Part AA voltaic cell designed to measure [Cu] isconstructed of a standard hydrogen electrode and ayou wanted to construct a calibration curve for howthe cell potential varies with the concentration ofcopper(II), what would you plot in order to obtain astraight line?Ifcopper metal electrode in the Cu?+ solution ofinterest.log[Cu²+]versus Eºcell[Cu²+]? versus E.cellCu2+] versus Ecellexp[Cu2+] versus EelSubmitPrevious AnswersCorrectPart BWhat would be the slope of the line?Express your answer using two significant figures..030SubmitPrevious Answers Request AnswerX Incorrect; Try Again; 4 attemptsremaining

Answered: Image /qna-images/answer/c72624c4-7d36-4ee4-ad38-7af204fd2f06.jpg

Part A A voltaic cell designed to measure [Cu] is If you wanted to construct a calibration curve for how the cell potential varies with the concentration of copper(II), what would you plot in order to obtain a straight line? constructed of a standard hydrogen electrode and a copper metal electrode in the Cu²+ solution of interest. log[Cu²+] versus E. cell [Cu2+]2 versus E. cell [Cu?+] versus E cell exp[Cu2+] versus Eºel Submit Previous Answers v Correct Part B What would be the slope of the line? Express your answer using two significant figures. ? .030 V Submit Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining

Part A A voltaic cell designed to measure [Cu] is If you wanted to construct a calibration curve for how the cell potential varies with the concentration of copper(II), what would you plot in order to obtain a straight line? constructed of a standard hydrogen electrode and a copper metal electrode in the Cu²+ solution of interest. log[Cu²+] versus E. cell [Cu2+]2 versus E. cell [Cu?+] versus E cell exp[Cu2+] versus Eºel Submit Previous Answers v Correct Part B What would be the slope of the line? Express your answer using two significant figures. ? .030 V Submit Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining

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

Similar questions

An electrochemical cell consists of a standard hydrogen electrode and a copper metal electrode. a. What is the potential of the cell at 25°C if the copper electrode is placed in a solution in which = 8.7 x 10-4 M? Ecell = b. The copper electrode is placed in a solution of unknown Cu+ |. The measured potential at 25°C is 0.223 V. What is | Cu²+ |? (Assume Cu²+ is reduced.) [C*] = Cu² 2+ M
Could you please solve the last two questions from the second picture?
A voltaic cell is constructed, based on the Zn/Sn2+ ion reaction. Zn + Sn2+ → Zn2+ + Sn The standard cell potential is 0.626 V. What is the cell potential be when [Zn2+]=1.2 M and [Sn2+]=0.8 M ?
A voltaic electrochemical cell is constructed using the following reaction. The half-cell components are separated by a salt bridge. Cr(s) + 3FE3+(aq)Cr3+(aq) + 3F22+(aq) Write the reactions that take place at the anode and at the cathode, the direction in which the electrons migrate in the external circuit, and the direction the anions in the salt bridge migrate. Use smallest possible integer coefficients. If a box is not needed, leave it blank. Enter the reaction that takes place at the anode. Include state symbols: + Enter the reaction that takes place at the cathode. Include state symbols: + In the external circuit, electrons migrate v the Cr electrode v the Fe3+, Fe2+ electrode. Anions migrate v the salt bridge the Fe3+, Fe2+ compartment. Submit from proach Show Tutor Steps to
Answer the following questions using the data in Appendix L of the textbook. a. Calculate the standard cell potential for a galvanic cell made with Ni and Ag. b. Calculate the standard cell potential for a galvanic cell made with Ni and Zn.
A cell is constructed by immersing a strip of silver in 0.10 M AgNO 3 solution and a strip of lead in 1.0 M Pb(NO 3) 2 solution. A wire and salt bridge complete the cell. What is the potential of the silver electrode in the cell? O a. 0.80 V O b. 0.83 V O C. 0.88 V O d. 0.86 V e. 0.74 V
A galvanic cell was formed using Avium and Beanium:[hypothetical elements] Reduction Potentials: Av3+(aq) + 3e- → Av(s) Eo = -0.48 V Bn4+(aq) + 4e- → Bn(s) Eo = +0.15 V a) Write a net ionic equation for this reaction. b) Write the cell notation for this cell. c) Which is the oxidizing agent? Explain how you know.
A galvanic (voltaic) cell consists of an electrode composed of nickel in a 1.0 M nickel(II) ion solution and another electrode composed of gold in a 1.0 M gold(III) ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C. Refer to the list of standard reduction potentials. E° V 'cell * TOOLS х10
Analyze the components of a voltaic electrochemical cell. A voltaic electrochemical cell is constructed using the following reaction. The half-cell components are separated by a salt bridge. Hg2+(aq) + Cu(s)→ Hg(I) + Cu²+(aq) Write the reactions that take place at the anode and at the cathode, the direction in which the electrons migrate in the external circuit, and the direction the anions in the salt bridge migrate. Use smallest possible integer coefficients. If a box is not needed, leave it blank. Enter the reaction that takes place at the anode. Include state symbols: + + Enter the reaction that takes place at the cathode. Include state symbols: + + In the external circuit, electrons migrate to v the Hg+ electrode from v the Cu electrode. In the salt bridge, anions migrate to the Cu compartment [from v) the Hg compartment.
Consider a voltaic cell that can be described like so. It is set up at standard conditions. A gold electrode is in contact with Au(NO3)3 (aq) and a lead electrode in contact with Pb(NO3)2 (aq) at 25 degrees C. Write true or false next to each of the following statements regarding the voltaic cell. I. Adding H20 to the lead half-cell will increase the measured cell potential. II. A salt-bridge is used to prevent charge buildup in the half-cells. III. This will result in the production of Pb2+ ions.
A student constructed a voltaic cell by combining Sn/Sn2+ and Zn/Zn2+ two half cells and measured a cell potential of 0.620 V. He then constructed a voltaic cell by combining Sn/Sn2+ and Ni/Ni2+ two half cells and measured a cell potential of 0.140 V. It is seen that the tin metal precipitated out of the solution in each above cell. Except for the reduction potential of Zn which is known as -0.763V, the reduction potentials of all the other two electrodes are unknown. a. Calculate the reduction potential of Sn2+ (aq)+ 2e- ---> Sn(s). b. Calculate the reduction potential of Ni2+(aq)+2e- ----> Ni(s) c. Write the cell reaction for the cell of Sn/Sn2+ and Zn/Zn2+
A voltaic cell is based on a nitrate/NO half-cell and a NiCl2/Ni half-cell. (Heads up, the chloride ions in this reaction are bystander ions.) Eo for NO-3 (aq) → NO(g) = +0.96 Eo for NiCl2 (aq) → Ni(s) = –0.28 What is the cell potential of the reaction when pH = 2.7, [NO3-] = 1.5 M, PNO = 0.010 atm and [Ni2+] = 0.21 M