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Resistance to antibiotics/antibacterials/antifungals in pathogenic microbes has been developing over the past few decades and has recently become a commonplace public-health peril. Thus, alternative nontoxic potent antibiotic agents are covertly needed to control antibiotic-resistant outbreaks. In an effort to combat the challenges posed by the co-occurrence of multidrug resistance, two terpyridine ligands 4′-(4-N,N′-dimethylaminophenyl)-2,2′:6′,2″-terpyridine (L1) and 4′-(4-tolyl)-2,2′:6′,2″-terpyridine (L2) have been designed, prepared and confirmed their structure by spectral studies. Thereafter, antimicrobial assay was performed against gram positive and negative bacterial strains along with fungal strains. Both compounds L1 and L2 exhibited remarkable inhibitory activities against bacteria, Escherichia coli and Staphylococcus aureus at MIC values 6.25 and 3.125 µg/ml, respectively. In addition, in silico molecular docking studies were ascertained with bacterial DNA gyrase and fungal demethylase. Furthermore, both L1 and L2 could bind Bovine Serum Albumin (BSA) protein and binding interaction has been studied with the help of UV-Visible and fluorescence spectroscopy. While fluorescence of BSA unperturbed in the presence of L2, an addition of L1 to the solution of BSA resulted significant quenching. The binding constant calculations at different temperature confirmed that the fluorescence quenching between BSA and L1 is predominantly static in nature. The toxicity of L1 and L2 was checked using Drosophila melanogaster. The toxicity analysis suggest both the dyes are non-cytotoxic in nature. Communicated by Ramaswamy H. Sarma

The objective of this study is to analyze and explain the factors influencing the value added growth in Turkish public and private manufacturing sectors during 1980–2001. With this aim in view, a Two-Deflator Growth Accounting (TDA) method is applied in the study. It is revealed that industries as a whole have positive value added growth with no negative contribution of capital. Although human capital’s contribution to the industrial sector’s growth as a whole and especially to public sector industries is not very significant, its contribution to the private sector industries remains significantly high. The overall contribution of raw labor is able to explain most of the contribution of labor to value-added growth in Turkish manufacturing industry during the period 1980–2001.

Studies on the Physiology of Rice VII: Effect of Varying Water Levels on Growth of Rice in Relation to Nitrogen Absorption

Physiological Studies on the Effect of Colchicine on Rice II

Derivation of Equations to Account for the Variation of Osmotic Pressure, Ph and Conductance of Sols of Polyacids with Dilution

Evaluation of Cell Constant of Porous Pads Made of Fine Particles and ? Potential of the Particles by Applying Correction for Surface Conductance

Studies on the Physiology of Rice VIII: The Effects of Low and High Temperature Germination with or without Short Days on Summer and Winter Varieties

Pure Chemistry Department, University College of Science, Calcutta-700 009 Manuscript received 26 September 1977, accepted 14 February 1978 In a previous publication it has been shown how Smolocbowski's equation may be modified to account for the electro-viscous effed of colloidal electrolytes. The constants in the modified equation determined from viscosity data implicitly contained a factor, g. This point has been clarified In the present paper and It has been shown that the same equation can be derived also from Booth's equation on the basis of certain assumptions. Some of the advantages of the modified equation and those which follow from it have been discussed. The modified equations have been subjected to test using fresh experimental data collected from the literature and have been found satisfactory. It has also been shown how the primary eletro-viscous effect varies with the concentration of the colloidal electrolyte In the sol under different conditions.

Chemistry Department, University College of Science and Technology, Calcutta-700 009 Manuscript received 12 June 1980, revised 5 May 1981, accepted 19 May 1981 By modifying Debye-H\(\ddot{u}\)ckel theory, as discussed in a previous paper, equation for the mean activity coefficient of an ion in solutions of strong electrolytes of the unibivalent type has been deduced. The equation has been subjected to test using available data on BaCl2 and K2SO4 and has been found satisfactory. Equations for the equivalent conductivity of solution of strong electrolytes of 1 : 1 and 2 : 1 types have also been deduced and subjected to test using the data available in the literature on KBr, NaCl, HCl and CaCl2 and have been found satisfactory. The equations can be expressed in the same cube root form as that of Ghosh.

