Stronger Ammonia

United States Pharmacopeia stronger ammonia water ammonia test solution normal (1 N) aqua ammonia chemically pure technical, Bh°... 

Ammonia TS, Stronger (15.2 A in NH3) (Ammonium Hydroxide Stronger Ammonia Water) Use ACS reagent-grade Ammonium Hydroxide, which is a practically saturated solution of ammonia in water, containing between 28% and 30% of NH3. 

Salts, smelling Ammonia-based preparations used as a restorative in hysterical syncope (fainting). Dry smelling salts (or vinaigrettes) are composed of ammonium chloride and potassium carbonate, perfumed with lavender liquid smelling salts are composed of ammonium carbonate dissolved in stronger ammonia water and alcohol, and perfumed with oils solidified smelling salts are similar preparations solidified with stearic acid. ... 

Ammoniaca ammoniacum aqua ammonia concentrated ammonia solution spirit of hartshorn stronger ammonia water. 

White powder darkens on exposure to light, d 5.56 mp 455 bp 1550. Soly in water (23 ) 1.93 mg/1 hydrochloric acid increases its soly. Sol in 250 parts of coned HC1, in 13 parts of 10% ammonia more sol in stronger ammonia and also at higher temps. Sol in solns of alkali cyanides, thiosulfates, ammonium carbonates appreciably sol in coned aq solns of ammonium chloride mercuric nitrate, and silver nitrate. The freshly pptd chloride dissolves more readily than tha dried precipitate. Insol in alcohol, or dil acida. Protect from light. 

Ammonia evolved in the cold (turns moist red litmus-paper blue). Methane may be evolved by stronger and more prolonged heating. 

It frequently happens that more than one volatile product is evolved, a fact which may be of considerable value. For example, benzamide, CeHjCONHt, will give off first ammonia, and then benzonitrile and benzene on stronger heating salicylamide, HOC H CONHj, will give off ammonia and then phenol. Sulphanilamide, NH,C,H,SO,NH (p. 181), gives off ammonia and aniline. 

The stronger base is derived from the weaker conjugate acid Therefore add a proton to ammonia to give its conjugate acid (ammonium ion) and a proton to pyridine to give its conjugate acid (pyridimum ion) then look up the values for each... 

Ammonium ion is a weaker acid than pyridimum ion therefore ammonia is a stronger base than pyridine... 

Hydrogen bonds between —OH groups are stronger than those between —NH groups as a comparison of the boiling points of water (H2O 100 C) and ammonia (NH3 —33 C) demonstrates... 

Alkylammes are slightly stronger bases than ammonia... 

The compound shown is a somewhat stronger base than ammonia Which nitrogen do you think IS protonated when it is treated with an acid" Write a structural formula for the species that results... 

Many of these reactions are reversible, and for the stronger nucleophiles they usually proceed the fastest. Typical examples are the addition of ammonia, amines, phosphines, and bisulfite. Alkaline conditions permit the addition of mercaptans, sulfides, ketones, nitroalkanes, and alcohols to acrylamide. Good examples of alcohol reactions are those involving polymeric alcohols such as poly(vinyl alcohol), cellulose, and starch. The alkaline conditions employed with these reactions result in partial hydrolysis of the amide, yielding mixed carbamojdethyl and carboxyethyl products. 

Reductions. Hydrazine is a very strong reducing agent. In the presence of oxygen and peroxides, it yields primarily nitrogen and water with more or less ammonia and hydrazoic acid [7782-79-8]. Based on standard electrode potentials, hydrazine in alkaline solution is a stronger reductant than sulfite but weaker than hypophosphite in acid solution, it falls between and Ti ( 7). 

Iron(III) bromide [10031-26-2], FeBr, is obtained by reaction of iron or inon(II) bromide with bromine at 170—200°C. The material is purified by sublimation ia a bromine atmosphere. The stmcture of inoa(III) bromide is analogous to that of inon(III) chloride. FeBr is less stable thermally than FeCl, as would be expected from the observation that Br is a stronger reductant than CF. Dissociation to inon(II) bromide and bromine is complete at ca 200°C. The hygroscopic, dark red, rhombic crystals of inon(III) bromide are readily soluble ia water, alcohol, ether, and acetic acid and are slightly soluble ia Hquid ammonia. Several hydrated species and a large number of adducts are known. Solutions of inon(III) bromide decompose to inon(II) bromide and bromine on boiling. Iron(III) bromide is used as a catalyst for the bromination of aromatic compounds. 

The lack of dependence on ionic strength in the first reaction indicates that it occurs between neutral species. Mono- or dichloramine react much slower than ammonia because of their lower basicities. The reaction is faster with CI2 because it is a stronger electrophile than with HOCl The degree of chlorination increases with decreasing pH and increasing HOCINH mol ratio. Since chlorination rates exceed hydrolysis rates, initial product distribution is deterrnined by formation kinetics. The chloramines hydrolyze very slowly and only to a slight extent and are an example of CAC. 

Similar reactions occur with ammonia and HOBr (19—25), but since HOBr is a stronger electrophile than HOCl, formation rates are faster. Because of rapid bromine transfer between bromamines, equihbrium concentrations of the respective bromamines are obtained quickly. Mon ohrom amine predominates at basic pH at high N Br ratios. Below pH 8.5, NHBr2 and NBr predominate. Tribromamine formation is favored at lower pH and higher Br N ratios. The bromamines are less stable than chloramines but are better disinfectants. 

The ahphatic alkyleneamines are strong bases exhibiting behavior typical of simple aUphatic amines. Additionally, dependent on the location of the primary or secondary amino groups iu the alkyleneamines, ring formation with various reactants can occur. This same feature allows for metal ion complexation or chelation (1). The alkyleneamines are somewhat weaker bases than ahphatic amines and much stronger bases than ammonia as the piC values iadicate (Table 2). 

With Ammonia and Amines. Ethylene oxide reacts with ammonia to form a mixture of mono-, di-, and triethanolamines. Nitrogen is a stronger nucleophile than oxygen (59). A small amount of water is essential for the reaction (60). 

Example A common misconception is that the conjugate base of a weak acid is strong. This is sometimes, but not always, true. It is tme, for exanple, for ammonia, which is a very weak acid (pK 36). Its conjugate base amide ion (H2N ) is a much stronger base than HO . It is not true, however, for acetic acid both acetic acid and its conjugate base acetate ion are weak. The conjugate base of a weak acid will be strong only when the acid is a weaker acid than water. 

Ammonia is, in fact, a poor choice for pH adjustment at higher temperatures. In practice, the lower alkylamines are effectively stronger bases than ammonia, not least because of the inductive effect of methylene groups. 

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