Alkali metal sulfite salt

Alkali metal azides, 1 79 2 139 Alkali metal cyanates, 2 86 Alkali metal pyrosulfites, 2 162 Alkali metal sulfites, 2 162 Alkaline earth azides, 1 79 Allanite, extraction of, 2 44 Allophanyl azide, formation of, from allophanyl hydrazide, 5 51 Allophanyl hydrazide (1-amino-biuret), 5 48 hydrazones of, 5 51 from methyl and ethyl alloph-anates, 5 50 salts of, 5 51... 

Other oxoacid salts of the alkali metals are discussed in later chapters, e.g. borates (p. 205), silicates (p. 347), phosphites and phosphates (p. 510), sulfites, hydrogensulfates, thiosulfates, etc. (p. 706) selenites, selenates, tellurites and tellurates (p. 781), hypohalites, halites, halates and perhalates (p. 853), etc. 

Although the alkali-metal ions are hydrated in aqueous solution, only the lithium and sodium ions retain their water of hydration in their solid salts. Hydrated potassium salts are known, but the water in such hydrates is generally anion water (Chap. 4) the ammonium ion often forms hydrated salts with the same anions as does the potassium ion (carbonate, oxalate, sulfite). 

The conversion of salt to hydroxide by use of a strongly basic anion-exchange resin, followed by titration with standard acid, is usually not so appropriate as the conversion of salt to acid because the resin-regeneration procedure is less convenient. Hydrolysis of the resin to give amines may occur, as well as absorption of carbon dioxide. The anion-exchange method can be used, for example, in the determination of alkali metal phosphates or sulfites. 

Sulfates are widely known in the environment and a few such as those of calcium, strontium, barium, and lead are insoluble. The sulfates of magnesium and the alkali metals are soluble and so are typically found in brines and salt deposits. Sulfites are rarer because of the ease of oxidation, but calcium sulfite, perhaps as the hemihydrate, can be detected on the surface of building stone in urban atmospheres containing traces of sulfur dioxide (Gobbi et al, 1998). 

The first examples reported by Sandmeyer date back to 1884. The many various preparative procedures differ mainly in the type and the preparation of the copper-cyanide complex which is used. In the Gattermann procedure KCN in the presence of Cu powder is used. Generally one tries to avoid the formation of HCN on the addition of alkali metal cyanide to the acidic medium by neutralizing the diazo-nium salt solution in advance with sodium or barium carbonate. Cyanogen, which is formed from CN ions on treatment with Cu" salts, is also a harmful by-product. In this case the addition of sodium hydrogen sulfite (equation 19) proved to be of great value. 

Conversion of Naphthols to Naphthylamines. Sulfurous Add Salts as Catalysts (Bucherer Reaction). The most general method for the replacement of —OH by —NHj groups in naphthols is the use of ammoniacal solutions containing salts of sulfurous acid. The alkali metal bisulfites are ordinarily employed in the preparation of primary amines but other compounds, such as the sulfite of methylamine (CH3-NHj)jSOj, can be used in making substituted amines. As can be seen from the reaction... 

MERCURIC BICHLORIDE (7487-94-7) HgClj Contact with acids or acid fumes evolves chloride and mercury vapors. Possible violent reaction with chlorine nitrate, sodium acetylide. Incompatible with albumin, alkalis, alkaloid salts, anhydrous ammonia, antimony, arsenic, borax, bromides, carbonates, chloric acid, copper, formates, gelatin, hydrozoic acid, infusions of cinchona, iron, lead and silver salts, lime water, light metals, methyl isocyanoacetate, oak bark or senna, phosphates, potassium, reduced iron, sodiiun, sodium peroxyborate, sulfides, sulfites, tannic acids, trinitrobenzoic acid, urea nitrate, vegetable astringents. Decomposed by sunlight. On small fires, use water spray, fog, foam, dry chemical powder, or CO2 extinguishers. 

White, odorless, tasteless, heavy powder slowly dec by sunlight into mercuric chloride and metallic mercury sublimes at 400-500 without melting, d 7.15. Practically insol in water (0-00020g/]00 ml H20 at 25 ) HCI or alkali and alkaline earth chlorides increase soly in water. Insol in alcohol. ether. Dec by solns of alkali iodides, bromides or cya -nides into the mercuric salt and metallic mecury solns of alkali chlorides act similarly but slowly. It is blackened by ammonia, caustic alkali and alkaline earth solns. Protect from light. Incompat Bromides, iodides, alkali chlorides, sulfates, sulfites, carbonates, hydroxides, lime water, acacia, ammonia, golden antimony sulfide, cocaine, cyanides, copper salts, hydrogen peroxide, iodine, iodoform, lead salts, silver salts, soap, sulfides. 

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