Analysis of Thermo Physical Properties of Binary Liquid Mixtures Containing Cyclic Diether with n-Alkanols (C₅-C₁₀) at 298.15 K: By Ultrasonic Velocity Measurements

Dhirendra Kumar Sharma^1*, Suneel Kumar¹, Akil Khan²

¹Department of Chemistry, Institute of Basic Science, Bundelkhand University, Jhansi, India.
²Department of Chemistry, Government College, Bandri, India.

DOI: 10.4236/ojpc.2025.152003                

Abstract

Ultrasonic velocity, viscosity and density measurements were calculated at 298.15 K for binary mixtures of cyclic diether (X₁) with primary alcohols. Based on the experimental data, several acoustical parameters were computed, including adiabatic compressibility (β_ad), specific acoustic impedance (Z), and molar volume (Vₘ). These parameters provide valuable insights into molecular interactions, structural modifications, and deviations from ideal behavior in the all studied mixtures. The excess properties have been fitted in Redlich-Kister equation. The results suggest the presence of molecular interactions in the studied mixtures, with dipole-induced interactions being the dominant force. These findings provide insight into the intermolecular interaction present in the studied mixtures, highlighting the influence of structural and electronic factors on their behavior.

Keywords

1, 3-Dioxolane, Density, Inter Molecular Interactions, Acoustical Impedance, Molar Volume, Ultrasonic Velocity

1. Introduction

Ultrasonic velocity measurements are widely recognized as a powerful tool for studying molecular interactions, structural properties, and thermodynamic behavior in both components [1]-[5]. Sound velocity is a key parameter for understanding molecular interactions and complex formation in liquid mixtures [6] [7]. The main use of cyclic diether and alkanols in many industrial processes such as pharmaceutical and cosmetics has greatly stimulated the need for extensive information on the thermodynamic, acoustic and transport properties of cyclic diether, alkanols and their mixtures. The work described in this paper belongs to a systematic study program concerning the measurement and mathematical description of various thermodynamic properties of binary liquid mixtures containing important compounds. The study of thermodynamic properties of binary mixtures of alkanols with 1,3-dioxolane is of great importance both from a practical and theoretical point of view. The experimental determined parameters in solute-solvent mixtures provide critical data for computing various thermodynamic and acoustical parameters. These parameters provide valuable information regarding interactions in the mixtures [8] [9]. Many researchers have extensively studied transport and thermodynamic properties of binary liquids, structural effects, and deviation from ideal behaviour [10]-[12]. The ultrasonic method is widely applicable in investigating the molecular interactions in liquid mixtures, because it provides insights into structural changes, compressibility, and bonding interactions at a molecular level. Density, sound velocity and viscosity determined have been widely utilized in liquid and liquid mixtures. Present paper investigates behavior of binary solutions, providing insights into their intermolecular forces and structural modifications.

2. Experimental Procedure

2.1. Materials

Cyclic diether (1,3-dioxolane) and primary alcohols (pentanol, hexanol, heptanol, octanol, nonanol and decanol) were purchased from CDH Ltd., New Delhi, India. All the chemicals were stored in dark bottles over freshly activated molecular sieve to minimize adsorption of moisture. All chemicals were purified by standard methods like distillation and fractional distillation under reduce pressure, and only the middle fractions were collected. Before use, the chemicals were stored over 0.4 nm molecular sieves for about 48 h to remove water and gas. It sounds like you’re ensuring the reliability of your experimental data by comparing the density, viscosity, and ultrasonic velocity of the studied chemicals with different citations [13]-[22]. This verification process is crucial for validating the liquid and liquid mixtures.

2.2. Apparatus and Procedure

Binary liquid mixtures are prepared by mixing appropriate volumes of the liquid components in the specially designed glass bottles with air tight Teflon coated caps and mass measurements performed on a analytical single pan balance (Model K-15 Deluxe, K Roy Instruments Pvt. Ltd.) with an accuracy of ± 0.00001 × 10⁻³ kg. The possible error in the mole fraction was estimated to be less than 1 × 10⁻⁴. Five samples were prepared for one system, and their density, viscosity and sound velocity were measured on the same day (Table 1).

Table 1. Practically values and Quoted data for densities (ρ), sound velocity (u), viscosity (η) of pure components at T = 298.15 K.

