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

Since we only answer 1 question in case of multiple question, we’ll answer the first question as the…

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

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Consider the oxidation/reduction reaction below:Fe(CN)63- + Ag(s) + Br- <--> Fe(CN)64- + AgBr(s)(a) Write the reaction in terms of two balanced half-reactions.(b) Express each half-reaction as a reduction reaction with its corresponding sign and value of standard electrode potential.(c) Arrange the oxidizing agents in (b) in order of decreasing effectiveness as electron acceptors.
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A voltaic cell is constructed that uses the following half-cellreactions:Cu+(aq) + e- ----->Cu(s)I2(s) + 2 e- ----->2 I-(aq)The cell is operated at 298 K with [Cu+] = 0.25 M and[I-] = 0.035 M. (a) Determine E for the cell at these concentrations.(b) Which electrode is the anode of the cell?(c) Is the answer to part (b) the same as it would be if the cellwere operated under standard conditions? (d) If [Cu+] wereequal to 0.15 M, at what concentration of I- would the cellhave zero potential?
What is the standard cell potential for the reaction below? Enter your answer with two decimal places and no units. Mg(s) + Br2() Mg2+(aq) + 2 Br"aq) The standard reduction potential is -2.37 V for the Mg2+/Mg half-cell and +1.09 V for the Bro/Br half-cell. Enter your answer in decimal format using two decimal places, (value + 2%).
is 0.085 correct or should it be 0.116? I got two answers and i’m not sure.
Consider the following half-reactions: Half-reaction E° (V) |Cl2(g) + 2e¯ → 2C1 (aq) 1.360V Co2+(aq) + 2e Mn2+(aq) + 2e → Co(s) -0.280V → Mn(s)-1.180V (1) The weakest oxidizing agent is: enter formula (2) The strongest reducing agent is: (3) The strongest oxidizing agent is: (4) The weakest reducing agent is: (5) Will CI"(aq) reduce Mn2+(aq) to Mn(s)? (6) Which species can be reduced by Co(s)? If none, leave box blank.
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