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.

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.

CONDUCTANCES OF CONCENTRATED AQUEOUS SOLUTIONS OF MIXED ELECTROLYTES

1958 ◽  
Vol 36 (10) ◽  
pp. 1325-1331 ◽  
Author(s):  
A. N. Campbell ◽  
E. M. Kartzmark ◽  
A. G. Sherwood
Keyword(s):  
Aqueous Solutions ◽  
Silver Nitrate ◽  
Ammonium Nitrate ◽  
Ion Concentration ◽  
Lithium Nitrate ◽  
Mixed Electrolytes ◽  
Salt Solutions ◽  
Concentrated Aqueous Solutions ◽  
The Mean

Equivalent conductances, viscosities, and densities were determined for solutions equimolar in two of the three salts lithium nitrate, ammonium nitrate, and silver nitrate. The three possible combinations of two salts were each studied at 25 °C and at 35 °C.The observed conductances and viscosities were compared with those of the single salt solutions at the same total ion concentration. The conductances were lower than the mean of the conductances of the single salt solutions. The viscosities were also lower than the mean viscosities.

CONDUCTANCE IN THE RANGE OF MEDIUM CONCENTRATION

1959 ◽  
Vol 37 (8) ◽  
pp. 1288-1293 ◽  
Author(s):  
A. N. Campbell ◽  
R. J. Friesen
Keyword(s):  
Experimental Data ◽  
Aqueous Solutions ◽  
Silver Nitrate ◽  
Ammonium Nitrate ◽  
Suitable Choice ◽  
Lithium Nitrate ◽  
Medium Concentration

Equivalent conductances, densities, and viscosities of aqueous solutions of ammonium nitrate, of silver nitrate, and of lithium nitrate were determined at 25 °C and at 35 °C at concentrations ranging from 0.01 N to 1.0 N.Experimental equivalent conductances have been compared with those calculated by the Wishaw–Stokes and Falkenhagen–Leist equations. Suitable choice of one parameter, the distance of closest approach, permits reproduction of the experimental data with an error of less than 0.5%. A study of the deviations of the calculated from the experimental conductances reveals that the distance of closest approach (so-called) varies appreciably with concentration and temperature.

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.

Reutilization of ammonia from wastewater using cation exchange resins

1994 ◽  
Vol 30 (9) ◽  
pp. 111-119 ◽  
Author(s):  
M. Buday
Keyword(s):  
Cation Exchange ◽  
Ammonium Nitrate ◽  
Ph Value ◽  
Pilot Scale ◽  
Ammonium Concentration ◽  
Ammonium Ions ◽  
High Concentration ◽  
Cation Exchange Resins ◽  
Nitrate Fertilizer ◽  
Exchange Resins

The paper deals with adsorption of ammonium ions from wastewater of ammonia and ammonium nitrate plant on cation exchange resins. The aim of the treatment was not only separation of ammonium ions but also their return to the technology of ammonium nitrate fertilizer. Therefore, it was desirable to obtain high concentration of eluate. The columns of cation exchangers were arranged in the so-called “coupled columns” technique. The results were obtained on the pilot scale (0.6 m3.h−1) and in full scale (50 −110 m3.h−1) plants. Nitric acid was used for the regeneration of the exhausted resins. Its concentration was in the range of 3.9 − 7.0 mol.1−1. The average ammonium concentration of the eluate was in the range of 0.95 − 2.35 mol.l−1. This parameter of the treatment process depended on the pH value of wastewater and on the concentration of the regenerant. The concentration of ammonium nitrate achieved in the eluate is sufficient for its utilization in the technology for the ammonium nitrate fertilizer production.

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