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- 4.In a certain conductivity cell, the resistance of a 0.01 M KCl solution is 150 Ω. Theknown molar conductivity of the solution is 141.27 Ω-1 cm2 mol-1. Calculate the cell constant (Kcell).*(Kcell unit is cm-1) 5. Using the same conductance cell as in Question No. 4, a student measured the resistanceof a 0.10 M NaCl solution to be 19.9Ω. Calculate the experimental value of the molarconductivity 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).Which will have greater molar conductivity and why? Sol A. 1mol KCldissolved in 200cc of the solution or Sol B. 1 mol KCl dissolved in 500cc of the solution.
- At 25°C the KCl solution has a type conductance of 0.14088 S/m and a resistance of 654 ohm. In the same cell, the 0.10 M NH3 solution has a resistance of 2524 ohm, the molar conductivity of the infinite dilution of NH4+ and OH- ions is 73.55x10-4 and 198.3x10-4. Count:A. NH3 conduction molarsb. Molar conductivity of the infinity to NH3) 0.025 M CH3COOH solution has a specific conductance of 2.33X10-4 Scm-1,and molar conductivity at infinite dilution is 364.13 S.Cm2.mol-1. What is itsdegree of dissociation?How is cell constant calculated from conductance values?
- A piece of an unknown weighing 12.50is placed in 49.7cm of water in a cylinder. The water level increases to 69.0cm3. whats the calculated value for the drnsity of the solid in g ml-1Why it is necessary to platinize the electrodes of a conductivity cellbefore it is used for conductance measurement?In a polarographic experiment of a 60 mL of 0.08 M Cu2+solution, a limitingcurrent was left on for 15 minutes. If the average current during the time of theexperiment is 6.0 μA, what fraction of the copper is removed from the solution? TheFaraday constant is 96485 C/mol of electron.
- A conductivity cell has a resistance of 250 Ω when filled with 0.02 M KCl at 25°C and 105 Ω when filled with 6 x 10-5 M ammonium hydroxide solution. The conductivity of 0.02 M KCl solution at 25°C is 0.277 Sm-1, and the limiting molar ionic conductivities of NH4 + and OH- are 7.34 x 10-3 and 0.0198 S m2mol-1 , respectively. Calculate the cell constant and degree of dissociation of ammonium hydroxide in the 6 x 10-5 M solution.The mobility of the NH4+ ion is known is 7,623 x 10 ^-8 m2/Vs. Count:a. The molar conductivity of the NH4+ ionb. Ion velocity, when a voltage of 15 V is applied to the cell with separate electrodes 25 cm awayc. The transport number of NH4 + ions in CH3COONH4 solution if the ion is mobility CH3COO is 4.239 x 10-8 m2/Vsd. The amount of current carried by the NH4+ and CH3COO ions when the appliance set is connectedwith a coulometer I2 electrolyzed for 60 minutes as much as 50 mL. 10 mL of This solution was reacted with 20 mL of 0.05 M Na2S2O3 solution according to the following reaction:2S2O32- + I2 → S4O62- + 2I-The conductivity of 0.20 M solution of KC1 at 298 K is 0.025 S cm-1. Calculate its molar conductivity.