Department of Chemistry, University College of Science & Technology,Calcutta-700009 Manuscript received 16 November 1976, revised 26 July 1977, accepted 3 October 1977 An equation has been deduced which can account quantitatively for the variation of the ratio, R, the specific viscosity of the sol containing added electrolyte to that of the original sol without any electrolyte, with the increase in concentration of the added electrolyte. The equation has been found to agree well with the data available in the literature on such systems as cols of agar, gum arabic, casein etc. with added electro­lytes containing counter ions of different valency.

30, Regent Estate, Calcutta.-700 032 Manuscript received 16 November 1981, accepted 28 September 1982 Evaluation of "Effective Ionic Diameter" 'A' from Hydration Number 'h' of a Strong Electrolyte Solution&nbsp

Department of Chemistry, University College of Science,Calcutta.-700 009 Manuscript received 8 February 1978, revised 3 May1978,accepted 27 July 1978 Simplified Derivation of an Equation for Electroviscous Effect

University College of Science, University of Calcutta, Calcutta-700 009 It has been shown in previous publications that the expression for K (Kappa) in the Debye-Heckel theory of strong electrolytes requires modification. The modified kappa, denoted by Km includes the 'effective ionic diameter', a within it and at constant a, its variation with the electrolyte concentration should follow the cube-root relationship. Introducing this Km, and the effect of ionic hydration on activity coefficient into the thermodynamic part of the equation of Onsager and Fuoss, equations have been deduced for the diffusion coefficient D, containing terms involving cube-root and first power of C, the concentration. The equations have been subjected to test using the data available in the literature on a few 1 : 1 and 2 : 1 electrolytes and have been found satisfactory upto a concentration of 0.1 M.

Department of Chemistry, University College of Science, Calcutta-790 009 Manuscript received 12 December 1978, accepted 6 June 1979 Smoluchowski's equation for electroviscous effect has been modified by the author. The modified equation has been applied to account for the viscous behaviour of the micelles of sodium dodecyl sulfate solution under different experimental conditions and has been found satisfactory. &nbsp

University College of Science & Technology, Calcutta-700 009. Manuscript receives 6 June 1977, accepted 9 July 1977 For Colloidal ampholytes, Smolucbowski's electroviscosity equation has been modified by taking into consideration the contribution of the ampholyte molecules to thespecific conductivity of the solution.

University College of Science. Department of Chemistry, Calcutta-700009 Manuscript received 29 July 1975,accepted 22 September 1975 As protein molecules at a concentration of about 0.2 per cent can cover the surface of particles of glass, quartz etc. so it has been assumed that the surface of a glass electrode, placed in a solution of concentration above 0.7 per cent of bovine serum mercapt-albumin (BSA) at isoionic pH or above it, is almost completely covered by the protein molecules. On the basis of this assumption and the theory of colloidal electrolytes proposed by the author equations have been deduced which can quantitatively account for the rise in pH of isoiouic (BSA) caused by the additon of neutral salts, without assuming anion binding. It has also been shown that the number of proton donors per mole of (BSA) (molecular weight 69,000), dissociating in the pH range 5.1 to about 7 S, is 12.6 and their pK is 6.18.

University College of Science, 92, Acharya Prafulla Chandra Road, Calcutta-700 009 Manuscriptreceived5 May1981, revised7 August 1981,accepted31 August 1981 It has been shownthat starting with Donnan's theory of membrane equilibrium for non-ideal solutions a modified expression for \(\chi\) (Kappa) of the Debye-Huckel theory of strong electrolytes can be deduced This modified expression for \(\chi\) is exactly tbe same as bas been deduced Jn a previous paper by applying Boltzmana formula to the distribution of the ions In tbe ion-atmosphere of the central positively charged ion, taking into coasideratioo the mesa activity coefficient of tbe ions of the electrolyte in solution.

