Current, A +100.0 +80.0 +60.0 +40.0 +20.0 0.0 -20.0 0.0 Limiting current Y X 4/2 E1/2 Z A+ ne P 1 -0.2 -0.4 -0.6 -0.8 -1.0 Eappl. V vs. SCE Why does current stop increasing and plateaus at -0.6 V
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- The resistance of a conductivity cell containing a 0.01 mol KCl solution cm-3 is 150 Ω and the conductivity of this KCl solution is 1.41 × 10-3 Ω-1 cm-1. The same conductivity cell resulting in a resistance of 51.40 Ω for 0.01 HCl solution mol cm-3. Calculate a cell constant and conductivity of the HCl solution.A conductivity cell filled with a 0.01 M KCl solution was found to have a resistance of 189 ohms at 25oC. When filled with 0.01 M HCl solution, the cell gave a resistance of 64.8 ohms at the same temperature. At 25oC, the conductivity of 0.01 M KCl solution was 1.4088 x 10-3 S cm-1. Calculate (a) the cell constant and (b) the conductivity of the HCl solution. answer is [0.266; 4.105 x 10-3] please explain. thank you!) 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?
- 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.Zinc is to be used as an internal standard for the polarographic analysis of thallium. A standard solution containing twice the concentration of zinc as Thallium has a diffusion current of 1.89 µA for Ti and 3.50 µA for Zn. A 10.0g alloy was dissolved in 500 mL, 25 mL of this solution was mixed with 25 mL of 1.0 x 10-3 M Zn 2+ solution. The diffusion currents of this final solution are 18.2µA for Tl+ and 14.5µA for Zn+. Calculate % Ti in the sample analysedb) 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).
- The electrolytic conductivity of NaCl solution at 18oC is 0.0124 ohm-1cm2 mol-1 and the resistance of the cell containing the solution at the same temperature is 50 ohm. The cell constant will be a. 0.62 b. 0.31 c. 0.124 d. 0.0002480.5M HA electrolyte with a degree of dissociation of 0.2; It is placed in a conductivity cell with a length of 0.9 cm and an area of 2cm2 and its conductivity is read as 300 mS. According to these data; a) Equivalent conductivity of the electrolyte b) Boundary equivalent conductivity c) Decomposition constantCalculate the hardness of water in terms of ppm CaCo3, V used, M EDTA, and Average M EDTA, Ave. ppm CaCO3
- The resistance of a conductivity cell containing a 0.02 M aqueous solution of KCl was fond to be 83 ohms at 298 K. The conductivity of the 0.02 M KCl solution at this temperature is 0.00277 S cm-1. When the cell was filled with a 0.005 M aqueous solution of K2SO4, it exhibited a resistance of 326 ohms at the same temperature. What is the molar conductivity of the potassium sulfate solution? [ answer should be 141 S cm2 mol-1]thank u0.5M HA sample with 0.2 dissociation; It is placed in a conductivity cell with a length of 0.9 cm and an area of 2 cm2 and its conductivity is read as 300 mS. For this purpose;a) Equivalent conductivity of the electrolyte ?b) Boundary equivalent conductivity ?c) Decomposition constant ?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.