Density and Viscosity of LiCl, LiBr, LiI and Kcl in Aqueous Methanol at 313.15K

Introduction

The density and viscosity data of electrolyte solutions have been extremely valuable in determining whether or not ion-solvent interactions exist in aqueous and non-aqueous solutions.¹ For a better knowledge of many physicochemical processes that occur in the chemical industry and in nature, Crystallization, desalination, waste water treatment, pollution control, oil recovery, heat and mass transfer, fluid flow, mineral transport and deposition, corrosion, and other processes all rely on the transport properties (viscosity and thermal conductivity) of aqueous electrolyte solutions in a wide range of solvent concentrations, solution temperatures, and pressures. In many applications, these processes take place at high temperatures and pressures. For understanding ion-solvent interactions, temperatures and concentration dependencies of the viscosity of aqueous electrolyte solutions are indeed important.^2-9

Viscosity is one of the important transport properties of electrolyte solutions and belongs to a dynamic state property, while density is one of the key thermodynamic features of electrolyte solutions and contributes to an equilibrium property.^10-12 Researchers have explored the use of density and viscosity of mixtures to derive thermodynamic properties like dynamic viscosity, kinematic viscosity, deviations in dynamic viscosity, excess molar volume, surface tension deviation, apparent molar volumes, etc.^13-16.  In this paper we report, limiting apparent molar volume (f⁰_v) of some lithium halides LiX (X= Cl Br I) in water + methanol at different temperature using density property. An attempt is to make determine the effect of variation of (f⁰_v) with methanol content for a given electrolyte. The viscosities of Lithium halides solution in (0, 20, 40, 50, 60, 80 and 100) mass % of methanol + water at different temperatures to see how changing the solvent content affects the viscosity B-coefficient.

Experimental

Water was distilled over alkaline KMnO4 in a rapid fit system, and then distilled again over H₂SO₄. The electric conductance of distilled water varied between 1×10^-6 and 9×10^-77 Ω^-1 cm^-1. Methanol with A.R. grade from SD Fine Chemical limited was directly used without further purification. LiCl anhydrous was from S D fine chemicals limited Mumbai product no. 230374, batch no. KO3Y/0703/1910/31 with purity 99%. LiBr anhydrous was from Sigma-Aldrich product no. 44987-3 batch no. MKBF4487V with purity 99.9%. LiI anhydrous was from  Sigma-Aldrich  product no. 43974-6 batch no. MKBD 2730 with purity 99.9%.KCl was from SD Fine Chemical limited Mumbai product no. 20198, batch no.KO5,H10Y/0710/1408/31 with purity 99.5%.

By mixing known quantities of water and methanol in glass-stoppered flasks, methanol + water mixes of compositions (0, 20, 40, 50, 60, 80, and 100) mass percent methanol were prepared. A bicapillary pycnometer was used to measure the density of the solution, with an accuracy of ± 1×10^-4 g/cm³ as described earlier^17-19. The pycnometer was placed in a temperature-controlled water bath with thermal stability of ± 0.01K for 15 min to attain thermal equilibrium. An Ubbelohde suspended level viscometer was used to measure viscosities^20-22. Water conductivity was used to calibrate the device. For the flow time measurements, an electronic digital stop watch with a readability of ±0.01s was employed.

Results and Discussion

The values of experimentally determined density for the pure liquids at are given in Table-1. Experimental densities (ρ) and viscosities (η) of pure liquids were in good agreement with literature values at different temperatures. The densities of LiCl, LiBr, LiI and KCl solutions having concentrations ranging between 0.005 to 0.05 M in 0, 20, 40, 50, 60, 80 and 100 wt % of water + methanol binary mixtures at different temperatures are measured. The observed densities ρ, of the solutions Lithium halides in water, methanol and methanol + water mixtures are used to calculate the apparent malar volumes f_v using the equation.

Table 1: Comparison of Experimental Densities (ρ) and Viscosities (η) of Pure Liquids    with Literature Values at different temperatures.

