the expansion depended upon the solution of some of its combined water by the muriatic acid. That muriatic acid and nitrous oxide have a slight affinity for each other, likewise appears from the absorption of nitrous oxide by aqueous solution of muriatic acid.
Thinking that nitrous oxide might attract muriatic acid from its solution in water, I exposed a minute quantity of fluid muriatic acid to nitrous oxide; but no alteration of volume took place in the gas.
b. 6 measures of nitrous oxide were mingled with 11 measures of sulphureous acid, saturated with water; after remaining at rest for six minutes, they filled a space nearly equal to 18 measures. Exposed to water, the sulphureous acid was absorbed, but not nearly so rapidly as when in a free state. Sulphur burnt with a vivid flame in the residual nitrous oxide. 7 measures of sulphureous acid were now mingled with 8 of nitrous oxide. They filled a space nearly equal to 15¾, and no farther expansion took place afterwards.
From these experiments it appears probable that sulphureous acid, and nitrous oxide, have some affinity for each other.
c. 11 measures of carbonic acid were mingled with 8 of nitrous oxide; they filled a space nearly equal to 19 measures. On exposing the mixture to caustic potash, the carbonic acid was absorbed, and the nitrous oxide remained pure. Hence it appears that carbonic acid and nitrous oxide do not combine with each other.
d. Oxygenated muriatic acid, and nitrous oxide, were mingled in a water apparatus: there was a slight appearance of condensation; but this was most probably owing to absorption by the water; on agitation, the oxygenated muriatic acid was absorbed, and the greater part of the nitrous oxide remained unaltered.
e. Sulphurated hydrogene and nitrous oxide, mingled together, neither expanded or contracted; exposed to solution of potash, the acid[154] only was absorbed.
f. 10 measures of nitrous gas were admitted to 12 of nitrous oxide at 59°. They filled a space equal to 22, and after remaining together for an hour, had undergone no change. Solution of muriate of iron absorbed the nitrous gas without affecting the nitrous oxide.
g. Nitrous oxide was successively mingled with oxygene, atmospheric air, hydrocarbonate, phosphorated hydrogene, hydrogene, and nitrogene, at 57°; it appeared to possess no action on any of them, and was separated by water, the gases remaining unaltered.
h. As nitrous oxide was soluble in ether, alcohol, and the other inflammable fluids, it was reasonable to suppose that its affinity for those bodies would enable them to unite with it in the aëriform state. At the suggestion of Dr. Beddoes I made the following experiment:
To 12 measures of nitrous oxide, at 54°, I introduced a single drop of ether; the gas immediately began to expand, and in four minutes filled a space equal to sixteen measures and a quarter. When an inflamed taper was plunged into the gas thus holding ether in solution, a light blue flame slowly passed through it.
A considerable diminution of temperature is most probably produced, from the great expansion of nitrous oxide during its combination with ether.
A drop of alcohol was admitted to 14 measures of nitrous oxide. In five minutes, the gas filled a space equal to fifteen and a third; but no farther diminution took place afterwards.
A minute quantity of oil of turpentine was introduced to 14 measures of nitrous oxide; it filled, in 4 minutes, a space rather less than 14; and no farther change took place afterwards. Most likely this contraction arose from the precipitation of the water dissolved in the gas by the stronger affinity of the oil for nitrous oxide. To ascertain with certainty if any oil had been dissolved by the gas, I introduced into it a small quantity of ammoniac. It immediately became slightly clouded, most probably from the formation of soap, by the combination of the dissolved oil with the ammoniac.
From these experiments we learn, that when nitrous oxide is mingled with either carbonic acid, oxygene, common air, hydrocarbonate, sulphurated hydrogene, hydrogene, or nitrogene, they may be separated from each other without making any allowance for contraction or expansion; but if a mixture of either muriatic acid, or sulphureous acid gas, with nitrous oxide, is experimented upon; in the absorption of the acid by alkalies, the apparent volume of gas condensed will be less than the real one, by a quantity equal to the sum of expansion from combination. Consequently a correction must be made on account of this circumstance.
Though alcohol, ether, essential oils, and the fluid inflammable bodies in general, dissolve nitrous oxide with much greater rapidity than water, yet as we are not perfectly acquainted with their action on unabsorbable gases, it is better to employ water for separating nitrous oxide from these substances; particularly as that fluid is more or less combined with all gases, and as we are acquainted with the extent of its action upon them.
