Additional Exercise 19.111An Ag/AgCl electrode dipping into 1.00 M HCI has a standard reduction potential of +0.2223 V.The half-reaction isAgCI(s) + eAg(s) +Cl"(aq)A second Ag/AgCl electrode is dipped into a solution containing Cl" at an unknown concentration.The cell generates a potential of 0.0522 V, with the electrode in the solution of unknown concentration having a negative charge.What is the molar concentration of CI in the unknown solution?[Cr] =%Dthe tolerance is +/-2%Click if you would like to Show Work for this question: Open Show Work Multi-Concept Problem 19.117At 25 °C, a galvanic cell was set up having the following half-reactions.Fe2+(aq) + 2eS Fe(s), E°Fe2+Cu2+(aq) + 2e S Cu(s), E°cu2+= -0.447 V= +0.3419 VThe copper half-cell contained 100 mL of 3.85 M CuSO4. The iron half-cell contained 31.6 mL of 0.312 M FeSO4. To the iron half-cell was added 43.5 mL of 0.662 M NaOH solution. The mixtuwas stirred and the cell potential was measured to be 1.175 V. Calculate the value of Ksp for Fe(OH),.Kspthe tolerance is +/-2%Click if you would like to Show Work for this question: Open Show Work

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Additional Exercise 19.111 An Ag/AgCl electrode dipping into 1.00 M HCI has a standard reduction potential of +0.2223 v. The half-reaction is AgC(s) + e= Ag(s) +CI(aq) A second Ag/AgCl electrode is dipped into a solution containing Cl" at an unknown concentration. The cell generates a potential of 0.0522 V, with the electrode in the solution of unknown concentration having a negative charge. What is the molar concentration of CI" in the unknown solution? [Cr] = the tolerance is +/-2% Click if you would like to Show Work for this question: Open Show Work

Additional Exercise 19.111 An Ag/AgCl electrode dipping into 1.00 M HCI has a standard reduction potential of +0.2223 v. The half-reaction is AgC(s) + e= Ag(s) +CI(aq) A second Ag/AgCl electrode is dipped into a solution containing Cl" at an unknown concentration. The cell generates a potential of 0.0522 V, with the electrode in the solution of unknown concentration having a negative charge. What is the molar concentration of CI" in the unknown solution? [Cr] = the tolerance is +/-2% Click if you would like to Show Work for this question: Open Show Work

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 66QAP: Consider a voltaic cell in which the following reaction takes place in basic medium at 25°C....

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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
Consider the voltaic cell 2 Ag+(aq) + Cd(s) 2 Ag(s) + Cd2+(aq) operating at 298 K. (a) Calculate the Ecell for this cell. (b) If (cone. Cd2+) = 2.0 M and (cone. Ag+) = 0.25 M, calculate Ecell. (c) If Ecell = 1.25 V and (cone. Cd2+) = 0.100 M, calculate(cone. Ag+).
Consider a voltaic cell in which the following reaction takes place in basic medium at 25°C. 2NO3-(aq)+3S2(aq)+4H2O3S(s)+2NO(g)+8OH(aq) (a) Calculate E°. (b) Write the Nernst equation for the cell E. (c) Calculate E under the following conditions: PNO=0.994atm,ph=13.7,[S2]=0.154M,[NO3-]=0.472M, .
Consider a voltaic cell in which the following reaction occurs. Zn(s)+Sn2+(aq)Zn2+(aq)+Sn(s) (a) Calculate E° for the cell. (b) When the cell operates, what happens to the concentration of Zn2+? The concentration of Sn2+? (c) When the cell voltage drops to zero, what is the ratio of the concentration of Zn2+ to that of Sn2+? (d) If the concentration of both cations is 1.0 M originally, what are the concentrations when the voltage drops to zero?
Sketch a galvanic cell, and explain how it works. Look at Figs. 17-1 and 17-2. Explain what is occurring in each container and why the cell in Fig. 17-2 works but the one in Fig. 17-1 does not.
What is wrong with the following statement: The best concentration cell will consist of the substance having the most positive standard reduction potential. What drives a concentration cell to produce a large voltage?
A metallurgist wants to gold-plate an object with a surface area of 17.21 in2. The gold plating must be 0.00200 in. thick (assume uniform thickness). (a) How many grams of gold (d=10.5g/cm3) are required? (b) How many minutes will it take to plate the object from a solution of AuCN using a current of 7.00 A? Assume 100% efficiency.
Consider the galvanic cell based on the following half-reactions: a. Determine the overall cell reaction and calculate b. Calculate G and K for the cell reaction at 25C. c. Calculate at 25C when [Au3+] = 1.0 102 M and [Tl+] = 1.0 104 M.
Calculate the voltages of the following cells at 25°C and under the following conditions: (a) Zn|Zn2+(0.50M)Cd2+(0.020M)|Cd (b) Cu|Cu2+(0.0010M)H+(0.010M)|H2(1.00atm)|Pt
Calculate the voltages of the following cells at 25°C and under the following conditions: (a) Cu|Cu+(0.80M)Hg22+(0.10M)|Hg|Pt (b) Cr|Cr3+(0.615M)Ni2+(0.228M)|Ni
Consider a galvanic cell based on the following half-reactions: a. What is the expected cell potential with all components in their standard states? b. What is the oxidizing agent in the overall cell reaction? c. What substances make up the anode compartment? d. In the standard cell, in which direction do the electrons flow? e. How many electrons are transferred per unit of cell reaction? f. If this cell is set up at 25C with [Fe2+] = 2.00 104 M and [La3+] = 3.00 103 M, what is the expected cell potential?