Q1) Plot the conductance on y-axis and time on x-axis. Q2) How to determine initial conductance (Go) and final conductance (Goo). Time Conductance (10-³s) 1.92 1.9 1.88 1.87 1.85 1.8 1.73 1.63 1.62 1.59 1 2345 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 1.58 1.56 1.54 1.51 1.48 1.47 1.45 1.43 1.40 1.39
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- 1. Part A Solution temperature = 24 °C Conductivity of instrument grade water = 1.043 uScm! Conductivity of deionised water = 1.74 µScm! Conductivity of tap water = 330 μScml On the basis of data above comment on conditions of the different water grades. 2. The experimental data for electrolytes in Part B are given below: Electrolyte c (M) K (ms.cm') HC1 0.01 5.06 KCI 0.01 1.415 NaCl 0.01 1.236 CaCl2 0.01 2.30 КОН 0.01 2.29 CH3OH 0.01 0.003 K2SO4 0.01 2.65 Calculate molar conductivity A of each electrolyte solution in Sm/mol above. Correct for the conductivity of deionized water.The molar conductivity of a 1.5 M solution of an electrolyte is found to be 138.9 S cm2 mol-1. Calculate the conductivity of this solution.b) In one conductivity cell, the resistance of a 0.1 M KCl solution is 1.5x102 Ω. The knownmolar conductivity of the solution is 101 Ω-1 cm2 mol-1 . Calculate the cell constant, Kcell. (Kcell unit is cm-1).
- (2) The molar conductivity of an acid at 0.2 M is 2.22 S.cm².mol and for same acid at infinite dilution is 0.0111 52¹. m².mol', what is the degree of dissociation: (D) 20 (A) 0.2 (B) 0.02 (C) 200 (E) 0.0021. The following molar conductivity data are obtained for a strong electrolyte: Concentration (M) Am (S m² mol-¹) 0.001 0.01237 0.01 0.01185 0.1 0.01067 What would be the approximate conductivity of the electrolyte at infinite dilution? A) 0.915 S m² mol-¹ B) 125 S m² mol-¹ C) 511 S m² mol"¹ D) 0.0125 S m² mol-¹ E) 0.243 S m² mol-¹(c) The data set below represents the surface tension data for aqueous solutions of 3- methylbutanoic acid [(CH3)2CHCH₂COOH] at 25°C. [C] [mol.dm³] 0 Y[mN.m'] 72.7 0.009 64.6 0.026 59.0 0.065 51.3 0.135 47.0 (i) Calculate the surface excess of 3-methylbutanoic acid (in mol.m2) and (ii) Hence estimate the molecular cross sectional area (in nm²) for this surface active molecule. (iii) Compare your estimate with the molecular cross sectional area one might expect for n-butanoic acid and account for the difference, if any, between the two surface active molecules.
- In this problem you will model the mixing energy of a mixture in a relatively simple way, in order to relate the existence of a solubility gap to molecular behavior. Consider a mixture of A and B molecules that is ideal in every way but one: The potential energy due to the interaction of neighboring molecules depends upon whether the molecules are like or unlike. Let n be the average number of nearest neighbors of any given molecule (perhaps 6 or 8 or 10). Let Uo be the average potential energy associated with the interaction between neighboring molecules that are the same (A-A or B-B), and let UAB be the potential energy associated with the interaction of a neighboring unlike pair (A-B). There are no interactions beyond the range of the nearest neighbors; the values of Uo and UAB are independent of the amounts of A and B; and the entropy of mixing is the same as for an ideal solution. Find an expression for the maximum temperature at which this system has a solubility gap.Part C A solution is formed when the solute unilormly disperses throughout (or dissolves in) the solvent The process can be described though three stops A hypothetical solution forms between a solid and a liquid The vakues of the thermodynamic Involved in the process are shown in the following table 1 separation of solvent-solvant particles, 2. breaking of solute-solute particles and 3. formation of solute-solvent interactions Action Enthalpy 145 kJ/mol 21.8 kJ/mol séparation of solute separation of solvent formation of solute-solvent interactions -85.7 kJ/mol solute The overall energy change for the solution process, AHa is the sum of the enthalpies of the threoe stepo. Whether AHs endothermic or exothermic depends on the relative magnitudes of AH, AH, and AH, where the subscript Indicates the step in the process corresponding to the enthalpy value Calculate the enthalpy of solution in kilojoules per mole of solute Enter your answer numerically in kilojoules per mole of solute. > View…120=233k×5 Find the value of k.
- For weak electrolytes, such as acetic acid, at very low concentrations the molar conductivity drops rapidly as the concentration increases. However, at higher concentration, there’s only a slight decrease in the molar conductivity. True FalseThe molar conductivity at infinite dilution of hydrobromic acid, sodium acetate, & sodium bromide at 298 K are 520.1 Scm2mol-1, 105.9 Scm2mol" 1, and 186.3 Scm?mol-1, respectively. Determine the molar conductivity at infinite dilution of acetic acid.What is the kinetic property observed in suspension? What is the optical property observed in solutions?