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.

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.

THE METAL–SOLUTION SILVER ION EXCHANGE

1956 ◽  
Vol 34 (1) ◽  
pp. 14-40 ◽  
Author(s):  
I. I. Tingley ◽  
I. H. S. Henderson ◽  
C. C. Coffin
Keyword(s):  
Silver Nitrate ◽  
Nitrate Solution ◽  
Silver Ions ◽  
Silver Nitrate Solution ◽  
Maximum Activity ◽  
Metallic Silver ◽  
Different Types ◽  
Cold Worked ◽  
Silver Nitrate Solutions ◽  
Nitrate Solutions

The exchange of silver ions between silver nitrate solutions and surfaces of metallic silver was studied, using radioactive silver (Ag110, 270 day half-life) as a tracer. Marked differences in behavior of surfaces prepared in different ways were observed. Crystalline (annealed and etched) surfaces exchanged rapidly to a depth of a few atomic layers, and about 80% of the acquired radioactivity was removed as quickly by exchange with inactive silver nitrate solution. Highly polished surfaces exchanged up to ten times as great an extent as the etched annealed surfaces, but required 40 hours' immersion to attain their maximum activity. The deactivation of polished surfaces by inactive solutions was inversely proportional to the period of immersion in active solution, with surfaces immersed for 17 hr. or more retaining all but 30% of their acquired activity. Abraded surfaces exchanged quickly and retained most of their activity, the extent of the exchange depending upon the ratio of “worked” to “unworked” material on the surface. Some evidence of comparatively rapid diffusion in the polish layers was obtained. The interior of cold-worked silver when exposed to the nitrate solution behaved similarly to abraded surfaces. Mechanisms for the behavior of these different types of surface are offered, and the data of other workers discussed.

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.

Pulsed-laser Irradiation to Suspended Carbon Particles in Aqueous Silver Nitrate Solution

2008 ◽  
Vol 37 (8) ◽  
pp. 818-819 ◽  
Author(s):  
Yoshiko Miura ◽  
Kazuko Yui ◽  
Hiroshi Uchida ◽  
Kiyoshi Itatani ◽  
Seiichiro Koda
Keyword(s):  
Silver Nitrate ◽  
Laser Irradiation ◽  
Nitrate Solution ◽  
Pulsed Laser ◽  
Silver Nitrate Solution ◽  
Carbon Particles ◽  
Pulsed Laser Irradiation

Controlling the Surface Plasmon Absorption of Silver Nanoparticles via Green Synthesis Using Pennisetum purpureum Leaf Extract

2018 ◽  
Vol 772 ◽  
pp. 73-77
Author(s):  
Ruelson S. Solidum ◽  
Arnold C. Alguno ◽  
Rey Capangpangan
Keyword(s):  
Silver Nanoparticles ◽  
Green Synthesis ◽  
Silver Nitrate ◽  
Surface Plasmon ◽  
Leaf Extract ◽  
Nitrate Solution ◽  
Silver Nitrate Solution ◽  
Absorption Peak ◽  
Plasmon Absorption ◽  
Surface Plasmon Absorption

We report on the green synthesis of silver nanoparticles utilizing theP.purpureumleaf extract. Controlling the surface plasmon absorption of silver nanoparticles was achieved by regulating the amount of extract concentration and the molarity of silver nitrate solution. The surface plasmon absorption peak is found at around 430nm. The surface plasmon absorption peak have shifted to lower wavelength as the amount of extract is increased, while plasmon absorption peak shifts on a higher wavelength as the concentration of silver nitrate is increased before it stabilized at 430nm. This can be explained in terms of the available nucleation sites promoted by the plant extract as well as the available silver ions present in silver nitrate solution.

The Action of Silver Salts on Solution of Ammonium Persulphate

1902 ◽  
Vol 23 ◽  
pp. 163-168 ◽  
Author(s):  
Hugh Marshall
Keyword(s):  
Silver Nitrate ◽  
Ammonium Salt ◽  
Potassium Salt ◽  
Nitrate Solution ◽  
Silver Nitrate Solution ◽  
General Description ◽  
Potassium Persulphate ◽  
Ammonium Persulphate ◽  
Silver Salts

Although the action of potassium persulphate on silver nitrate solution was one of the first persulphate reactions observed (vol. xviii. p. 64), I had not until lately paid any special attention to the behaviour of the ammonium salt in this respect. It appears, however, that in the latter case there are additional actions of great interest, not possible with the potassium salt. A general description of these will be given now, but there are still some points deserving of further investigation.

scholarly journals The New Complexes of Tris(2-Methoxy-5-Bromophenyl)Stibine with Silver Nitrate

