Ammonia, smell

Consider using urea in formulations with alkaline pH and for which ammonia smell is not a problem, since it is a cheap and effective hydrotrope. 

Methyl, dimethyl, trimethyl, and ethyl amines are gases under standard conditions. Most common alkyl amines are liquids, and high molecular weight amines are, quite naturally, solids at standard temperatures. Additionally, gaseous amines possess a characteristic ammonia smell, while liquid amines have a distinctive fishy smell. 

Wason S, Stephan M, Breide C. 1990. Ingestion of aromatic ammonia smelling salts capsules. AmJDis Child 144(2) 139-140. 

Colorless liquid with a strong ammonia smell density 0.707 at 20°C (68°F) boils at 55°C (131°F) freezes at -50°C (-58 F) soluble in water, alcohol, and most organic solvents strongly alkaline forms a hydrate. 

IV. Diagnosis is based on a history of exposure and description of the typical ammonia smell, accompanied by typical irritative or corrosive effects on the eyes,... 

Increase in top gas hydrogen water leak Flame yellow/orange water leak Loss of burden water leak Ammonia smell water leak. 

Ammonia hydroxide Household ammonia Smelling salts... 

The first amines, from Ci to C5, show physical properties close to ammonia, i.e. a high solubility in water, and a characteristic ammonia smell. Their solubility decreases rapidly with their molecular weight hexylamine C6H13NH2 has a very low solubility in water (1.2% at room temperature). 

To test for positive ions, add 300 milligrams of the sample to be tested to water and mix. Filter the slurry and divide the filtered solution into two parts. To one part of the solution add a drop of a saturated sodium sulfate solution. Barium or strontium will come out of the solution as a white precipitate. A flame test on a platinum wire, using the part of the solution that was not treated with sodium sulfate, identifies barium or strontium. A green flame is produced by barium salts and a red flame is produced by strontium salts. To find the quantities of barium and strontium, add sodium sulfate until no more precipitation is formed. Filter and weigh the precipitate. The untreated aqueous solution may be flame tested for sodium and potassium. A yellow and violet flame is produced respectively, although the potassium test is diffcult. NH4 can be detected by an ammonia smell after the solution has been made basic with sodium hydroxide. 

The cartilaginous fishes include the sharks and rays, whose flesh is rich in connective tissue and relatively low in fat, although they do accumulate oils in their livers. The concentrations of vitamins and minerals are very similar to those in white fish. These fishes contain urea in relatively large amounts, and so protein values based on total nitrogen are overestimated. The ammonia smell of cooked sharks and rays is not an indication that the fish is spoiled but rather is the result of enzymatic degradation of urea. 

Ammonia is a colourless gas at room temperature and atmospheric pressure with a characteristic pungent smell. It is easily liquefied either by cooling (b.p. 240 K) or under a pressure of 8-9 atmospheres at ordinary temperature. Some of its physical and many of its chemical properties are best understood in terms of its structure. Like the other group head elements, nitrogen has no d orbitals available for bond formation and it is limited to a maximum of four single bonds. Ammonia has a basic tetrahedral arrangement with a lone pair occupying one position ... 

All ammonium salts evolve ammonia on heating with alkali. Ammonia may be delected by (a) its smell, (b) its action in turning red litmus blue and (c) the orange-brown colour produced with Nessler s reagent. This is a very sensitive test. 

Ammonia is a volatile compound as evidenced by the strong smell of even dilute solutions. This volatility presents a possible source of determinate error. Will this determinate error be negative or positive ... 

At room temperature and atmospheric pressure ammonia is a colourless, alkaline gas with a pungent smell. It dissolves readily in water. Physical properties are summarized in Table 9.6. The effect of temperature on vapour pressure of anhydrous ammonia is shown in Figure 9.2. 

Organic fluorine as a separate industry that began in the late 1920s with the discovery by Midgle of fluorocarbons for use as refrigerants. Ammonia was unsuitable because of the hazard and unpleasant smell from minute leaks. Sulfur dioxide had similar problems. The best refrigerant was... 

Reactions.—Add a few drops of alcohol to the same quantity of apetic acid, and an equal volume of concentrated sulphuric acid. Warm gently and notice the fruity smell of ethyl acetate. Neutralise a few drops of acetic acid by adding e.xcess of ammonia and boiling until neutral. Let cool and add a drop of ferric chloride. The red colour of ferric acetate is produced On boiling, basic ferric acetate is precipitated. 

