Solution of Chlorinated Lime

Preparation and Properties of Lead(IV) Oxide, a. Prepare a saturated transparent solution of chlorinated lime and a solution of 3 g of lead acetate in 5 ml of water. Add an equal volume of a lead acetate solution heated to 50 °C to the first solution while stirring it. Heat the reaction mixture to 100-110 °C. Wash the precipitate first with water by decantation, and next with a dilute nitric acid solution (what ions are washed off here ). Filter off the product, again wash it two or three times on the funnel with water and dry it at 100 °C. Keep the preparation. Write the equation of the reaction. 

Mix the linseed meal gradually with the water, and add the solution of chlorinated lime, with constant stirring. 

Antidotes.—Solution of chlorinated lime, with an emollient drink. 

Solution of Chlorinated Lime with Boric Acid, B.P.C. (Eusol). 

The presence of acetanilide in these residues may be confirmed by boilin the residue for two to three minutes with HCl, and when cool, adding a few drops of 0 5 per cent, of chlorinated lime solution, in such a manner that the liquids do not mix. A fine blue colour results if acetanilide be present. 

Calcium hypochlorite may be prepared by passing chlorine into a slurry of lime and sodium hydroxide. Alternatively, chlorine is passed into a solution of hydrated lime to produce bleaching powder, CaCl(0Cl) H20 ... 

Ag2C03 = 2 AgCl + 2HC10 + C02 Another way to increase the yield is to pass additional chlorine into soda or lime solutions of chlorine Cl2 + Na2C03 + H20 = NaClO +... 

The precipitation of basic calcium hypochlorites can be nsed to ranove calcium chloride. The excess calcium that is not associated with calcium hypochlorite can be precipitated by adding sulfate or carbonate, but this is less effective, and does not remove other impurities that remain in the calcium hypochlorite after the solution is evaporated. In either case, the conversion of lime to calcium hypochlorite is reduced by the amount of calcium salts that are removed from the process. In an earlier process, a concentrated lime slurry is chlorinated at 40-45 C to form crystals of hemibasic calcium hypochlorite. These are ranoved by filtration and snspended in a slurry of chlorinated lime. Chlorine is then added to make calcinm hypochlorite dihydrate crystals that are removed by filtration. The filtrate is mixed with lime to precipitate dibasic calcium hypochlorite. The dibasic calcium hypochlorite is ranoved by filtration, snspended in recycled liquor, and chlorinated to form crystals of calcium hypochlorite dihydrate. Throughout the process, seed crystals are used and the filtrates are recycled. " Alternatively, slow chlorination at 15°C is used to directly produce calcium hypochlorite dihydrate instead of the hanibasic compound in the first step. Dibasic calcium hypochlorite is made from the filtrate and processed as before. " ... 

Early demand for chlorine centered on textile bleaching, and chlorine generated through the electrolytic decomposition of salt (NaCl) sufficed. Sodium hydroxide was produced by the lime—soda reaction, using sodium carbonate readily available from the Solvay process. Increased demand for chlorine for PVC manufacture led to the production of chlorine and sodium hydroxide as coproducts. Solution mining of salt and the avadabiHty of asbestos resulted in the dominance of the diaphragm process in North America, whereas soHd salt and mercury avadabiHty led to the dominance of the mercury process in Europe. Japan imported its salt in soHd form and, until the development of the membrane process, also favored the mercury ceU for production. 

Sodium bicarbonate may be prepared by the ammonia-salt (Solvay) process. Carbon dioxide is passed through a solution of sodium chloride in ammonia water. Sodium bicarbonate is precipitated and the ammonium chloride remains in solution. The ammonium chloride is heated with lime to regenerate ammonia (see Alkali AND CHLORINE PRODUCTS). 

Bleach Liquor. Bleach Hquor or lime bleach Hquor is an aqueous solution of calcium hypochlorite and calcium chloride. It typically contains 30—35 g/L of available chlorine, though it may be as high as 85 g/L. It has been used in pulp bleaching, when it can be made more cheaply than sodium hypochlorite. It is prepared on site by chlorinating lime solutions. 

Chlorination of lime slurried in strong NaOCl solution, followed by cooling to — 15°C, precipitates about 80% of the av CI2 as large hexagonal crystals of a triple salt Ca(OCl)2 NaOCl NaCl -12H20 [64147-46-2] (182). The recovered triple salt, free of much of the lime impurities, is treated with chlorinated lime slurry to produce neutral calcium hypochlorite dihydrate crystals [22464-76-2]. 

Two cocrystallization processes employ dibasic crystals as intermediates. The PPG process (199—202) is discussed under commercial processes. The PPC process (203) forms dibasic crystals from lime and recovered filtrates. The dibasic crystals are separated from thek mother liquor by decantation, slurried in caustic solution and chlorinated to produce a cocrystalline slurry of Ca(OCl)2 and NaCl. The slurry is sent to a flotation cell where the larger salt crystals settle out and the smaller hypochlorite crystals float to the top with the aid of ak and flotation agent. The hypochlorite slurry is centrifuged the cake going to a dryer and the centrate to the flotation cell. The salt-rich bottoms from the flotation cell are centrifuged and washed with dibasic mother Hquor. The centrates are recycled to the precipitation step. 

Theory Chlorinated lime reacts with acetic acid to produce a mole each of calcium acetate, hydrochloric acid and hydrochlorous acid. The two acids interact to give water and chlorine, and the latter reacts with HI to liberate iodine that can be estimated by titrating with 0.1 N sodium thiosulphate solution. The various reactions involved may be expressed as given below ... 

Other agents are also available, which are used to remove pigmentation of teeth e.g. weak ammonia solution is used to remove iodine stains, hypochlorite or iodine solution are used to remove silver stains, hypochlorites are used to remove iron stains of teeth and for dye stains, chlorinated lime and acetic acid are used. 

Put some chlorinated lime into a test tube and pour a 20% hydrochloric acid solution over it. Write the equation of the reaction. 

Add a solution of 1 iV sulphuric acid to a part of the prepared chlorinated lime solution until the reaction is acid and carefully smell the product. Write the equation of the reaction. What happens to chlorinated lime when its concentrated solution is heated ... 

Put a little chlorinated lime into test tube 7, and pour a concentrated ammonia solution into dropping funnel 2. Add the ammonia solution dropwise to the chlorinated lime and collect the evolved nitrogen in test tube 3 by putting it over the end of the gas-discharge tube. Write the equation of the reaction. See whether... 

Preparation of Nickel(III) Oxide. Pour a little of a sodium hydroxide solution into a small amount of a nickel sulphate one while stirring, and then add a chlorinated lime (calcium hypochlorite) solution (which must be absolutely transparent). Let the mixture stand for several hours until the evolution of oxygen bubbles stops. Next heat it up to boiling. Let the mixture settle and wash the precipitate by decantation. Write the equation of the reaction. 

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