INVESTIGATION ON VISCOUS SYNERGY AND INVESTIGATION ON VISCOUS SYNERGY AND ANTAGONISM OF SOME LIQUID MIXTURES AND ANTAGONISM OF SOME LIQUID MIXTURES AND ION-SOLVENT INTERACTION OF ION-SOLVENT INTERACTION OF SOME COMPOUNDS IN VARIOUS SOME COMPOUNDS IN VARIOUS SOLVENT SYSTEMS SOLVENT SYSTEMS BY BY Anuradha Sinha Anuradha Sinha Supervisor : Dr. Mahendra Nath Roy Supervisor : Dr. Mahendra Nath Roy Department of Chemistry Department of Chemistry University of North Bengal University of North Bengal
Transcript
INVESTIGATION ON VISCOUS SYNERGY AND INVESTIGATION ON VISCOUS SYNERGY AND ANTAGONISM OF SOME LIQUID MIXTURES AND ANTAGONISM OF SOME LIQUID MIXTURES AND
ION-SOLVENT INTERACTION OF ION-SOLVENT INTERACTION OF SOME COMPOUNDS IN VARIOUS SOME COMPOUNDS IN VARIOUS
SOLVENT SYSTEMSSOLVENT SYSTEMS
BYBY
Anuradha SinhaAnuradha Sinha Supervisor : Dr. Mahendra Nath RoySupervisor : Dr. Mahendra Nath Roy
Department of ChemistryDepartment of ChemistryUniversity of North BengalUniversity of North Bengal
Contents Contents
CHAPTER I : Necessity of the Research CHAPTER I : Necessity of the Research WorkWork
CHAPTER II : General IntroductionCHAPTER II : General Introduction CHAPTER III : Experimental SectionCHAPTER III : Experimental Section CHAPTER IV : Viscous Synergy and CHAPTER IV : Viscous Synergy and
Antagonism and Isentropic Compressibility Antagonism and Isentropic Compressibility of Ternary Mixtures Containing 1,3-of Ternary Mixtures Containing 1,3-Dioxolane, Water and Monoalkanols at Dioxolane, Water and Monoalkanols at 303.15 K303.15 K
CHAPTER V : Solute-Solvent and Solute-Solute CHAPTER V : Solute-Solvent and Solute-Solute Interactions of Resorcinol in Mixed 1,4-Interactions of Resorcinol in Mixed 1,4-DioxaneDioxaneWater Systems at Different Water Systems at Different TemperaturesTemperatures
CHAPTER VI : Investigation on Viscous CHAPTER VI : Investigation on Viscous Antagonism of Binary and Ternary Liquid Antagonism of Binary and Ternary Liquid Mixtures and its Relation to Concentration at Mixtures and its Relation to Concentration at (303.15, 313.15 and 323.15) K(303.15, 313.15 and 323.15) K
CHAPTER VII : Excess Molar Volumes, Viscosity CHAPTER VII : Excess Molar Volumes, Viscosity Deviations and Isentropic Compressibility of Deviations and Isentropic Compressibility of Binary Mixtures Containing 1,3-Dioxolane and Binary Mixtures Containing 1,3-Dioxolane and Monoalcohols at 303.15 KMonoalcohols at 303.15 K
CHAPTER VIII : Ion-Solvent and Ion-Ion CHAPTER VIII : Ion-Solvent and Ion-Ion Interactions of some Tetraalkylammonium, Interactions of some Tetraalkylammonium,
Alkali Metals and Ammonium Halides in Alkali Metals and Ammonium Halides in
i-Amyl Alcohol at 298.15 K by Conductometric i-Amyl Alcohol at 298.15 K by Conductometric TechniqueTechnique
CHAPTER IX : Studies of Viscous Antagonism, CHAPTER IX : Studies of Viscous Antagonism, Excess Molar Volume and Isentropic Excess Molar Volume and Isentropic Compressibility in Aqueous Mixed Solvent Compressibility in Aqueous Mixed Solvent Systems at Different TemperaturesSystems at Different Temperatures
CHAPTER X : Densities, Viscosities and CHAPTER X : Densities, Viscosities and Sound Speeds of some Acetate Salts in Sound Speeds of some Acetate Salts in Binary Mixtures of Tetrahydrofuran and Binary Mixtures of Tetrahydrofuran and Methanol at (303.15, 313.15 and 323.15) KMethanol at (303.15, 313.15 and 323.15) K
CHAPTER XI : Concluding RemarksCHAPTER XI : Concluding Remarks
Necessity of the Research WorkNecessity of the Research Work
Object and Application of the WorkObject and Application of the Work
The molecular interactions play a very The molecular interactions play a very important role in various physico-chemical processes important role in various physico-chemical processes occurring in nature. occurring in nature.
