Normal sodium

The following factors are the equivalent of 1 mL of normal sodium thiosulfate. Where the normality of the solution being used is other than normal, multiply the factors given in the table below by the normality of the solution employed. 

After the apparatus has been fitted together the caustic soda solution is run in slowly and the flask shaken. The liquid is no more ammonia is evolved be ascertained by testing a drop litmus paper. If the operation is titrated with half-normal sodium methyl orange as indicator. 

The dislillale ia collected in a oOO c.c. Krkniueyar flask having a mark upon it 1c indicate the level of 2o0 c.c. Phenolpbthalein solution and a an tEcicnt excess of deci-normal sodium hydroxide solution ar,r lulded to the distillate and tho excess of alkali determined by lack-titralina. 

When the normal sodium bisulphite compound is dissolved in water and submitted to steam distillation, half of the citral passes over, the remainder being converted into the sodium salt of the so-called stable citraldihydrodisulfonic acid —... 

Ester found in 5 less the amount of ester equivalent to the volume of deci-normal sodium hydroxide used up in the blank experiment. 

Isolation of Inosine by Ion Exchange Method Half of the above clear centrifugate (1.15 liters) is treated with 250 cc of anion exchange (bicarbonate form) and stirred together therewith for 16 hours at room temperature. The pH value is increased thereby to about 4 to 5. The ion exchanger is filtered off under suction and washed 3 times, each time with 150 cc of water. The solution is brought to a pH value of 7 by means of normal sodium hydroxide (total volume of the solution about 1.55 liters), and concentrated to a volume of about 100 cc under vacuum. 

The pH of the medium is adjusted with 10-normal sodium hydroxide solution to pH 7.5. 

To a solution of 130 g. (0.6 mole) of arsanilic acid (Org. Syn. 3, 13) in 600 cc. (0.6 mole) of normal sodium hydroxide is added 52 g. (0.62 mole) of sodium bicarbonate and 70 g. (0.75 mole) of chloroacetamide (Org. Syn. 7, 16). The mixture is heated 011 a water bath to 90-1000 and a steady evolution of carbon dioxide occurs. At the end of two hours, when gas evolution has practically ceased, the mixture is cooled to 40° C., stirred vigorously and 150 cc. of 1 1 hydrochloric acid poured in rapidly. /i-Arsonophenylglycinamide crystallizes at once and, after cooling to room temperature, is filtered by suction and washed once with 2 per cent hydrochloric acid (Note 1), then with cold water. The crude product thus obtained is contaminated with some arsanilic acid and possibly other products. These are removed during purification. The crude product is suspended in about 400 cc. of water and with vigorous stirring, treated carefully with 25 per cent aqueous sodium hydroxide until solution is just complete. At this point the mixture is still acid to litmus and an excess of sodium hydroxide is to be avoided to prevent decomposition of the product. About 15 g. of boneblack... 

A venturi meter with a 50 mm throat is used to measure a flow of slightly salty water in a pipe of inside diameter 100 mm. The meter is checked by adding 20 cm3/s of normal sodium chloride solution above the meter and analysing a sample of water downstream from the meter. Before addition of the salt, 1000 cm- of water requires 10 cm3 of 0.1 M silver nitrate solution in a titration. 1000 cm3 of the downstream sample required 23.5 cm3 of 0.1 M silver nitrate. If a mercury-under-water manometer connected to the meter gives a reading of 20S mm, what is the discharge coefficient of the meter Assume that the density of the liquid is not appreciably affected by the salt. 

From this equation we can calculate the actual crystal radius (for use in normal sodium chloride type crystals) from Ru the univalent crystal radius. A knowledge of the repulsion exponent n is needed, however. This can be derived from the experimental measurement of the compressibility of crystals. Bom11 and Herzfeld,12 give the values in Table III, obtained in this way. 

Monitor the following serial laboratories for comparison to baseline values every 6 hours in the first 24 hours and daily thereafter until normalized sodium, serum creatinine, blood urea nitrogen, serum lactate, glucose, bilirubin, hemoglobin, hematocrit, platelets, prothrombin time, partial thromboplastin time, arterial blood gases, and pH. 