The esters are, for the most pait, colourless liquids or solids of low m. p., with a fruity smell and insoluble in water. They are hydrolysed by potash (most readily with alcoholic potash) and give amides with ammonia,... 

Contains Nitrogen.—First test the original solid ni liquid by heating in a hard-glass tube with soda-lime (p. 2), and notice if the smell is that of ammonia (ammonia salt, amide or cyanide), an amine (amine or amino-acid) or a pyridine base (alkaloid). 

Aininonhni oi amine salts, if present, emit the smell of ammonia or amine if the salt of an insoluble oiganic base is present amine, alkalniif), it may be precipitated as a liquid or solid Salts of aliphatic bases and bases such as benzylanvne... 

The alkaline sodium sulphite solution may be replaced by saturated amtnonlum sulphite solution prepared as follows. Pass sulphur dioxide into a mixture of 1 part of concentrated ammonia solution (sp. gr. 0-88) and two parts of crushed ice in a freezing mixture imtil the liquid smells strongly of sulphur dioxide, and then neutralise with ammonia solution. This solution slowly deposits ammonium sulphite crystals and contains about 0-25 g. of SOj per ml. Use 60 ml. of this ice-cold ammonium sulphite solution to which 8 ml. of concentrated ammonia solution are added. After the addition of the solution of p-nitrophenyldiazonium chloride, allow the mixture to stand for 1 hour in a freezing mixture, filter oft the yellow precipitate of ammonium p-nitrophenyUiydrazine disulphonate, heat it on a water bath with 20 ml. of concentrated hydrochloric acid at 70-80° for 7 minutes, cool the blood-red solution, and dissolve the resulting precipitate of p-nitrophenylhydr-azine hydrochloride and ammonium salts in water, and isolate the base as above. 

Possible danger to respiratory tract from fumes ammonia, acetone, nail polish remover, heated sulfur, moth balls Make sure there is good ventilation. Never smell fumes directly. Wear a mask. Leave foul area and notify your teacher immediately. 

Carothers claimed that he kept going only because he finally received one of Illinois few scholarships, 750 embellished with esteem. But he must also have persevered because he loved chemistry. As he admitted, even the smell of his laboratory coat, saturated with the inexpressibly pungent and complicated odors of lab no. 219 [filled him] with a nostalgia to return to the atmosphere of sweetly blended sulfur dioxide, bromine, chlorine, ammonia, hydrogen chloride, phosgene, chloroacetone, etc., etc., etc. ... 

Test Ttibe 3 6 M NH3 1 carefully smelled all tubes to begin with and this tube was definitely ammonia. Since I was able to rule out this tube initially, I then mixed a small amount of known ammonia with all other tubes. As I mixed the ammonia with the other tubes, I noticed considerable heat being produced in tubes 1, 4 and 7, which I suspected was due to an acid present. With tube 1, smoke appeared, which led me to believe that tube 1 was the HC1 which produced a white cloud (smoke) of NH4C1. Tubes 1 and 3 were now ruled out. I then noticed precipitates formed in tubes 8 (blue), tube 6 (blue), tube 5 (white), tube 10 (brownish-grey) and tube 7 (white). When excess ammonia was added to tube 10, the precipitate dissolved. When excess ammonia was added to test tube 8, the precipitate dissolved and the solution turned dark blue indicative of Cu2+. When I added excess ammonia to test tube 6, the precipitate dissolved and the solution turned a medium blue color, indicative of the presence of Ni(NH3)62+. 

The solution is diluted with 200 c.c. of water and boiled until a sample, when mixed with dichromate solution, no longer smells of nitrosobenzene but of quinone (ten to fifteen minutes). To the cooled solution 2 g. of dichromate dissolved in water are added, a downward condenser is attached to the flask containing the mixture, and steam is passed through. The quinone is carried over with the steam. On the mechanism of its formation in this reaction compare p. 310. Test the residue in the flask for ammonia. 

In order to convert it into phenyl azide ( diazobenzeneimide ) the perbromide is added in three or four portions to about 10 c.c. of well-cooled concentrated ammonia solution. A vigorous reaction takes place, resulting in the formation of the pungent smelling phenyl azide, which is purified by steam distillation. It can also be distilled in a vacuum without decomposition. Since it explodes when rapidly heated it must be handled cautiously. 

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