Reactions sodium oxides with water

A base can be prepared by the reaction of sodium oxide with water. Give the reaction and the name of the base product. 

Introduce a solution of 15 g. of the diazo ketone in 100 ml. of dioxan dropwise and with stirring into a mixture of 2 g. of silver oxide (1), 3 g. of sodium thiosulphate and 5 g. of anhydrous sodium carbonate in 200 ml. of water at 50-60°. When the addition is complete, continue the stirring for 1 hour and raise the temperature of the mixture gradually to 90-100°. Cool the reaction mixture, dilute with water and acidify with dilute nitric acid. Filter off the a-naphthylacetic acid which separates and recrys-talhse it from water. The yield is 12 g., m.p. 130°. 

Properties of Tellurium(IV) Oxide. 1. Test the reaction of tellu-rium(IV) oxide with water, and also with solutions of sodium hydroxide and hydrochloric acid with heating. Write the equations of the reactions. 

This is essentially a two-step reaction, with hypochlorous acid being generated from the reaction of bleach with water and then the hypochlorous acid oxidizing the sodium bromide component. 

Both sodium and potassium salts are natural constituents of body tissues and fluids as Na+ and K+ ions, respectively, and are not themselves toxic at normal physiological levels. The oxides and hydroxides of both these metals are very caustic, corrosive substances that damage exposed tissue. Oxides are formed by the combustion of sodium and potassium organometallics, and hydroxides are produced by the reaction of the oxides with water or by direct reaction of the organometallics with water, as shown below for cyclopentadienylsodium ... 

This reaction involves the reduction of the dichromate ion by ammonium ion. Chromic oxide is also made by heating sodium dichro-mate with sulfur, and leaching out the sodium sulfate with water ... 

Cleaning Up The aqueous layer from the first part of the reaction should be neutralized with sodium carbonate, diluted with water, and flushed down the drain. The aqueous layer containing hydrosulfite, saturated sodium chloride, and sodium hydroxide are treated with household bleach (5.25% sodium hypochlorite solution) until no further reaction is evident. After neutralizing the solution with dilute hydrochloric acid, the solution is diluted with water and flushed down the drain. Shake the mixture of silver oxide, silver, and sodium sulfate with water to dissolve the sodium sulfate, and then recover the mixture of silver and silver oxide by vacuum filtration. 

Write balanced equations for the following reactions (a) barium oxide with water, (b) iron(II) oxide with perchloric acid, (c) sulfur trioxide with vrater, (d) carbon dioxide with aqueous sodium hydroxide. 

Note that the 2— charged oxide attacks and forms a bond with a partially positive hydrogen atom of the water molecule. The subsequent breaking (represented by a discontinuity in the bond) of the O—H bond produces two hydroxide ions. The equilibrium constant for Equation (11.9) is greater than 10, so this reaction lies far to the right. Taking sodium oxide as an example, the full reaction of an ionic oxide with water is represented in Equation (11.10) ... 

Poly (ethylene glycol)s are made by reaction of ethylene oxide with water, ethylene glycol, or diethylene or triethylene glycol using sodium or potassium hydroxide catalyst. 

Evidence for the solvated electron e (aq) can be obtained reaction of sodium vapour with ice in the complete absence of air at 273 K gives a blue colour (cf. the reaction of sodium with liquid ammonia, p. 126). Magnesium, zinc and iron react with steam at elevated temperatures to yield hydrogen, and a few metals, in the presence of air, form a surface layer of oxide or hydroxide, for example iron, lead and aluminium. These reactions are more fully considered under the respective metals. Water is not easily oxidised but fluorine and chlorine are both capable of liberating oxygen ... 

Prepare a saturated solution of sodium sulphide, preferably from the fused technical sodium polysulphide, and saturate it with sulphur the sulphur content should approximate to that of sodium tetrasulphide. To 50 ml. of the saturated sodium tetrasulphide solution contained in a 500 ml. round-bottomed flask provided with a reflux condenser, add 12 -5 ml. of ethylene dichloride, followed by 1 g. of magnesium oxide to act as catalyst. Heat the mixture until the ethylene dichloride commences to reflux and remove the flame. An exothermic reaction sets in and small particles of Thiokol are formed at the interface between the tetrasulphide solution and the ethylene chloride these float to the surface, agglomerate, and then sink to the bottom of the flask. Decant the hquid, and wash the sohd several times with water. Remove the Thiokol with forceps or tongs and test its rubber-like properties (stretching, etc.). 

Mercuric Sulfate. Mercuric s Af2iX.e.[7783-35-9] HgSO, is a colorless compound soluble ia acidic solutions, but decomposed by water to form the yellow water-iasoluble basic sulfate, HgSO 2HgO. Mercuric sulfate is prepared by reaction of a freshly prepared and washed wet filter cake of yellow mercuric oxide with sulfuric acid ia glass or glass-lined vessels. The product is used as a catalyst and with sodium chloride as an extractant of gold and silver from roasted pyrites. 

The standard potential for the anodic reaction is 1.19 V, close to that of 1.228 V for water oxidation. In order to minimize the oxygen production from water oxidation, the cell is operated at a high potential that requires either platinum-coated or lead dioxide anodes. Various mechanisms have been proposed for the formation of perchlorates at the anode, including the discharge of chlorate ion to chlorate radical (87—89), the formation of active oxygen and subsequent formation of perchlorate (90), and the mass-transfer-controUed reaction of chlorate with adsorbed oxygen at the anode (91—93). Sodium dichromate is added to the electrolyte ia platinum anode cells to inhibit the reduction of perchlorates at the cathode. Sodium fluoride is used in the lead dioxide anode cells to improve current efficiency. 

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