Department of Pure Chemistry, University College of Science and Technology, Calcutta-700 009 Manuscript received 13 October 1982,accepted 19 March 1983 Viscosity Equation of Strong Electrolyte Solutions Involving Cube Root and First Power of Concentration and "Effective Ionic Diameter" &nbsp

Department of Chemistry, University College of Science & Technology, Calcutta-700009 Manuscript received 19 July 1978, accepted 14 December 1978 Combining Smoluchowski's electroviscous equation with the author's equation* to account for the variation of specific conductivity of colloidal electrolytes with dilution the following equation has been deduced R=1\(+\)\(\frac{m(\propto-\propto_0)}{m_0+(\propto-\propto_0)}\) where R represents the ratio of the specific viscosity of the polyacrylic acid sol to which some alkali has been added and 4 its degree of dissociation to that of the sol to which no alkali has been added and its degree of dissociation is \(\propto_o\)and m and mo are constants. In the case of polyacrylic acid sol values of R calculated by using this equation agree well with those observed when \(\propto\) is varied from 0 038 to 0.80. In the case of polymethacrylic acid sols values of R calculated by using this equation upto \(\propto\)=0.1 and above\(\propto\)=0.34 agree well with those observed provided m is given a separate value for each of these two ranges of \(\propto\).The value of m upto \(\propto\)=0.1 is smaller than that above \(\propto\)=0.34. It has been shown on the basis of the arguments used in the deduction of the equation that the increase of m between \(\propto\)=0.1 and \(\propto\)=0.34 is caused by the transformation of the macromolecules of polymethacrylic acid from the folded to the unfolded form.

University College of Science and Technology, Calcutta.-700 009 Manuscript received 25 .August 1981, revised 7 January 1982, accepted 28 April 1982 In previous publications, the author has deduced an equation to account for the variation of the mean activity coefficient of the ions of strong electrolytes of 1 : 1 type in solutions of low concentrations, 0.001 to 0.1 m, by modifying the Debye-Mickel expression for k. This equation has been combined with that derived by Glueckauf to account for the effect of hydration on the activity coefficient of ions of the aforesaid type, using volume fraction statistics. The combined equation has been subjected to test using the data available in the literature on HCI, LiCI, NaCI, KCI and CsCI in the concentration range 0.2 m to 4 m and has been found satisfactory.

Department of Postgraduate Studies & Research in Chemistry, RanchiUniversity, Ranchi-834 008 Manuscript received 1 December 1984, revised 10 October 1985, accepted 17 January 1986 Synthesis of sodium, potassium and ammonium salts of heteropoly-5-molybdo-1-v anado tellurate anion [TeVMO5O14]7-are reported. They are characterised by chemical analysis, ir and uv spectra. Thermal stability of the compounds has been examined by DTA and TGA studies The average molecular weight of sodium 5- molybdo-1-vanadotellurate has been determined by cryoscopy in Na2So410H2O­Na2SO4 H2O system and further been confirmed by Weissenberg Xray crystal diffrac­tion method.

Department of Chemistry, University College of Science and Technology, Calcutta-700 009 Manuscript received 14 September 1981, revised 23 February 1982, accepted 28 September 1982 In previous publications the expression for \(k\) (Kappa) of the Debye.Hückel theory of strong electrolytes has been modified. In this paper using this modified\(k\) (Kappa) equations have been deduced for λ, the equivalent conductance of solutions of strong electrolytes. These equations cover a wide range of concentration from 0.00002 N to 0.1 N of solutions of 1 : 1 strong electrolytes and according to them λ varies as (C)1/2,C representing concentration in moles per liter. The equations have been subjected to test using the data available in the literature on HCI, KCI, NaCI, KNO3and AgNO3and have been found satisfactory. It has been found that A, the "effective diameter", of the ions occurring in the equations, has different values in the different zones of concentration of the electrolytes used. The value of A of each of the chlorides above 0 001 N is much smaller than that below it. In the case of each of the nitrates, A has the highest value below 0 0008 N and the lowest value above 0.005 N. Within the range 0.005 N to 0.0008 N, it has an intermediate value. Since the change in A indicates change in hydration of the ions, the effect of its change on the size and mobility of the ions has been considered.&nbsp

