A 20.00-mL aliquot of 0.100 M Fe²+ solution is titrated with 0.100 M Ce+. (a) Calculate the potential of the indicator cathode with respect to SHE after addition of 10, 18.00, 19.80, 19.98, 20.00, 20.02, 20.20, 22.00, 30.00, and 40.00 mL of cerium(IV). noi nagonblad b) Draw a titration curve for these data. (msleya do ava muñɔɔ ɔrt to limow odi to lautnolog di sin

A 20.00-mL aliquot of 0.100 M Fe²+ solution is titrated with 0.100 M Ce+. (a) Calculate the potential of the indicator cathode with respect to SHE after addition of 10, 18.00, 19.80, 19.98, 20.00, 20.02, 20.20, 22.00, 30.00, and 40.00 mL of cerium(IV). noi nagonblad b) Draw a titration curve for these data. (msleya do ava muñɔɔ ɔrt to limow odi to lautnolog di sin

Principles of Instrumental Analysis

7th Edition

ISBN:9781305577213

Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Chapter23: Potentiometry

Section: Chapter Questions

Problem 23.23QAP: The following cell was found to have a potential of —0.492 V: Ag|AgCl(sat’d)||HA(0.200 M),NaA(0.300...

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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.
A 40.00-mL aliquot of 0.05000 M HNO2 is diluted to 75.00 mL and titrated with 0.0800 M Ce4+. The pH of the solution is maintained at 1.00 throughout the titration; the formal potential of the cerium system is 1.44V a. Calculate the potential of the indicator electrode with respect to a saturated calomel reference electrode after the addition of 5.00, 10.00, 15.00, 25.00, 40.00, 49.00, 49.50, 49.60, 49.70, 49.80, 49.90, 49.95, 49.99, 50.00, 50.01, 50.05, 50.10, 50.20, 50.30, 50.40, 50.50, 51.00, 60.00, 75.00 and 90.00 mL of Cerium (IV). b. Draw a titration curve for these data. c. Generate a first- and second-derivative curve for these data. Does the volume at which the second-derivative curve crosses zero correspond to the theoretical equivalence point? Why or why not?
Calculate the potential of the solution in the titration of 50.0 mL 0.100 M Fe2+ in 1.00 M HClO4 with 0.0167 M Cr2O72- at 10.00 mL titrant added.
Calculate the potential in the solution (vs. NHE) in the titration of 50.0 mL of 0.100 M Fe2+in 1.00 M HClO4 with 0.0167 M Cr2O7 2− at 10, 25, 50 and 60 mL titrant added.
50.00 ml of 0.1000 M Fe(CN)64- solution is titrated with 0.05000 M Tl3+ solution potentiometrically using S.C.E. and Pt electrodes. Calculate the values of the potential when 10.0, 50.0 and 60.0 ml of titrant have been added.
Sometimes it is not possible to indicate the end point of a titration.a) How can one proceed then and what is the name of the type of titration that can be performed? Briefly describe. An example in which this method can be used is in the determination of mercury, which forms strong complexes with EDTA, but for which there is no suitable indicator that can indicate the end point. b) You are given the task of determining the Hg2 + concentration in a sample solution? After adding an excess of EDTA, the sample solution is titrated with a magnesium solution. 20.00 ml of a 0.0452 M EDTA solution was added to 30.00 ml of sample solutionThe excess EDTA was determined by adding 0.0500 M Mg 2+ solution, consuming 4.37 ml to the end point.
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.
Calculate the potential in the solution in the titration of 50.0 mL of 0.100 M Fe2+ in 1.00 M HCl4 with 0.0167 M Cr2O7 2- at 10.0, 25.0, 50.0 and 60.0 titrant added.
Calculate the potential in the solution (vs. NHE) in the titration of 50.0 mL of 0.100 M Fe2+in 1.00 M HClO4 with 0.0167 M Cr2O7 2− at 10, 25, 50 and 60 mL titrant added. Please answer it clearly
Consider the titration of 25.0 mL of 0.010 0 M Sn21 by 0.050 0 M Tl31 in 1 M HCl, using Pt and saturated calomel electrodes. (a) Write a balanced titration reaction. (b) Write two half-reactions for the indicator electrode. (c) Write two Nernst equations for the cell voltage. (d) Calculate E at the following volumes of Tl31: 1.00, 2.50, 4.90, 5.00, 5.10, and 10.0 mL. Sketch the titration curve.
Consider the titration of 100.0 mL of 0.010 0 M Ce4+ in 1 M HClO4 with 0.040 0 M Cu+ to give Ce3+ and Cu2+. Calculate the potential of the indicator electrode after adding 24.5 mL of Cu+.
The concentration of ammonia in a cleaning product was determined by back titration.Firstly, 10.00 cm3 of the cleaning product was pipetted into a large conical flask,containing 250.00cm3 of 0.50 mol/l HCl to give Solution A.Following a period of reaction and shaking, 50.00cm3 of Solution A was removed anddiluted to 250 cm3 with water in a volumetric flask to give Solution B.20 cm3 samples of Solution B were titrated against 0.05 mol/l Na2CO3 solution, givingan average titre of 12.45 cm3. i) Write equations for the reactions that have taken place.ii) Determine the concentration of NH3 in the original cleaning product in mol/l,g/l, ppm, and % w/v.