Infectious Diseases Society of America.

A new model for calculating the viscosity of aqueous solutions has been developed. Parameters for 74 solutes were established based on a critical review of the literature for solutions of one solute in water, with over 9000 points included. The average difference between the calculated and experimental viscosities is less than 0.1 %, and the standard deviation of this difference is 3.7 % of the average experimental viscosity. The model was validated by estimating published viscosity for systems of more than one solute in water. The average difference between experimental and calculated values for 1700 points is −2.7 %, and the standard deviation of this difference is 16 % of the average experimental viscosity. The median standard deviation of the difference between experimental and calculated values is 3.5 % of the experimental viscosity. The solutes studied are (NH4)2SO4, AlCl3, BaCl2, Ca(NO3)2, CaCl2, Cd(NO3)2, CdCl2, CdSO4, CoCl2, CoSO4, Cr2(SO4)3, CrCl3, Cu(NO3)2, CuCl2, CuSO4, Fe2(SO4)3, FeCl2, FeSO4...

Model for Calculating the Viscosity of Aqueous Solutions

A compendium of phase change enthalpies published in 2010 is updated to include the period 1880–2015. Phase change enthalpies including fusion, vaporization, and sublimation enthalpies are included for organic, organometallic, and a few inorganic compounds. Part 1 of this compendium includes organic compounds from C1 to C10. Part 2 of this compendium, to be published separately, will include organic and organometallic compounds from C11 to C192. Sufficient data are presently available to permit thermodynamic cycles to be constructed as an independent means of evaluating the reliability of the data. Temperature adjustments of phase change enthalpies from the temperature of measurement to the standard reference temperature, T = 298.15 K, and a protocol for doing so are briefly discussed.

Phase Transition Enthalpy Measurements of Organic and Organometallic Compounds. Sublimation, Vaporization and Fusion Enthalpies From 1880 to 2015. Part 1. C1-C10

A new model for calculating the density of aqueous solutions of electrolytes has been developed. Parameters for 59 electrolytes were established on the basis of an extensive critical review of the published literature for solutions of one electrolyte in water, with over 10 700 points included. The average difference between the calculated and experimental density of solutions of water and one electrolyte is 0.10 kg m-3 with a standard deviation of 1.44 kg m-3. The model was validated by predicting the density of systems of two or more electrolytes in water. The average difference between experimental and calculated values for over 1600 points is 0.003 kg m-3 with a standard deviation of 1.39 kg m-3. The electrolytes studied are AlCl3, Al2(SO4)3, BaCl2, CaCl2, CdCl2, CdSO4, CoCl2, CoSO4, CrCl3, Cr2(SO4)3, CuCl2, CuSO4, FeCl2, FeSO4, FeCl3, Fe2(SO4)3, HCl, HCN, HNO3, H3PO4, H2SO4, KCl, K2CO3, KNO3, KOH, K2SO4, LiCl, Li2SO4, MgCl2, MgSO4, MnCl2, MnSO4, NaBr, NaCl, NaClO3, Na2CO3, NaF, NaHCO3, NaH2PO4, Na2HPO...

Model for Calculating the Density of Aqueous Electrolyte Solutions

Mechanistic study into the enhanced transdermal permeation of a model β-blocker, propranolol, by fatty acids: a melting point depression effect

Excess thermodynamic functions for a simple eutectic: m-aminophenol-pyrogallol systems

Solutal convection during growth of organic NLO crystals

Crystallization behavior and nature of complexation have been studied for the naptha-lene-picric acid and anthracene-picric acid systems. Phase diagrams were determined experimentally to get the exact compositions of eutectics and molecular complexes. Data on crystallization velocity obey the relation V = u(ΔT) n where ΔT is undercooling, u and n are constant. Experimental values of heats of fusion do not go in subordination with mixture law. Infra-red and ultraviolet-visible spectral studies indicate the charge transfer interactions in both systems.

Chemistry of Organic Eutectics and Molecular Complexes: Naphthalene-Picric Acid and Anthracene-Picric Acid Systems

Bone remodeling is the continuous process by which old bone is removed by bone-resorbing cells, the osteoclasts and replaced by new bone synthesized by bone forming cells, the osteoblasts. Osteoporosis is characterized by a progressive loss of bone mass and microarchitecture, which leads to increased fracture risk. Denosumab, a human monoclonal antibody resembling natural IgG2 immunoglobulin, has antiresorptive activity and is distinguished from other antiresorptive drugs. It mimics osteoprotegerin (OPG) that binds to RANKL and hence does not allow RANKL to bind with RANK receptor, thereby inhibiting osteoclast differentiation, activation and survival exerting primarily antiresorptive action. Denosumab trials have shown its efficacy in postmenopausal women with osteoporosis, unresectable giant cell tumor of bone and significant effect in non-metastatic prostate cancer and delay in the time-to-first skeletal related events (SRE) and subsequent SRE with denosumab than zoledronic acid in patients. It is available as 60 mg/ml in pre-filled syringes and approved for osteoporosis in postmenopausal women (60 mg s.c. twice yearly), unresectable giant cell tumor of bone in adults and skeletally mature adolescents (120 mh s.c. monthly), prevention of skeletal-related events and to increase bone mass in patients at high risk for fracture including androgen deprivation therapy for non-metastatic prostate cancer or adjuvant aromatase inhibitor therapy for breast cancer. Denosumab offers advantages of twice yearly dosing in osteoporosis and monthly dosing in giant cell tumor of bone with its novel mechanism of action and better tolerability.

Denosumab: A bone antiresorptive drug

Small children have a tendency to put everything in the mouth; hence, poisoning due to accidental ingestion of commonly available household toxic substances is quite common in infants and small children. A wide variety of medications and substances can cause serious illness or kill a child who ingests just a single dose in small quantity. Camphor is one such substance easily available in many Indian households and is not a very well-recognised potentially fatal toxic compound. Around 3-5 mL of 20% camphor oil or > 30 mg/Kg is a potentially lethal dose.1,2 We report the case of a 31/2-year-old girl presenting with afebrile generalised tonic seizures. The causal association of accidental camphor ingestion was suspected based on smell of camphor in vomitus.

N.P. Singh

Papers

Excess thermodynamic functions for a simple eutectic: m-aminophenol-pyrogallol systems

Solutal convection during growth of organic NLO crystals

Chemistry of Organic Eutectics and Molecular Complexes: Naphthalene-Picric Acid and Anthracene-Picric Acid Systems

Denosumab: A bone antiresorptive drug

Camphor poisoning-An unusual cause of seizure.