Department of Chemistry, Ranchi University, Ranchi-834 009 Department of Chemistry, Gossner College, Ranchi-834 001 Central Fuel Research Institute, Ranchi Manuscript received 16 March 1984, revised 26 December 1984,accepted 15 February 1985 Synthesis and Characterisation of Mixed Heteropoly Molybdotungstotellurate

Department or Chemistry, University College of Science. Calcutta-700 009 Manuscript recived 4 August 1983, accepted 17 February 1984 The expression for k (kappa) of the Debye-Huckel theory of strong electrolytes has been modified in previous publications. The expression for krn, the modified kappa, includes the effective ionic diameter, a, which occurs in the denominator along with D, the dielectric constant and T, the absolute temperature. It follows from theory that In the concentration range of a solution in which a remains constant, Km should vary according to cube root or concentration, C. Equations have been deduced containing Km to account for the variation of relative apparent molal heat contents in dilute "strong electrolyte'' solutions when their concentrations are varied. The equations have been subjected to test using the data available in the literature on NaCI, KCI, KNO2 , NaOH, HCI, BaCI2. and Li2SO4 so far and have bees found satisfactory.

Of 807 women 45 years or less who had Lippes loop IUDs inserted in 1969- 1970 at a south Calcutta clinic, 552 were interviewed at home to study post-IUD fertility in 1980-1981. 48 were excluded due to early menopause, separation or death of spouse. Pregnancy rates in the remaining 504 women were 1.2% for the 1st 24 months, 0% at 48 and 0.2% for 49-96 months for those using contraception, compared to 6.9, 7.3, and 1.6% at 12, 48 and 132 months for those not using contraception. 7.5%, 8.1% and 9.9% of the women not using contraception were not pregnant at 12, 28 and 132 months. 18.2% of these women had been sterilized, while 12.8% were using an IUD, 11.7% were using natural birth control, and 5.7% used condoms. 4.6% retained the original IUD for 11 years. There was a 1.2% failure rate among IUD acceptors during use of a re-inserted IUD. Women had fewer subsequent pregnancies if they had more children when accepting the IUD, intended to limit family size, or were older. Those with all daughters wanted more children and were less likely to use contraception. Since the overall fertility rate after marriage was 335, use of the IUD in this population was estimated to reduce fertility by 86%.

University College of Science, Calcutta-700 009 Manuscript received 6 May 1987, accepted 13 November 2987 In previous publications, Jones and Dole's equation for the viscosity of solutions of the strong electrolytes had been modified and its modified B-coefficient has been identified with the Einstein expression 2.5\(\bigtriangledown\)where \(\bigtriangledown\) represents the volume fraction per unit concentration of the electrolyte. It has been shown that the modified B-coefficient varies linearly with (h — \(\phi\)/18), where h is the hydration number, \(\phi\)the apparent molal volume of the electrolyte and 18 the molecular volume of water at 25°. This relationship has been subjected to further test using fresh data collected from the literature and has been found satisfactory. It has also been shown that the partial molal entropy of hydration of a strong electrolyte in solution varies linearly with the absolute temperature in the range 298.2 — 473.2 K.

Department of Chemistry, University College of Science, 92, Acharya Prafulla Chandra Road, Calcutta-700 009 Manuscript received 18 September 1979, accepted 9 January 1980 Equations deduced in previous publications to account for the variation of specific conductivity of different types of colloidal electrolytes with dilution (by water) have been subjected to further test using relevant data available in the literature on benzopurpurine 4 B and its isomer prepared from meta-tolidine and also on azrechtic acid, a polyelectrolyte, extracted from the gum of the plant Azadirechta Indica. The equations have been found to hold good in these cases, the concentration and the corresponding specific conductivity varying over a wide range.