The redox titration we did in lab used 0.010 M Cr2072¯ to titrate 0.060 M and 20 mL Fe2+ The titration use Pt electrode to indicate the potential of the solution and use SCE as the reference electrode, calculate the cell potential at half of the equivalent ½ Ve, at 7.0 mL, Ve and 13 mL of Cr20,2-? E for SCE is 0.241 V, Eº (Cr2O¬2- +14 H*+6e ----2Cr³+ + ZH2O) = 1.36 V

The redox titration we did in lab used 0.010 M Cr2072¯ to titrate 0.060 M and 20 mL Fe2+ The titration use Pt electrode to indicate the potential of the solution and use SCE as the reference electrode, calculate the cell potential at half of the equivalent ½ Ve, at 7.0 mL, Ve and 13 mL of Cr20,2-? E for SCE is 0.241 V, Eº (Cr2O¬2- +14 H*+6e ----2Cr³+ + ZH2O) = 1.36 V

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 23.26QAP

See similar textbooks

Similar questions

Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.
The cell Ag|AgCl(sat’d)||H+(a = x)|glass electrode has a potential of —0.2094 V when the solution in the right-hand compartment is a buffer of pH 4.006. The following potentials are obtained when the buffer is replaced with unknowns: (a) —0.2806 V and (b) —0.2132 V. Calculate the pH and the hydrogen ion activity of each unknown. (c) Assuming anuncertainty of 0.001 Vin the junction potential, what is the range of hydrogen ion activities withinwhich the true value might be expected to lie?
What cathode potential (versus SCE) would be required to lower the total Hg(II) concentration of the following solutions to 1.00 10-6 M (assume reaction product in each case is elemental Hg): (a) an aqueous solution of Hg2+? (b) a solution with an equilibrium SCN- concentration of 0.100 M? Hg2+ + 2SCN- Hg(SCN)2(aq) = Kf = 1.8 107 c) a solution with an equilibrium Br- concentration of 0.100 M? HgBr42++ 2e- Hg(l) + 4Br- E0= 0.223 V
The saturated calomel electrode. abbreviated SCE. is often used as a reference electrode in making electrochemica1 measurements. The SCE is composed of mercury in contact with a saturated solution of calomel (Hg2Cl2). The electrolyte solution is saturated KCI. is +0.242 V relative to the standard hydrogen electrode. Calculate the potential for each of the following galvanic cells containing a saturated calomel electrode and the given half-cell components at standard conditions. In each case. indicate whether the SCE is the cathode or the anode. Standard reduction potentials are found in Table 17.1. a. Cu2++2eCu b. Fe3++e-Fe2+ c. AgCl+e-Ag+Cl- d. Al3++3eAl e. Ni2++2eNi
Calculate the electrode potentials for the following systems: (a) Cr2O72-(5.00 10-3 M),Cr3+(2.50 10-2 M),H+ (0.100 M)|Pt (b) UO22+(0.100 M),U4+ (0.200 M),H+ (0.600 M)|Pt
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.