THE SULPHURIC ACID SOLVENT SYSTEM: PART II. CONDUCTIVITY MEASUREMENTS ON SOLUTIONS OF SOME ACIDS

1961 ◽  
Vol 39 (6) ◽  
pp. 1266-1273 ◽  
Author(s):  
J. Barr ◽  
R. J. Gillespie ◽  
E. A. Robinson
Keyword(s):  
Dissociation Constant ◽  
Sulphuric Acid ◽  
Dissociation Constants ◽  
Solvent System ◽  
Acid Dissociation ◽  
Acid System ◽  
Conductivity Measurements ◽  
Acid Dissociation Constants ◽  
Strong Base ◽  
System Part

Conductivity measurements have been made on solutions of the following substances in sulphuric acid: HClO4, HSO3F, HSO3Cl, HPO2F2, HAs(HSO4)4, CH3SO3H, and CF3CO2H. Of these substances HSO3F, HSO3Cl, HAs(HSO4)4, and probably HClO4, behave as acids, CF3CO2H is a non-electrolyte, and HPO2F2, and probably CH3SO3H, are bases of the sulphuric acid system. Acid dissociation constants for HSO3F, HSO3Cl, and HAs(HSO4)4 have been determined by comparing the conductivities of their solutions with those of H2S2O7, whose dissociation constant is known from other measurements, and also by conductimetric titration with a strong base, e.g. KHSO4. These acids of the sulphuric acid system decrease in strength in the order HSO3F > HAs(HSO4)4 > HSO3Cl > HClO4.

THE SULPHURIC ACID SOLVENT SYSTEM: PART I. ACID-BASE REACTIONS

1960 ◽  
Vol 38 (8) ◽  
pp. 1363-1370 ◽  
Author(s):  
R. H. Flowers ◽  
R. J. Gillespie ◽  
E. A. Robinson
Keyword(s):  
Electrical Conductivity ◽  
Sulphuric Acid ◽  
Dissociation Constants ◽  
Solvent System ◽  
Conductivity Measurements ◽  
Acid Base ◽  
Acid And Base ◽  
System Part ◽  
Acids And Bases ◽  
Good Agreement

Acid–base reactions in the solvent sulphuric acid are discussed. Such reactions are conveniently studied by electrical conductivity measurements. A relation between the composition at which the conductivity has a minimum value and the strengths of the acid and base is derived. Values of the dissociation constants of acids and bases obtained in this way are shown to be in good agreement with values obtained by other methods.

The trifluoroacetic acid solvent system. Part V. Cryoscopic measurements

1976 ◽  
Vol 54 (19) ◽  
pp. 3031-3037 ◽  
Author(s):  
Michael G. Harriss ◽  
John B. Milne
Keyword(s):  
Trifluoroacetic Acid ◽  
Dissociation Constants ◽  
Freezing Point ◽  
Solvent System ◽  
Ion Pair ◽  
Conductivity Measurements ◽  
Cast Doubt ◽  
System Part ◽  
Triple Ions ◽  
Cryoscopic Constant

Measurement of freezing point depressions for the non-electrolytes, CCl4. CH3SO2F, and (CF3CO)2O permit calculation of the cryoscopic constant for trifluoroacetic acid, HOTFA. Water is shown to give freezing point depressions lower than those for non-electrolytes and this is attributed to association. Freezing point depressions for NaOTFA, KOTFA, and CsOTFA have been measured and accounted for in terms of ion-pair dissociation constants previously determined from electrical conductivity measurements. The results cast doubt on the existence of triple ions in this solvent.

