THE CONDUCTANCES OF STRONG SOLUTIONS OF STRONG ELECTROLYTES AT 95°

1952 ◽  
Vol 30 (2) ◽  
pp. 128-134 ◽  
Author(s):  
A. N. Campbell ◽  
E. M. Kartzmark
Keyword(s):  
Silver Nitrate ◽  
Ammonium Nitrate ◽  
Strong Solutions ◽  
Partial Molar Volumes ◽  
Concentrated Solutions ◽  
Temperature Coefficients ◽  
Equivalent Conductance ◽  
Strong Electrolytes ◽  
Made In ◽  
Nitrate Solutions

Measurements of conductance and fluidity of silver nitrate and of ammonium nitrate solutions, over a range of concentration varying from 0.05  N to 14  N (silver nitrate) and from 0.08  N to 15  N (ammonium nitrate) have been made. In both cases, a maximum is observed in the specific conductances but in neither case does a minimum occur in the plot of equivalent conductance against concentration. While the equivalent conductance in very dilute solutions is proportional to [Formula: see text], in very concentrated solutions it appears to be directly proportional to C. Temperature coefficients of conductance and of fluidity are evaluated and their theoretical importance discussed. Partial molar volumes of water in these solutions are evaluated.

scholarly journals CONDUCTANCES OF STRONG SOLUTIONS OF STRONG ELECTROLYTES

1950 ◽  
Vol 28b (2) ◽  
pp. 43-55 ◽  
Author(s):  
Alan N. Campbell ◽  
Elinor M. Kartzmark
Keyword(s):  
Silver Nitrate ◽  
Ammonium Nitrate ◽  
Nitrate Solution ◽  
Strong Solutions ◽  
Silver Nitrate Solution ◽  
Weak Electrolyte ◽  
Strong Electrolytes ◽  
Conductance Ratio ◽  
Silver Nitrate Solutions ◽  
Nitrate Solutions

The conductances, densities, and viscosities of solutions of silver nitrate and of ammonium nitrate, at 25 °C., have been determined at concentrations ranging from 0.1 N to saturation (about 9 and 11 N respectively). By way of comparison, the same data have been obtained for the weak electrolyte acetic acid, up to 99.7% by weight concentration. It is shown that the weak electrolyte, at these concentrations, deviates even more from the Ostwald dilution law than do the strong electrolytes. Various attempts have been made to correct the conductance for viscosity. In addition to the older methods, two new attempts have been made, viz.; sugar was added to N/10 silver nitrate (used as the basis for these calculations) until its viscosity became equal to each of the silver nitrate solutions in turn. The conductance of a N/10 silver nitrate solution containing enough sugar to make its viscosity exactly equal to that of any given silver nitrate solution was used in the evaluation of the conductance ratio. Again, the viscosities of silver nitrate solutions at different temperatures were determined and the conductance found at the temperature at which the viscosity had become equal to that of N/10 silver nitrate at 25 °C. This conductance was used as the numerator in the conductance ratio. All attempts, however, resulted in "overcorrection", that is, in an apparently increasing equivalent conductance, with increasing concentration, after a certain concentration is reached. It is shown that a remarkable agreement exists, in the case of ammonium nitrate, with the Walden modification of the Ostwald formula.

Viscosity, electrical conductivity and density of the system ammonium nitrate-dimethyl sulphoxide

1984 ◽  
Vol 49 (5) ◽  
pp. 1109-1115
Author(s):  
Jindřich Novák ◽  
Zdeněk Kodejš ◽  
Ivo Sláma
Keyword(s):  
Electrical Conductivity ◽  
Aqueous Solutions ◽  
Ammonium Nitrate ◽  
Transport Properties ◽  
Calcium Nitrate ◽  
Dimethyl Sulphoxide ◽  
Present System ◽  
Empirical Equations ◽  
Concentrated Solutions ◽  
Nitrate Solutions

The density, viscosity, and electrical conductivity of highly concentrated solutions of ammonium nitrate in dimethyl sulphoxide have been determined over the temperature range 10-60 °C and the concentration range 7-50 mol% of the salt. The variations in the quantities as a function of temperature and concentration have been correlated by empirical equations. A comparison is made between the transport properties for the present system, aqueous solutions of ammonium nitrate, and calcium nitrate solutions in dimethyl sulphoxide.