For the synthesis of amino acids, the reaction of an a-haloalkyl boronic ester 4 with sodium azide and a phase-transfer catalyst in dichloromethane/water requires a large excess of azide in order to form the a-azidoalkyl boronic ester 5 with only 1-2% epimer34. With the exception of R1 = benzyl, where epimerization of 4 is relatively rapid, bromoalkyl boronic esters are preferred. Chloroalkyl boronic esters react so slowly that the azide and dichloromethane may generate hazardously explosive diazidomethane65,66. Chain extension of 5 to 6 proceeds normally. Sodium chlorite, which is known to oxidize aldehydes to carboxylic acids67-69, also oxidizes a-chloroalkyl boronic esters to carboxylic acids34. The azido acid is hydrogenated to the amino acid. 

To a solution of 122 g. of pure salicylaldehyde (Note 1) in 1000 cc. of normal sodium hydroxide solution at room temperature, is added 1420 g. of 3 per cent hydrogen peroxide. The mixture darkens slightly in color and the temperature rises to 45-50°. The solution is allowed to stand for fifteen to twenty hours, whereupon a few drops of acetic acid are added in order to neutralize any excess alkali, and the solution evaporated to complete dryness on the water bath under reduced pressure. 

By heating sulphuric acid with sodium hydrosulphate between 200° and 300 , G. F. Brindley 30 obtained crystals of sodinm trihydro-disulphate, NaH3(S04)2 and C, Schultz, by cooling a soln. of normal sodium sulphate in nearly seven times... 

J. J. Watts and W. A. Richards patented the preparation of this salt by removing the proper quantity of carbon dioxide from sodium hydrocarbonate by adding sodium hydroxide, sodium carbonate, or the hydroxides of the alkaline earths, and crystallizing the soln. at about 35° C. Winkler obtained it from carbonated liquor of the ammonia-soda process and T. M. Chatard by the spontaneous evaporation of soln. of normal sodium carbonate which had been exposed to the air some time and thereby absorbed carbon dioxide. There is a fairly general agreement that a temp, below 35° is not favourable to the formation of trona and that the crystals develop better in sodium chloride soln. and excess of the normal carbonate also favours the formation of trona. J. J. Watts and W. A. Richards say that if an excess of the hydrocarbonate be used, it crystallizes out unchanged. T. M. Chatard studied the influence of the composition of the soln. on the formation of trona, and obtained the results indicated in Table LIV with soln. containing a mol. of the normal carbonate. H. N. McCoy and C. D. Test have studied the conditions under which the sesquiearbonate is formed, and their results are summarized in Fig. 73. 

Nitro-l-diazonapbtbalene, the normal sodium salt, ppt (from ale + eth), begins to decomp below 100° the isodiazo sodium salt, dk-yel ndls (from ale + eth), dec at l65°(Ref 2)... 

Quantitative Determination. — Dissolve 1 gm. of tartaric acid in 50 cc. of water, and titrate with normal sodium hydroxide solution, using phenolphthalein as indicator. 

Low-Sodium Milk (Hargrove and Alford 1974). Low-Sodium milk is available in some areas as a specialty product for consumers who require low-sodium foods. It is produced by passing normal milk over an ion-exchange resin which replaces the sodium of the milk with potassium. The normal sodium content of milk is reduced from 50 mg/100 ml to approximately 3 mg/100 ml other components of the milk remain essentially the same. 

The heat of formation of liquid arsenic trifluoride has been obtained 1 indirectly by determining the heats of dissolution of the trifluoride and of a mixture of arsenious oxide and sodium fluoride in about one litre of normal sodium hydroxide solution. The value obtained was 198,300 calories. Assuming Trouton s constant to be 21, the heat of vaporisation is about -7000 calories, so that the heat of formation of gaseous arsenic trifluoride is 191,300 calories. 

The oxidation of arsenites by oxygen in the presence of sodium hydroxide is affected by the presence of other types of catalysts (see p. 175). Thus in the presence of copper sulphate and with less alkali than corresponds with Na3As03, the velocity of oxidation is very small, but with an increased amount of sodium hydroxide present, copper hydroxide or oxide is formed and the action is accelerated, and indeed copper oxide itself may be used as catalyst.2 With an excess of sodium hydroxide and a suitable quantity of copper oxide, normal sodium arsenite may be completely oxidised to arsenate in a few hours. Similarly the presence of an excess of sodium carbonate facilitates oxidation.3... 

Aluminium Arsenates.—The orthoarsenate, A1As04, is obtained 2 in the form of elongated lens-shaped crystals when normal sodium orthoarsenate is heated with an excess of aluminium sulphate in a sealed tube at 220° C. The crystals are hexagonal in structure, with a0 = 5-030 and c0 = 5-612 A. the form is similar to that of quartz.3... 

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