2021 ◽  
Vol 13 (1) ◽  
pp. 21-30
Author(s):  
O.K. Sharutina ◽  
Keyword(s):  
Diffraction Analysis ◽  
Silver Nitrate ◽  
Silver Atom ◽  
Nitrate Solution ◽  
Silver Nitrate Solution ◽  
X Ray Diffraction ◽  
Space Group ◽  
X Ray ◽  
Crystallographic Characteristics ◽  
Group A

By mixing solutions of tris(2-methoxy-5-bromophenyl)antimony and silver nitrate in a methanol : acetonitrile mixture (1:1 vol.), nitrato-O,O'-(acetonitrile)[tris(2-methoxy-5-bromophenyl)antimony]silver complex with the general formula [(C6H3ОMe-2-Br-5)3SbAg(μ2-NO3)(Ме3CN)]2•2[(C6H3ОMe-2-Br-5)3SbAgNO3(Ме3CN)] (1) has been obtained. An addition of silver nitrate solution in the methanol : acetonitrile mixture to the tris(2-methoxy-5-bromophenyl)antimony dioxane solution has led to the formation of a small amount of dark crystals of the ionic complex [(2-MeО-5-Br-C6H3)3SbAg(H2O)Sb(C6H3Br-5-OMe-2)3]+[(2-MeО-5-Br-C6H3)3SbAg(m-NO3)3 AgSb(C6H3Br-5-OMe-2)3]-×3C4H8O2 (2). Complexes 1 and 2 have been characterized by IR spectroscopy, and their structures have been determined by X-ray diffraction analysis. The IR spectra of complexes 1 and 2 contain the bands characterizing the Sb-O, Sb-C, С≡N-, and NO3-group band vibrations. X-ray diffraction analysis of the complexes has been carried out on an automatic four-circle D8 Quest Bruker diffractometer (МоКα radiation, λ = 0.71073 Å, graphite monochromator) at 293 K. Crystallographic characteristics of 1: triclinic, P-1 space group, a = 9.32(3), b = 17.50(7), c = 17.97(5) Å, a = 97.56(14), β = 92.90(19), g = 99.45(19) grad., V = 2859(16) Å3, Z = 2, rcalc = 2.069 g/cm3, 2: monoclinic, С2/с space group, a = 17.417(14), b = 21.041(15), c = 32.01(2) Å, a = 90, β = 97.79(3), g = 90 grad., V = 11624(15) Å3, Z = 4, rcalc = 2.006 g/cm3. In the monomeric and dimeric molecules of crystal 1, nitrate ligands are chelating and bridging, respectively. In the cation of complex 2, the silver atom is bonded to two antimony ligands, the third coordination site is occupied by a water molecule. In the dimeric anion there are one antimony ligand and three bridging nitrate groups surrounding each silver atom.

scholarly journals The Synthesis and Stability Study of Silver Nanoparticles Prepared by Using p-Aminobenzoic Acid as Reducing and Stabilizing Agent

2018 ◽  
Vol 18 (3) ◽  
pp. 421 ◽  
Author(s):  
Dian Susanthy ◽  
Sri Juari Santosa ◽  
Eko Sri Kunarti
Keyword(s):  
Silver Nanoparticles ◽  
Reaction Time ◽  
Silver Nitrate ◽  
Tap Water ◽  
Nitrate Solution ◽  
Silver Nitrate Solution ◽  
Stability Study ◽  
Synthesis Process ◽  
Aminobenzoic Acid ◽  
Stabilizing Agent

A study to examine the performance of p-aminobenzoic acid as both reducing agent for silver nitrate to silver nanoparticles (AgNPs) and stabilizing agent for the formed AgNPs has been done. The synthesis of AgNPs was performed by mixing silver nitrate solution as precursor with p-aminobenzoic acid solution and heating it in a boiling water bath. After the solution turned to yellow, the reaction stopped by cooling it in tap water. The formed AgNPs were analyzed by using UV-Vis spectrophotometry to evaluate their SPR absorption in wavelength range of 400–500 nm. The synthesis process was highly depend on the pH, reaction time, and mole ratios of the reactants. The synthesis only occur in pH 11 and at reaction time 30 min, the particle size of the formed AgNPs was 12 ± 7 nm. Longer reaction time increased the reducing performance of p-aminobenzoic acid in AgNPs synthesis but decreased its stabilizing performance. The increase of silver nitrate amount relative to p-aminobenzoic acid in the synthesis increased the reducing and stabilizing performance of p-aminobenzoic acid and the optimum mole ratio between AgNO3 and p-aminobenzoic acid was 5:100 (AgNO3 to p-aminobenzoic acid).

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