THE NORMAL BOILING POINTS AND OTHER PHYSICAL PROPERTIES OF STRONG SOLUTIONS OF SILVER NITRATE AND OF AMMONIUM NITRATE

1950 ◽  
Vol 28b (4) ◽  
pp. 161-169 ◽  
Author(s):  
Alan N. Campbell ◽  
Elinor M. Kartzmark
Keyword(s):  
Acetic Acid ◽  
Physical Properties ◽  
Distribution Coefficient ◽  
Silver Nitrate ◽  
Ammonium Nitrate ◽  
Temperature Coefficient ◽  
Boiling Point ◽  
Strong Solutions ◽  
Normal Boiling Point ◽  
Boiling Points

The present paper is a record of certain of the physical properties of solutions of silver nitrate and of ammonium nitrate, which were made by us in connection with our work on conductance. Some of these properties were actually used in calculations, others not, but they are collected here in their entirety. The properties described are: (1) normal boiling point; (2) densities and partial molar volume of water in solution; (3) viscosities at different concentrations and temperatures, as compared with those of a typical nonelectrolyte, urea; (4) the temperature coefficient of fluidity compared with the temperature coefficient of conductance; (5) the distribution coefficient of acetic acid between ether and solutions of silver nitrate.

THE ELECTRICAL CONDUCTANCES OF AQUEOUS SOLUTIONS OF SILVER NITRATE AND OF AMMONIUM NITRATE AT THE TEMPERATURES 221.7 °C. AND 180.0 °C, RESPECTIVELY

1954 ◽  
Vol 32 (12) ◽  
pp. 1051-1060 ◽  
Author(s):  
A. N. Campbell ◽  
E. M. Kartzmark ◽  
M. E. Bednas ◽  
J. T. Herron
Keyword(s):  
Aqueous Solutions ◽  
Silver Nitrate ◽  
Molten Salt ◽  
Ammonium Nitrate ◽  
Molten State ◽  
Equivalent Conductance ◽  
Electrical Conductances ◽  
Straight Line

The specific and equivalent conductances (which also involve the densities) of aqueous solutions of silver nitrate and of ammonium nitrate, ranging in concentration from 0.1 M to that of the pure molten salt, have been determined at temperatures of 221.7 °C and 180.0 °C, respectively. It has been found that when the equivalent conductance is plotted against logarithm of the concentration, a straight line is obtained in the region of concentrations greater than about 6 M or less. Hence the equivalent conductance can be calculated from the relation[Formula: see text]where D = the slope and Λa = equivalent conductance at the limiting experimental concentration, Ca (in the molten state).

TRANSFERENCE NUMBERS AND CONDUCTANCES IN CONCENTRATED SOLUTIONS: SILVER NITRATE AND SILVER PERCHLORATE AT 25.00 °C

1959 ◽  
Vol 37 (12) ◽  
pp. 1959-1963 ◽  
Author(s):  
A. N. Campbell ◽  
K. P. Singh
Keyword(s):  
Aqueous Solutions ◽  
Silver Nitrate ◽  
Transference Number ◽  
Transference Numbers ◽  
Concentrated Solutions ◽  
Equivalent Conductance ◽  
Ion Formation ◽  
Silver Perchlorate ◽  
Complex Ion

The transference numbers, equivalent conductances, densities, and viscosities of aqueous solutions of silver nitrate and of silver perchlorate have been determined from a concentration of 0.1 M up to 7.6 M, for silver nitrate, and up to 5.6 M for silver perchlorate. In both cases the cation transference number increases considerably with increasing concentration. Certain anomalies in the results for silver perchlorate raise the possibility of complex ion formation here. Similar anomalies appear in the behavior of equivalent conductance with respect to concentration.The results of the conductance measurements have been compared with the values calculated from the equations of Wishaw and Stokes and of Falkenhagen and Leist.

