The selectivity coefficient, Kg-r. for a K* ion-selective electrode is 0.00649. When the electrode is placed into a 5.01 x 105 M K* solution at pH 6.58, the potential is -0.164 V vs. SCE. If the pH of the solution is lowered to 1.37 and the ionic strength is kept constant, what is the potential of the electrode? Assume f= 1 for the electrode. %3D

The selectivity coefficient, Kg-r. for a K* ion-selective electrode is 0.00649. When the electrode is placed into a 5.01 x 105 M K* solution at pH 6.58, the potential is -0.164 V vs. SCE. If the pH of the solution is lowered to 1.37 and the ionic strength is kept constant, what is the potential of the electrode? Assume f= 1 for the electrode. %3D

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter21: Potentiometry

Section: Chapter Questions

Problem 21.23QAP

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.
At what pH does Ecell = 0.00 V for the reduction of dichromate by iodide ion in acid solution, assuming standard-state concentrations of all species except H+ ion?
A 0.2g sample of toothpaste containing fluoride was treated with 50 cm3 of a suitable buffer solution and diluted to 100 cm3. Using a fluoride ion-selective electrode, a 25.00 cm3 aliquot of this solution gave cell potentials of –155.3 mV before and –176.2 mV after spiking with 0.1 cm3 of a 0.5 mg/cm3 fluoride standard. Calculate the pF– corresponding to each cell potential and the percentage by weight of fluoride in the toothpaste.
An ion selective electrode for NO2- has the following values of Log k for the listed interferents. Interferent Logk F- -3.1 SO42- -4.1 I- -1.2 NO3- -3.3 Which ion is the most serious interferent? Why? For what activity of this interferent is the potential (E) equivalent to a solution in which aNO2- = 2.75 x 10-4 ?
When the difference in pH across the membrane of a glass electrode at 25C is 4.63 pH units, how much voltage is generated by the pH gradient? Assume that the constant in Equation 15-6 is 1.00.
Given the following: A cell SCE // Ag2CrO4 (saturated), CrO42- (xM) /AG is used for the determination of pCrO4- (ESCE = -0.244 V at 25 C). The half reaction at indicator electrode is: Ag2CrO4(s) + 2e-   2 Ag(s) + CrO42- (E0 = +0.446 V) What is pCrO4, given the cell potential of 0.402? What type of indicator electrode is Ag in this situation?
A fluoride ion-selective electrode has a selectivity coefficient KPot F2, OH2 5 0.1. What will be the change in electrode potential when 1.0 104 M F at pH 5.5 is raised to pH 10.5?