Potassium acid sulfite

The sodium and potassium salts of S02 are simpler and more pleasant to use as they do not have the odor of the pure liquid or the 5% water solution. They are rapidly soluble in must where they react with a small portion of the natural acid present to liberate S02. There are two sodium salts of S02 available, Na2S03 (neutral sodium sulfite) and NaHS03 (sodium acid sulfite). The latter compound introduces less sodium into the wine and removes less acid from the wine for an equivalent amount of S02 liberated. Potassium acid sulfite and potassium pyrosulfite (potassium metabisulfite) are the two salts of potassium with S02 that are readily available, soluble in grape juice, and capable of yielding S02 upon reaction with the acid of the juice. Potassium salt is recommended when it is desired to keep the wine low in sodium ion content for diet reasons. The salts should be edible or food product grade, that is, free of heavy metals and other toxic impurities. They must be stored in tightly closed containers or they will react with the water vapor and... 

Synonyms E228 potassium acid sulfite potassium bisulphite potassium hydrogen sulfite. 

Synonyms Potassium acid sulfite Potassium hydrogen sulfite... 

Sodium or potassium hydrogen sulfite reacts with several thiiranes to give disulfides of /3-mercaptosulfonic acid salts (76EGP122086). Potassium thiocyanate in dimethylformamide or aqueous ethanol isomerizes thiiranes (Scheme 84) (72CJC3930). 1,2-Dithiols are obtained by treatment of thiiranes with NaBH2S3 obtained from sodium borohydride and sulfur (73TL1401). 

Compounds which can be regarded as analogous to reduction products are 1,6-covalent adducts produced by various weak acids including potassium hydrogen sulfite and purine (165) and the 2-oxopurine (166) (75Jcs(pi)224o). 

S03H)ONH2 Hydroxylamine-O-sulfonic acid, 5 122, 123 SOsKH Potassium hydrogen sulfite, 2 167... 

With sodium or potassium hydrogen sulfite allyl alcohol gives the salt of 3-hydroxypropanesulfonic acid,63 the free acid from which gives a 90% yield of propanesultone when heated gradually to 200°. Hydrogen sulfites can also be added to unsaturated fatty acids,64 acrylonitrile,29 and alkenedicarboxylic acids and their esters.65... 

Write the chemical formula for each of the following compounds, and indicate the oxidation state of the group 6A element in each (a) selenous acid, (b) potassium hydrogen sulfite, (c) hydrogen teUuride, (d) carbon disulfide, (e) calcium sulfate, (f) cadmium sulfide, (g) zinc teUuride. 

Because of its high solubility and the small effect of temperature, as shown in Fig. 21, potassium sulfite is more difficult to prepare than sodium sulfite. Foerster and earlier workers found it necessary to proceed from a solution of the acid sulfite. The pyrosulfite may be crystallized readily from water. Both salts oxidize rapidly in air when moist but are stable when dry. 

Potassium metabisulfite (potassium pyrosulfite) is used as an antifermenting agent in breweries and wineries, and to bleach straw. Sodium bisulfite (sodium acid sulfite) is mainly used in pharmaceutical products, as disinfectant or bleach, and in the dye industry. Sodium sulfite is used in photographic developers, for fixing prints, bleaching textile fibers, and as a preservative in the food industry. 

Different CL reactions in liquid phase have been applied with analytical purposes. These include luminol, tris(2,2 -bipyridyl)ruthenium(II), lucigenin, lophine, peroxyoxa-late derivatives, acidic potassium permanganate, sulfite, gallic acid, morphine, codeine, pyrogallol acridinium esters, and others. Table 19.2 summarizes some of the commonly used CL reactions in liquid phase and their analytical application in different areas. 

Potassium Acetate Potassium Acid Sulfate Potassium Acid Tartrate Potassium Antimonate Potassium Bicarbonate Potassium Bichromate Potassium Bisulfate Potassium Bisulfite Potassium Bitartrate Potassium Borate Potassium Bromate Potassium Bromide Potassium Carbonate Potassium Chlorate Potassium Chloride Potassium Chromate Potassium Cyanide Potassium Dichromate Potassium Ferricyanide Potassium Ferrocyanide Potassium Fluoride Potassium Hexacyanoferrate (III) Potassium Hydrogen Carbonate Potassium Hydrogen Sulfate Potassium Hydrogen Sulfite Potassium Hydroxide Potassium Hypochlorite Potassium Hyposulfite Potassium lodate Potassium Iodide Potassium Manganate Potassium Nitrate Potassium Perborate Potassium Perchlorate Potassium Permanganate Potassium Peroxydisulfate Potassium Persulfate... 

Palmitic Acid 57-10-3 Phosphorus (V) Oxide 1314-56-3 Potassium Hydrogen Sulfite 7773-03-7... 

Because of the time and expense involved, biological assays are used primarily for research purposes. The first chemical method for assaying L-ascorbic acid was the titration with 2,6-dichlorophenolindophenol solution (76). This method is not appHcable in the presence of a variety of interfering substances, eg, reduced metal ions, sulfites, tannins, or colored dyes. This 2,6-dichlorophenolindophenol method and other chemical and physiochemical methods are based on the reducing character of L-ascorbic acid (77). Colorimetric reactions with metal ions as weU as other redox systems, eg, potassium hexacyanoferrate(III), methylene blue, chloramine, etc, have been used for the assay, but they are unspecific because of interferences from a large number of reducing substances contained in foods and natural products (78). These methods have been used extensively in fish research (79). A specific photometric method for the assay of vitamin C in biological samples is based on the oxidation of ascorbic acid to dehydroascorbic acid with 2,4-dinitrophenylhydrazine (80). In the microfluorometric method, ascorbic acid is oxidized to dehydroascorbic acid in the presence of charcoal. The oxidized form is reacted with o-phenylenediamine to produce a fluorescent compound that is detected with an excitation maximum of ca 350 nm and an emission maximum of ca 430 nm (81). 

The problem describes a salt of a pol3/protic acid and asks for ion concentrations. To determine concentrations of all ions, we need to consider more than one equilibrium. This is done in stages, starting with the dominant equilibrium. We apply the seven-step strategy. The problem asks for the concentrations of the ions in aqueous potassium sulfite, in which the major species are, SO], and H2O. The potassium ion is a spectator ion. 

Sulfonation of anthraquinone to form the 1-sulfonic acid is achieved at approximately 120°C with 20% oleum in the presence of mercury or a mercury salt as a catalyst [2], Without this catalyst, the reaction produces the 2-sulfonic acid. Exchange with aqueous ammonia (30%) at about 175°C under pressure converts the potassium salt of 1-sulfonic acid to 1-aminoanthraquinone in 70 to 80% yield. To avoid sulfite formation, the reaction is performed in the presence of an oxidant, such as m-nitrobenzosulfonic acid, which destroys sulfite. 

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