The boundary equivalent conductivity of the 0.1 M electrolyte with a resistance of 0.33 ohms was determined as 320 Scm-2mol-1 and the conductivity ratio was determined as 0.55. According to this information, the electrolyte; a) Equivalent conductivity b) Self conductivity c) Find the cell constant of the electrode used.

The boundary equivalent conductivity of the 0.1 M electrolyte with a resistance of 0.33 ohms was determined as 320 Scm-2mol-1 and the conductivity ratio was determined as 0.55. According to this information, the electrolyte; a) Equivalent conductivity b) Self conductivity c) Find the cell constant of the electrode used.

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter4: Least-squares And Calibration Methods

Section: Chapter Questions

Problem 5P

See similar textbooks

Similar questions

The boundary equivalent conductivity of the 0.1 M electrolyte with a resistance of 0.33 ohms was determined as 320 Scm-2mol-1 and the conductivity ratio was determined as 0.55. According to this information, the electrolyte; a) Equivalent conductivityb) Self conductivityb) Find the cell constant of the electrode used.
Why it is necessary to platinize the electrodes of a conductivity cellbefore it is used for conductance measurement?
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.
Provide as many error sources in your calibration of the ion-selective electrode (ISE) as you can.
what the different between Equivalent conductance and molar conductance
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.
Create a calibration curve. Electrode potential (mV) vs. log [Ca2+]. (complete with, the equations of the best fit line, and the correlation coefficient) log[Ca 2+] Electrode potential (mV) -5 -105.4 -105.1 -106.5 -6 -120.9 -120.3 -120.6 -4.4 -96.6 -97.2 -96.5 -4 -85.5 -85.8 -85.2 -3 -56.6 -56.2 -56.4 -2 -26.6 -27.1 -27.1
A bare silver wire electrode is dipped into a solution 0.05M in KNO3 (supporting electrolyte) and saturated in AgBr (Ksp = 5.0 x 10-13), and connected to the back of an mV/pH meter along with a saturated calomel reference electrode. Calculate the potential of the silver indicator electrode. Calculate the cell potential.
The forward-bias voltage (V) required to maintain a PN diode current (I) is a function of the temperature (T). (a) Derive an expression for δV/δT (b) What is a typical value for a silicon diode? (c) Compare the result of (b) with a numerical value extracted.
The conductance of several salts in a binary mixture of water and a dipolar aprotic solvent ethylene carbonate are reported at 25 °C in a solvent 80% ethylene carbonate by mass. Calculate Λ°m for NaI and KI in this solvent.
The exchange current density at the electrode Pt| Fe3+| Fe2+ is 2.4 x 10-3 A cm-2, How many electrons are transported through the double layer per second in the cell (area of 1 cm2 each)? Estimate the number of times per second that a single atom on the surface takes part in an electron transfer event, assuming that the atom occupies 280 pm2 of the surface of the electrode
2) Name the advantages of glass electrode in potentiometric measurements (please write correctly and concisely).