Chemical	Density, ρ (g.cm−3)		Sound velocity, u (m.s−1)		Viscosity, η (mPa s)
	Experimental	Quote Values	Experimental	Quote Values	Experimental	Quote Values
1,3-Dioxolane	1.0616	1.057717	1340	133817	0.5885	0.587817
		1.058617		133818		0.587317
Pentanol	0.8124	0.810813	1198	119716	3.3978	3.541113
		0.810713		126822		3.542413
Hexanol	0.8176	0.818713	1306	130415	4.6091	4.592413
		0.815215		130315		4.593213
Heptanol	0.8196	0.818713	1325	132715	5.9066	5.944313
		0.819719		1327.3724		5.9443224
Octanol	0.8236	0.821613	1350	134814	7.1508	7.660513
		0.821813		134722		7.598113
Nonanol	0.8248	0.824415	1366	136515	8.9258	9.023021
		0.82422415		136424		9.020024
Decanol	0.8292	0.826715	1378	138015	11.8027	11.82515
		0.826419		137924		11.82915

2.3. Measurements

Density: The density was determined at the experimental temperature using a 25 mL capacity specific gravity bottle immersed in the thermostatic bath. The volume of the bottle at the experimental temperature viz 298.15K was ascertained using distilled water.

Sound velocity: Sound velocity determined by the multi-frequency interferometer at 3 MHz and 298.15 K, A fixed frequency generator working at 3 MHz. its resonant frequency, the crystal undergoes rapid mechanical oscillations, generating ultrasonic waves. These waves can propagate through the liquid in the vessel, creating effects like cavitation, acoustic streaming, or enhanced mixing.

The ultrasonic velocity (U) was determined using the following formula:

U = λ. f (1)

Viscosity: An experimental setup for measuring the viscosity by Ostwald viscometer. The viscometer was calibrated using distilled water at 298.15 K, and multiple measurements (five repetitions) were taken for each sample to ensure accuracy. The uncertainty in viscosity measurement is given as ± 0.005 × 10⁻³ mPa·s, indicating high precision.

3. Theoretical

The molar volume (V_m) has been determined as:

V_m = $\frac{\left(X_1{M}_1+ X_2{M}_2\right)}{\rho }$ (2)

The adiabatic compressibility $({\beta }_{ad})$ is typically measuring the equation:

${\beta }_{ad}$ = $\frac{1}{u^2\rho }$ (3)

where ρ in (g/cm³ or kg/m³), u in (m/s or cm/s).

This equation is based on the relationship between compressibility and the propagation of sound waves in a medium. The lower the speed of sound in a liquid, the higher its compressibility.

The acoustic impedance was determined by

Z = ρ. u (4)

To calculate the excess parameters of all acoustical properties were computed using the relation:

$A^E$ = $A_{exp.}$ − A_ideal (5)

where A_ideal = ($X_1{A}_1$ + $X_2{A}_2$ ), A is any acoustical parameter and $X_1{A}_1$ and $X_2{A}_2$ is mole fractions of cyclic diether and primary alcohols.

4. Result and Discussion

The practically determined density (ρ), viscosity ($\eta$ ) and sound velocity (u) for the binary liquid at 298.15K are reported in Table 2. Table 2 represents the calculated values of adiabatic compressibility$({\beta }_{ad}),$ molar volume (V_m) and acoustic impedance (Z) for the binary mixtures and their excess data are presented in Table 3.

A perusal of Table 2 shows the mole fraction (X₁) of cyclic diether increases, density and ultrasonic velocity increase, while viscosity decreases. This trend can be explained by molecular interactions in the system: When 1,3-Dioxolane is added, it likely leads to closer packing of molecules due to molecular interactions, such as dipole-induced dipole forces.

Table 2. Density (ρ), sound velocity (u), viscosity (η), calculated adiabatic compressibility $({\text{β}}_{\text{ad}}),$ molar volume (Vₘ), and acoustic impedance (Z), of liquid mixtures of cyclic diether vs alkanols at experimental temperature.