Re-examination of the Kirkwood–Westheimer theory of electrostatic effects. III. Dissociation constants of cis-3- and trans-4-substituted cyclohexanecarboxylic acids in water–dimethyl sulfoxide mixtures

1978 ◽  
Vol 56 (8) ◽  
pp. 1130-1133 ◽  
Author(s):  
Jitka Kirchnerova ◽  
Patrick G. Farrell ◽  
John T. Edward ◽  
Jean-Claude Halle ◽  
Robert Schaal
Keyword(s):  
Dimethyl Sulfoxide ◽  
Dissociation Constant ◽  
Dissociation Constants ◽  
Solvent Composition ◽  
Potentiometric Method ◽  
Acid Dissociation ◽  
Electrostatic Effects ◽  
Acid Dissociation Constants ◽  
Cyclohexanecarboxylic Acid

Acid dissociation constants of two cis-3- and of four trans-4-substituted cyclohexanecarboxylic acids in water – dimethyl sulfoxide mixtures of varying composition were determined by a potentiometric method. Results have been analyzed according to the model of Kirkwood and Westheimer, and shown to differ from calculated values because of certain oversimplifications built into the model. Dissociation constant differences between cyclohexanecarboxylic acid and the compounds studied vary only slightly with changing solvent composition.

THE SULPHURIC ACID SOLVENT SYSTEM: PART VI. THE BASICITIES OF COMPOUNDS CONTAINING SULPHUR–OXYGEN BONDS

1964 ◽  
Vol 42 (5) ◽  
pp. 1113-1122 ◽  
Author(s):  
S. K. Hall ◽  
E. A. Robinson
Keyword(s):  
Nitrogen Atom ◽  
Sulphuric Acid ◽  
Solvent System ◽  
Dimethyl Sulphoxide ◽  
Strong Base ◽  
Weak Bases ◽  
System Part ◽  
Sulphur Trioxide ◽  
Basic Behavior

Cryoscopic and conductimetric studies of a variety of compounds containing S—O bonds have shown that dimethyl sulphoxide behaves as a strong base in sulphuric acid whereas dialkyl sulphones behave as weak bases. In contrast diaryl sulphones and aryl sulphonic acids behave as non-electrolytes.A correlation is established between the basicities of the alkyl sulphones, H2SO4, and the HSO4− ion, and their sulphur–oxygen stretching frequencies. This relation is used to predict the basicities of other compounds containing S—O bonds. In particular it is shown that the basicity of monomeric sulphur trioxide is similar to that of sulphuric acid, and sulphamide is shown to behave as a strong base in sulphuric acid, which implies protonation on a nitrogen atom rather than on oxygen, since the S—O stretching frequencies indicate only weakly basic behavior for O-protonation.

scholarly journals Acid dissociation constants of tetracyanohydroxooxomolybdate(IV) ion

1973 ◽  
Vol 26 (3) ◽  
pp. 671 ◽  
Author(s):  
M Aijaz Beg ◽  
Kabir-ud-Din ◽  
RA Khan
Keyword(s):  
Hydrochloric Acid ◽  
Dissociation Constant ◽  
Titration Curve ◽  
Dissociation Constants ◽  
Acid Dissociation ◽  
Thermodynamic Quantities ◽  
Method Of Least Squares ◽  
Acid Dissociation Constants ◽  
Ph Titration ◽  
The Third

The third dissociation constant of tetracyanohydroxooxomolybdic acid, H3[MoO(OH)(CN)4], has been obtained in the temperature range 25-50�C from the pH-titration curve of its tripotassium salt against hydrochloric acid. The values of pK3 fitted an equation of Harned- Robinson type: �������������������� pK3 = (1730.72/T)-6.19+0.0308T) obtained by the method of least squares. ��� Thermodynamic quantities ΔG�, ΔH�, ΔS�, and ΔC�p for the process have been evaluated at 30�C.

THE COPPER(II) SYN-PHENYL-2-PYRIDYL KETOXIME SYSTEM PART I

1965 ◽  
Vol 43 (1) ◽  
pp. 64-74 ◽  
Author(s):  
T. L. Meek ◽  
G. E. Cheney
Keyword(s):  
Metal Ions ◽  
Dissociation Constants ◽  
Acid Dissociation ◽  
Geometric Isomers ◽  
Copper Chelate ◽  
Acid Dissociation Constants ◽  
System Part

A survey has been made of the reactions of both geometric isomers of phenyl-2-pyridyl ketoxime with metal ions. The complexes of copper(II) with the syn-phenyl isomer have been investigated. Acid dissociation constants of both geometric isomers, and of the 2:1 copper chelate of the syn-phenyl oxime have been determined.

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