Bases concentration

Sulfates. Indium metal and its oxides dissolve in warm sulfuric acid to give a solution of the trisulfate [13464-82-9], In2(S0 2- It is a white, crystalline, deUquescent soHd, readily soluble in water that forms double salts with alkaLi sulfates and some organic substituted ammonium bases. Concentration of the acidified trisulfate solution produces indium acid sulfate crystal [57344-73-7], In(HS0 2> other reaction conditions give basic sulfates. [Pg.81]

OU- and water-resistant treatments have been reported which iavolve blends of fluoropolymers and alkoxysUane or alkoxysUoxane materials, dehvered as 100% actives (90) or from solvent or emulsion (91), fluotinated alkoxysUoxane emulsions (92), and self-emulsifying fluotinated alkoxysUane-based concentrates (93). [Pg.311]

Bismuth trioxide is practically insoluble in water it is definitely a basic oxide and hence dissolves in acids to form salts. Acidic properties are just barely detectable, eg, its solubiUty slightly increases with increasing base concentration, presumably because of the formation of bismuthate(III) ions, such as Bi(OH) g and related species. [Pg.130]

One 1-ml aliquot is added to 1.0 ml of freshly-distilled 1,2-dibromo-ethane (bp 132°C) in an oven-dried flask which contains a static atmosphere of nitrogen or argon. After the resulting solution has been allowed to stand at 25°C for 5 min, it Is diluted with 10 rat of water and titrated for base content (residual base) to a phenolphthalein endpoint with standard 0.100 M hydrochloric acid. The second 1-mL aliquot is added cautiously to 10 ml of water and then titrated for base content (total base) to a phenol phthalein endpoint with standard aqueous 0.100 M hydrochloric acid. The methyllithium concentration is the difference between the total base and residual base concentrations.2 Alternatively, the methynithiura concentration may be determined by titration with a standard solution of sec-butyl alcohol employing 2,2 -bipyridyl as an indicator. [Pg.105]

SO that a plot of k against the conjugate base concentration yields as the slope this plot is shown in Fig. 6-6, where it is seen that the slopes are essentially the same at the three pH values. [Pg.270]

The following tables give a comparison of the stability of various silyl ethers to acid, base, and TBAF. The reported half-lives vary as a function of environment and acid or base concentration, but they help define the relative stabilities of these silyl groups. [Pg.138]

Fig. 2-13. The effect of acid and base concentration on the resolution of propranolol on teicoplanin CSP (250 x 4.6 mm) in the new polar organic mode. The flow rate was 2.0 mL min at ambient temperature (23 °C).

An example of the effect of acid and base concentration on the separation of propranolol is shown in Fig. 2-13. In this case, the baseline separation is achieved by adjusting the concentration without changing the acid/base ratio. [Pg.48]

Hartshorn and Ridd48 showed that there is a negligible solvent isotope effect on nitrating anilinium ions in sulphuric acid and deuterated sulphuric acid (cf. an earlier less accurate determination by Brickman and Ridd48). The absence of a solvent isotope effect also argues against reaction on the free base because the free base concentration would be lower by a factor of about four in the deuterium-containing medium. Consequently, the differences in the rate coefficients in Table 6... [Pg.25]

The log rate versus acid strength curve for the latter compound is of the exact form expected for reactions of the free base, whilst that of the former compound is intermediate between this form and that obtained for the nitration of aniline and phenyltrimethylammonium ion, i.e. compounds which react as positive species. That these compounds react mainly or entirely via the free base is also indicated by the comparison of the rate coefficients in Table 8 with those in Table 5, from which it can be seen that the nitro substituent here only deactivates weakly, whilst the chloro substitutent appears to activate. In addition, both compounds show a solvent isotope effect (Table 9), the rate coefficients being lower for the deuterium-containing media, as expected since the free base concentration will be lower in these. [Pg.27]

Some diazonium couplings are subject to base catalysis and in these cases kinetic isotope effects are observed but since the rate of catalysed reaction is not linearly related to the base concentration (see p. 7), the SE3 mechanism is ruled out and the Se2 mechanism must operate, viz. [Pg.53]

A higher base concentration or substitution of one or two gas-dispersion tubes leads to clogging of the inlet to the trap. [Pg.18]