Temp. K)	ro (g/ cm3)		h0 (m Pa s )
	Expl.	Lit.	Expl.	Lit.
Water
298.15	0.99706	0.997127	0.8944	0.894928
		0.9970528		0.890329
303.15	0.99570	0.995727	0.7987	0.80030
308.15	0.99405	0.99440630	0.7195	0.72127
313.15	0.99208	0.992327	0.6538	0.65427
		0.992231		0.6526332
Methanol
298.15	0.78662	0.7866228	0.5490	0.54433
303.15	0.78139	(0.7825-	0.5126	0.50727
		0.78181)33
308.15	0.77640	0.77699034	0.4787	0.47427
313.15	0.77130	0.772327	0.4477	0.45027

Where ρ and ρ₀ are the densities of solution and solvents respectively, C is the concentration in mol liter^-1.  The densities ρ and apparent molar volumes f_v, for LiCl, LiBr, LiI and KCl in different methanol + water mixtures at 313.15 K are given in the Table-2 and Table-3. The densities and viscosities of LiCl, LiBr, LiI and KCl were found to increase with the increase in concentration of electrolytes. f_v varied linearly with C^1/2 over the concentration range. The electrolytes’ limiting partial molar volume (f⁰_v) was calculated using computerised least square fitting of the Masson equation-2.

Table 2: Densities ρ, apparent molar volumes f_v, and viscosities ɳ, for LiCl and LiBr in different methanol + water mixtures at 313.15K

