Conversion constants for redox potentials measured versus different reference electrodes in acetonitrile solutions at 25°C

The electrophilic properties of 34 solvents have been characterized by the Acceptor Number (AN) which has been derived from31P-n.m.r. measurements of triethylphosphine oxide dissolved in the respective solvents. Relationships are found between the acceptor numbers and theZ-values,E
T-values andY-values, as well as the free energies of solvation of anions and the redox potentials of the hexacyanoferrate(III)—hexacyanoferrrate(II) system in different solvents. The new parameter provides—together with the donor number—a useful guide in choosing the most appropriate solvent for a given reaction.

The acceptor number — A quantitative empirical parameter for the electrophilic properties of solvents

Empirical parameters for donor and acceptor properties of solvents

The division of thermodynamic solvation free energies of electrolytes into contributions from individual ionic constituents is conventionally accomplished by using the single-ion solvation free energy of one reference ion, conventionally the proton, to set the single-ion scales. Thus, the determination of the free energy of solvation of the proton in various solvents is a fundamental issue of central importance in solution chemistry. In the present article, relative solvation free energies of ions and ion−solvent clusters in methanol, acetonitrile, and dimethyl sulfoxide (DMSO) have been determined using a combination of experimental and theoretical gas-phase free energies of formation, solution-phase reduction potentials and acid dissociation constants, and gas-phase clustering free energies. Applying the cluster pair approximation to differences between these relative solvation free energies leads to values of −263.5, −260.2, and −273.3 kcal/mol for the absolute solvation free energy of the proton in me...

/pdf/single-ion-solvation-free-energies-and-the-normal-hydrogen-26dyitnfeg.pdf

Single-Ion Solvation Free Energies and the Normal Hydrogen Electrode Potential in Methanol, Acetonitrile, and Dimethyl Sulfoxide

Application of macrocyclic compounds in chemical analysis

Solvation of ions. XVI. Solvent activity coefficients of single ions. Recommended extrathermodynamic assumption

Cuprous hydrometallurgy: Part II. The electrowinning of copper from cuprous sulphate solutions containing organic nitriles

Copper is processed via solutions of copper salts, both cupric and cuprous, in acidified aqueous solutions containing organic nitriles. Methods of producting solutions of cuprous salts include reduction of cupric salts and oxidation of copper and copper sulphides. Solutions of cuprous salts are thermally or electrochemically disproportionated to produce copper and solutions of cupric salts.

Method of producing copper and composition therefor

Method of preparing cuprous sulfate and bisulfate solutions from materials containing copper and impurities by a leaching process are disclosed The leaching composition contains sulfuric acid, cupric ions, water and an organic nitrile The leaching composition may be used with copper sulfide ores in particulate form The cuprous solutions resulting from the leaching can be treated by disproportionation methods to recover pure copper

Method of producing cuprous sulfate and bisulfate solutions

Cuprous hydrometallurgy: Part I. Electrorefining copper via acidic solutions of cuprous sulphate containing organic nitriles

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