Hydrochloric acid, solution tables

The samples of crosslinked polystyrene with different divinylbenzene (DVB) contents and different particle sizes as well as the sample of uncrosslinked polystyrene as suspensions were nitrated either with nitric acid in a mixture of acetic anhydride and acetic acid according to the published procedures (8,9) or in the standard sulfuric acid medium frequently used for nitrations of benzenoid derivatives (samples 3-18, 3-20, 3-22, 3-24 as listed in Table I). The samples of the resulting nitropolystyrei were then reduced to the corresponding aminopolystyrenes using stannous chloride in hydrochloric acid solution (Table I). 

Hydrogen Chloride—Water System. Hydrogen chloride is highly soluble in water and this aqueous solution does not obey Henry s law at ah concentrations. Solubhity data are summarized in Table 5. The relationship between the pressure and vapor composition of unsaturated aqueous hydrochloric acid solutions is given in Reference 12. The vapor—Hquid equiHbria for the water—hydrogen chloride system at pressures up to 1632 kPa and at temperatures ranging from —10 to +70° C are documented in Reference 13. 

Much of the information available on resistance of nickel-iron alloys to corrosion by mineral acids is summarised by Marsh. In general, corrosion rates decrease sharply as the nickel content is increased from 0 to 30-40%, with little further improvement above this level. The value of the nickel addition is most pronounced in conditions where hydrogen evolution is the major cathodic reaction, i.e. under conditions of low aeration and agitation. Results reported by Hatfield show that the rates of attack of Fe-25Ni alloy in sulphuric and hydrochloric acid solutions, although much lower than those of mild steel, are still appreciable (Tables 3.35 and 3.36). In solutions of nitric acid, nickel-iron alloys show very high rates of corrosion. 

Table 3.50 Corrosion of Type I Ni-Resisi, casi iron and carbon steel in unaerated hydrochloric acid solutions at room temperature...

The silver reductor has a relatively low reduction potential (the Ag/AgCl electrode potential in 1M hydrochloric acid is 0.2245 volt), and consequently it is not able to effect many of the reductions which can be made with amalgamated zinc. The silver reductor is preferably used with hydrochloric acid solutions, and this is frequently an advantage. The various reductions which can be effected with the silver and the amalgamated zinc reductors are summarised in Table 10.11. ... 

Since the distribution of the chlorooxo-osmate species present in the hydrochloric acid solution that is loaded on the generator is affected by the acid concentration C5), a series of generators were prepared using a range of hydrochloric acid concentrations to dissolve the potassium osmate precipitate. The results obtained with these generators are included in Table... 

Preparation from Borax. Dissolve 12 g of borax in 25 ml of water in a beaker with heating. What is the reaction of the solution to litmus and what is it due to Write the molecular and net-ionic equations of the borax hydrolysis reaction. How can the hydrolysis of borax be facilitated Calculate what amount of a 25% hydrochloric acid solution is needed to prepare boric acid from 12 g of borax. Measure off the calculated amount of acid, and taking a small excess amount, pour the acid into the hot borax solution. Let the solution cool slowly. What substance crystallizes Filter off the crystals on a Buchner funnel, dry them between filter paper sheets, and recrystallize them from hot water, guiding yourself by the table of solubilities. Determine the product yield (in per cent). Keep the prepared boric acid for the following experiments. 

The ultraviolet absorption spectra of gemifloxacin mesylate were recorded on A Shimadzu UV-1601 PC double beam spectrophotometer with matched 1-cm quartz cells in water, methanol, 0.1 N hydrochloric acid, and 0.1 N sodium hydroxide solutions. Figure 4.1 shows the recorded absorption spectra of these solutions. The recorded spectra were essentially identical and exhibiting two peak maxima for each spectrum at 266 and 340, 272 and 342,272 and 344, and 262 and 342 nm for the solutions in water, methanol, 0.1 N hydrochloric acid and 0.1 N sodium hydroxide, respectively. The molar absorptivity of gemifloxacin mesylate was found to be moderately affected by the solvent used. The calculated molar absorptivity in water, methanol, 0.1 N hydrochloric acid, and 0.1 N sodium hydroxide solutions at the two maxima was tabulated in Table 4.1. However, the position of the maxima, as compared to water, was slightly red shifted for methanol and 0.1 N hydrochloric acid solutions and slightly blue shifted for 0.1 N sodium hydroxide solution. 

By way of example, Figure 6.2 shows a first order rate plot for the stirred contact of sodium form styrenesulfonate cation exchange resin (12% DVB) with 0.001 M hydrochloric acid solution at 25 C. The system data and calculated rate constant are given in Table 6.1. The activation energy may be found from the temperature dependence of the rate constant and was found to equal 16.7 kj eq. This same data is redeployed later according to more rigorous diffusion theory. 