LiCl					LiBr
C/ mol.dm-3	ρ /g.cm-3	fv / cm3. mol -1		ɳ / mPa s	C/ mol.dm-3		ρ /g.cm-3		fv /cm3. mol-1		ɳ / mPa s
0 % Methanol
0.0050	0.99228	18.99		0.6603	0.0059		0.99252		25.39		0.6603
0.0120	0.99244	19.09		0.6612	0.0103		0.99279		25.45		0.6608
0.0160	0.99253	19.14		0.6617	0.0160		0.99314		25.55		0.6614
0.0207	0.99264	19.19		0.6622	0.0206		0.99343		25.59		0.6619
0.0257	0.99276	19.24		0.6628	0.0270		0.99382		25.68		0.6625
0.0310	0.99288	19.28		0.6634	0.0303		0.99402		25.70		0.6628
0.0351	0.99298	19.31		0.6639	0.0360		0.99437		25.75		0.6633
0.0420	0.99313	19.36		0.6646	0.0400		0.99461		25.80		0.6637
0.0454	0.99321	19.38		0.6650	0.0462		0.99499		25.88		0.6643
0.0508	0.99334	19.42		0.6656	0.0515		0.99531		25.93		0.6647
20 % Methanol
0.0051	0.95795	13.05		0.9663	0.0053		0.95814		24.68		0.9680
0.0105	0.95811	13.10		0.9677	0.0123		0.95858		24.81		0.9705
0.0168	0.95830	13.15		0.9691	0.0162		0.95882		24.88		0.9717
0.0201	0.95840	13.17		0.9698	0.0203		0.95908		24.95		0.9728
0.0256	0.95856	13.21		0.9710	0.0267		0.95948		25.02		0.9745
0.0305	0.95871	13.24		0.9720	0.0294		0.95965		25.05		0.9752
0.0365	0.95888	13.27		0.9732	0.0347		0.95998		25.11		0.9765
0.0413	0.95903	13.29		0.9741	0.0408		0.96036		25.17		0.9779
0.0474	0.95921	13.32		0.9753	0.0457		0.96067		25.20		0.9791
0.0510	0.95931	13.33		0.9760	0.0528		0.96111		25.26
40 % Methanol
0.0058	0.92147	9.74		1.4296	0.0051		0.92162		22.35		1.1280
0.0127	0.92170	9.75		1.4368	0.0111		0.92202		22.30		1.1318
0.0155	0.92180	9.75		1.4393	0.0158		0.92233		22.27		1.1344
0.0209	0.92198	9.76		1.4438	0.0220		0.92274		22.24		1.1375
0.0268	0.92218	9.77		1.4483	0.0247		0.92292		22.23		1.1388
0.0336	0.92240	9.78		1.4532	0.0314		0.92337		22.20		1.1419
0.0355	0.92247	9.78		1.4545	0.0350		0.9236		22.18		1.1435
0.0400	0.92262	9.78		1.4575	0.0428		0.92412		22.15		1.1468
0.0467	0.92284	9.79		1.4619	0.0448		0.92426		22.14		1.1476
0.0525	0.92303	9.80		1.4656	0.0513		0.92469		22.12
50 % Methanol
0.0052	0.90038	7.05	1.1174		0.0065	0.90065		17.83		1.1086
0.0103	0.90056	7.00	1.1263		0.0104	0.90093		17.77		1.1122
0.0168	0.90080	6.96	1.1354		0.0153	0.90128		17.70		1.1162
