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.

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.

VAPOR PRESSURES OF AQUEOUS SOLUTIONS OF SILVER NITRATE, OF AMMONIUM NITRATE, AND OF LITHIUM NITRATE

1956 ◽  
Vol 34 (2) ◽  
pp. 151-159 ◽  
Author(s):  
A. N. Campbell ◽  
J. B. Fishman ◽  
G. Rutherford ◽  
T. P. Schaefer ◽  
L. Ross
Keyword(s):  
Aqueous Solutions ◽  
Silver Nitrate ◽  
Direct Determination ◽  
Lithium Ion ◽  
Silver Ions ◽  
Lithium Nitrate ◽  
Vapor Pressures ◽  
Heats Of Dilution ◽  
Water Of Hydration

This paper is devoted to the direct determination of the vapor pressures of solutions of the nitrates of silver, of ammonium, and of lithium, at temperatures varying from 30 °C. to 105 °C. and at concentrations varying from 10 to 85 weight % (for lithium nitrate, the limited solubility precluded measurements beyond 65%). From the vapor pressures, the enthalpies of evaporation of water (by a modification of the Clapeyron–Clausius equation), the differential heats of dilution, and the activities of water (as compared with the mole fractions of the solvent) have been calculated. From the results we conclude that the water of hydration of the ammonium and silver ions (if, indeed, these ions are hydrated at all) is very loosely attached, while that of the lithium ion is strongly bound.

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).

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.

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.

scholarly journals Experimental data on the removal of acid orange 10 dye from aqueous solutions using TiO2/Na-Y zeolite and BiVO4/Na-Y zeolite nanostructures: A comparison study

Data in Brief ◽  
2021 ◽  
Vol 35 ◽  
pp. 106869
Author(s):  
Behzad Rahimi ◽  
Nayereh Rezaie-Rahimi ◽  
Negar Jafari ◽  
Ali Abdolahnejad ◽  
Afshin Ebrahimi
Keyword(s):  
Experimental Data ◽  
Aqueous Solutions ◽  
Comparison Study ◽  
Y Zeolite ◽  
Acid Orange ◽  
Acid Orange 10

scholarly journals Multi-Component Adsorption of Benzene, Toluene, Ethylbenzene, and Xylene from Aqueous Solutions by Montmorillonite Modified with Tetradecyl Trimethyl Ammonium Bromide

2013 ◽  
Vol 2013 ◽  
pp. 1-10 ◽  
Author(s):  
H. Nourmoradi ◽  
Mehdi Khiadani ◽  
M. Nikaeen
Keyword(s):  
Experimental Data ◽  
Aqueous Solutions ◽  
Structural Changes ◽  
Freundlich Isotherm ◽  
Isotherm Models ◽  
Ammonium Bromide ◽  
Order Kinetic ◽  
Multicomponent Adsorption ◽  
Benzene Toluene ◽  
Kinetic And Isotherm Models

Multicomponent adsorption of benzene, toluene, ethylbenzene, and xylene (BTEX) was assessed in aqueous solutions by montmorillonite modified with tetradecyl trimethyl ammonium bromide (TTAB-Mt). Batch experiments were conducted to determine the influences of parameters including loading rates of surfactant, contact time, pH, adsorbate concentration, and temperature on the adsorption efficiency. Scanning electron microscope (SEM) and X-ray diffractometer (XRD) were used to determine the adsorbent properties. Results showed that the modification of the adsorbent via the surfactant causes structural changes of the adsorbent. It was found that the optimum adsorption condition achieves with the surfactant loading rate of 200% of the cation exchange capacity (CEC) of the adsorbent for a period of 24 h. The sorption of BTEX by TTAB-Mt was in the order ofB<T<E<X. The experimental data were fitted by many kinetic and isotherm models. The results also showed that the pseudo-second-order kinetic model and Freundlich isotherm model could, respectively, be fitted to the experimental data better than other available kinetic and isotherm models. The thermodynamic study indicated that the sorption of BTEX with TTAB-Mt was achieved spontaneously and the adsorption process was endothermic as well as physical in nature. The regeneration results of the adsorbent also showed that the adsorption capacity of adsorbent after one use was 51% to 70% of original TTAB-Mt.

scholarly journals Measurement and Prediction of Densities of Ternary Aqueous Mixtures Involving Sodium Polyacrylate

2004 ◽  
Vol 4 (1) ◽  
pp. 64
Author(s):  
Z. A. Noor Fadzlina ◽  
T. T. Teng ◽  
M. Abdul Rahman
Keyword(s):  
Experimental Data ◽  
Aqueous Solutions ◽  
Percentage Error ◽  
Sodium Polyacrylate ◽  
Aqueous Systems ◽  
Aqueous Mixtures ◽  
Density Prediction ◽  
Density Values ◽  
Good Agreement

The densities of the binary aqueous solutions of sodium polyacrylate (NaPM) at 20°C, 25°C, and 300C up to 0.17 m and LiCI at 25°C and 300C up to 3.13 m were measured using a vibrating tube digital densitimeter. The measured experimental data were then fitted to the polynomial d = do + IA;m'. The densities of the ternary aqueous systems NaPM-NaCI, NaPM-LiCI, and NaPM-sucrose were also =1 measured from 20°C to 30°C. The isopycnotic equation, Imi / moi was used to predict the densities of the ternary aqueous systems mentioned. The results show that predicted and observed density values are in good agreement. The overall percentage error of density prediction for the system NaPM-NaCI-H20 is 0.067. For the system NaPM-LiCI-HP,the overall percentage error is 0.074; and, for the system NaPM-sucrose-H20, the overall percentage error is 0.065.

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