By pursuing the subject of the solution of essential oils in gases, we may probably discover a mode of obtaining them in a state of absolute dryness. For if other gases as well as nitrous oxide, have a stronger affinity for oils than for water, water most probably will be precipitated from them during their solution of oils; and after their saturation with oil, it is likely that they are capable of being deprived of that substance by ammoniac.
VI. Action of aëriform Nitrous Oxide in the Alkalies.
History of the discovery of the combinations
of Nitrous Oxide with the Alkalies.
a. When nitrous oxide in a free state is exposed to the solid caustic alkalies and alkaline earths, at common temperatures, it is neither absorbed nor acted upon; when it is placed in contact with solutions of them in water, a small quantity is dissolved; but this combination appears to depend on the water of the solution, for the gas can be expelled unaltered, at the temperature of ebullition.
b. Caustic potash was exposed to nitrous oxide for 13 hours: the diminution was not to one fiftieth, and this slight condensation most probably depended upon its combination with the water of the gas.
Concentrated solution of potash absorbed a fourth of its bulk of nitrous oxide. When the impregnated solution was heated, globules of gas were given out from it rapidly; but the quantity collected was too small to examine.
Soda, whether solid or in solution, exhibited exactly the same phænomena with nitrous oxide. The solution of soda absorbed near a quarter of its bulk of gas.
c. 11 measures of ammoniacal gas were mingled with 8 measures of nitrous oxide over dry mercury, both of the gases being saturated with water. No change of appearance was produced by the mixture, and they filled, after two minutes, a space equal to 19. On the introduction of a little water, the ammoniac was absorbed, and the nitrous oxide remained unaltered, for it was dissolved by water as rapidly as if it had never been mingled with ammoniac.[155]
7 measures of nitrous oxide, exposed to 6 measures of solution of ammoniac in water, was in an hour diminished to 4½ nearly. When the solution was heated over mercury, permanent gas was produced, which was unabsorbable by a minute quantity of water, and soluble in a large quantity; consequently it was nitrous oxide.
d. Nitrous oxide was exposed to dry caustic strontian; it underwent a diminution of nearly one fortieth, which most likely was owing to the combination of the strontian with its water.
11 measures of nitrous oxide were agitated in contact with 8 of strontian lime water: nearly 4 measures were absorbed. The impregnated solution exposed to heat, rapidly gave out its gas; 3 measures were soon collected, which mingled with a small quantity of hydrogene, and inflamed by the taper, gave a smart detonation.
e. Nitrous oxide exposed to lime and argil, both wet and dry, was not in the slightest degree acted upon.
From these experiments it is evident that nitrous oxide in the aëriform state cannot be combined either with the alkalies, or the alkaline earths. That a combination may be effected between nitrous oxide and these substances, it must be presented to them, in the nascent state.
The salts composed of the alkalies and nitrous oxide, are not analogous to any other compound substances, being possessed of very singular properties. Before these properties are detailed, it may not be amiss to give an account of the accidental way in which I discovered the mode of combination.
In December, 1799, designing to make a very delicate experiment, with a view to ascertain if any water was decomposed during the conversion of nitrous gas into nitrous oxide, by sulphite of potash, I exposed 200 grains of crystalised sulphite of potash, containing great superabundance of alkali, to 14 cubic inches of nitrous gas, containing one eighteenth nitrogene. The alkali was employed to preserve any ammoniac that might be formed, in the free state, as it would otherwise combine with sulphureous acid.[156]
The volume of gas diminished with great rapidity; in two hours and ten minutes it was reduced to 6⁴/₅, which I considered as the limit of diminution. Accidentally, however, suffering it to remain for three hours longer, I was much surprised by finding that not quite 2 cubic inches remained, which consisted of nitrous oxide, mingled with the nitrogene that existed before the experiment.
In accounting theoretically for this phænomenon, different suppositions necessarily presented themselves.
1st, It was possible, that though sulphite of potash, and potash, separately possessed no action on free nitrous oxide, yet in combination they might exert such affinities upon it as either to absorb it, or make it enter into new combinations.