Synergy and antagonism give the mutual Synergy and antagonism give the mutual enhancement or decrement of the physico-chemical, enhancement or decrement of the physico-chemical, biological or pharmaceutical activity between biological or pharmaceutical activity between different components of a given mixture.different components of a given mixture.
Applicable in manufacture of pharmaceuticals, Applicable in manufacture of pharmaceuticals, foodstuffs, cosmetics, industrial products. foodstuffs, cosmetics, industrial products.
High-energy primary and secondary batteries, High-energy primary and secondary batteries, wet double-layer capacitors and super capacitors, wet double-layer capacitors and super capacitors, electro-deposition and electroplating.electro-deposition and electroplating.
Non-aqueous electrolyte solutions are broadly Non-aqueous electrolyte solutions are broadly used in electrochromic displays and smart windows, used in electrochromic displays and smart windows, photoelectrochemical cells, electromachining, photoelectrochemical cells, electromachining, etching, polishing and electro-synthesis. etching, polishing and electro-synthesis.
Organic and inorganic synthesis, studies Organic and inorganic synthesis, studies
of reaction mechanisms and extraction. of reaction mechanisms and extraction.
Energy transport, heat transport, mass Energy transport, heat transport, mass transport and fluid flow. transport and fluid flow.
Non-aqueous systems have been of Non-aqueous systems have been of immense importance to the technologist and immense importance to the technologist and theoretician as many chemical processes occur theoretician as many chemical processes occur in these systems. in these systems.
General IntroductionGeneral Introduction Investigation on Viscous Synergy and Antagonism Investigation on Viscous Synergy and Antagonism
Viscous synergy is the term used in application to the Viscous synergy is the term used in application to the interaction between the components of a system that causes interaction between the components of a system that causes the total viscosity of the system to be greater than the sum of the total viscosity of the system to be greater than the sum of the viscosities of each component considered separately.the viscosities of each component considered separately.
Investigation on Ion-Solvent InteractionInvestigation on Ion-Solvent Interaction
Source and Purification of the Source and Purification of the Chemicals used Chemicals used
SolventsSolvents
1,3-Dioxolane (C1,3-Dioxolane (C33HH66OO22), M.W. 74.08, LR, India, was ), M.W. 74.08, LR, India, was
heated under reflux with PbOheated under reflux with PbO22 for 2 hrs., then cooled for 2 hrs., then cooled
and filtered. After adding xylene to the filtrate, the and filtered. After adding xylene to the filtrate, the mixture was distilled. mixture was distilled.
PrPr44NBr, BuNBr, Bu44NBr, BuNBr, Bu44NI were purified by NI were purified by
recrystallisation. The crystallised salts were dried in recrystallisation. The crystallised salts were dried in vacuum. The salts were stored in glass bottles in vacuum. The salts were stored in glass bottles in darkened desiccator over fused CaCldarkened desiccator over fused CaCl22. .
LiBr, NHLiBr, NH44Br were dried at ~ 80-100ºC in vacuum Br were dried at ~ 80-100ºC in vacuum
oven for 48 hrs before use.oven for 48 hrs before use.
Experimental MethodExperimental Method
Measurement of Density Measurement of Density
Ostwald-Sprengel type pycnometer Ostwald-Sprengel type pycnometer Calibration at different temperatures with doubly distilled Calibration at different temperatures with doubly distilled
water and THF. water and THF. The precision of the density measurement was The precision of the density measurement was 0.0003 %. 0.0003 %.
Thermostatic water bath maintained with an accuracy ofThermostatic water bath maintained with an accuracy of 0.01 K. 0.01 K.
Measurement of ViscosityMeasurement of Viscosity
Ubbelohde viscometer Ubbelohde viscometer The precision of the viscosity measurement was The precision of the viscosity measurement was 0.004 %. 0.004 %.
Measurement of Ultrasonic SpeedMeasurement of Ultrasonic Speed
Ultrasonic speeds were measured, with an accuracy Ultrasonic speeds were measured, with an accuracy of ± 0.2 %, using a single-crystal variable-path of ± 0.2 %, using a single-crystal variable-path ultrasonic interferometer operating at 4 MHz. ultrasonic interferometer operating at 4 MHz.
Measurement of ConductanceMeasurement of Conductance
Systronics Conductivity-TDS meter 308 Systronics Conductivity-TDS meter 308 Dip-type immersion conductivity cell Dip-type immersion conductivity cell The entire conductance data was found to be ± 0.3 % The entire conductance data was found to be ± 0.3 %
precise. precise.
Viscous Synergy and Antagonism and Isentropic Viscous Synergy and Antagonism and Isentropic Compressibility of Ternary Mixtures Containing Compressibility of Ternary Mixtures Containing
1,3-Dioxolane, Water and Monoalkanols at 303.15 K1,3-Dioxolane, Water and Monoalkanols at 303.15 Kcalccalc == ∑∑ w w ii ii ; ; ρ ρ calccalc == ∑∑ w w ii ρ ρ ii
I I SS = (= (expexp – – calccalc ) / ) / calccalc = = / / calccalc
The negative value of IThe negative value of ISS gives I gives IAA..
FF = = maxmax / / 00
KKSS = = 11/ (/ (uu22 ρ ρ))
nn
KKSS EE == K KSS –– x xi i K KS,iS,i
i = 1i = 1
Experimental (expt.) and literature (lit.) values of densities (ρ) and
viscosities (η) along with the expt. speeds of sound (u) of the pure solvents
1,3-dioxolane cannot easily disrupt the molecukar package between branched isomers and water1,3-dioxolane cannot easily disrupt the molecukar package between branched isomers and water
Investigation on Viscous Antagonism of Binary and Investigation on Viscous Antagonism of Binary and Ternary Liquid Mixtures and Its Relation to Ternary Liquid Mixtures and Its Relation to
Concentration at (303.15, 313.15 and 323.15) KConcentration at (303.15, 313.15 and 323.15) K Calculated (calc) and experimental (expdensities of ethylene glycol +
tetrahydrofuran and ethylene glycol + 1,4-dioxane against the respective
Studies of Viscous Antagonism, Excess Molar Studies of Viscous Antagonism, Excess Molar Volume and Isentropic Compressibility in Aqueous Volume and Isentropic Compressibility in Aqueous
Mixed Solvent Systems at Different TemperaturesMixed Solvent Systems at Different Temperatures
nn
Δη Δη = = η η – – Σ Σ xxii ηηii
ii =1 =1
nn
VVEE = Σ = Σ xxii MMii (1/ρ –1/ρ (1/ρ –1/ρii ) )
i=1i=1
water + ethylene glycol +water + ethylene glycol +
DMSO > DO > DMF > THF DMSO > DO > DMF > THF
-7
-6
-5
-4
-3
-2
-1
0
1
0 0.1 0.2 0.3 0.4 0.5 0.6 0.7 0.8 0.9 1
x A
Δ η
x
10
2
/ (
P )
Fig.1: Viscosity deviations (Δη) of : (■), water (A) + ethylene glycol (B) +
dimethylsulphoxide (C) mixtures with mole fraction of water (xA) at
298.15 K.
HH22O + CHO + CH22OH +OH +
CH CH22OHOH
ΔηΔη CH CH33
< N-C-H < < H< N-C-H < < H33C-S-CHC-S-CH33
CHCH33 O O O O
(THF) (DMF) (DO) (DMSO)(THF) (DMF) (DO) (DMSO)
IIAA and and VVE E ((weakest molecular interaction with THFweakest molecular interaction with THF)) CHCH33
> N-C-H > > H> N-C-H > > H33C-S-CHC-S-CH33
CHCH33 O O O O
Excess Molar Volumes, Viscosity Deviations and Excess Molar Volumes, Viscosity Deviations and Isentropic Compressibility of Binary Mixtures Isentropic Compressibility of Binary Mixtures Containing 1,3-Dioxolane and Monoalcohols Containing 1,3-Dioxolane and Monoalcohols
at 303.15 Kat 303.15 K nn
GG*E*E == R T R T [[ ln ln V V – ( – ( ΣΣ x xii ln ln ii V Vii ) ] ) ]
ii=1=1
nn nn
ln ln η η == Σ Σ xxii ln ln ηηi i ++ dd11 Π Π xxii i=1 i=1i=1 i=1
kk
YYEE == x x11 x x22 ∑ A ∑ A J -1J -1 ((xx11 –– x x22 )) J – 1J – 1
J=1J=1
σ = [ ( Yσ = [ ( YEEexp.exp. – Y – YEE
cal.cal. ) )22/ ( n – m ) ] / ( n – m ) ] 1 / 21 / 2
(▲); 2 -propanol (x); 1-butanol (o); 2-butanol (●); t -butanol (■); i -amyl
alcohol (∆).
CHCH33OH…….OH…….
(1,3-dioxolane)(1,3-dioxolane) most favorable intermolecular complexation through H-bonding most favorable intermolecular complexation through H-bonding
alcohols as Lewis acids and the cyclic diether as a Lewis basealcohols as Lewis acids and the cyclic diether as a Lewis base
The negative The negative VVEE andand K KSSEE values indicate the presence of strong donor- values indicate the presence of strong donor-
acceptor interaction between the oxygen and hydrogen atoms of the acceptor interaction between the oxygen and hydrogen atoms of the cyclic diether and the alcohols.cyclic diether and the alcohols.
The branched isomers fit into the structure of cyclic diether more easily The branched isomers fit into the structure of cyclic diether more easily compared to the linear isomer. compared to the linear isomer.
∆∆ηη and and GG*E*E and and dd1 1 values are found to be positive where charge-transfer values are found to be positive where charge-transfer and hydrogen-bonding interactions lead to the formation of complex and hydrogen-bonding interactions lead to the formation of complex species between unlike molecules.species between unlike molecules.
Ion-Solvent and Ion-Ion Interactions of some Ion-Solvent and Ion-Ion Interactions of some Tetraalkylammonium, Alkali Metals and Tetraalkylammonium, Alkali Metals and
Ammonium Halides in i-Amyl Alcohol at 298.15 K Ammonium Halides in i-Amyl Alcohol at 298.15 K
by Conductometric Techniqueby Conductometric Technique
d d == (( M M // N. N. )) 1/31/3 = 1.183= 1.183 (( M M // ) ) 1/31/3
== p p [[ 00 ( (1 1 + + RRXX ) +) + E ELL ]] p p = = 1 1 –– a a ((1 1 -- ) ) == 1 1 –– K KAA c c 22 f f 22
– – ln f ln f = = k k //2 2 ((1 1 ++ k R k R )) == e e22//ε kε kBB T T
KKAA = = KKRR / (/ (1 1 –– a a ) = ) = KKRR ((1 1 ++ K KSS))
00 == 1 1 / / 6 П r T6 П r T
MeMe44 N N++ > Et > Et44 N N++ > Bu > Bu44 N N++ > Pr > Pr44 N N++
However, in case of alkali metal and ammonium halides the trend However, in case of alkali metal and ammonium halides the trend is:is:
LiLi++ > NH > NH44+ + > Na> Na++
LiBr NaI NH4Br
Bu4NI
Bu4NBr
Pr4NBr
Et4NBr
Me4NCl
0
2000
4000
6000
8000
10000
12000
14000
16000
18000
20000
Electrolytes
K A
/
( d
m
3 . m
ol -1
)
Fig.1: The electrolytes; tetraalkylammonium, alkali metals and
ammonium halides with their association constant (KA) values in pure i-
amyl alcohol at 298.15 K.
MeMe44 NCl > Et NCl > Et4 4 NBr > BuNBr > Bu44 NI > Pr NI > Pr4 4 NBr > BuNBr > Bu44 NBr NBr
and, LiBr > NaI > NHand, LiBr > NaI > NH44 Br Br
LiBr
NaI
NH4Br
Bu4NI
Bu4NBrPr4NBr
Et4NBrMe4NCl
0
2
4
6
8
10
12
14
16
18
Electrolytes
Λ o
x
10
4 /
( S
. m
2 .
mo
l -1 )
Fig.2: The electrolytes; tetraalkylammonium, alkali metals and
ammonium halides with their limiting molar conductance () values in
pure i-amyl alcohol at 298.15 K.
LiBr
NaI
NH4Br
Bu4NI
Bu4NBrPr4NBr
Et4NBrMe4NCl
0
0.1
0.2
0.3
0.4
0.5
0.6
0.7
Electrolytes
Λ o
η
x
10
6 /
( S
. m
2.
mo
l -1.
P )
Fig.3: The electrolytes; tetraalkylammonium, alkali metals and
ammonium halides with their Walden’s product () in pure i-amyl
alcohol at 298.15 K.
KKA A Ion-dipole interactionIon-dipole interaction
RR44NN+……+……HO-CH-CHHO-CH-CH22-CH-CH22-CH-CH33
CHCH33
(i-amyl alcohol)(i-amyl alcohol)
BuBu44NI > BuNI > Bu44NBr NHNBr NH44++ > Na > Na++ Li Li++ > Na > Na++
size of Isize of I-- > Br > Br – – size of Lisize of Li++ < Na < Na++
increase of the Walden product indicates the weak solvation of the ions increase of the Walden product indicates the weak solvation of the ions in the pure solvent OR higher is the limiting molar conductance value, in the pure solvent OR higher is the limiting molar conductance value, lower is the solvationlower is the solvation
Walden’s product decreases in the increasing order of the radii:Walden’s product decreases in the increasing order of the radii:
MeMe44 N N++ > Et > Et4 4 NN++ > Pr > Pr4 4 NN++ > Bu > Bu44 N N+ + and Liand Li++ > Na > Na++ > NH > NH44++
Densities, Viscosities and Sound Speeds of some Densities, Viscosities and Sound Speeds of some Acetate Salts in Binary Mixtures of Tetrahydrofuran Acetate Salts in Binary Mixtures of Tetrahydrofuran
and Methanol at (303.15, 313.15 and 323.15) Kand Methanol at (303.15, 313.15 and 323.15) K VVφφ == M M // 00 –– 1000 (1000 ( - - 0 0 ) / () / (c c 00 ))
VVφ φ == V Vφφ00 ++ S SVV
** √c √c
EE22 == E Eφφ+ [(1000 –+ [(1000 – c E c Eφφ )( 2000 +)( 2000 + S SEE c c3/23/2 ))--11]]SSE E cc1/21/2
EEφφ = = αα00 V Vφφ + (+ (α α -- α α00 ) 1000) 1000 c c -1-1
strong ion-solvent interactions between NH4+ ion and THF +
MeOH molecules and Strong ion-ion interactions between Li+ ion and THF + MeOH molecules
The smaller ions show a stronger affinity towards the
ionic association while the larger ions seems to be responsible for the inability to ion-pair formation.
SV* values is found to increase as mass % of THF
increases along with the rise in temperature. This is reflected to accommodation of more and more solute molecules in the empty space left in the packing of associated solvent molecules resulting in an increased ion-pairing.
Rise in temperature is attributed to violent thermal agitation resulting in increasing the force of ion-ion interactions.
AA–coefficients - the ion-atmosphere effects –coefficients - the ion-atmosphere effects
BB–coefficients -solvation of the ions and their effects –coefficients -solvation of the ions and their effects on the structure of the solvent in the near on the structure of the solvent in the near environment of the solute particlesenvironment of the solute particles
small small AA values indicate weak ion-ion interactions and values indicate weak ion-ion interactions and positive positive BB values suggest the presence of strong ion- values suggest the presence of strong ion-solvent interactionssolvent interactions
BB–coefficients decreases from NH–coefficients decreases from NH44++ to Li to Li++ as mass % as mass %
of THF increases and decreases with rise in of THF increases and decreases with rise in temperature, thus, indicating weakest ionic solvation temperature, thus, indicating weakest ionic solvation for Lifor Li++-salt-salt
∆μ0*2 i.e. the contribution per mole of the solute to free energy of activation
The change observed in Z (acoustic impedance) ) with conc. is attributed to change of ultrasonic speed. This behavior is due to association of molecules and formation of molecular aggregates.
The increase in Lf (intermolecular free length) implies increase in number of free ions showing the occurrence of ionic dissociation.
The change of r΄ (relaxation strength) with conc. may be interpreted in terms of increase in intermolecular forces due to increase in conc. and subsequent decrease in the relaxation of the molecules.
RA (relative association) is used to understand the interaction influenced by the breaking of the solvent structure on addition of solute and the solvation of the solute simultaneously produced.
Solute–Solvent and Solute–Solute Interactions of Solute–Solvent and Solute–Solute Interactions of Resorcinol in Mixed 1,4-Dioxane–Water Systems at Resorcinol in Mixed 1,4-Dioxane–Water Systems at
Different TemperaturesDifferent Temperatures
VVφφ00 == aa00 + a+ a11.T .T ++ aa22. T. T22
ΦΦ00EE = ( = ( δVδV
00// δT δT )) PP == aa00 + 2 a + 2 a22 T T
( ( δ cδ cPP / / δ P δ P )) TT == – (– ( δ δ 22 V Vφφ00// δ T δ T 22 )) PP
0
20
40
60
80
100
120
140
0 0.05 0.1 0.15 0.2 0.25 0.3 0.35 0.4 0.45 0.5
√ c / ( mol. dm - 3 ) 1 / 2
Vφ
x
10
6 /
( m
3 . m
ol -
1 )
Fig.1(a): Apparent molar volumes (Vφ) against square root of molar
concentration (√c) of resorcinol in 1,4 -dioxane + water mixtures and pure
1,4-dioxane at 303.15 K. Graphical points: 10 mass % DO (▲); 20 mass %
DO (○); 30 mass % DO (●); 100 mass % DO (Δ).
-0.2
-0.1
0
0.1
0.2
0.3
0.4
0 0.05 0.1 0.15 0.2 0.25 0.3 0.35 0.4 0.45 0.5
√ c / ( mol. dm - 3 ) 1 / 2
(
/
0 –
1 )
÷ √
c /
( m
ol.
dm
- 3
) -
1 /
2
Fig. 2(a): (/ 0 –1) /√ c against square root of molar concentration (√c) of
resorcinol in 1,4-dioxane + water mixtures and pure 1,4-dioxane at 303.15
K. Graphical points: 10 mass % DO (▲); 20 mass % DO (○); 30 mass % DO
(●); 100 mass % DO (Δ).
Limiting apparent molar expansibilities (Φ0E) for resorcinol in 1,4-dioxane
+ water mixtures and pure 1,4-dioxane at (303.15, 313.15 and 323.15) K.
Fig. 3: Apparent molal adiabatic compressibility (ΦK) against square root
of molal concentration (√ m) of resorcinol in 1,4-dioxane + water mixtures
at 303.15 K. Graphical points: 10 mass % DO (▲); 20 mass % DO (○); 30
mass % DO (●).
H OH…………......
…………….
O-H
O-H
(Resorcinol) (DO)
Vφ0 values indicates the presence of strong solute-solvent
interactions, and these interactions are strengthened with a rise in temperature and weakened with an increase in the amount of 1,4-dioxane in the mixed solvent under investigation, suggesting larger electrostriction at higher temperature and lower amount of 1,4-dioxane in the mixture.
SSVV** results indicate the presence of weak results indicate the presence of weak
solute-solute interactions which decrease with solute-solute interactions which decrease with a rise in temperature attributing to more a rise in temperature attributing to more violent thermal agitation that decreases the violent thermal agitation that decreases the ionic dissociation and it increases with an ionic dissociation and it increases with an increase in the amount of 1,4-dioxane in the increase in the amount of 1,4-dioxane in the mixture which results in a decrease in mixture which results in a decrease in solvation of ions. solvation of ions.
Negative ( Negative ( δδ22VVφφ00/ / δTδT2 2 ))PP values suggested that values suggested that
resorcinol acts as a structure breaker in these resorcinol acts as a structure breaker in these solvent mixtures solvent mixtures
Concluding RemarksConcluding Remarks Most of the present day knowledge on non-aqueous Most of the present day knowledge on non-aqueous
solutions have come from studies on various thermodynamic solutions have come from studies on various thermodynamic properties, e.gproperties, e.g.., density, transport properties, e.g, density, transport properties, e.g.., viscosity, , viscosity, conductance as well as acoustic properties, e.g., ultrasonic conductance as well as acoustic properties, e.g., ultrasonic speed.speed.
Molecular interactions are very complex in nature, if careful Molecular interactions are very complex in nature, if careful judgement is used, valid conclusions can be drawn in many judgement is used, valid conclusions can be drawn in many cases relating to degree of structure and order of the system.cases relating to degree of structure and order of the system.
Extensive studies of the different physico-chemical, Extensive studies of the different physico-chemical, biological or pharmaceutical activity between different biological or pharmaceutical activity between different components of a given mixture will be of sufficient help in components of a given mixture will be of sufficient help in understanding the nature of the different interactions prevailing understanding the nature of the different interactions prevailing in systems.in systems.
The The National SymposiumNational Symposium on Current Trends in Chemical on Current Trends in Chemical Research, organized and hosted by the Department of Research, organized and hosted by the Department of Chemistry, Gauhati University, Guwahati, Assam, India Chemistry, Gauhati University, Guwahati, Assam, India from 27th to 28th February, from 27th to 28th February, 20042004 on the topic “ on the topic “Studies on Studies on Viscous Synergy and Antagonism of Liquid Mixtures at Viscous Synergy and Antagonism of Liquid Mixtures at Various TemperaturesVarious Temperatures”.”.
The 42nd The 42nd Annual ConventionAnnual Convention of Chemists, organized by of Chemists, organized by the Indian Chemical Society, Kolkata, and hosted by Visva-the Indian Chemical Society, Kolkata, and hosted by Visva-Bharati University, Santiniketan, India during 9th to 13th Bharati University, Santiniketan, India during 9th to 13th February, February, 20062006 on the topic “ on the topic “Viscous Synergy and Viscous Synergy and Antagonism and Isentropic Compressibility of Ternary Antagonism and Isentropic Compressibility of Ternary Mixtures containing 1,3-Dioxolane, Water and Mixtures containing 1,3-Dioxolane, Water and Monoalkanols at 303.15 KMonoalkanols at 303.15 K”.”.
List of PublicationsList of Publications Investigations of Viscous Antagonism of Binary Liquid Mixtures in Investigations of Viscous Antagonism of Binary Liquid Mixtures in
the Temperature Range, 303.15 K to 323.15 K, the Temperature Range, 303.15 K to 323.15 K, Journal of Teaching Journal of Teaching and Research in Chemistryand Research in Chemistry, , 20042004, , 1111, 12-20., 12-20.
Excess Molar Volumes, Viscosity Deviations and Isentropic Excess Molar Volumes, Viscosity Deviations and Isentropic Compressibility of Binary Mixtures Containing 1,3-Dioxolane and Compressibility of Binary Mixtures Containing 1,3-Dioxolane and Monoalcohols at 303.15 K, Monoalcohols at 303.15 K, Journal of Solution ChemistryJournal of Solution Chemistry, , 20052005, , 3434, , 1311-1325.1311-1325.
Investigation on Viscous Antagonism of Ternary Liquid Mixtures Investigation on Viscous Antagonism of Ternary Liquid Mixtures and its Relation to Concentration, and its Relation to Concentration, Journal of the Indian Chemical Journal of the Indian Chemical SocietySociety, , 20052005, , 8282, 814-818., 814-818.
Solute-Solvent and Solute-Solute Interactions of Resorcinol in Mixed 1,4-Solute-Solvent and Solute-Solute Interactions of Resorcinol in Mixed 1,4-Dioxane-Water Systems at Different Temperatures, Dioxane-Water Systems at Different Temperatures, International International Journal of Thermo-physicsJournal of Thermo-physics, , 20052005, , 2626, 1549-1563., 1549-1563.
Ion-Solvent and Ion-Ion Interactions of some Tetraalkylammonium, Ion-Solvent and Ion-Ion Interactions of some Tetraalkylammonium, Alkali metals and Ammonium Halides in Isoamyl Alcohol at 298.15 K by Alkali metals and Ammonium Halides in Isoamyl Alcohol at 298.15 K by Conductometric Technique, Conductometric Technique, Journal of the Indian Chemical SocietyJournal of the Indian Chemical Society, , 20062006, , 8383, 160-164., 160-164.
Viscous Synergy and Antagonism and Isentropic Compressibility of Viscous Synergy and Antagonism and Isentropic Compressibility of Ternary Mixtures containing 1,3-Dioxolane, Water and Monoalkanols at Ternary Mixtures containing 1,3-Dioxolane, Water and Monoalkanols at 303.15 K, 303.15 K, Fluid Phase EquilibriaFluid Phase Equilibria, , 20062006, , 243243, 133-141., 133-141.
Studies of Viscous Antagonism, Excess Molar Volume and Isentropic Studies of Viscous Antagonism, Excess Molar Volume and Isentropic Compressibility in Aqueous Mixed Solvent Systems at Different Compressibility in Aqueous Mixed Solvent Systems at Different Temperatures, Temperatures, Physics and Chemistry of LiquidsPhysics and Chemistry of Liquids, , 20062006, , 4444, 303-314., 303-314.
Densities, Viscosities and Sound Speeds of some Acetate Salts in Binary Densities, Viscosities and Sound Speeds of some Acetate Salts in Binary Mixtures of Tetrahydrofuran and Methanol at (303.15, 313.15 and Mixtures of Tetrahydrofuran and Methanol at (303.15, 313.15 and 323.15) K, 323.15) K, Journal of Chemical and Engineering DataJournal of Chemical and Engineering Data, , 20062006, , 51, 51, 1415-1423.1415-1423.
Electrical Conductances of Some Ammonium and Electrical Conductances of Some Ammonium and Tetraalkylammonium Halides in Aqueous Binary Mixtures of 1,4-Tetraalkylammonium Halides in Aqueous Binary Mixtures of 1,4-Dioxane at 298.15 K, Dioxane at 298.15 K, Pakistan Journal of Scientific and Industrial Pakistan Journal of Scientific and Industrial ResearchResearch, , 20062006, , 4949, 153-159., 153-159.
Conductivity Studies of Sodium Iodide in Pure Tetrahydrofuran Conductivity Studies of Sodium Iodide in Pure Tetrahydrofuran and Aqueous Binary Mixtures of Tetrahydrofuran and 1,4-Dioxane and Aqueous Binary Mixtures of Tetrahydrofuran and 1,4-Dioxane at 298.15 K, at 298.15 K, Physics and Chemistry of LiquidsPhysics and Chemistry of Liquids, in press. , in press.
