Match the applications with the type of metallic indicator electrode First kind Second kind Third kind Redox indicator [Choose ] [Choose ] potentiometric titration of iron (II) measuring the activity of EDTA anion using a mercury electrode measuring the activity of calcium ion using a mercury electrode measuring the activity of fluoride ion using a fluoride selective electrode Sensing silver ion acitivity using silver electrode [Choose]

An electrode is prepared by dipping a silver strip into a solution saturated with silver thiocyanate, AgSCN, and containing 0.10 M SCN . The cell potential of the voltaic cell constructed by connecting this electrode as the cathode to the standard hydrogen half-cell as the anode is 0.45 V. What is the solubility product of silver thiocyanate?

An electrochemical cell is made by placing an iron electrode in 1.00 L of 0.15 M FeSO4 solution and a copper electrode in 1.00 L of 0.040 M CuSO4 solution. a What is the initial voltage of this cell when it is properly constructed? b Calculate the final concentration of Cu2+ in this cell if it is allowed to produce an average current of l.25 amp for 375 s.

An electrochemical cell is made by placing a zinc electrode in 1.00 L of 0.200 M ZnSO4 solution and a copper electrode in 1.00 L of 0.0100 M CuCl2 solution. a What is the initial voltage of this cell when it is properly constructed? b Calculate the final concentration of Cu2+ in this cell if it is allowed to produce an average current of 1.0 amp for 225 s.

Calculate the cell potential of a cell operating with the following reaction at 25C, in which [Cr2O32] = 0.020 M, [I] = 0.015 M, [Cr3+] = 0.40 M, and [H+] = 0.60 M. Cr2O72(aq)+6I(aq)+14H+(aq)2Cr3+(aq)+3I2(s)+7H2O(l)

Use Table 17.1 to predict what reaction, if any, will occur if sulfur is added to acidic aqueous solutions of the following species at standard conditions. (a) MgBr2 (b) Sn(NO3)2(c) Cr(ClO3)2

Using data from Table 17-1, place the following in order of increasing strength as reducing agents (all under standard conditions). Cu+,F,H,H2O,I2,K

Electrolysis of an alkaline earth metal chloride using a current of 5.00 A for 748 s deposits 0.471 g of metal at the cathode. What is the identity of the alkaline earth metal chloride?

A galvanic cell is based on the following half-reactions: In this cell, the copper compartment contains a copper electrode and [Cu2+] = 1.00 M, and the vanadium compartment contains a vanadium electrode and V2+ at an unknown concentration. The compartment containing the vanadium (1.00 L of solution) was titrated with 0.0800 M H2EDTA2, resulting in the reaction H2EDTA2(aq)+V2+(aq)VEDTA2(aq)+2H+(aq)K=? The potential of the cell was monitored to determine the stoichiometric point for the process, which occurred at a volume of 500.0 mL H2EDTA2 solution added. At the stoichiometric point, was observed to be 1 .98 V. The solution was buffered at a pH of 10.00. a. Calculate before the titration was carried out. b. Calculate the value of the equilibrium constant, K, for the titration reaction. c. Calculate at the halfway point in the titration.

A galvanic cell is constructed in which the overall reactionis Cr2O72(aq)+14H2O+(aq)+6I(aq)2Cr3+(aq)+3I2(s)+21H2O(l) Calculate E for this cell. At pH 0, with [Cr2O72]=1.5M and [I]=0.40M, the cell potential is found to equal 0.87 V. Calculatethe concentration of Cr3+(aq) in the cell.