15. The mobility of a NO3 ion in aqueous solution is 7.40 x 105 m² V-¹ s¹ at 25°C. The potential difference between two electrodes placed in the solution is 4.00 V. If the electrodes are 5.00 mm apart, what is the drift speed of the ion? a) 59.2 µm s b) 5.21 um s c) 34.7 μm s¹ d) 17.3 μm s¹

15. The mobility of a NO3 ion in aqueous solution is 7.40 x 105 m² V-¹ s¹ at 25°C. The potential difference between two electrodes placed in the solution is 4.00 V. If the electrodes are 5.00 mm apart, what is the drift speed of the ion? a) 59.2 µm s b) 5.21 um s c) 34.7 μm s¹ d) 17.3 μm s¹

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter21: Potentiometry

Section: Chapter Questions

Problem 21.11QAP

See similar textbooks

Similar questions

The following cell was found to have a potential of —0.492 V: Ag|AgCl(sat’d)||HA(0.200 M),NaA(0.300 M)|H2(1.00 atm),Pt Calculate the dissociation constant of HA, neglecting the junction potential.
The mobility of a Rb+ ion in aqueous solution is 7.92 x 10-8 m2 s-1 V-1 at 25 °C. The potential difference between two electrodes placed in the solution is 35.0 V. If the electrodes are 8.00 mm apart, what is the drift speed of the Rb+ ion?
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.
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 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!
The mobility of a Li+ ion in an aqueous solution is 4.01×10−8 m2s−1 V−1 at 25°C. The potential difference between two electrodes in the solution placed 1.0 cm apart is 12.0 V. What is the lithium ion current rate? (Use μms-1 for your answer)
An ion selective electrode is utilised to determine the concentration of Ca2+ in the presence of Mg2+. The selectivity coefficient for the electrode kij is 0.015. If the concentrations of Ca2+ and Mg2+ are 50 and 500 ppm, respectively, calculate the change in potential (in mV) when the temperature of the measurement cell is increased from 20oC to 40oC.
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 u
A conductivity cell was calibrated using 0.01 M KCl (κ = 1.4087x10-3 S/cm) and the measured resistance was 688 Ω. a. Determine the cell constant (include units). b. Determine the molar conductivity, Λm for a 0.0100 M AgNO3 solution in the same cell with a resistance reading of 777Ω.
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 analysed
(a) State Kohlrausch’s law of independent migration of ions. Mention one application of Kohlrausch’s law.(b) The resistance of a conductivity cell containing 10-3 M KC1 solution at 25 °C is1500 Q. What is the cell constant if conductivity of 10-3 M KC1 solution at 25 °C is 1.5 X 10-4 S cm-1?
1. Purification of chromium can be achieved by electrorefining chromium from an impure chromium anode onto a pure chromium cathode in an electrolytic cell. How many hours will it take to plate 15.5 kg15.5 kg of chromium onto the cathode if the current passed through the cell is held constant at 42.0 A42.0 A? Assume the chromium in the electrolytic solution is present as Cr3+Cr3+.