Mole fraction 1,3-Dioxolane (x1)	Density (ρ) g.cm−3	Speed of Sound (u) ms−1	Viscosity ($\eta$ ) mPa.s	Adiabatic compressibility $({\beta }_{ad})$ × 10−7Pa−1	Molar volume (Vm) × 10−3 cm3.mole−1	Acoustic impedance (Z) × 10−4 g.cm..s−1
1,3-Dioxolane + Pentanol
0	0.8124	1198	3.3978	8.5770	0.1085	0.0973
0.0939	0.8276	1284	2.3973	7.3290	0.1049	0.1062
0.1942	0.8436	1290	1.8970	7.1233	0.1012	0.1088
0.2941	0.8640	1296	1.4437	6.8909	0.0972	0.1119
0.3942	0.8836	1300	1.1866	6.6966	0.0934	0.1148
0.4787	0.9068	1304	1.0904	6.4853	0.0897	0.1182
0.5999	0.9316	1310	0.9311	6.2551	0.0855	0.1220
0.6972	0.9596	1318	0.7717	5.9991	0.0816	0.1264
0.7928	0.9876	1324	0.7171	5.7762	0.0779	0.1307
0.9035	1.0260	1332	0.6489	5.4934	0.0735	0.1366
1.0000	1.0616	1340	0.5885	5.246	0.0697	0.1422
1,3-Dioxolane + Hexanol
0	0.8176	1306	4.6091	7.1709	0.1249	0.1067
0.0912	0.8252	1317	3.3826	6.9867	0.1207	0.1086
0.1955	0.8432	1320	2.3306	6.8065	0.1146	0.1113
0.2923	0.8584	1322	1.9839	6.6657	0.1094	0.1134
0.3982	0.8792	1325	1.5720	6.4786	0.1034	0.1164
0.4942	0.8992	1327	1.3059	6.3154	0.0981	0.1193
0.6059	0.9264	1330	1.0343	6.1024	0.0919	0.1232
0.6976	0.9508	1332	0.9131	5.9279	0.0868	0.1266
0.8018	0.9836	1335	0.7680	5.7045	0.0809	0.1313
0.8914	1.0168	1337	0.7304	5.5018	0.0758	0.1359
1.0000	1.0616	1340	0.5885	5.2460	0.0697	0.1422
1,3-Dioxolane + Heptanol
0	0.8196	1325	5.9066	6.9497	0.1417	0.1085
0.0928	0.8304	1334	4.3181	6.7671	0.1352	0.1107
0.1905	0.8412	1334	3.2577	6.6802	0.1286	0.1122
0.2939	0.8592	1335	2.5895	6.5304	0.1208	0.1147
0.3894	0.8740	1335	1.9926	6.4199	0.1141	0.1166
0.4818	0.8916	1336	1.5315	6.2837	0.1075	0.1191
0.6021	0.9184	1337	1.2190	6.0912	0.0989	0.1227
0.6952	0.9420	1337	1.0959	5.9387	0.0922	0.1259
0.7892	0.9756	1338	0.9903	5.7255	0.0850	0.1305
0.9006	1.0156	1339	0.7057	5.4918	0.0770	0.1359
1.0000	1.0616	1340	0.5885	5.2460	0.0697	0.1422
1,3-Dioxolane + Octanol
0	0.8296	1350	7.1508	6.6622	0.1581	0.1111
0.0885	0.8296	1350	5.6095	6.6139	0.1509	0.1119
0.1967	0.8464	1349	3.9321	6.4923	0.1408	0.1141
0.2998	0.8560	1348	3.2616	6.4291	0.1324	0.1153
0.3902	0.8712	1348	2.4284	6.3168	0.1243	0.1174
0.4963	0.8876	1348	1.9058	6.2002	0.1153	0.1196
0.6008	0.9140	1347	1.3631	6.0301	0.1055	0.1231
0.6925	0.9340	1348	1.1376	5.8921	0.0978	0.1259
0.7975	0.9676	1348	0.9141	5.6875	0.0883	0.1304
0.8940	1.0104	1348	0.7652	5.4466	0.0792	0.1362
1.0000	1.0616	1340	0.5885	5.2460	0.0697	0.1422
1,3-Dioxolane + Nonanol
0	0.8248	1366	8.9258	6.4976	0.1749	0.1126
0.0876	0.8336	1366	6.8601	6.4289	0.1656	0.1138
0.1913	0.8404	1363	5.8531	6.4051	0.1556	0.1145
0.2942	0.8504	1359	4.4022	6.3671	0.1453	0.1155
0.3963	0.8692	1355	3.1558	6.2662	0.1339	0.1177
0.4959	0.8844	1352	2.3340	6.1859	0.1237	0.1195
0.6050	0.9092	1349	1.7321	6.0439	0.1119	0.1226
0.6947	0.9332	1346	1.3334	5.9145	0.1023	0.1256
0.7993	0.9648	1343	0.9642	5.7466	0.0913	0.1295
0.9013	1.0084	1340	0.8031	5.5228	0.0803	0.1351
1	1.0616	1340	0.5885	5.2460	0.0697	0.1422
1,3-Dioxolane + Decanol
0	0.8292	1378	11.8027	6.4976	0.1908	0.1142
0.0881	0.8364	1374	8.5615	6.4289	0.1803	0.1149
0.191	0.8396	1370	7.8207	6.4051	0.1693	0.1150
0.2921	0.8560	1366	5.5340	6.3671	0.1561	0.1169
0.3937	0.8672	1362	4.2319	6.2662	0.1442	0.1181
0.4956	0.8824	1358	3.4173	6.1859	0.1320	0.1198
0.604	0.9076	1353	2.5370	6.0439	0.1183	0.1227
0.7129	0.9308	1348	1.5262	5.9145	0.1055	0.1254
0.7983	0.9616	1344	1.1637	5.7466	0.0946	0.1292
0.8971	1.0040	1340	0.8623	5.5228	0.0824	0.1345
1	1.0616	1340	0.5885	5.246	0.0697	0.1422