THE ELECTRICAL CONDUCTANCE OF STRONG ELECTROLYTES: A TEST OF STOKES EQUATION

1955 ◽  
Vol 33 (5) ◽  
pp. 887-894 ◽  
Author(s):  
A. N. Campbell ◽  
E. M. Kartzmark
Keyword(s):  
Silver Nitrate ◽  
Ammonium Nitrate ◽  
Stokes Equation ◽  
Electrical Conductance ◽  
Lithium Nitrate ◽  
High Concentration ◽  
Empirical Observation ◽  
Semiempirical Equation ◽  
Strong Electrolytes ◽  
The Stokes Equation

The equation recently put forward by Wishaw and Stokes, purporting to reproduce the equivalent conductance of concentrated solutions of strong electrolytes, has been tested by applying it to the experimental data of Campbell, Kartzmark et alii. The agreement between the calculated and observed values of Λ is astonishingly good, in the case of lithium nitrate up to a concentration of 7 molar. The deviations found for silver nitrate and ammonium nitrate are attributed to ion-pair formation and a dissociation "constant" deduced (for silver nitrate) which does show approximate constancy; a similar calculation by Stokes for ammonium nitrate shows even better constancy. Since the Stokes' equation is fully theoretical and contains only quantities to which physical meaning can be attached, it is to be preferred to any empirical, or semiempirical, equation. The Stokes' equation, being merely an extension of the Debye–Hückel– Onsager concept, cannot be expected to apply to concentrations greater than, say, 5 N. Attention is again drawn to the empirical observation that in the region of very high concentration the plot of Λ versus log C is a true straight line.

scholarly journals The silver voltameter. Part III.―The solvent properties of silver nitrate solutions

1914 ◽  
Vol 91 (623) ◽  
pp. 53-71 ◽  
Keyword(s):  
Silver Nitrate ◽  
Silver Chloride ◽  
Pure Water ◽  
Quantitative Measurements ◽  
Appreciable Increase ◽  
Solvent Properties ◽  
Made In ◽  
Silver Nitrate Solutions ◽  
Nitrate Solutions

In an earlier paper by Mr. F. E. Smith and a second paper by the author in conjunction with Mr. F. E. Smith it was shown that the weight of silver deposited by a given current was influenced in a very important degree by impurities in the silver nitrate solutions. The most important impurities are those which are capable of exerting a reducing action upon the silver nitrate. But there is also a group of substances to be considered which are soluble in silver nitrate solutions, though almost insoluble in water: these are precipitated when the silver nitrate solutions are impoverished at the cathode by the passage of the current and cause an appreciable increase in the weight of the deposit. They may be removed by diluting the silver nitrate solutions, filtering off the precipitation will be freely soluble in the concentrated mother-liquor from which the crystals have separated, and may be got rid of the usual way by draining on the pump and rinsing cautiously with water. In view of the importance of these impurities in the experimental determination of the electrochemical equivalent of silver, and the interest of the problem from the standpoint of the theory of solutions, it appeared to be desirable to pursue the matter further and to make quantitative measurements of the solvent properties of silver nitrate solutions for some typical substances which are insoluble, or nearly so, in pure water. The present paper includes measurements of the solubility of silver chloride, bromide, iodide, and sulphide. The solubility of the iodide has already been investigated somewhat fully by Hellwig, but only a few incidental measurements have been made in the case of the other salts.

Induction period of the crystallization of silver nitrate solutions in ethylene glycol

1991 ◽  
Vol 56 (10) ◽  
pp. 2142-2147
Author(s):  
Ivo Sláma
Keyword(s):  
Ethylene Glycol ◽  
Silver Nitrate ◽  
Induction Period ◽  
Glass Forming Ability ◽  
Transformation Theory ◽  
Concentration Region ◽  
Glass Forming ◽  
Temperature Transformation ◽  
Silver Nitrate Solutions ◽  
Nitrate Solutions

The dependence of the induction period of crystallization on supercooling was examined for the silver nitrate-ethylene glycol system over the concentration region of silver nitrate lome fraction of 0 to 0.12. Addition of AgNO3 to ethylene glycol was found to increase considerably the critical induction period of crystallization, although to a lesser extent than Ca(NO3)2, CaCl2, ZnCl2, LiCl and LiNO3 do. The effect of these salts on the critical induction period of crystallization in dimethylsulfoxide, dimethylformamide, dimethylacetamide and methanol was compared in terms of the solvent-rich composition limit of the glass-forming ability. By using the TTT(Time-Temperature-Transformation) theory, it has been deduced that the effect of the salts on the critical induction period of crystallization of ethylene glycol is probably due to the different dependences of viscosity on their concentration in ethylene glyco in the supercooling region.

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