0.0200	0.90091	6.94	1.1394		0.0211	0.90169		17.63		1.1205
0.0260	0.90113	6.91	1.1463		0.0263	0.90206		17.58		1.1241
0.0296	0.90126	6.89	1.1502		0.0319	0.90246		17.53		1.1279
0.0362	0.90150	6.86	1.1570		0.0340	0.90261		17.51		1.1292
0.0418	0.90171	6.84	1.1625		0.0416	0.90315		17.46		1.1340
0.0456	0.90184	6.83	1.1660		0.0445	0.90336		17.44		1.1358
0.0513	0.90205	6.81	1.1712		0.0502	0.90376		17.41
60 % Methanol
0.00497	0.86746	2.96	1.0232		0.0055	0.86767		14.63		1.0103
0.0111	0.86770	2.98	1.0369		0.0105	0.86804		14.64		1.0160
0.0158	0.86789	2.99	1.0456		0.0164	0.86848		14.65		1.0220
0.0205	0.86808	3.00	1.0534		0.0216	0.86886		14.66		1.0268
0.0251	0.86826	3.01	1.0604		0.0263	0.86921		14.67		1.0310
0.0314	0.86851	3.02	1.0695		0.0313	0.86958		14.68		1.0353
0.0356	0.86868	3.03	1.0752		0.0362	0.86994		14.69		1.0395
0.0409	0.86889	3.04	1.0821		0.0392	0.87017		14.69		1.0419
0.0452	0.86906	3.05	1.0875		0.0462	0.87068		14.70		1.0475
0.0505	0.86927	3.06			0.0509	0.87103		14.71
80 % Methanol
0.0050	0.83033	-1.20	0.7993		0.0056	0.83055		10.85		0.7873
0.0100	0.83054	-1.16	0.8098		0.0102	0.8309		10.98		0.7921
0.0165	0.83083	-1.12	0.8209		0.0153	0.8313		11.09		0.7968
0.0196	0.83096	-1.10	0.8256		0.0214	0.83177		11.21		0.8020
0.0249	0.83119	-1.08	0.8332		0.0253	0.83207		11.30		0.8051
0.0306	0.83143	-1.05	0.8407		0.0327	0.83264		11.42		0.8108
0.0364	0.83168	-1.01	0.8480		0.0345	0.83278		11.46		0.8122
0.0407	0.83187	-0.99	0.8531		0.0388	0.83311		11.54		0.8154
0.0454	0.83207	-0.97	0.8586		0.0464	0.83369		11.63		0.8209
0.0520	0.83236	-0.95			0.0517	0.8341		11.69
100 % Methanol
0.0053	0.77248	-1.75	0.0053		0.0059	0.77273		7.55		0.4597
0.0100	0.77269	-1.68	0.0100		0.0103	0.77308		8.12		0.4598
0.0155	0.77293	-1.65	0.0155		0.0167	0.77359		8.56		0.4605
0.0206	0.77315	-1.61	0.0206		0.0214	0.77397		8.69		0.4612
0.0269	0.77342	-1.56	0.0269		0.0259	0.77432		8.97		0.4620
0.0290	0.77351	-1.54	0.0290		0.0326	0.77485		9.19		0.4633
0.0365	0.77384	-1.50	0.0365		0.0371	0.7752		9.50		0.4642
0.0403	0.77401	-1.49	0.0403		0.0413	0.77553		9.62		0.4651
0.0450	0.77421	-1.47	0.0450		0.0447	0.7758		9.62		0.4659
0.0492	0.77439	-1.45	0.0492		0.0498	0.7762		9.88

