Specific gravity hydrochloric acid

Ethyl Benzoate.—This ester has not been found, so far, to occur naturally in essential oils. It has, however, been prepared by synthetic processes, for example, by condensing ethyl alcohol with benzoic acid by means of dry hydrochloric acid gas. Its odour is very similar to that of methyl benzoate (q.v.), but not quite so strong. It is an oil of specific gravity I OfilO, refractive index 1 5055, and boiling-point 213° at 745 mm. It is soluble in two volumes of 70 per cent, alcohol. 

Ethyl Cinnamate.—The cinnamic ester of ethyl alcohol is a natural constituent of a few essential oils, including camphor oil and storax. It is formed synthetically by condensing cinnamic acid and ethyl alcohol by dry hydrochloric acid gas. It has a soft and sweet odour, and is particularly suitable for blending in soap perfumes. It is an oil at ordinary temperatures, melting at 12°, and boiling at 271°. Its specific gravity is 1 0546, and its refractive index 1 5590. 

The label on a bottle of concentrated hydrochloric acid. The label gives the mass percent of HCI in the solution (known as the assay] and the density (or specific gravity) of the solution. The molality, molarity, and mole fraction of HCI in the solution can be calculated from this information. 

Mix 400 mL of pure concentrated hydrochloric acid with 250-400 mL of distilled water so that the specific gravity of the resultant acid is 1.10 (test with a hydrometer). Insert a thermometer in the neck of a 1 L Pyrex distillation flask so that the bulb is just opposite the side tube, and attach a condenser to the side tube use an all-glass apparatus. Place 500 mL of the diluted acid in the flask, distil the liquid at a rate of about 3-4 mL min-1 and collect the distillate in a small Pyrex flask. From time to time pour the distillate into a 500 mL measuring cylinder. When 375 mL has been collected in the measuring cylinder, collect a further 50 mL in the small Pyrex flask watch the thermometer to see that the temperature remains constant. Remove the receiver and stopper it this contains the pure constant boiling point acid. Note the barometric pressure to the nearest millimetre at intervals during the distillation and take the mean value. Interpolate the concentration of the acid from Table 10.5. 

Hydrochloric acid is to be obtained in the cheapest form possible. This is as 18 Baume acid, which is 27.9% hydrochloric acid (specific gravity =1.142). The material will be shipped by 8,000 gal tank truck from a site less than 200 miles away. 

Nickel was first isolated in 1751, and a relatively pure metal was prepared in 1804. In nature, nickel is found primarily as oxide and sulfide ores (USPHS 1977). It has high electrical and thermal conductivities and is resistant to corrosion at environmental temperatures between -20°C and +30°C (Chau and Kulikovsky-Cordeiro 1995). Nickel, also known as carbonyl nickel powder or C.I. No. 77775, has a CAS number of 7440-02-0. Metallic nickel is a hard, lustrous, silvery white metal with a specific gravity of 8.9, a melting point of about 1455°C, and a boiling point at about 2732°C. It is insoluble in water and ammonium hydroxide, soluble in dilute nitric acid or aqua regia, and slightly soluble in hydrochloric and sulfuric acid. Nickel has an atomic weight of 58.71. Nickel is... 

A pharmacist mixes 100 mL of 35% (w/w) hydrochloric acid with enough purified water to make 400 mL. If the specific gravity of hydrochloric acid is 1.20, calculate the percentage strength (w/v) of the final solution. 

Commercial grade, concentrated hydrochloric acid is about 37.5% HCl by weight and has a normality of 12 and specific gravity 1.19. 

How many volumes of a 37% hydrochloric acid (starting concentration Si HCl = [HCl] = 37%) have to be mixed with volumes of water (starting concentration S2 [HCl] = 0%) to get a 10% hydrochloric acid (It is more precise to take the densities instead of concentrations, especially when there is a high difference in specific gravity as shown in this example.)... 

Sodium iodate dissolves copiously in warm dil. sulphuric acid without decomposition but it is decomposed by hydrochloric acid. The presence of potassium iodide causes potassium iodate to dissolve more readily than in pure water and although A. Ditte says that a double salt is not obtained from the soln., yet the phenomenon is probably due to the formation of a complex salt in soln. J, N. Bronsted measured the solubility of potassium iodate in aq. soln. of potassium hydroxide. Potassium iodate does not dissolve in alcohol. According to H. L. Wheeler, 100 grms. of water at 23° dissolve 21 grms. of rubidium iodate, and 26 grms. of caesium iodate at 24°. The specific gravity of a sat. aq. soln. of lithium iodate 52 at 18° is 1 568 thesp. gr. of soln. of potassium iodate calculated by G. T. Gerlach. from P. Kremers data, are ... 

In this connection, it is well to know that the percentage of HC1 in an aqueous solution is very readily calculated from the specific gravity. The decimal portion of the latter value is multiplied by 2, and the decimal point moved two places to the right. Thus, if the specific gravity is 1.166, the solution will contain 166 X 2 = 33.2 per cent HC1 by weight. A simple calculation will therefore enable the student to determine the weight of hydrochloric acid to be added of any convenient density, in order to supply the requisite water. 

To obtain the gold in a perfectly pure stats, however, the precipitated powder is boiled with hydrochloric acid of specific gravity 1 1, which is then decanted, and the resides is boiled twice with fresh acid. The gold is not washed between these successive treatments with add, which remove the last traces of iron, and nearly all tlie chloride of silver,... 

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