Viscosity of Aqueous Sodium Fluoride and Sodium Periodate Solutions. Ionic Energies and Entropies of Activation for Viscous Flow

Nightingale, E. R.; Benck, Ralph F.

doi:10.1021/j150580a050

Cited by 42 publications

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“…This has been done in light of Nightingale (27) and Feakins (28) formulations. It has been mentioned already that these tetracyclines have been used as therapeutic and prophylatic agents against bacterial activity.…”

Section: Resultsmentioning

confidence: 99%

Ultrasonic and thermodynamic studies of tetracyclines in solutions

Pandey¹,

Mishra²,

Shukla³

et al. 1987

Can. J. Chem.

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. Can. J. Chem. 65, 303 (1987).The ultrasonic velocity, U , density, and viscosity of aqueous and non-aqueous (water + dioxan) solutions of tetracycline hydrochloride and chlorotetracycline have been measured at two different temperatures. Partial molal volumes, $, , partial molal compressibility, $kr Vand's interaction coefficients, Q and C , and thermodynamic activation parameters AG*, AS*, and AH* of these solutions have been computed from the ultrasonic velocity, density, and viscosity data. The results are interpreted in terms of solute-solvent interaction.

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Section: Resultsmentioning

confidence: 99%

Ultrasonic and thermodynamic studies of tetracyclines in solutions

Pandey¹,

Mishra²,

Shukla³

et al. 1987

Can. J. Chem.

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“…Smaller monovalent ions generally have large electric fields at their surface and thus are structure makers. As explained by Nightingale, , the structure-making ability of the large IO 3 - and BrO 3 - is due to the low π-bond character of the halogen−oxygen bonds effectively delocalizing the electronic charge, allowing greater interaction between the ion and water molecules.…”

Section: Introductionmentioning

confidence: 97%

Ion-Specific Strength of Attractive Particle Networks

et al. 1999

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The shear yield stress of alumina suspensions was measured by the vane tool technique, as a function of high concentration of various counterions. Slurries at pHs below the isoelectric point were coagulated with the sodium salts of IO3 -, BrO3 -, Cl-, NO3 -, and ClO4 -. Structure maker ions (IO3 - and BrO3 -) produced the strongest particle networks, while structure breaker ions (ClO4 -, NO3 -, and Cl-) produced weaker networks. Electrokinetic results (ζ potentials) suggest the structure makers adsorb inside the shear plane in greater quantities and are thus more efficient in collapsing the double layer. The high yield stresses in the case of IO3 - cannot be fully explained by the concept of truncating the van der Waals attraction at a distance related to the size of the ion. When the possibility of either an additional attraction or a closer distance of approach is considered, the results can be adequately explained. Similar results were observed for zirconia.

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“…Because of their larger size, these ions are less hydrated or unhydrated. Due to minimum hydration of H 2 32 ΡΟϊ ions, the activation energy for viscous flow in solution decreases from that of pure solvent even though the ion itself increases the bulk viscosity of the solution [19]. This causes an increase in the movement of ions, leading to higher tracerdiffusion rate.…”

Section: Methodsmentioning

confidence: 99%

Tracer-diffusion of H₂ ³²PO₄ ^¯ Ions in Electrolyte Solutions in Agar Gel Medium

Baluja

Shukla

1984

Radiochimica Acta

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The tracer-diffusion coefficients of H^'PO, ions have been determined in sodium and potassium nitrate solutions immobilized in 2.5 % agar gel over the concentration range 10"' -1.0 Μ at 298 K. Comparison of the experimental and theoretical values indicates failure of the Onsager-Fuoss theory at higher concentrations of electrolyte solutions. The observed results are explained on the basis of water-gel, ion-water and ion-ion interactions. Diffusion rates are also determined at various gel concentrations at different temperatures (298 -323 K), keeping the electrolyte (KNO,) concentration constant at 10"' M. The obstruction effect of gel calculated in terms of formation factor F is observed to increase with increasing gel concentration. The results are explained on the basis of EYRING's theory of diffusion. centage was varied from 0.5-5.0%, keeping the electrolyte concentration constant at 10" 2 M. After the gel had set, both ends of the tube were tightly corked and kept in an automatically regulated thermostat at the desired temperature.After allowing the diffusion to proceed for a definite time (24 hrs), the gel columns on both sides of the zone were sliced into 0.5 cm samples. These samples were carefully transferred to aluminium planchettes and dehydrated in a hot air oven at 65 °C. The radioactivity in each sample was counted by an end window Geiger-Muller counter under the conditions of constant geometry.

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Viscosity of Aqueous Sodium Fluoride and Sodium Periodate Solutions. Ionic Energies and Entropies of Activation for Viscous Flow

Cited by 42 publications

References 0 publications

Ultrasonic and thermodynamic studies of tetracyclines in solutions

Ultrasonic and thermodynamic studies of tetracyclines in solutions

Ion-Specific Strength of Attractive Particle Networks

Tracer-diffusion of H₂ ³²PO₄ ^¯ Ions in Electrolyte Solutions in Agar Gel Medium

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Viscosity of Aqueous Sodium Fluoride and Sodium Periodate Solutions. Ionic Energies and Entropies of Activation for Viscous Flow

Cited by 42 publications

References 0 publications

Ultrasonic and thermodynamic studies of tetracyclines in solutions

Ultrasonic and thermodynamic studies of tetracyclines in solutions

Ion-Specific Strength of Attractive Particle Networks

Tracer-diffusion of H2 32PO4 ¯ Ions in Electrolyte Solutions in Agar Gel Medium

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Tracer-diffusion of H₂ ³²PO₄ ^¯ Ions in Electrolyte Solutions in Agar Gel Medium