 

Table 3: Densities ρ, apparent molar volumes f_v, and viscosities ɳ, for LiI and KCl in different methanol + water mixtures at 313.15K

LiI							KCl
C/mol. dm-3		ρ /g.cm-3		fv/cm3 .mol -1		ɳ/mPa s	C/mol. dm-3		ρ /g.cm-3		fv/cm3 .mol -1		ɳ/mPa s
0 % Methanol
0.0051		0.99265		37.23		0.6599	0.0054		0.99241		29.26		0.6599
0.0101		0.99314		37.27		0.6603	0.0099		0.99261		29.48		0.6601
0.0156		0.99367		37.30		0.6607	0.0158		0.99287		29.78		0.6604
0.0201		0.99411		37.32		0.6610	0.0203		0.99307		29.96		0.6605
0.0251		0.99459		37.34		0.6613	0.0253		0.99329		30.08		0.6607
0.0299		0.99505		37.36		0.6616	0.0296		0.99348		30.19		0.6609
0.0344		0.99549		37.38		0.6619	0.0352		0.99373		30.24		0.6610
0.0400		0.99603		37.40		0.6623	0.0402		0.99395		30.31		0.6612
0.0500		0.99699		37.43		0.6629	0.0450		0.99416		30.39		0.6613
							0.0501		0.99438		30.48		0.6615
20 % Methanol
0.0053		0.95833		36.12		0.9749	0.0152		0.95854		27.01		0.9663
0.0109		0.95888		36.25		0.9799	0.0208		0.95882		26.64		0.9666
0.0201		0.95979		36.38		0.9860	0.0254		0.95904		26.86		0.9669
0.0251		0.96028		36.45		0.9888	0.0304		0.95928		27.01		0.9672
0.0313		0.96089		36.51		0.9920	0.0352		0.95950		27.41		0.9674
0.0349		0.96125		36.55		0.9938	0.0401		0.95974		27.32		0.9677
0.0398		0.96173		36.60		0.9961	0.0463		0.96003		27.55		0.9679
0.0523		0.96296		36.71		1.0014	0.0504		0.96022		27.70		0.9681
0.0554		0.96326		36.74		1.0027	0.0554		0.96046		27.70		0.9683
40 % Methanol
0.0056		0.92187		30.81		1.1244	0.0152		0.92211		22.01		1.1223
0.0098		0.92231		30.77		1.1258	0.0202		0.92237		22.24		1.1223
0.0199		0.92338		30.70		1.1287	0.0254		0.92265		22.42		1.1223
0.0261		0.92403		30.66		1.1305	0.0305		0.92292		22.59		1.1223
0.0306		0.92451		30.64		1.1317	0.0351		0.92316		22.78		1.1223
0.0354		0.92502		30.62		1.1330	0.0401		0.92342		22.99		1.1223
0.0412		0.92563		30.59		1.1346	0.0451		0.92368		23.16		1.1223
0.0496		0.92652		30.56		1.1368	0.0503		0.92395		23.30		1.1223
0.0551		0.92710		30.54		1.1382	0.0551		0.92420		23.40		1.1223
50 % Methanol
0.0047	0.90071		25.78		1.1029		0.0051	0.90048		19.65		1.0990
0.0107	0.90137		25.65		1.1064		0.0108	0.90080		20.17		1.1000
0.0203	0.90244		25.50		1.1114		0.0201	0.90131		20.92		1.1016
0.0249	0.90295		25.44		1.1136		0.0266	0.90167		21.22		1.1027
0.0319	0.90373		25.36		1.1169		0.0318	0.90195		21.51		1.1037
0.0350	0.90408		25.33		1.1184		0.0351	0.90212		21.73		1.1043
0.0399	0.90462		25.27		1.1206		0.0416	0.90247		21.93		1.1054
0.0504	0.90579		25.18		1.1252		0.0497	0.90291		22.13		1.1069
0.0551	0.90632		25.14		1.1273		0.0551	0.90319		22.27		1.1079
60 % Methanol
0.0049	0.86782		22.27		1.0070		0.0054	0.86759		14.86		1.0007
0.0109	0.86851		22.23		1.0125		0.0094	0.86784		15.18		1.0019
0.0225	0.86984		22.18		1.0217		0.0230	0.86866		15.77		1.0058
0.0254	0.87017		22.17		1.0238		0.0267	0.86888		16.00		1.0069
0.0301	0.87071		22.16		1.0272		0.0305	0.86911		16.21		1.0080
0.0352	0.87129		22.15		1.0307		0.0362	0.86944		16.52		1.0097
0.0410	0.87196		22.13		1.0347		0.0430	0.86984		16.78		1.0117
0.0498	0.87297		22.11		1.0406		0.0528	0.87041		17.17		1.0146
0.0551	0.87358		22.10		1.0441		0.0551	0.87055		17.22		1.0153
80 % Methanol
0.0061	0.83083		19.39		0.7858		0.0058	0.83049		11.92		0.7788
0.0110	0.83140		19.56		0.7900		0.0106	0.83079		12.07		0.7804
0.0199	0.83245		19.77		0.7967		0.0203	0.83141		12.72		0.7837
0.0242	0.83295		19.86		0.7998		0.0255	0.83174		12.90		0.7856
0.0319	0.83385		19.99		0.8049		0.0317	0.83213		13.23		0.7877
0.0354	0.83426		20.06		0.8072		0.0365	0.83243		13.37		0.7894
0.0413	0.83495		20.15		0.8110		0.0401	0.83265		13.50		0.7907
0.0508	0.83605		20.30		0.8169		0.0512	0.83334		13.83		0.7946
0.0551	0.83655		20.36		0.8195		0.0551	0.83358		13.94		0.7960
100 % Methanol
0.0067	0.77307		15.13		0.4574		0.0057	0.77266		2.60		0.4638
0.0103	0.77351		15.46		0.4569		0.0107	0.77302		2.99		0.4653
0.0197	0.77464		16.10		0.4567		0.0206	0.77373		3.50		0.4686
0.0253	0.77531		16.44		0.4570		0.0261	0.77412		3.76		0.4705
0.0312	0.77602		16.71		0.4574		0.0309	0.77446		3.92		0.4721
0.0357	0.77656		16.93		0.4579		0.0358	0.77481		4.08		0.4738
0.0410	0.77719		17.18		0.4585		0.0411	0.77518		4.29		0.4756
0.0520	0.77850		17.60		0.4600		0.0508	0.77586		4.62		0.4790
0.0551	0.77887		17.71		0.4604		0.0556	0.77619		4.77		0.4806