Table VI Predicted rate constants and half-lives for methylparaben dissolved in dilute hydrochloric acid solution, at 25°C.

The form in which cocaine is administered is an important determinant of abuse liability (see Table 6.2). Street cocaine, which takes the form of a white powder, is produced by combining a paste made from coca leaves with a hydrochloric acid solution to form a salt—cocaine hydrochloride. Because it is a salt, street cocaine is water soluble and can be injected or taken intranasally (sniffed or snorted). Intranasal cocaine can produce intense effects, but because it causes constriction of blood vessels in the nose, absorption is slowed. By the way, it is this vasoconstriction that results in inflammation and tissue damage of the mucous membranes of the nose in chronic intranasal users. Overdo.se deaths, psychosis, and dependence are all possible consequences of intranasal cocaine but are less common than with injected cocaine. Because sniffing was the major method of administration on the street until the late 1980s, the hazards of cocaine abuse were underestimated. 

Values of/x = Ac/A may be calculated from Kohlrausch s measurements of electrical conductivity of hydrochloric acid solutions. /h and fci can be evaluated from the potentiometric measurements on hydrochloric acid solutions performed by Scatchaed. These data are very reliable since the concentration chain was so arranged as to eliminate diffusion potentials. In this way, ScATCHARD determined the mean activity coefficient V/h/ci instead of the individual ion activities. If we assume that in a potassium chloride solution/ = /ci— which is plausible when we recall that both ions have the same structure—and that fci is the same in hydrochloric acid solutions and potassium chloride solutions of the same concentration, then we can calculate/h and fci in hydrochloric acid solutions. Naturally these values are not strictly correct since the effect of the potassium ions on the activity of the chloride ions probably is different from that of the hydrogen ions at the same ionic strength. In the succeeding table are given values of /x, /h, and fci calculated by the above method. 

SvERRE Stene has measured the pH of a number of phosphate buffer mixtures, biphthalate solutions, and borate buffers with the hydrogen electrode at 150 . He found that the pH of biphthalate-hydrochloric acid solutions at 150° was about 0.2 unit greater than at 20°, the pH of biphthalate-sodium hydroxide mixtures was 0.7 greater than at 20°, while that of boric acid-borate buffers diminished with increasing temperature. Solutions of the latter system with pH s up to 9.0 were 0.5 unit less at 150°, 0.6 unit less for pH 9.2, 0.8 unit less for 9.6, and a whole unit for pH 10.0. Because certain assumptions introduced in his calculations were not entirely justified, these data must be accepted with reserve. Thus the boric acid-borate solutions behave differently from other buffers consisting of a weak acid and one of its salts. Walbum (table, page 250) also has found this diminution of pH with temperature. 

Sorensen states that the triphenylmethane dyes also show a pronounced salt error. However, metanil yellow extra (diazo-sulfonic acid indicator) is serviceable. Sorensen examined three 0.01 N hydrochloric acid solutions with methyl violet, mauveine, methyl green, and metanil yellow extra. Solution A contained only acid, B contained in addition 0.1 N KCl, whereas C was 0.3 N with respect to this salt. The pH s measured colorimetrically with each of these four indicators are compared with those determined electrometrically and with the values calculated from the nature of the three solutions. These findings are summarized in the following table. 

Kraus and Nelson, working at Oak Ridge National Laboratory in the USA, found that in aqueous hydrochloric acid solutions a number of metal ions form anionic complexes and are strongly taken up by anion-exchange resins. For most metal ions, a plot of the D value of several thousand is attained. An illustration of such plots for most of the metallic elements in the periodic table was published by Kraus and Nelson in 1956... 

Chemical Stability. The wire made from PPT(I) exhibited good chemical resistance. For example, there was no change in electrical resistance after the wire was submerged in 5% hydrochloric acid solution or gasoline at room temperature for 24 hours or was boiled in 40% sodium hydroxide solution, lubricating oil, benzene or ethyl alcohol for 24 hours. These properties are shown in Table V. 

The members of the team use the hydrochloric acid solution to standardize the sodium hydroxide solution, which in turn is used to titrate the acetic acid solution. In table 1.2 are the results of one member of each of 25 teams that participated in the competition in 1997 at the University of New South Wales, Sydney. 

Table 3.3 Current efficiency in electrodialysis of hydrochloric acid solution and electrical resistance of anion exchange membranes and composite membranesa...

Table 17.2 Activities in Aqueous Hydrochloric Acid Solutions at 25°C.

The importance of this problem is underlined by the data in Table 4 concerning the behaviour of ARMCO iron in 1 N HCl solutions inhibited with the commercial product Borg P16 at a temperature of 75 °C. Borg P16 is a specific commercial inhibitor of the corrosion of iron and carbon steels in hydrochloric acid solutions and is a derivative of the commercial product Rodine 213. This inhibitor is used both for the acid cleaning of steam generators and for pickling baths. 

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