Solutions containing approximately 1.6JH butyllithium in hexane were purchased either from Alfa Inorganics, Inc., or from Foote Mineral Company, The concentration of butyllithium in these solutions can be determined either by a double titration procedure2 or by dilution with anhydrous tetrahydro furan followed by titration with 2-butanol in the presence of a 2,2 -bipyridyl indicator.3 In either ease the total base concentration in the reagent is determined by titration with standard aqueous acid. [Pg.124]

NaOMe solutions, no correlation was found between reaction rates and either or stoichiometric base concentration but where the rates were successfully correlated by a linear free energy equation similar to those given above. [Pg.336]

If the hydride ion comes from 39, the final step is a rapid proton transfer. In the other case, the acid salt is formed directly, and the alkoxide ion acquires a proton from the solvent. Evidence for this mechanism is (1) The reaction can be first order in base and second order in substrate (thus going through 39) or, at higher base concentrations, second order in each (going through 40) and (2) when the reaction was run in D2O, the recovered alcohol contained no a deuterium, indicating that the hydrogen comes from another mole of aldehyde and not from the medium. [Pg.1565]

As we have already seen, base concentrations around 10 M are common. This concentration is a bit lower but still in the range that we would expect for laboratory solutions. [Pg.246]

Each concentration measure is convenient for some types of calculations but inconvenient for others. Consequently, a chemist may need to convert a concentration from one measure to another. Example illustrates the conversion from a mass-based concentration, percent by mass, to a mole-based concentration, molality. Mole... [Pg.832]

To convert between molarity and the other mole-based concentration measures, we must relate volume to mass and number of moles. Whereas molar mass lets us convert between mass and moles, we need density to convert... [Pg.833]

In a first set of experiments, the impact of the sodium hydroxide concentration (0.1, 1.0, 2.0 M) and gas-flow direction (co-current, counter-flow) was analysed (50 ml h liquid flow, 65 pm film thickness) [5]. The higher the base concentration, the higher is the conversion of carbon dioxide. For aU concentrations, complete absorption is achieved, but at different carbon dioxide contents in the gas mixture. The higher the carbon dioxide content, the higher is the gas flow velocity and the larger must be the sodium hydroxide concentration for complete absorption. The gas flow direction had no significant effect on carbon dioxide absorption as the gas velocities were still low, so that no pronounced co- or counter-flow operation was realized. [Pg.640]

A local high concentration of ba.se was considered to be the reason of significant amounts of by-product Q formed at low speed of rotation. At higher speed, fa.ster dispersion of the base throughout the reaction mixture would occur and local base concentrations would be decreased. This is likely to be the reason of the decrease of by-product formation with increasing rotation speed (see Fig 5.3-11). [Pg.218]

The use of a diesel-based concentrate with hydroxypropylguar gum has been evolved from the batch-mixed dry powder types [778], The application of such a concentrate reduces system requirements. Companies can benefit... [Pg.245]

Gran plot for titration of a strong acid with a strong base. If to V ml of a strong acid (concentration CA) V ml of a strong base (concentration Cb) have been added, CH + will be given by... [Pg.109]

For all the amphiprotic solvents in the pure state the cation (or acid) concentration is by definition equal to the anion (or base) concentration in other words, the pure solvent is neutral therefore, adding a solute such as HC1 makes the solution acidic, whereas a solute such as NaOH makes it basic. [Pg.249]

The authors studied, as they call it, "acid-base equilibria in glacial acetic acid however, as they worked at various ratios of indicator-base concentration to HX or B concentration, we are in fact concerned with titration data. In this connection one should realize also that in solvents with low e the apparent strength of a Bronsted acid varies with the reference base used, and vice versa. Nevertheless, in HOAc the ionization constant predominates to such an extent that overall the picture of ionization vs. dissociation remains similar irrespective of the choice of reference see the data for I and B (Py) already given, and also those for HX, which the authors obtained at 25° C with I = p-naphthol-benzein (PNB) and /f B < 0.0042, i.e., for hydrochloric acid K C1 = 1.3 102, jjrfflci 3 9. IQ-6 an jjHC1 2.8 10 9 and for p-toluenesulphonic acid Kfm° = 3 7.102( K ms 4 0.10-6) Kmt = 7 3.10-9... [Pg.279]

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