4.1. Excess Molar Volume ($V_m^E$ )

Calculation of molar volume (V_m) and deviation in molar volume ($V_m^E$ ) for liquid mixtures of cyclic diether with primary alcohols at experimental temperature using experimental density values (ρ). These values reported in Table 2 and Table 3. As the mole fraction of cyclic diether (X₁) increases, molar volume (Vm) decreases for all binary mixtures. This suggests that 1,3-Dioxolane molecules may be filling the voids between alcohol molecules. The reduction in molar volume often points to dipole-induced dipole interactions, where the presence of 1,3-Dioxolane alters the hydrogen bonding network of the alcohols.

These positive values of $V_m^E$ are indicate volume expansion upon mixing. This suggests that intermolecular interactions are weaker in the pure components. The hydrogen bonds in primary alcohols are break and the formation of new, but weaker dipole-induced dipole interactions with 1,3-Dioxolane contribute to positive excess molar volumes. The physical contributions comparing of dispersive forces or weak dipole-dipole interaction lead to positive $V_m^E$ values. Chemical contributions include breaking up of associate present in pure liquids resulting in positive $V_m^E$ and specific interaction like formation of strong hydrogen bonds, charge-transfer complex and other complex forming interactions including strong dipole-dipole interaction between component molecules. The trend is consistent across all liquid mixtures. From Marcus [23], alkanols molecules are joined by hydrogen bonding in pure liquid state (Figure 1). The graphical analysis of ($V_m^E$ ) vs. X₁ in Figure 2 should exhibit a positive deviation, possibly showing a peak, indicating the strongest deviation at a particular composition. This behavior highlights that molecular interactions change non-linearly with composition.

Figure 1. Hydrogen bonding present in cyclic diether—n-Alkanols.

Figure 2. Excess molar volume ($V_m^E$ ) versus mole fraction (X₁) of the 1,3-dioxolane at experimental temperature.

4.2. Excess Adiabatic Compressibility (${\beta }_{ad}^E$ )

The deviation of adiabatic compressibility (${\beta }_{ad}^E$ ) of liquid mixtures provides valuable insights into the intermolecular interactions between cyclic diether and primary alcohols at experimental temperature. When excess adiabatic compressibility (${\beta }_{ad}^E$ ) values is positive. This suggests that weaker intermolecular forces (such as dipole-induced dipole interactions) dominate over stronger hydrogen bonds. When excess adiabatic compressibility (${\beta }_{ad}^E$ ) values is negative [24] then, the mixture is less compressible than expected. This indicates stronger molecular interactions. Tighter molecular packing reduces compressibility [25]. When considering excess adiabatic compressibility (${\beta }_{ad}^E$ ), then it is known that contributions heptanol, octanol, nonanol and decanol gives positive values, while pentanol and hexanol contribute negative values. Having in mind the various contributions operating in the studied systems, then the positive values of excess adiabatic compressibility (${\beta }_{ad}^E$ ), in Figure 3 can be attributed mainly to the disruption of the H-bonded structures as the alkanol molecule. The negative values of excess adiabatic compressibility (${\beta }_{ad}^E$ ), in the lack of c-atom region indicate that complex formation occurred through π… HO bonding between the π electron cloud of the aromatic ring of 1,3-dioxolane and the hydroxyl group of alkanol.

