Sulfite potassium solutions

Mercury(II) oxide dissolves in neutral sodium or potassium sulfite solution forming sulfitomercurate(II) ion ... 

A sample of potassium sulfite solution is mixed with an excess of dilute hydrochloric acid. 

In the potassium salt cycle, the gas is first scrubbed with water or sulfuric acid solution to remove particulate and sulfur bioxide. It is then contacted with a potassium sulfite solution which removes SO2 by the foUowing reaction ... 

Analytical Methods. A classical and stiU widely employed analytical method is iodimetric titration. This is suitable for determination of sodium sulfite, for example, in boiler water. Standard potassium iodate—potassium iodide solution is commonly used as the titrant with a starch or starch-substitute indicator. Sodium bisulfite occurring as an impurity in sodium sulfite can be determined by addition of hydrogen peroxide to oxidize the bisulfite to bisulfate, followed by titration with standard sodium hydroxide (279). 

Potassium sulfite is commonly used as a food preservative, because the sulfite anion undergoes reactions that release sulfur dioxide, an effective preservative. Determine the concentrations of the ionic species present in a solution of potassium sulfite that is 0.075 M. 

HF (aq.). The earliest determination of the heat of formation of fluorine compounds was made by Berthelot and Moissan,1 who measured the heat of reaction between fluorine and an aqueous alkaline solution of potassium sulfite but their data are of historical interest only. Guntz1 found the heat of solution of hydrogen fluoride to be 11.8 von Wartenberg and Fitzner1 gave, for HF (g) (ideal) =HF (aq.), Q = 11.56. von... 

To prepare the necessary potassium sulfite Dissolve 44g of potassium metabisulfite m a solution of lOOg of potassium hydroxide in one liter of water, add 5 drops of phenol-phthalem indicator and then more of the 10% potash solution until a pink color just forms. Add the latter solution drop by drop from a separatory funnel KHSO f KOH ------- KaSOs + H 0]... 

Potassium pentachloronitrido-osmate(VI), 6 206 Potassium permanganate, solution of, standardization of, for determination of average atomic weight of rare earth elements in oxalates, 2 60, 61 Potassium pyrosulfite, 2 166 and its f-hydrate, 2 165, 167 Potassium rare earth sulfates, 2 47 Potassium selenocyanate, 2 186 Potassium sulfites, KHSO , in solution, 2 167... 

Trimethyl Telluronium Picrate1 Trimethyl telluronium iodide, prepared from 1.6 g of dimethyl tellurium diiodide, potassium sulfite, and methyl iodide, is dissolved in water and a saturated aqueous solution of picric acid is added until precipitation of the telluronium picrate ceases. The solid is filtered off, washed with cold water, and dried in air yield 0.3 g (20% based on dimethyl tellurium diiodide) m.p. 127° (dec.). 

A beaker containing dilute hydrochloric acid is poured into a beaker containing a solution of potassium sulfite. 

Biphasic basic oxidation using technical grade (50-60%) 3-chloroperbenzoic acid affords this oxaziridine in - 4 hr In a 2-L, three-necked, Morton-flask equipped with a mechanical stirrer was placed 22.6 g (0.083 mol) of crude (+)-[(7,7-dimethoxycamphoryl)sulfonyl]imine, 42.6 g (0.13 mol) of 3-chloroperoxybenzoic acid (50-60%) in 450 mL of methylene chloride, and 450 mL of saturated potassium carbonate solution. The reaction mixture was stirred vigorously until the oxidation was complete as indicated by TLC (Note 27) at which time 500 mL of water was added, the organic layer was separated and the aqueous layer was extracted with methylene chloride (2 x 500 mL). The combined organic extracts were washed with saturated sodium sulfite (300 mL) and water (300 mL), and dried over anhydrous magnesium sulfate. 

Sulfite Ion. The reaction of NO with sulfite ion and several of the reactions discussed subsequently can be explained by a reaction sequence in which a base attacks NO to form BNO in the first step, followed by a rapid reaction of the BNO radical with a second molecule of NO. In several of these reactions the dimer BN2O2 is formed, although NO does not dimerize to a measurable extent at room temperature (17). The reaction of sulfite ion with NO is an example of this reaction type. When nitric oxide is bubbled into a cooled (0° C.) basic aqueous solution of potassium sulfite, a white solid which has the empirical formula K2SO3N2O2 precipitates (10). 

Add 5.0 mL of 0.01 M sodium hydrogen sulfite solution (NaHS03) to the potassium permanganate solution while stirring. Record your observations. 

Solutions of Sodium and Potassium Sulfite and Bisulfite. Oxygen free, pure sulfite and bisulfite solution containing sodium or potassium ions are stable for more than a year at room temperature. However, at 100°C or above, the sulfate spectrum can be observed already after a few days. Elemental sulfur does not immediately appear. Sometimes, at intermediate and high pH, thiosulfate can be observed in a few experiments. The appearance of these species indicates that they are intermediates in the auto-redox reaction Equations I-III, or that they are formed in a secondary reaction of sulfur (IV) with the product elemental sulfur. The latter reactions are already known. They occur during the degradation of elemental sulfur... 

All A-halo compounds can be readily determined by analysis based on their oxidizing action. They liberate two equivalents of iodine from acidified potassium iodide solution almost instantaneously (1 mmole of A-monohalo compound is equivalent to 20 ml of O.In-thiosulfate solution). The liberation of iodine from hydrogen iodide involves production of the amine or amide parent of the halo compound. Sodium sulfite and hydrogen sulfide also reduce N-halo compounds. UV and IR spectroscopic methods have been worked out for determination of JV-halo compounds.399... 

Replacement of the nitro group by a sulfo group is particularly easy in the nitroanthraquinone series, when these compounds are boiled for several hours with sodium or potassium sulfite in aqueous solution.495,496... 

Oxidation by potassium permanganate is usually carried out in acetic or sulfuric acid solution. Isolation of the sulfone must include separation from the precipitate of manganese(iv) oxide hydrate, which, in the case of sparingly soluble sulfones, is effected by reduction of this precipitate by just sufficient sodium hydrogen sulfite solution or by sulfur dioxide soluble sulfones can be isolated by addition of water after filtration from the hydrated manganese oxide or by acidification and extraction with ether. 

Acetone (1 mole) is shaken with a concentrated aqueous solution of sodium hydrogen sulfite (1 mole). The mixture becomes warm and is allowed to cool, then a concentrated aqueous solution of potassium cyanide (1 mole) is dropped in with good shaking, whereupon the solution again becomes warm. The mixture is cooled again and the oily layer of acetone cyanohydrin is separated from the aqueous layer, which is then extracted several times with ether. The cyanohydrin layer and ether extracts are united, washed with sodium hydrogen sulfite solution to remove acetone, and then with saturated sodium chloride solution, and freed from ether. Completely alkali-free acetone cyanohydrin boils at 82°/23 mm and melts at-19°. 

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 sulfite forms no hydrates, but the pyrosulfite forms the compound K2S205-%H20, which is probably, the double salt K2S205-4KHS03. In solution, the pyrosulfite is converted to the hydrogen sulfite. 

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