Electrolytes compounds

Structures such as (26) were demonstrated [103] to he fairly easily reduced at a Pt electrode. Thus, when R = Ph, an anion radical (E° = —1.26 V vs Ag/Agl/I 0.1 M) of high stahihty is formed. However, macroelectrolyses of the compounds (26) could not he achieved at all since whatever the amount of electricity passed through the cell, the starting material was totally recovered. The compounds (26) are expected to react slowly with the tetraalky-lammonium salt R4N+ and the reaction would correspond to an indirect reduction of the electrolyte. Compounds (26), with R = primary alkyl groups, led - even in DMF-to strong self-inhibition explained by the adsorption of produced... 

The variation of a with formal concentration is shown in figure 9-2. Weak electrolytes (compounds that are only partially dissociated) dissociate more as they are diluted. o-Hydroxyben-zoic acid is more dissociated than p-hydroxybenzoic acid at the same formal concentration because the ortho isomer is a stronger acid. Box 9-2 and Demonstration 9-1 illustrate weak-acid properties. 

Overpotential Departure from equilibrium (reversible) potential due to passage of a net current. Concentration overpotential results from concentration gradients adjacent to an electrode surface. Surface overpotential results from irreversibilities of electrode kinetics. Supporting (inert or indifferent) electrolyte Compounds that increase the ionic conductivity of the electrolyte but do not participate in the electrode reaction. 

Electrolyte — Compounds that dissociate (- dissociation) into -> ions upon dissolution in -> solvents or/and upon melting and which provide by this the - ionic conductivity. Also, compounds that possess in the solid state a rather high ionic conductivity are called - solid electrolytes. - True electrolytes are those which are build up of ions in the solid state (or pure form), whereas potential electrolytes are those which form ions only... 

Weak acids and bases ionize only slightly in aqueous solution. Because their solutions conduct electricity poorly, they are called weak electrolytes. Compounds whose solutions do not conduct electricity at all are called non-electrolytes. An outline of the electrolytic properties of compounds is presented in Table 9.2. 

Thus, compounds must be both soluble and ionic to be written in the form of their separate ions. A listing of water-soluble compounds was given in Table 8.3. In addition to the compounds listed there, all strong acids are water soluble. In summary strong electrolytes—compounds that dissociate or ionize extensively in aqueous solution—include the following ... 

Electrolyte—Compounds that ionize in a solution electrolytes dissolved in the blood play an important role in maintaining the proper functioning of the body. 

Citrate compounds are salting-out electrolytes — they tie up water molecules in the liquid and as a result help force the formation of liquid crystals or lamellar stmctures. It is sometimes possible to reverse this trend by the addition of salting-in electrolytes, compounds with high lyotropic numbers (>9.5) which can raise the cloud point of a liquid formulation [26], This permits increased concentration without the onset of structuring. 

The coUigative properties of electrolytes require a slightly different approach than the one used for the coUigative properties of nonelectrolytes. The reason is that electrolytes dissociate into ions in solution, and so one unit of an electrolyte compound separates into two or more particles when it dissolves. (Remember, it is the number of solute particles that determines the coUigative properties of a solution.) For example, each unit of NaCl dissociates into two ions—Na and Cl. Thus the coUigative properties of a 0.1 m solution of NaCl should be twice as great as those of a 0.1 m solution con-... 

Intercalation of poly(ethylene oxide) into a lithium-ion exchanged clay gives an interesting class of layered silicate nanocomposites that are lithium-ion electrolytes. Compounds have been prepared by intercalation from methanol/water solutions and by melt intercalation. Melt intercalation typically gives samples with higher polymer contents than the solution method and with higher lithium-ion conductivity though the conductivity is probably still too low for practical applications. 

Table II shows the mean-force potentials for a dilute solution of the electrolyte compound Y =...

Emf measurements yield reliable standard potentials only when data analysis uses well-founded extrapolation methods which take into luxoimt association of the electrolyte compounds A knowledge of reliable standard potentials is important for electrochemistry in non-aqueous solutions, especially for solvation studies and technological investigations. A comprehensive survey of these questions is in preparation. Data analysis with the help of Eqs. (28) gives and R values which are compatible with those from other methcKls. Table V illustrates the satisfactory agreement of activity coefficients from emf measurements, y (emO, and heats of dilution, y (4>H ), both evaluated by appropriate methods. 

Ion solvation is the transfer process of the separated ions of a pure electrolyte compound Y from the vacuum to the infinitely dilute solution in a solvent S. In the case of ionophoric electrolytes the solvation quantities are related to... 

Table VI shows the limiting anion conductances determined from the measurements underlying Fig. 5. Extrapolations were made by taking into account the association of the electrolyte compounds KSCN and Mc4NSCN in methanol via Eqs. (37). As a result, the theoretical requirement of equal limiting anion conductances is fulfilled within the limits of experimental error.

The ions and ion pairs of an electrolyte compound Y = which is involved in... 

A perusal of recent literature shows an increasing interest in technical applications and applied research based on non-aqueous electrolyte properties. The assortment of solvents with widely varying properties, an almost unlimited number of solvent mixtures and soluble electrolyte compounds provides flexibility in tackling a given problem. The unique properties of non-aqueous solutions can be the key in solving special technical problems. 

In principle, the dissociation of electrolytes obeys to the law of mass actions as described in Chapter 12 for conventional chemical reactions. For evaluation, the Gibbs energies of formation of the compounds involved are needed. For some of the most important electrolyte compounds, they are listed in Appendix D. 

Standard Thermodynamic Properties for Selected Electrolyte Compounds... 

Electrochemistry uses mean composition variables based on the mole numbers of the ions in the solution produced by the electrolyte compounds that are the solutes. 

Born process Hypothetical process for calculating the energy of transfer of an electrolyte compound from a vacuum into a solvent where the electrolyte exhibits complete dissociation into ions. 

ELECTROLYTE SOLUTIONS are solutions of electrolyte compounds in pure or mixed solvents such that the solutions become electric conductors in which current is carried by the movement of ions. They exhibit specific properties due to the more or less complete dissociation of their solutes into ions. Aqueous electrolyte solutions are involved in numerous biological, biochemical, geological, and technical processes. Nonaqueous electrolyte solutions are intensively studied owing to unique properties for their application in various new technologies such as high-energy batteries, electrodeposition, nonemissive displays, solar cells, phase-transfer catalysis, or electroor-ganic synthesis. 

The molar quantity AsoiZ corresponds to the transfer of 1 mol of electrolyte compound from its pure state to... 

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