Figure 3. Excess adiabatic compressibility (${\beta }_{ad}^E$ ) versus mole fraction (X₁) of the 1,3-dioxolane at experimental temperature.

The excess adiabatic compressibility (${\beta }_{ad}^E$ ) values of 1,3-dioxolane and primary alkanols is insightful or aligns well with molecular interaction principles. When excess adiabatic compressibility (${\beta }_{ad}^E$ ) is negative, it shows that the experimental liquid mixture is less compressible from ideal mixing. When excess adiabatic compressibility (${\beta }_{ad}^E$ ) values is positive, it means the mixture is more compressible than expected. This occurs when dispersion forces (van der Waals interactions) dominate over specific hydrogen bonding, leading to: (1) Weaker inter molecular forces in the mixture than in pure components. (2) Increased free volume and looser packing, allowing the liquid to be more compressible. (3) Possible disruption of alcohol-alcohol hydrogen bonding without strong alternative interactions.

The excess adiabatic compressibility (${\beta }_{ad}^E$ ) values of 1,3-Dioxolane with alcohols are expected to follow a trend based on the strength of intermolecular interactions and molecular packing efficiency. Given your previous observations values of (${\beta }_{ad}^E)$ negative or positive, order is reflected to relative dominance of dipole-dipole interactions, hydrogen bonding, and dispersion forces in each binary mixture.

Since shorter alcohols have stronger hydrogen bonding interactions, leading to more negative (${\beta }_{ad}^E$ ) and longer alcohols exhibit increased dispersion forces, leading to more positive (${\beta }_{ad}^E$ ).

Table 3. Calculated excess adiabatic compressibility (${\beta }_{ad}^E$ ), excess molar volume ($V_m^E$ ), and excess specific acoustic impedance (Z^E) and excess viscosity (η^E), of liquid mixtures of cyclic diether vs alkanols at experimental temperature.

