Measure the cell potentials of Cells A-DCell 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 CellCell 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 equilibriumreaction: 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 isfilled with 0.10 M AGNO3. Silver electrodes placed in each half-cell. The cell potential was measured by connecting the black cliponto the silver electrode in the half-cell with the saturated solution and the red clip onto the silver electrode in the half-cell to thehalf-cell with the 0.10 M AgNO3. Let x and y represent the concentrations of the silver ion and the oxalate ion, respectively. Thevoltage 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:Voltmeter6. Draw the Voltaic Cell Diagram for this electrochemical cell.Salt Bridge7. 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 donot use numbers.)9. a) Calculate the unknown silver ion concentration based on the measured E cell, value of n, andthe 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 literaturevalue, then there is a calculation error. Check your math.

Calculation of cell potential is done using Nernst equation: E=E∘-0.0591nlogPR

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

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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