2dly. It was more probable that the caustic potash, though incapable of condensing aëriform nitrous oxide, was yet possessed of a strong affinity for it when in the nascent state, and that the nitrous oxide condensed in the experiment had been combined in this state with the free alkali.
To ascertain if the compound of potash and sulphite of potash with sulphate, was capable of acting upon nitrous oxide, I suffered a quantity of this substance to remain in contact with the gas for near a day: no change whatever took place.
To determine whether the diminution of nitrous oxide depended upon its absorption in the nascent state, by the peculiar compound of potash and sulphite of potash, or if it was simply owing to the alkali.
I mingled a solution of sulphite of potash with caustic soda; the salt, after being evaporated at a low temperature, was exposed to nitrous gas. The nitrous oxide formed was absorbed, but in rather less quantities than when alkaline sulphite of potash was employed.
Hence it was evident that the alkali was the agent that had condensed the nitrous oxide in those experiments, for soda is incapable of combining either with sulphate, or sulphite of potash.
To ascertain whether any change in the constitution of the nitrous oxide had been produced by the condensation, I introduced a small quantity of sulphite of potash, with excess of alkali, that had absorbed nitrous oxide, into a long and thin cylindrical tube filled with mercury; and inclining it at an angle of 35° with the plane of the mercury, applied the heat of a spirit lamp to that part of the tube containing the salts; when the glass became very hot, gas was given out with rapidity; in less than a minute the tube was full. This gas was transfered into another tube, and examined; it proved to be nitrous oxide in its highest state of purity;[157] for a portion of it absorbed by common water, left no more than a residuum of ¹/₁₅, and sulphur burnt in it with a vivid rose-colored flame.
Being now satisfied that the alkalies were capable of combining with nitrous oxide; to investigate with precision the nature of these new compounds, I proceeded in the following manner.
VII. Combination of Nitrous Oxide with Potash.
a. Into a solution of sulphite of potash, which had been made by passing sulphureous acid gas from a mercurial airholder into caustic potash dissolved in water, I introduced 17 grains of dry potash. The whole evaporated at a low temperature, gave 143 grains of salt. This salt was not wholly composed of sulphite of potash and potash; it contained as well, a minute quantity of carbonate, and sulphate of potash, formed during the evaporation.[158]
120 grains of it finely pulverised, and retaining the water of crystalisation, were exposed to 15 cubic inches of nitrous gas, over mercury. The nitrous gas diminished with great rapidity, and in three hours a cubic inch and nine tenths only remained, which consisted of nearly one third nitrous oxide, and two thirds nitrogene that had pre-existed in the nitrous gas. The increase of weight of the salt could not be determined, as some of it was lost by adhering to the vessel in which the combination was effected, and to the mercury. It presented no distinct series of crystalisations, even when examined by the magnifier; rendered green vegetable blues, and its taste was very different from that of the remaining quantity of salt that had been exposed to the atmosphere. A portion of it strongly heated over mercury, gave out gas with great rapidity, which had all the properties of the purest nitrous oxide.
When water was poured upon some of it, no gas was given out, and the whole was equably and gradually dissolved. Alcohol, as well as ether, appeared incapable of dissolving any part of it.
When muriatic acid was introduced into it, confined by mercury, a rapid effervescence took place. Part of the gas disengaged was sulphureous acid, and carbonic acid; the remainder was nitrous oxide.
b. I made a number of experiments upon salts procured in the manner I have just described, with a view to obtain the compound of nitrous oxide and potash, free from admixture of other salts.
When the mixed salt was boiled in alcohol or ether, no part of it appeared to be dissolved. Finding that little or no gas was given out during the ebullition of concentrated solutions of the mixed salts, I attempted to separate the sulphate, sulphite, and carbonate of potash, from the combination of nitrous oxide and potash, by successive evaporations and crystalisations. But though in this way it was nearly freed from sulphate of potash, yet the extreme and nearly equal solubility of the other salts, prevented me from completely separating them from each other.
By exposing, however, very finely pulverised sulphite of potash, mingled with alkali, for a great length of time to nitrous gas, it was almost wholly converted into sulphate; and after the separation of this solution, evaporation, and crystalisation, at a low temperature, I obtained the new combination, mingled with very little carbonate of potash, and still less of sulphite.