Mole fraction 1,3-Dioxolane (x1)	Excess adiabatic compressibility (${\beta }_{ad}^E$ ) × 10−7Pa−1			Excess viscosity (ηE) mPa.s	Excess molar volume ($V_m^E$ ) × 10−3 cm3.mole−1		Excess acoustic impedance (ZE) × 10−4 g.cm.s−1
1,3-Dioxolane + Pentanol
0	-			-	-		-
0.0939	−93.514			−0.7367	0.0469		−47.19498
0.1942	−80.677			−0.9552	0.2682		−27.73692
0.2941	−70.644			−1.1280	0.1192		−14.35296
0.3942	−56.727			−1.1038	0.2446		−1.68484
0.4787	−49.711			−0.9627	0.1860		−5.86255
0.5999	−32.372			−0.7815	0.2867		−22.3876
0.6972	−25.563			−0.6675	0.1314		−21.7466
0.7928	−15.997			−0.4535	0.1568		−21.869
0.9035	−7.400			−0.2108	0.0076		−12.5556
1.0000	-			-	-		-
1,3-Dioxolane + Hexanol
0	-			-	-		-
0.0912	−12.864			−0.8597	0.7779		−13.3654
0.1955	−11.193			−1.4925	0.4810		−24.1169
0.2923	−93.762			−1.4500	0.6245		−36.6767
0.3982	−77.201			−1.4361	0.4952		−44.1104
0.4942	−61.541			−1.3162	0.4919		−49.8688
0.6059	−45.638			−1.1387	0.3860		−50.6217
0.6976	−32.537			−0.8912	0.3783		−48.7995
0.8018	−20.169			−0.6174	0.2564		−39.1249
0.8914	−1.060			−0.2947	0.0816		−24.5556
1.0000	-			-	-		-
1,3-Dioxolane + Heptanol
0	-			-	-		-
0.0928	2.457			−1.0951	0.1293		−9.44037
0.1905	5.504			−1.6358	0.5357		−27.9265
0.2939	8.146			−1.7541	0.2168		−37.8571
0.3894	13.359			−1.8431	0.4437		−50.2419
0.4818	15.486			−1.8128	0.4770		−56.9538
0.6021	16.733			−1.4856	0.4818		−60.7204
0.6952	17.334			−1.1136	0.5437		−60.5022
0.7892	12.039			−0.7193	0.0752		−46.2414
0.9006	7.647			−0.4114	0.1264		−29.2001
1.0000	-			-	-		-
1,3-Dioxolane + Octanol
0		-	-			-	-
0.0885		7.713	−1.0951			0.6846	−19.3955
0.1967		10.869	−1.6358			0.0682	−31.1779
0.2998		19.142	−1.7541			0.8340	−51.1151
0.3902		20.728	−1.8431			0.6824	−58.7113
0.4963		24.082	−1.8128			1.0462	−69.5677
0.6008		21.867	−1.4856			0.5270	−67.3609
0.6925		21.066	−1.1136			0.8545	−67.9767
0.7975		15.476	−0.7193			0.6410	−55.3057
0.8940		5.051	−0.4114			0.0624	−27.5923
1.0000		-	-			-	-
1,3-Dioxolane + Nonanol
0		-	-			-	-
0.0876		4.101	−1.3354			−0.0127	−13.8972
0.1913		14.688	−1.4778			0.8880	−37.811
0.2942		23.767	−2.0708			1.3824	−58.0273
0.3963		26.458	−2.4659			0.7277	−66.163
0.4959		30.889	−2.4573			0.9917	−77.6885
0.6050		30.351	−2.1496			0.6632	−79.1657
0.6947		28.662	−1.8005			0.4673	−76.1285
0.7993		24.941	−1.2976			0.5023	−67.4371
0.9013		15.325	−0.6083			0.1749	−42.0859
1		-	-			-	-
1,3-Dioxolane + Decanol
0		-	-			-	-
0.0881		7.94	−2.2532			0.2115	−18.0838
0.191		20.585	−1.8401			1.6598	−45.848
0.2921		23.249	−2.9930			0.7076	−55.1023
0.3937		30.026	−3.1558			1.1236	−71.7103
0.4956		34.182	−2.8276			1.2487	−83.06
0.604		33.522	−2.4923			0.6457	−83.7183
0.7129		34.915	−2.2819			1.0260	−87.4645
0.7983		28.826	−1.6867			0.5040	−73.6965
0.8971		18.727	−0.8801			0.1778	−48.3816
1		-	-			-	-

4.3. Deviation of Viscosity (η^E)

A deviation in viscosity (η^E) of 1,3-dioxolane + n-alkanol of liquid mixtures at experimental temperature are important for understanding molecular interactions in these systems. Based on Edward Peters’ principle, higher density or viscosity reflects stronger intermolecular interactions. A perusal of Figure 4 show that the excess viscosity (η^E) is negative for all prepared liquid mixtures at experimental temperature. The excess viscosity (η^E) can be positive or negative. Negative excess viscosity (η^E < 0), implies weaker interactions. It suggests the disruption of alcohol-alcohol hydrogen bonding by 1,3-dioxolane molecules, leading to lower resistance to flow and decreased viscosity.

Figure 4. Excess viscosity (η^E) versus mole fraction (X₁) of the 1,3-dioxolane at experimental temperature.

4.4. Acoustic Impedance (Z)

An specific impedance (Z) of liquid mixtures investigated in this study showed either positive or negative at experimental temperature. These values are presented in Table 3 and Figure 5. A perusal of Table 3 indicates the specific acoustic impedance (Z) values of all liquid are decrease but the increase in the mole fraction of dicyclic ether (X₁).

Figure 5. Excess acoustic impedance (Z^E) versus mole fraction (X₁) of the 1,3-dioxolane at experimental temperature.

Figure 4 illustrates the differences of excess specific acoustic impedance (Z) for six binary liquid mixtures, A perusal of Figure 4 indicates the values of acoustic impedance (Z) is negative for all experimental liquid mixtures at experimental temperature.

5. Conclusion

This research article reports experimental study of sound velocity, viscosity and density and its derived excess parameters. The positive value of excess molar volume shows the presence of weak molecular interactions between the two components. All the computed parameters and its values show the presence of hydrogen bonding and dipole-dipole interaction in liquid mixtures.

Acknowledgements

The authors thanks to Uttar Pradesh Council of Science and Technology, Lucknow (No. CST/CHEM/D-648) for financial support (Project ID: 3409).

Conflicts of Interest

The authors declare no conflicts of interest regarding the publication of this paper.

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