Homework Help is Here – Start Your Trial Now!
Science
Chemistry
Measure the cell potentials of Cells A-D Cell A: Zn(s) | Zn²*(0.10 M) || Sn²*(0.010 M) | Sn(s) Cell B. Ag(s) | Ag*(0.010 M| Cu²*(0.10 M) | Cu(s) Cell C. Cu(s) | Cu2+(0.10 M) || Sn²+(0.10 M) | Sn(s)_

Measure the cell potentials of Cells A-D Cell A: Zn(s) | Zn²*(0.10 M) || Sn²*(0.010 M) | Sn(s) Cell B. Ag(s) | Ag*(0.010 M| Cu²*(0.10 M) | Cu(s) Cell C. Cu(s) | Cu2+(0.10 M) || Sn²+(0.10 M) | Sn(s)_

Chemistry
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...
See similar textbooks
icon
Related questions
Question
Measure the cell potentials of Cells A-D Cell A: Zn(s) | Zn*(0.10 M) || Sn²*(0.010 M) | Sn(s) Cell B. Ag(s) | Ag+(0.010 M) || Cu2+(0.10 M)| Cu(s) Cell C. Cu(s) | Cu2+(0.10 M) || Sn²+(0.10 M) | Sn(s)_ Cell D. Mg(s) | Mg2+(1.00 M) || Cu²+(0.00010 M)| Cu(s)_ Concentration Cell Cell E. Ag(s) | Ag:C2O4(s)| Ag+(x M), C2O,2- (v M| Ag*(0.10 M) | Ag(s) A saturated solution of Ag.C2O4(s) is made by placing solid Ag2C2O4 in water and stirring over night to establish the equilibrium reaction: Ag.C20:(s) 2 2 Ag*(ag)+ C2O42-(gg). The voltaic cell was prepared by filling the one of the half-cells with a saturated solution of Ag2C2O4(s) and the other half-cell is filled with 0.10 M AGNO3. Silver electrodes placed in each half-cell. The cell potential was measured by connecting the black clip onto the silver electrode in the half-cell with the saturated solution and the red clip onto the silver electrode in the half-cell to the half-cell with the 0.10 M AgNO3. Let x and y represent the concentrations of the silver ion and the oxalate ion, respectively. The voltage was measured to be 0.149 V.
Transcribed Image Text:Measure the cell potentials of Cells A-D Cell A: Zn(s) | Zn*(0.10 M) || Sn²*(0.010 M) | Sn(s) Cell B. Ag(s) | Ag+(0.010 M) || Cu2+(0.10 M)| Cu(s) Cell C. Cu(s) | Cu2+(0.10 M) || Sn²+(0.10 M) | Sn(s)_ Cell D. Mg(s) | Mg2+(1.00 M) || Cu²+(0.00010 M)| Cu(s)_ Concentration Cell Cell E. Ag(s) | Ag:C2O4(s)| Ag+(x M), C2O,2- (v M| Ag*(0.10 M) | Ag(s) A saturated solution of Ag.C2O4(s) is made by placing solid Ag2C2O4 in water and stirring over night to establish the equilibrium reaction: Ag.C20:(s) 2 2 Ag*(ag)+ C2O42-(gg). The voltaic cell was prepared by filling the one of the half-cells with a saturated solution of Ag2C2O4(s) and the other half-cell is filled with 0.10 M AGNO3. Silver electrodes placed in each half-cell. The cell potential was measured by connecting the black clip onto the silver electrode in the half-cell with the saturated solution and the red clip onto the silver electrode in the half-cell to the half-cell with the 0.10 M AgNO3. Let x and y represent the concentrations of the silver ion and the oxalate ion, respectively. The voltage was measured to be 0.149 V.
For the concentration cell, cell E only: Finding the Ksp for Ag2C204. and the reaction is not even a Redox rxn! Perform the following considering the SPONTANEOUS direction of the electrochemical cell: Voltmeter 6. Draw the Voltaic Cell Diagram for this electrochemical cell. Salt Bridge 7. a) Write the half-reaction that takes place in the anode including the concentration of the ion, even if its x. b) Write the half-reaction that takes place in the cathode including the concentration of the ion. c) Write the overall cell reaction including the concentrations of the ions, even if its x. 8. Symbolically, write the Nernst equation for each of these electrochemical cells, including the LMA for Q. (Symbolically means you do not use numbers.) 9. a) Calculate the unknown silver ion concentration based on the measured E cell, value of n, and the known ion concentration. Show all the values plugged into this equation. b) Calculate the unknown oxalate ion concentration based on the saturated solution of Ag2C2O4(s). 10. A saturated solution of Ag.C204(s) was placed in one of the half-cells and the equilibrium reaction: Ag.C2O4(s) 2 2 Ag*(ag) +C20,2-(ag). Write the Ksp expression for this equilibrium reaction. 11. Calculate the value of the Ksp for silver oxalate. The literature value for the K.of Ag2C2O4(s) = 1.3 x 10-11. If your calculated value is not of the same magnitude (x 10-11) as the literature value, then there is a calculation error. Check your math.
Transcribed Image Text:For the concentration cell, cell E only: Finding the Ksp for Ag2C204. and the reaction is not even a Redox rxn! Perform the following considering the SPONTANEOUS direction of the electrochemical cell: Voltmeter 6. Draw the Voltaic Cell Diagram for this electrochemical cell. Salt Bridge 7. a) Write the half-reaction that takes place in the anode including the concentration of the ion, even if its x. b) Write the half-reaction that takes place in the cathode including the concentration of the ion. c) Write the overall cell reaction including the concentrations of the ions, even if its x. 8. Symbolically, write the Nernst equation for each of these electrochemical cells, including the LMA for Q. (Symbolically means you do not use numbers.) 9. a) Calculate the unknown silver ion concentration based on the measured E cell, value of n, and the known ion concentration. Show all the values plugged into this equation. b) Calculate the unknown oxalate ion concentration based on the saturated solution of Ag2C2O4(s). 10. A saturated solution of Ag.C204(s) was placed in one of the half-cells and the equilibrium reaction: Ag.C2O4(s) 2 2 Ag*(ag) +C20,2-(ag). Write the Ksp expression for this equilibrium reaction. 11. Calculate the value of the Ksp for silver oxalate. The literature value for the K.of Ag2C2O4(s) = 1.3 x 10-11. If your calculated value is not of the same magnitude (x 10-11) as the literature value, then there is a calculation error. Check your math.
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 2 steps

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Activities
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS