Acoustic and volumetric properties of betaine hydrochloride drug in aqueous D(+)-glucose and sucrose solutions Suresh Ryshetti a , Akash Gupta b , Savitha Jyostna Tangeda a,⇑ , Ramesh L. Gardas b,⇑ a Department of Chemistry, Kakatiya University, Warangal 506009, India b Department of Chemistry, Indian Institute of Technology Madras, Chennai 600036, India article info Article history: Received 11 January 2014 Received in revised form 16 May 2014 Accepted 20 May 2014 Available online 29 May 2014 Keywords: Density Speed of sound Betaine hydrochloride drug Co-sphere overlap model Hepler’s constant abstract The densities (q) and speeds of sound (u) of betaine hydrochloride (B.HCl) drug (0.01 to 0.06) mol kg 1 in (0.10, 0.20 and 0.30) mol kg 1 aqueous D(+)-glucose and sucrose solutions are reported as a function of temperature at T = (293.15 to 313.15) K and atmospheric pressure. The values of density (q) and speed of sound (u) are obtained with high precision. These values have been used to estimate the apparent molar volume (V 2,/ ), partial molar volume (V 1 2 ), transfer partial molar volume (D t V 1 2 ), apparent molar isentropic compressibility (K s,2,/ ), partial molar isentropic compressibility (K 1 s;2 ), transfer partial molar compressibility (D t K 1 s;2 ), hydration number (N H ), partial molar expansion (E 1 2 ) and Hepler’s constant (@ 2 V 1 2 /@T 2 ) P . Furthermore, pair (V AB and K AB ) and triplet (V ABB and K ABB ) interaction coefficients have been computed from the values of D t V 1 2 and D t K 1 s;2 . The co-sphere overlap model is used to understand the values of D t V 1 2 and D t K 1 s;2 . The positive values of (@ 2 V 1 2 /@T 2 ) P indicate structure making ability of betaine hydrochloride in aqueous D(+)-glucose and sucrose solutions at the temperatures and compositions investigated. Ó 2014 Elsevier Ltd. All rights reserved. 1. Introduction Volumetric and acoustic properties are powerful tools to ana- lyze the behavior of various solutes such as drugs, amino acids, proteins, peptides, carbohydrates and ionic liquids in aqueous and non-aqueous solutions [1–5]. Drug-macromolecular interac- tions are playing a significant role in understanding the activity of drugs in biological systems [6]. It is difficult to study the drug activity directly in complex biological processes and the mecha- nism of these molecular processes is not yet clearly understood. Attempts are being made to interpret these drug-molecular inter- actions through thermophysical properties such as density and speed of sound [7,8]. Most of the biochemical processes occur in aqueous media. The (drug + water) molecular interactions and their temperature dependence play an important role in under- standing the drug action across the biological membrane [9]. Many researchers have studied the density, speed of sound and viscosity of (drug + water) and (drug + water + alcohol) systems and inter- preted the results in terms of (hydrophilic + hydrophilic) and (hydrophilic + hydrophobic) interactions [10–12]. The detailed literature survey reveals that thermophysical properties of the drugs in aqueous carbohydrate solutions have not been reported. This prompted us to investigate the volumetric and acoustic prop- erties of betaine hydrochloride (B.HCl) drug in water and aqueous D(+)-glucose and sucrose solutions. B.HCl drug, used as the stomach acidifier and digestive aid for the human body, finds applicability in treating abnormally low lev- els of potassium, food allergies, yeast infection, diarrhea, hay fever, thyroid disorders, etc. However more systematic studies are needed to gather the evidence to rate the effectiveness of B.HCl for these uses. In the present study, we have examined the molec- ular interactions of B.HCl drug in aqueous D(+)-glucose and sucrose solutions at low concentrations in the form of solutes and co-solutes. The experimental values of density (q) and speed of sound (u) of (0.01 to 0.06) mol kg 1 B.HCl drug in (0.1, 0.2 and 0.3) mol kg 1 aqueous D(+)-glucose and sucrose solutions have been measured at T = (293.15 to 313.15) K and atmospheric pres- sure. The results are used to calculate several parameters such as partial molar properties, hydration numbers, pair and triplet interaction coefficients and Hepler’s constant. These parameters are used to interpret the (hydrophilic + hydrophilic), (hydro- philic + hydrophobic), electrostatic interactions, structure mak- ing/breaking ability of B.HCl drug in aqueous D(+)-glucose and sucrose solutions. To the best of our knowledge from the literature survey, the values of density and speed of sound of B.HCl drug in http://dx.doi.org/10.1016/j.jct.2014.05.015 0021-9614/Ó 2014 Elsevier Ltd. All rights reserved. ⇑ Corresponding authors. Tel.: +91 9908455351 (S.J. Tangeda). Tel.: +91 44 22574248 (R.L. Gardas). E-mail addresses: [email protected](S.J. Tangeda), [email protected](R.L. Gardas). J. Chem. Thermodynamics 77 (2014) 123–130 Contents lists available at ScienceDirect J. Chem. Thermodynamics journal homepage: www.elsevier.com/locate/jct
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J. Chem. Thermodynamics 77 (2014) 123–130
Contents lists available at ScienceDirect
J. Chem. Thermodynamics
journal homepage: www.elsevier .com/locate / jc t
Acoustic and volumetric properties of betaine hydrochloride drugin aqueous D(+)-glucose and sucrose solutions
http://dx.doi.org/10.1016/j.jct.2014.05.0150021-9614/� 2014 Elsevier Ltd. All rights reserved.
Suresh Ryshetti a, Akash Gupta b, Savitha Jyostna Tangeda a,⇑, Ramesh L. Gardas b,⇑a Department of Chemistry, Kakatiya University, Warangal 506009, Indiab Department of Chemistry, Indian Institute of Technology Madras, Chennai 600036, India
a r t i c l e i n f o a b s t r a c t
Article history:Received 11 January 2014Received in revised form 16 May 2014Accepted 20 May 2014Available online 29 May 2014
Keywords:DensitySpeed of soundBetaine hydrochloride drugCo-sphere overlap modelHepler’s constant
The densities (q) and speeds of sound (u) of betaine hydrochloride (B.HCl) drug (0.01 to 0.06) mol � kg�1
in (0.10, 0.20 and 0.30) mol � kg�1 aqueous D(+)-glucose and sucrose solutions are reported as a functionof temperature at T = (293.15 to 313.15) K and atmospheric pressure. The values of density (q) and speedof sound (u) are obtained with high precision. These values have been used to estimate the apparentmolar volume (V2,/), partial molar volume (V12 ), transfer partial molar volume (DtV
1s;2), hydration number (NH), partial molar expansion (E12 ) and Hepler’s constant
(@2V12 /@T2)P. Furthermore, pair (VAB and KAB) and triplet (VABB and KABB) interaction coefficients have beencomputed from the values of DtV
12 and DtK
1s;2. The co-sphere overlap model is used to understand the
values of DtV12 and DtK
1s;2. The positive values of (@2V12 /@T2)P indicate structure making ability of betaine
hydrochloride in aqueous D(+)-glucose and sucrose solutions at the temperatures and compositionsinvestigated.
� 2014 Elsevier Ltd. All rights reserved.
1. Introduction
Volumetric and acoustic properties are powerful tools to ana-lyze the behavior of various solutes such as drugs, amino acids,proteins, peptides, carbohydrates and ionic liquids in aqueousand non-aqueous solutions [1–5]. Drug-macromolecular interac-tions are playing a significant role in understanding the activityof drugs in biological systems [6]. It is difficult to study the drugactivity directly in complex biological processes and the mecha-nism of these molecular processes is not yet clearly understood.Attempts are being made to interpret these drug-molecular inter-actions through thermophysical properties such as density andspeed of sound [7,8]. Most of the biochemical processes occur inaqueous media. The (drug + water) molecular interactions andtheir temperature dependence play an important role in under-standing the drug action across the biological membrane [9]. Manyresearchers have studied the density, speed of sound and viscosityof (drug + water) and (drug + water + alcohol) systems and inter-preted the results in terms of (hydrophilic + hydrophilic) and(hydrophilic + hydrophobic) interactions [10–12]. The detailed
literature survey reveals that thermophysical properties of thedrugs in aqueous carbohydrate solutions have not been reported.This prompted us to investigate the volumetric and acoustic prop-erties of betaine hydrochloride (B.HCl) drug in water and aqueousD(+)-glucose and sucrose solutions.
B.HCl drug, used as the stomach acidifier and digestive aid forthe human body, finds applicability in treating abnormally low lev-els of potassium, food allergies, yeast infection, diarrhea, hay fever,thyroid disorders, etc. However more systematic studies areneeded to gather the evidence to rate the effectiveness of B.HClfor these uses. In the present study, we have examined the molec-ular interactions of B.HCl drug in aqueous D(+)-glucose and sucrosesolutions at low concentrations in the form of solutes andco-solutes. The experimental values of density (q) and speed ofsound (u) of (0.01 to 0.06) mol � kg�1 B.HCl drug in (0.1, 0.2 and0.3) mol � kg�1 aqueous D(+)-glucose and sucrose solutions havebeen measured at T = (293.15 to 313.15) K and atmospheric pres-sure. The results are used to calculate several parameters such aspartial molar properties, hydration numbers, pair and tripletinteraction coefficients and Hepler’s constant. These parametersare used to interpret the (hydrophilic + hydrophilic), (hydro-philic + hydrophobic), electrostatic interactions, structure mak-ing/breaking ability of B.HCl drug in aqueous D(+)-glucose andsucrose solutions. To the best of our knowledge from the literaturesurvey, the values of density and speed of sound of B.HCl drug in
124 S. Ryshetti et al. / J. Chem. Thermodynamics 77 (2014) 123–130
aqueous D(+)-glucose and sucrose solutions have not been reportedat the concentrations and temperatures investigated in this paper.
2. Experimental
All chemicals (shown in table 1) were used after drying overP2O5 in vacuum desiccators at room temperature for 48 h. Freshlyprepared doubly distilled, degassed water with a specific conduc-tance less than 1 � 10�6 S � cm�1 was used for the preparation ofaqueous solutions. The aqueous solutions were prepared on massbasis at room temperature over a concentration range (0.01 to0.06) mol � kg�1 and kept in airtight bottles to minimize exposureof solutions to air. The mass measurements were done on an elec-tronic analytical balance (Sartorius, Model CPA225D) with a preci-sion of ±0.01 mg. We have measured the density (q) and speed ofsound (u) of solutions on the same day of sample preparation byusing Anton Paar DSA 5000M instrument. The instrument was cal-ibrated with doubly distilled water and dry air at the investigatedtemperatures; uncertainties in the measurements of density (q)and speed of sound (u) at 3 MHz frequency are ±5 � 10�3 kg �m�3
and ±0.5 m � s�1, respectively. The experiments were carried outat T = (293.15 to 313.15) K with an accuracy of ±0.01 K. The tem-peratures were controlled by a Peltier thermostat (PT 100) whichis in-built on Anton Paar DSA 5000M instrument [13].
3. Results and discussion
The densities (q) and speeds of sound (u) of B.HCl drug in water,aqueous glucose and sucrose solutions of various molalities atT = (293.15 to 313.15) K are given in table 2. The plots of density(q) and speed of sound (u) vs. molality (m) of B.HCl drug in waterat different temperatures are shown in figures 1 and 2, respec-tively. The comparison of experimental density (q) values withavailable literature data for dilute solution of D(+)-glucose andsucrose are presented in supporting information (table ST1). Asshown in table ST1, experimental density data of aqueous solutionof D(+)-glucose and sucrose are in good agreement with availableliterature data (relative deviations are within 0.1%) at T = (293.15and 298.15) K. However deviations are larger up to 0.3% for aque-ous solution of D(+)-glucose at T = (303.15 and 308.15) K. Thesedeviations can be due essentially to the purity of the sample andalso from the experimental technique adopted. As shown in thesupporting information (figure S1), experimental speeds of sound(u) values are in good agreement with available literature datafor aqueous solution of D(+)-glucose at T = 298.15 K and similartrends are observed at other studied temperatures and for aqueoussolution of sucrose also. As shown in table 2, the decreasing valuesof density (q) or increasing values of speed of sound (u) withincrease in temperature suggests the consequence of temperatureon the solvation behavior of solute. Values of the apparent molarvolume (V2,/) and apparent molar isentropic compressibility(Ks,2,/) have been calculated from the values of density (q) andspeed of sound (u) by using the following equations (1) and (2),respectively [14], the values of V2,/ and Ks,2,/ are reported in table3 and these values increase with the temperature, concentrationsof solute and co-solute.
V2;/ ¼ ½M=q� � ½1000ðq� qoÞ=ðmqqoÞ�; ð1Þ
TABLE 1Provenance and mass fraction purity of the chemicals used.
Compound Mass fraction purity CAS No. Source
Betaine HCl 0.990 590-46-5 Sigma Aldrich Co.
D(+)-glucose 0.980 50-99-7 Finar Chemical Ltd.
Sucrose 0.995 57-50-1 Himedia Laboratories
Ks;2;/ ¼ ½jsM=q� � ½1000ðjosq� jsqoÞ=ðmqqoÞ�; ð2Þ
where M and m are molar mass and molality of B.HCl drug, q and qo
refer to the density of solution and solvent (water or water + D(+)-glucose/sucrose), js and jo
s represent the isentropic compressibilityof solution and solvent, respectively. Values of isentropic compress-ibility (js) are calculated from the values of density (q) and speed ofsound (u) by using the relation [15]:
js ¼ 1=ðu2qÞ: ð3Þ
Values of the partial molar volume (V12 ) and partial molar isen-tropic compressibility (K1s;2) for B.HCl drug in water, aqueous glu-cose and sucrose solutions are reported by the least-squarefitting of the linear plots of V2,/ and Ks,2,/ against the molality(m) of B.HCl drug, respectively [16].
V2;/ ¼ V12 þ Sv �m; ð4Þ
Ks;2;/ ¼ K1s;2 þ Sk �m: ð5Þ
Here Sv and Sk are the experimental slopes. These values areaccountable for the (solute + solute) interactions. The experimentalslopes Sv and Sk are semi-empirical parameters which depend onsolvent, solute, and temperature, and for large organic solutesthese values are not of much significance [6]. The partial molarproperties (infinite dilution apparent molar properties) i.e. V12and K1s;2 indicate the (solute + solvent) interactions at infinite dilu-tion and their values are given in table 4. In the present study, posi-tive values of V12 and negative values of K1s;2 account for strong(solute + solvent) interactions between B.HCl drug and water or(water + aqueous glucose/sucrose) solutions [14]. The values ofV12 and K1s;2 increase with increasing the temperature for B.HCldrug in water and all the investigated concentrations of D(+)-glu-cose and sucrose, mainly due to releasing of water molecules fromthe second solvation layer of the ionic (AN+(CH3)3/Cl�)/hydrophilic(ACOOH) groups of B.HCl drug [17]. The values of V12 and K1s;2increase with the concentration of D(+)-glucose and sucrose, whichsuggests that, for the systems studied, the extent of molecularinteractions such as (ionic + hydrophilic) and (hydrophilic + hydro-philic) increase with solute concentration. These results (table 4)are also useful in understanding the effects of temperature andcomposition on the molecular interactions of B.HCl drug in aque-ous D(+)-glucose and sucrose solutions. Furthermore, these molec-ular interactions can be understood on the basis of the co-sphereoverlap model which is developed by Gurney et al. [18,19].Such possible interactions in a ternary mixture (B.HCl drug +water + D(+)-glucose/sucrose) can be regarded as follows:(i) ionic/(hydrophilic + hydrophilic) interactions between the ionic(AN+(CH3)3/Cl�)/hydrophilic (ACOOH) groups of B.HCl drugand (AOH, AC = O, and AOA) groups of D(+)-glucose/sucrose.(ii) ionic/(hydrophilic + hydrophobic) interaction between theionic (AN+(CH3)3/Cl�)/hydrophilic (ACOOH) groups of B.HCl drugand ACH2/ACH groups of D(+)-glucose/sucrose. (iii) (Hydropho-bic + hydrophobic) interaction between the ACH2 groups of B.HCldrug and ACH2/ACH groups of D(+)-glucose/sucrose.
Values of the transfer partial molar volume (DtV12 ) and transfer
partial molar isentropic compressibility (DtK1s;2) of B.HCl drug
in aqueous glucose and sucrose solutions are obtained from thefollowing equation [20]:
5 reveals that the values of DtX12 are free from (solute + solute)
interactions and therefore furnish information about (solute +solvent) interactions [21]. The positive values of DtX
12 indicate the
TABLE 2Density (q) and speed of sound (u) of B.HCl in water, aqueous D(+)-glucose and sucrose solutions at T = (293.15 to 313.15) K and pressure p = 0.1 MPa.a
FIGURE 1. Plot of density (q) vs. molality (m) of B.HCl drug in water attemperatures, T = �, 293.15 K; j, 298.15 K; N, 303.15 K; �, 308.15 K; ⁄, 313.15 K.
1480
1490
1500
1510
1520
1530
1540
0 0.02 0.04 0.06
u / m
.s-1
m / mol kg-1
FIGURE 2. Plot of speed of sound (u) vs. molality (m) of B.HCl drug in water attemperatures, T = �, 293.15 K; j, 298.15 K; N, 303.15 K; �, 308.15 K; ⁄, 313.15 K.
TAB
LE2
(con
tinu
ed)
m/(
mol�k
g�1)
10�
3q
/(kg�m�
3)
u/(m�s�
1)
10�
3q
/(kg�m�
3)
u/(m�s�
1)
10�
3q
/(kg�m�
3)
u/(m�s�
1)
10�
3q
/(kg�m�
3)
u/(m�s�
1)
10�
3q
/(kg�m�
3)
u/(m�s�
1)
T=
293.
15K
298.
15K
303.
15K
308.
15K
313.
15K
0.01
951
1.03
8481
1515
.10
1.03
7097
1527
.83
1.03
5505
1538
.96
1.03
3716
1548
.42
1.03
1749
1556
.31
0.02
780
1.03
8742
1516
.03
1.03
7357
1528
.70
1.03
5761
1539
.83
1.03
3962
1549
.31
1.03
1989
1557
.15
0.03
918
1.03
9099
1517
.26
1.03
7704
1529
.89
1.03
6106
1541
.03
1.03
4301
1550
.48
1.03
2317
1558
.30
0.04
702
1.03
9341
1518
.01
1.03
7939
1530
.60
1.03
6335
1541
.81
1.03
4523
1551
.21
1.03
2535
1559
.02
0.05
708
1.03
9645
1519
.07
1.03
8236
1531
.55
1.03
6627
1542
.79
1.03
4808
1552
.18
1.03
2809
1560
.00
aSt
anda
rdu
nce
rtai
nti
esu
are
u(m
)=
2�1
0�5
mol�k
g�1,u
(T)
=0.
01K
and
u(p)
=0.
01M
Pa,u
(u)
=0.
5m�s�
1an
du(
q)
=5�1
0�3
kg�m�
3.m
ism
olal
ity
ofbe
tain
eh
ydro
chlo
ride
inpe
rkg
ofw
ater
/wat
er+
suga
r.Th
ew
ater
base
isu
sed
for
bin
ary
mix
ture
s,w
hil
eth
ew
ater
and
suga
rba
seis
appl
ied
for
tern
ary
mix
ture
s.M
olal
ity
ofsu
gar
inpe
rkg
ofw
ater
ispr
epar
edw
ith
stan
dard
un
cert
ain
tyof
3�1
0�5
mol�k
g�1.
126 S. Ryshetti et al. / J. Chem. Thermodynamics 77 (2014) 123–130
presence of strong (solute + solvent) interactions in all solutionsinvestigated. According to the co-sphere overlap model, ionic/(hydrophilic + hydrophilic) (first type) interactions lead to positivevalues of DtX
type) and (hydrophobic + hydrophobic) (third type) interactionslead to negative values of DtX
12 . In the present study, the positive
values of DtX12 indicate the presence of ionic/(hydrophilic + hydro-
philic) (first type) interactions in aqueous D(+)-glucose and sucrosesolutions. Moreover, these interactions increase with increase in theconcentration of D(+)-glucose and sucrose. The higher DtX
12 values
for sucrose solutions as compared to D(+)-glucose solutions areaccountable for more ionic/(hydrophilic + hydrophilic) (first type)interactions in sucrose solutions. The values of DtX
12 increase with
temperature and this may be ascribed to decreasing of electrostrict-ed water molecules around the ionic (AN+(CH3)3/Cl�)/hydrophilic(ACOOH) groups of B.HCl drug [17].
The values of V12 can be explained by Shahidi’s equation [22]:
V12 ¼ Vv�w þ Vvoid � V shrinkage; ð7Þ
TABLE 3Apparent molar volumes (V2,/) and apparent molar isentropic compressibilities (Ks,2,/) of B.HCl in water, aqueous D(+)-glucose and sucrose solutions at T = (293.15 to 313.15) Kand pressure p = 0.1 MPa.a
a Standard uncertainties u are u(m) = 2 � 10�5 mol � kg�1, u(T) = 0.01 K and u(p) = 0.01 MPa. m is molality of betaine hydrochloride in per kg of water/water + sugar. The waterbase is used for binary mixtures, while the water and sugar base is applied for ternary mixtures. Molality of sugar in per kg of water is prepared with standard uncertainty of3 � 10�5 mol � kg�1.
S. Ryshetti et al. / J. Chem. Thermodynamics 77 (2014) 123–130 127
where Vv�w is the van der Waal’s volume, Vvoid is the volume associ-ated with voids and Vshrinkage is the shrinkage volume due toelectrostriction. The Vv�w and Vvoid are assumed to be constant inD(+)-glucose and sucrose solutions; Vshrinkage is the shrinkage vol-ume caused by interactions of hydrogen bonding groups of solutewith water molecules [13]. The positive values of DtV
12 indicate
the decrease in Vshrinkage in the presence of D(+)-glucose and sucrose[23], which is found to decrease with increasing temperature andthe concentration of D(+)-glucose and sucrose.
The values obtained for transfer partial molar volume (DtV12 )
and transfer partial molar isentropic compressibility (DtK1s;2) of
B.HCl drug in aqueous glucose and sucrose solutions can also beexpressed as follows [24]:
DtX12 ¼ 2XABmB þ 3XABBm2
B þ � � � ; ð8Þ
where A stands for solute and B for co-solute, the constants XAB (VAB
or KAB) and XABB (VABB or KABB) are pair and triplet volumetric orcompressibility interaction coefficients, respectively. The values ofDtX
12 have been fitted in equation (8) to get XAB (VAB or KAB) and
XABB (VABB or KABB) interaction coefficients, which are given in table6. The XAB and XABB values are positive for all solutions investigated.This may be due to strong (solute + solvent) interactions in the solu-tions investigated [25,26].
The hydration numbers (NH) of B.HCl drug in aqueous D(+)-glu-cose and sucrose solutions have been calculated at temperaturesinvestigated by using the method reported by Millero et al. [27] as:
TABLE 4Partial molar properties V12 and K1s;2 of B.HCl in aqueous D(+)-glucose and sucrose solutions at T = (293.15 to 313.15) K and pressure p = 0.1 MPa.a
106V12 /(m3 �mol�1) 106K1s;2/(m3 �mol�1 � GPa�1)
T = 293.15 K 298.15 K 303.15 K 308.15 K 313.15 K 293.15 K 298.15 K 303.15 K 308.15 K 313.15 K
a Standard uncertainties u are u(T) = 0.01 K and u(p) = 0.01 MPa. The water base is used for binary mixtures, while the water and sugar base is applied for ternary mixtures.Molality of betaine hydrochloride in per kg of water/water + sugar is prepared with standard uncertainty of 2 � 10�5 mol � kg�1. Molality of sugar in per kg of water is preparedwith standard uncertainty of 3 � 10�5 mol � kg�1.
TABLE 5Transfer partial molar properties DtV
12 and DtK
1s;2of B.HCl in aqueous D(+)-glucose and sucrose solutions at T = (293.15 to 313.15) K and pressure p = 0.1 MPa.a
106DtV12 /(m3 �mol�1) 106DtK
1s;2/(kg �m3 �mol�2 � GPa�1)
T = 293.15 K 298.15 K 303.15 K 308.15 K 313.15 K 293.15 K 298.15 K 303.15 K 308.15 K 313.15 K
a Standard uncertainties u are u(T) = 0.01 K and u(p) = 0.01 MPa. The water base is used for binary mixtures, while the water and sugar base is applied for ternary mixtures.Molality of betaine hydrochloride in per kg of water/water + sugar is prepared with standard uncertainty of 2 � 10�5 mol � kg�1. Molality of sugar in per kg of water is preparedwith standard uncertainty of 3 � 10�5 mol � kg�1.
TABLE 6Pair XAB and triplet XABB interaction coefficients of B.HCl in aqueous D(+)-glucose and sucrose solutions at T = (293.15 to 313.15) K and pressure p = 0.1 MPa.a
T/K From volume From compressibility
106VAB/(m3 �mol�2 � kg) 106VABB/(m3 �mol�3 � kg2) 106KAB/(m3 �mol�2 � kg � GPa�1) 106KABB/(m3 �mol�3 � kg2 � GPa�1)
a Standard uncertainties u are u(T) = 0.01 K and u(p) = 0.01 MPa. The water base is used for binary mixtures, while the water and sugar base is applied for ternary mixtures.Molality of betaine hydrochloride in per kg of water/water + sugar is prepared with standard uncertainty of 2 � 10�5 mol � kg�1. Molality of sugar in per kg of water is preparedwith standard uncertainty of 3 � 10�5 mol � kg�1.
128 S. Ryshetti et al. / J. Chem. Thermodynamics 77 (2014) 123–130
NH ¼ � K1s;2 ðelectÞ=ðK1s � V11 Þ
h i; ð9Þ
where K1s;2 (elect) is the electrostriction partial molar compressibil-ity, K1s is the compressibility of bulk water or bulk solvent, V11 is themolar volume of bulk water or bulk solvent. The K1s;2 (elect) valuescan be calculated by using the equation:
K1s;2 ðelectÞ ¼ K1s;2 ðsoluteÞ � K1 ðintÞ; ð10Þ
where K1 (int) is the intrinsic partial molar isentropic compressibil-ity of solute. It is assumed that K1 (int) � 0 [27], then K1s;2 (elect)becomes equal to K1s;2 (solute). The NH values (table 7) for theB.HCl drug studied are less in the presence of D(+)-glucose/sucrose
TABLE 8Partial molar expansions (E12 ) of B.HCl in aqueous D(+)-glucose and sucrose solutions at T = (293.15 to 313.15) K and pressure p = 0.1 MPa.a
a Standard uncertainties u are u(T) = 0.01 K and u(p) = 0.01 MPa. The water base is used for binary mixtures, while the water and sugar base is applied for ternary mixtures.Molality of betaine hydrochloride in per kg of water/water + sugar is prepared with standard uncertainty of 2 � 10�5 mol � kg�1. Molality of sugar in per kg of water is preparedwith standard uncertainty of 3 � 10�5 mol � kg�1.
TABLE 9The values of (@C1p;2/oP)T and (o2V12 /oT2)P of B.HCl in aqueous D(+)-glucose and sucrose solutions at T = (293.15 to 313.15) K and pressure p = 0.1 MPa.a
a Standard uncertainties u are u(T) = 0.01 K and u(p) = 0.01 MPa. The water base is used for binary mixtures, while the water and sugar base is applied for ternary mixtures.Molality of betaine hydrochloride in per kg of water/water + sugar is prepared with standard uncertainty of 2 � 10�5 mol � kg�1. Molality of sugar in per kg of water is preparedwith standard uncertainty of 3 � 10�5 mol � kg�1.
S. Ryshetti et al. / J. Chem. Thermodynamics 77 (2014) 123–130 129
as compared to their values in water, and these values decreasewith further increase in concentration of D(+)-glucose/sucrose. Thevalues of NH also decrease with the increase in temperature. Theseresults indicate the effect of temperature and concentrations ofD(+)-glucose and sucrose on the dehydration of B.HCl drug in solu-tions studied.
The temperature dependence of V12 can be determined by thefollowing expression.
V12 ¼ a0 þ a1T þ a2T2; ð11Þ
where T is the temperature in Kelvin. The values of coefficients ao,a1 and a2 were estimated by the least-squares fitting of the valuesof V12 in equation (11). The partial molar expansion (E12 ) can beincurred by differentiating equation (11) with respect to tempera-ture and these E12 values are shown in table 8.
E12 ¼ ð@V12 =@TÞP ¼ a1 þ 2a2T: ð12Þ
It is clear from table 8 that the positive values of E12 indicate thepresence of strong (solute + solvent) interactions in all solutionsinvestigated. Further these E12 values increase with increasing tem-perature at all compositions of D(+)-glucose and sucrose. Roy et al.also observed the increasing E12 values along with increasing tem-perature in a ternary mixture [28].
The qualitative information on hydration of solutes in solutionscan be obtained with the help of Hepler’s equation on the basis ofthe sign of the expression [29].
@C1p;2=@P� �
T¼ �Tð@2V12 =@T2ÞP: ð13Þ
It has been suggested that the positive values of (o2V12 /oT2)P (ornegative values of ((@C1p;2/oP)T) are associated with structure mak-ing and negative values of (o2V12 /oT2)P (or positive values of((@C1p;2/oP)T) for structure breaking nature of solute molecules insolutions [29]. In the present investigation (table 9), the positive
values of (o2V12 /oT2)P indicate the structure making effect of theB.HCl drug in D(+)-glucose and sucrose solutions, which increaseswith increasing the concentrations of D(+)-glucose and sucrose.
4. Conclusions
In the present study, the partial molar properties, transfer par-tial molar properties, pair and triplet interaction coefficients andhydration numbers have been computed from the densities (q)and speeds of sound (u) of B.HCl drug in water, aqueous D(+)-glu-cose and sucrose solutions. These parameters indicate the presenceof ionic/(hydrophilic + hydrophilic) interactions between the ionic(AN+(CH3)3/Cl�)/hydrophilic (ACOOH) groups of B.HCl drug and(AOH, AC = O, and AOA) groups of D(+)-glucose/sucrose and arebeing influenced by the concentration of D(+)-glucose and sucroseas well as the experimental temperatures. The decrease in electro-striction of water molecules around the ionic (AN+(CH3)3/Cl�)/hydrophilic (ACOOH) groups of B.HCl drug has been noted withincreasing temperature and concentration of D(+)-glucose andsucrose. The positive values of (o2V12 /oT2)P indicate the structuremaking ability of B.HCl drug in D(+)-glucose and sucrose solutions.
Acknowledgments
One of the authors (Suresh Ryshetti) is thankful to UniversityGrants Commission (UGC), Govt. of India for the financial supportin form of Junior Research Fellowship (JRF). Authors are thankfulto Council of Scientific and Industrial Research (CSIR) and Depart-ment of Science and Technology (DST) for their financial support.
Appendix A. Supplementary data
Supplementary data associated with this article can be found, inthe online version, at http://dx.doi.org/10.1016/j.jct.2014.05.015.
[2] G.R. Hedwig, J. Chem. Thermodyn. 23 (1991) 123–127.[3] R.L. Gardas, D.H. Dagade, J.A.P. Coutinho, K.J. Patil, J. Phys. Chem. B 112 (2008)
3380–3389.[4] R.D. Lisi, S. Milioto, M. Castagnolo, A. Inglese, J. Solution Chem. 19 (1990) 767–
791.[5] A. Kumar, T. Singh, R.L. Gardas, J.A.P. Coutinho, J. Chem. Thermodyn. 40 (2008)
32–39.[6] M.J. Iqbal, M.A. Chaudhry, J. Chem. Thermodyn. 41 (2009) 221–226.[7] D.V. Jahagirdhar, B.R. Arbad, S.R. Mirgane, M.K. Lande, A.G. Shankarwar, J. Mol.
Liq. 75 (1998) 33–43.[8] A.L. Surdo, C. Shin, F. Millero, J. Chem. Eng. Data 23 (1978) 197–201.[9] S.S. Dhondge, S.P. Zodape, D.V. Parwate, J. Chem. Thermodyn. 48 (2012) 207–
212.[10] H. Kumar, K. Kaur, J. Chem. Eng. Data 58 (2013) 203–208.[11] P. Sharma, S. Chauhan, V.K. Syal, M.S. Chauhan, Int. J. Thermophys. 29 (2008)
643–655.[12] P. Sharma, S. Chauhan, M.S. Chauhan, V.K. Syal, Indian J. Pure Appl. Phys. 46
(2008) 839–843.[13] V. Singh, P.K. Chhotaray, R.L. Gardas, J. Chem. Thermodyn. 71 (2014) 37–49.
[14] A.K. Nain, R. Pal, R.K. Sharma, J. Chem. Thermodyn. 43 (2011) 603–612.[15] S.H. Baluja, A. Solanki, N. Kachhadia, Russ. J. Phys. Chem. A 81 (5) (2007) 742–
746.[16] A. Pal, N. Chauhan, J. Mol. Liq. 149 (2009) 29–36.[17] M. Riyazuddeen, A. Usmani, J. Chem. Eng. Data 56 (2011) 3504–3509.[18] R.W. Gurney, Ionic Processes in Solution, McGraw Hill, New York, 1953.[19] H.S. Frank, M.W. Evans, J. Chem. Phys. 13 (1945) 507–532.[20] Z. Yan, W. Jianji, J. Lu, J. Chem. Eng. Data 46 (2001) 217–222.[21] A. Pal, S. Soni, J. Chem. Eng. Data 58 (2013) 18–23.[22] F. Shahidi, P.G. Ferrell, J.T. Edwards, J. Solution Chem. 5 (1976) 807–816.[23] T.S. Banipal, J. Kaur, P.K. Banipal, A.K. Sood, K. Singh, J. Chem. Eng. Data 56
(2011) 2751–2760.[24] W.G. McMillian, J. Mayer, J. Chem. Phys. 13 (1945) 276–305.[25] A. Pal, S. Kumar, J. Chem. Thermodyn. 37 (2005) 1085–1092.[26] T.S. Banipal, H. Singh, P.K. Banipal, J. Chem. Eng. Data 55 (2010) 3827–3881.[27] F.J. Millero, L.S. Antonio, S. Charles, J. Phys. Chem. 82 (1978) 784–792.[28] M.N. Roy, R.K. Das, A. Bhattacharjee, Russ. J. Phys. Chem. A 84 (13) (2010)
2201–2210.[29] L.G. Hepler, Can. J. Chem. 47 (1969) 4613–4617.