 

Where ‘f⁰_v’ is the limiting partial malar volume at infinite dilution and S_v is the experimental slope. The f⁰_v and S_v values are presented in Table-4. The f⁰_v is regarded as a measure of solute-solvent interactions. The f⁰_v for LiCl, LiBr and LiI is increases regularly as the size of Lithium halide increases. As the solvent composition varies, the values of f⁰_v vary as well. Various researchers have seen a shift in f⁰_v with different concentrations of other solvents in water in the case of electrolytes.^23-25 The S_v values of LiCl are negative in water and methanol mixtures at 50 % methanol indicating some ion-ion interactions shown in Table-4. Similarly, the S_v values of LiBr are negative in water and methanol mixtures at 40 % and 50 % methanol and LiI shows it negative at 40, 50, 60 % methanol indicating ion-ion interactions. The negative slope indicating the ionic dissociation of the electrolytes²⁶.

Table 4: Apparent molar volumes, (f⁰_v, cm³ mol^-1) and experimental slopes (S_v cm³ L^1/2  mol^-3/2), along with correlation coefficient, γ, of Lithium halides  in different water  + methanol at 313.15K.

Electrolyte	Mass %   methanol	f0v, /cm3 mol-1	Sv /cm3 L1/2  mol-3/2	γ
LiCl
	0	18.79	2.78	0.9998
	20	12.91	1.86	0.9993
	40	9.17	0.39	0.9868
	50	7.16	-1.56	-0.9996
	60	2.91	0.64	0.9951
	80	-1.33	1.63	0.9960
	100	-1.89	2.01	0.9975
LiBr
	0	25.09	3.58	0.9955
	20	24.41	3.75	0.9993
	40	22.46	-1.48	-0.9991
	50	18.07	-2.99	-0.9992
	60	14.59	0.54	0.9933
	80	10.41	5.65	0.9988
	100	6.50	15.19	0.9951
LiI
	0	37.14	1.31	0.9995
	20	35.85	3.77	0.9998
	40	30.94	-1.70	-0.9998
	50	26.05	-3.87	-0.9999
	60	22.34	-1.02	-0.9983
	80	18.91	6.15	0.9997
	100	13.74	16.91	0.9999
KCl
	0	28.74	8.00	0.9891
	20	25.58	9.00	0.8923
	40	20.40	12.90	0.9981
	50	18.52	16.50	0.9962
	60	13.68	14.83	0.9943
	80	10.81	13.35	0.9968
	100	1.59	13.39	0.9996

 

The f⁰_v values for lithium halides in water and water + methanol are plotted against molecular weight of corresponding halide ions using an equation of the form

Where ‘b’ is constant and f⁰_v (Li) is the limiting ionic partial molar volume of Li⁺ ions. The plot of f⁰_v of electrolytes versus molecular weight of corresponding halide ions is given in the Fig.-1. An excellent linear relationship was observed for all lithium halides solutions in all solvents with γ greater than 0.9999. The extrapolation of graphs of f⁰_v versus molecular weight of halide ion to zero ionic formula weight gives the partial molar volume of Li⁺ ion. The Table-5 represents the value of ionic partial malar volumes of all the ions in all solvents at 313.15K. It demonstrates that the ionic partial molar volumes of halides ions (X-) fluctuate with the solvent composition over time, peaking at 20% methanol. There are no more holes in the binary solvents at 20% methanol, and the dissolving of the third component, the solute, necessitates the solvent’s maximum expansion to accommodate the solute. As a result, there should be a peak in the partial molar volume of the halides ions (X-).

Figure 1: Plots of φ0v versus Molecular weights of Cl–, Br–, I– in different methanol + water mixtures at 313.15 K. Click here to View figure

Table 5: Ionic partial molar volumes, ϕ⁰_v of ions in various methanol + water mixtures at 313.15K

%Methanol	K+	Cl–	Br–	I–	Li+
0	20.71	8.03	14.33	26.38	10.76
20	16.81	8.77	20.27	31.71	4.14
40	13.56	6.84	20.13	28.61	2.33
50	11.80	6.72	17.63	25.61	0.44
60	6.93	6.75	18.43	26.18	-3.84
80	3.63	7.18	18.92	27.42	-8.51
100	-4.19	5.78	14.17	24.41	-7.67

 

The viscosities of solutions of the LiCl, LiBr, LiI and KCl  in water methanol and methanol-water mixtures are measured at 313.15 K . The observed viscosities η, of Lithium halides in water, methanol and methanol + water mixtures at 313.15K are analysed with the help of Jones-Dole equation²².

Where η is the viscosity of the solution and η_o is the viscosity of the solvent, and C is the molar concentration. A is the measure of long range Columbic forces between ions, while B reflects the effect of ion- solvent interactions. Plots of (η_r – 1) /C^1/2  versus C^1/2  for the electrolytes are straight lines with intercept equal to A, and  the slope give the values of the  viscosity B-coefficients. The A and B coefficients obtained with a computerised least square method are listed in Table-6. Fig.-2 depicts plots of (ɳr – 1)/C1/2 versus C1/2 of LiCl in different methanol + water mixtures at 313.15 K.