The minute quantity of sulphite chiefly appeared in very small crystals; distinct from the mass of salt, which possessed no regular crystalisation, and was almost wholly composed of the new compound, intimated mingled with a little carbonate. The new compound, as nearly as I could estimate from the quantity of nitrous oxide absorbed, consisted of about 3 alkali, to 1 of nitrous oxide, by weight.
It exhibited the following properties:
1. Its taste was caustic, and possessed of a pungency different from either potash or carbonate of potash.
2. It rendered vegetable blues green, which might possibly depend upon the carbonate of potash mixed with it.
3. Pulverised charcoal mingled with a few grains of it, and inflamed, burnt with flight scintillations. Projected into zinc in a state of fusion, a slight inflammation was produced.
4. When either sulphuric, muriatic, or nitric acid was introduced to it under mercury, it gave out nitrous oxide, mingled with a little carbonic acid.
5. Thrown into a solution of sulphurated hydrogene, gas was disengaged from it, but in quantities too minute to be examined.
6. When carbonic acid was thrown into a solution of it in water, gas was disengaged; on examination it proved to be nitrous oxide.
7. A concentrated solution of it kept in ebullition in a cylinder, confined by mercury, gave out a few globules of gas, which were too minute to be examined, and probably consisted of common air previously contained in the water.
c. In the experiments made to ascertain these properties all the salt was expended, otherwise I should have endeavoured to ascertain what quantity of gas would have been liberated by heat from a given weight; and likewise what would have been the effects of admixture of it with oil. When some of the mixed salt was mingled with oil of turpentine, part of it was dissolved, and the fluid became white; but no gas was given out. On this coarse experiment, however, I cannot place much dependance. If the combination of nitrous oxide and potash is capable of combining with oil without decomposition, barytes and strontian[159] will probably separate the oil from it, and thus it may possibly be obtained in a state of purity.
In a rough experiment made on the conversion of nitrous gas into nitrous oxide, by concentrated solution of sulphite of potash with excess of alkali, very little of the nitrous oxide was absorbed. Hence it is probable that water lessens the affinity of potash for nascent nitrous oxide.
VIII. Combination of Nitrous Oxide with Soda.
The union of nitrous oxide with soda is effected in the same manner as with potash. The alkali, mingled by solution and evaporation, with either sulphite of soda, or of potash, is exposed to nitrous gas; the nitrous oxide is condensed by it at the moment of generation, and the combination effected.
As far as I have been able to observe, nitrous oxide is not absorbed to so great an extent by soda, as potash.
I have not yet been able to obtain the combination of nitrous oxide with soda in its pure state. To the attainment of this end, difficulties identical with those noticed in the last section present themselves. It is extremely difficult to procure the soda perfectly free from carbonic acid, and though by using sulphite of potash the sulphate formed is easily separated, yet still evaporation and crystalisation will not disengage the sulphite and carbonate from the new compound.
The compound of soda and nitrous oxide, mingled with a little sulphite and carbonate of soda, was rapidly soluble, both in warm and cold water, without effervescence. Its solution, heated to ebullition, gave out no gas. The taste of the solid salt was caustic, and more acrid than that of the mixture of carbonate and sulphite of soda. When cast upon zinc in fusion, it burnt with a white flame. When heated to 400° or 500°, it gave out nitrous oxide with rapidity. Nitrous oxide was expelled from it by the sulphuric, muriatic, and carbonic acids, I believe, by sulphurated hydrogene.[160]
IX. Combination of Nitrous Oxide with Ammoniac.
I attempted to effect this combination by converting nitrous gas into nitrous oxide, by sulphite of ammoniac, wetted with strong solution of caustic ammoniac; but without success; for the whole of the nitrous oxide produced remained in a free state.
When I exposed sulphite of potash, mingled by solution and evaporation with highly alkaline carbonate of ammoniac,[161] to nitrous gas, the diminution was nearly one fourth more than if pure sulphite of potash had been employed. Hence it appears most likely that ammoniac is capable of combination with nitrous oxide in the nascent state.
In the experiments on the conversion of nitrous gas into nitrous oxide, by nascent hydrogene, and by sulphurated hydrogene, [Res. I. Divis. V]. probably the water formed at the same time with the ammoniac and nitrous oxide, prevented them from entering into combination; possibly the peculiar compound was formed, but in quantities so minute as not to be distinguished from simple ammoniac;[162] for even the existence of ammoniac in these processes, is but barely perceptible.
