Inert salts

The ernes of ionic surfactants are usually depressed by tire addition of inert salts. Electrostatic repulsion between headgroups is screened by tire added electrolyte. This screening effectively makes tire surfactants more hydrophobic and tliis increased hydrophobicity induces micellization at lower concentrations. A linear free energy relationship expressing such a salt effect is given by ... 

Hydrogenation. Hydrogenation is one of the oldest and most widely used appHcations for supported catalysts, and much has been written in this field (55—57). Metals useflil in hydrogenation include cobalt, copper, nickel, palladium, platinum, rhenium, rhodium, mthenium, and silver, and there are numerous catalysts available for various specific appHcations. Most hydrogenation catalysts rely on extremely fine dispersions of the active metal on activated carbon, alumina, siHca-alumina, 2eoHtes, kieselguhr, or inert salts, such as barium sulfate. 

The rate of a reaction that shows specific acid (or base, or acid-base) catalysis does not depend on the buffer chosen to adjust the pH. Of course, an inert salt must be used to maintain constant ionic strength so that kinetic salt effects do not distort the pH profile. 

To consider the convective mass transfer problem of a rotating hemisphere electrode, we assume that sufficient inert salts are present in the electrolyte that the migrational... 

The competition between ion-pair and radical-pair collapse can be predictably modulated by the polarity of the solvent and by the addition of inert salt. 

Such competition between ion-pair collapse of MT+, C(N02)f and the radical-pair collapse of MT+, NO is also readily modulated by the addition of inert salt.14 The description of the solvent and salt effects in equations (82) and (83) is further confirmed by direct kinetics analysis of the decay of the cation radical MT+ on the nanosecond/microsecond timescale. 

The explanation for the dichotomy between aromatic nitration versus de-alkylative oxidation in equation (84) lies in the dynamics of ion-radical triad (which is predictably modulated by solvent polarity and added inert salt). For example, the nonpolar dichloromethane favors aromatic nitration via a radical-pair collapse of ArH+, NO, 239 i.e.,... 

The application of the concept of a reactive-ion micelle is illustrated by addition of cyanide ion to N-alkylpyridinium ions (Fig. 3) and rate constants are compared in Table 4. Second-order rate constants are essentially independent of substrate hydrophobicity and are only slightly affected by added inert salts. They are also very similar to second-order rate constants in water. 

In equilibrium analysis studies carried out in the presence of an inert salt (medium salt NX) and small (trace) concentrations of the reactants, only the terms involving have to be considered in Eq. (6.33), while those involving can be neglected. Nevertheless, as the main difficulty... 

Gap Sensitivity. Blends of NG 15 and inert salt 85% (the latter sifted first thru 20 mesh/sq cm screen) were packed in two identical 30—32mtn diam paper tubes, and placed end-to-end on dry sand a definite distance apart. Detonation of... 

Dubnov [53] also describes experiments which prove that the activity of an inert salt increases with its fineness (Table 104). The figures in the Table refer to sodium chloride. An explosive charge containing 35 or 40% sodium chloride was detonated in a methane-air mixture. 

Content of inert salt % Charge limit 8 Lead block expansion cm3 Heat of detonation kcal/kg Calculated temperature °C ... 

Studies of sensitization of inert salts (such as NaCl, Amm sulfate and Amm chloride) used in safety expls by HE s (such as NG, DEGcDN, RDX PETN) were described. 

Dynamit 4 (Get). NG 36.0—39.5, NC (from surplus smokeless propint) 0.5—4, alkali nitrate and/or K perchlorate 40—50, vegetable meal and/or solid hydrocarbons 1—7 inorganic inert salts 7—12%... 

Figure 8-1, Demonstration 8-1, and Color Plate 3 show that the concentration quotient in Equation 8-1 decreases if you add the inert salt KN03 to the solution. That is, the equilibrium constant is not really constant. This chapter explains why concentrations are replaced by activities in the equilibrium constant and how activities are used.

Addition of an inert salt increases the solubility of an ionic compound. 

Electrodes respond to the activity of uncomplexed analyte ion. Therefore, ligands must be absent or masked. Because we usually wish to know concentrations, not activities, an inert salt is often used to bring all standards and samples to a high, constant ionic strength. If activity coefficients are constant, the electrode potential gives concentrations directly. 

To determine the concentration of a dilute analyte with an ion-selective electrode, why do we use standards with a constant, high concentration of an inert salt ... 

The simplest method to lower the temp of expln is to incorporate in the formulation an addnl amt of an inert salt, such as NaCl,... 

Unfortunately, liquid ammonia possesses a very intense absorption band at 15,320 A. (2 i and/or 2vz) so that this region is inaccessible for quantitative measurements even with a 1 mm. cell. If ND8 is used as the solvent instead of NH8, no intense overtone or combination bands of the solvent occur in the spectral region of interest (Figure 1). The spectra of dilute solutions of lithium, sodium, potassium, calcium, and barium in liquid ND8, and the perturbations arising from concentration changes, temperature changes, and the presence of inert salts have been investigated. 

B Rate coefficients for these reactions have been shown to be increased in value on addition of inert salts. 

Co-solvent effects are generally more difficult to interpret than are kinetic salt effects, largely because the addition of a new solvent produces much more violent changes in the reaction medium than does addition of an inert salt. The mechanism of substitution may therefore be affected by addition of a co-solvent this is es-picially true of reactions proceeding by mechanism SE2, where the SE2(open) and SE2(cyclic) transition states may be regarded as the two extremes of a whole range of transition states. 

In this particular case, it is known that the substitution in methanol itself is accelerated by the addition of inert salts, and hence that mechanism SE2(open) probably obtains in solvent methanol. The most reasonable interpretation of the co-solvent effect is, therefore, that mechanism SE2(open) obtains in all four reaction media, and that the transition state is stabilised relative to the reactants in the more aqueous media. 

It would be expected39 that in the ionisation of a neutral substrate, the addition of inert salts should produce considerable rate accelerations. In the race-misation of ( —)-a-carbethoxybenzylmercuric bromide by mechanism SE1 in solvent dimethylsulphoxide, however, the addition of inert salts was found to result in either rate acceleration (e.g. with LiN03) or retardation (e.g. with LiC104)43. 

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