Table 6: Parameters of Jones – Dole Equation A and B along with correlation coefficient, γ, for Lithium halides in different water + methanol at 313.15K

Electrolyte	Mass % methanol	A / dm3/2.mol-1/2	B / dm3.mol-1	γ
LiCl
	0	0.0085	0.1471	0.9995
	20	0.0162	0.1645	0.9997
	40	0.0883	0.2053	0.9998
	50	0.2171	0.3354	1.0000
	60	0.3009	0.538	1.0000
	80	0.3584	0.6271	1.0000
	100	-0.0276	0.8181	0.9999
LiBr
	0	0.0090	0.1180	0.9991
	20	0.0414	0.1392	0.9995
	40	0.0596	0.2303	0.9999
	50	0.0866	0.3471	0.9999
	60	0.1077	0.5428	1.0000
	80	0.1292	0.6135	1.0000
	100	-0.1322	0.8034	1.0000
LiI
	0	0.0045	0.0859	0.9987
	20	0.1415	0.1159	0.9995
	40	0.0150	0.2003	0.9999
	50	0.0395	0.3106	0.9999
	60	0.0755	0.4915	1.0000
	80	0.0985	0.5708	1.0000
	100	-0.1862	0.7240	1.0000
KCl
	0	0.0089	0.0230	09724
	20	0.0143	0 .0125	0.9417
	40	0.0045	-0.0141	-0.9906
	50	-0.0032	0.1721	0.9998
	60	-0.0029	0.3026	0.9943
	80	-0.0074	0.4728	1.0000
	100	-0.0152	0.7809	0.9999

 

Figure 2: Plots of (ɳr – 1)/C1/2 versus C1/2 of LiCl in different methanol + water mixtures at 313.15 K. Click here to View figure

There is a slow variety in ionic B esteems as the methanol content in the blended dissolvable increments. Both methanol and water are solvents which have intermolecular hydrogen holding. The expansion of methanol to water, first reinforces the three dimensional construction of the water, then, at that point further expansion of methanol causes depolymerisation of water structure, however intermolecular communication among methanol and water lead to arrangement of methanol-water edifices with a greater hydrodynamic element.

The B values of all lithium halides electrolytes (LiCl, LiBr, and LiI) are positive in all solvent compositions and continuously increases with increase of methanol. These positive B-parameters indicate structure making tendency of lithium halides in these solvent mixture. The B-coefficient of the KCl solutions in 50 to 100 wt% methanol are positive and continuously increases with increases of methanol. These positive B-parameters indicate structure making tendency of KCl in these solvents mixtures. The B- coefficient of KCl falls from solution in water to those in 20 to 40 wt % methanol but then rises again in the subsequent solvent mixtures. A-coefficients either positive or negative are very low in magnitudes indicating weak solute- solute interaction.

In summary, density and viscosity of four alkali chlorides and iodides namely LiCl, LiBr, LiI and KCl in aqueous methanol at 313.15 K were calculated using the electrolytes’ experimental densities, apparent molar volumes, and limiting apparent molar volumes. The experimental data on viscosity of these electrolytes were interpreted using the Jones-Dole equation for strong electrolyte solutions.  The densities and viscosities of LiCl, LiBr, LiI and KCl were found to increase with the increase in concentration of electrolytes. The apparent molar volumes varied linearly with C^1/2 over the concentration range. Our investigation on density and viscosity of the electrolytic solution studied in the revealed that when the dielectric constant of the solvent decreases, so also the solvent-solvent interactions in these systems. Furthermore, the experimental densities and viscosities of pure liquids were found to be in acceptable concurrence with reported values at various temperatures. In all solvent compositions, the B values of all lithium halide electrolytes are positive and increase with increasing methanol concentration. These positive B-parameters imply that lithium halides in these solvent mixtures have a tendency to form structures.

Acknowledgement

Authors would like to thank principals of SSGM College, Kopargaon and Arts, Science and Commerce College, Surgana for permission and providing necessary research facilities. Dr. Aapoorva Hiray, Coordinator, MG Vidyamandir institute, is gratefully acknowledged for continuous support. NCL, Pune is acknowledged for literature survey.

Conflict of interest

On behalf of all authors, the corresponding author states that there is no conflict of interest

Funding Source

There are no funding Source

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