If it should be proved by future experiments, that in the decomposition of nitrous gas by nascent hydrogene, a peculiar compound of nitrous oxide, water and ammoniac, is formed, it will afford proofs in favor of the doctrine of predisposing affinity;[163] for then this decomposition might be supposed to depend upon the disposition of oxygene, hydrogene and nitrogene to assume the states of combination in which they might form a triple compound, of water, nitrous oxide, and ammoniac.
Nitrous oxide might probably be made to combine with ammoniac by exposing a mixture of nitrous gas and aëriform ammoniac, to the sulphites.
It is probable that nitrous oxide may be combined with ammoniac, by means of double affinity. Perhaps sulphate of ammoniac and the combination of potash with nitrous oxide mingled together in solution, would be converted into sulphate of potash and the compound of nitrous oxide, and ammoniac.
X. Probability of forming Compounds of Nitrous Oxide
and the Alkaline Earths.
I attempted to combine nitrous oxide with lime and strontian, by exposing sulphites of lime and strontian with excess of earth, to nitrous gas; but this process did not succeed: the diminution took place so slowly as to destroy all hopes of gaining any results in a definite time. Sulphite of potash is decomposable by barytes, strontian, and lime;[164] consequently it was impossible to employ this substance to effect the combination.
As the dry sulphures, when well made, convert nitrous gas into nitrous oxide, it is probable that the union of the earths with nascent nitrous oxide may be effected by exposing nitrous gas to their sulphures, containing an excess of earth.
Perhaps the combination of nitrous oxide with strontian may be effected by introducing the combination of potash and nitrous oxide into strontian lime water.
It is probable that nitrous oxide may be combined with clay and magnesia, by exposing these bodies, mingled with sulphite of potash or soda, to nitrous gas.
XI. Additional Observations on the combinations
of Nitrous Oxide with the Alkalies.
A desire to complete physiological investigations relating to nitrous oxide, has hitherto prevented me from pursuing to a greater extent, the experiments on the combination of this substance with the alkalies, &c. As soon as an opportunity occurs, I purpose to resume the subject.
The observations detailed in the foregoing sections are sufficient to show that nitrous oxide is capable of entering into intimate union with the fixed alkalies: and as the compounds formed by this union are insoluble in alcohol, decomposable by the acids, and heat, and possessed of peculiar properties, they ought to be considered as a new class of saline substances.
If it is thought proper, on a farther investigation of their properties, to signify them by specific names, they may, according to the usually adopted fashion of nomenclature, be called nitroxis: thus the nitroxi of potash would signify the salt formed by the combination of nitrous oxide with potash.
Future experiments must determine the different affinities of nitrous oxide for the alkalies, and alkaline earths.
With regard to the uses of these new compounds it is difficult to form a guess. When they are obtained pure, and fully saturated with nitrous oxide, on account of the low temperature at which their gas is liberated, they will probably constitute detonating compounds. From their facility of decomposition by the weaker acids, they may possibly be used medicinally, if ever the evolution of nitrous oxide in the stomach should be found beneficial in diseases.
XII. The properties of Nitrous Oxide resemble those of Acids.
If we were inclined to generalise, and to place nitrous oxide among a known class of bodies, its properties would certainly induce us to consider it as more analogous to the acids than to any other substances; for it is capable of uniting with water and the alkalies, and is insoluble in most of the acids. It differs, however, from the stronger acids, in not possessing the sour taste,[165] and the power of reddening vegetable blues: and from both the stronger and weaker acids, in not being combinable when in a perfectly free state, at common temperatures, with the alkalies. If it should be proved by future experiments, that condensation by cold gave it the capability of immediately forming neutro-saline compounds with the alkalies; it ought to be considered as the weakest of the acids. Till those experiments are made, its extraordinary chemical and physiological properties are sufficient to induce us to consider it as a body sui generis.
It is a singular fact that nitrous gas, which contains in its composition a quantity of oxygene so much greater than nitrous oxide, should nevertheless possess no acid properties. It is uncombinable with alkalies, very little soluble in water, and absorbable by the acids.