Question 11 Match the statement with the correct electrode being described. saturated calomel electrode silver/silver chloride electrode metallic electrode of the first kind metallic electrode of the second kind liquid-membrane electrode A. specific to indicator ions with a fixed concentration B. contains a saturated KCI solution with AgCl C. non-selective redox occurs D. specific to the indicator ion but can also precipitate or complex E. contains a saturated KCI solution with mercury

Question 11 Match the statement with the correct electrode being described. saturated calomel electrode silver/silver chloride electrode metallic electrode of the first kind metallic electrode of the second kind liquid-membrane electrode A. specific to indicator ions with a fixed concentration B. contains a saturated KCI solution with AgCl C. non-selective redox occurs D. specific to the indicator ion but can also precipitate or complex E. contains a saturated KCI solution with mercury

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

1. Equilibrium constant: 2. Greater or less ?
A 100.0 mL solution of 0.0200 M Fe3+ in 1 M HClO4 is titrated with 0.100 M Cu+, resulting in the formation of Fe2+ and Cu2+. A Pt indicator electrode and a saturated Ag∣∣AgCl electrode are used to monitor the titration. Calculate the values of ? for the cell after each of the given volumes of the Cu+Cu+ titrant have been added. 10.0 ml E = ? V 19.5 ml E = ? V
A. Why is the titration of the oxalate in the green salt with KMnO4 performed prior to carrying out the redox titration for iron content? (Why can’t you do them the other way – iron first then oxalate?) B. In a titration using 0.02000 M KMnO4 solution, the following data were obtained: Buret readings: FINAL = 15.31 mL INITIAL = 5.02 mL How many moles of KMnO4 were used?
Asymmetry potential is encountered with which of the following electrodes? a. Ion-exchanger electrode b. PVC-based electrode c. Pt electrode d. pH electrode
Which of the following is most suitable for filtering the crystalline precipitate BaSO4 out of the precipitating medium? a. Buchner funnel b. Gooch crucible c. Ashless filter paper d. Sintered glass crucible
Which of the statements below are true for the titration of Fe2t with standard Ce? I. The indicator electrode potential before the addition of Cet solution is calculated using the Fea+ half-reaction after calculating the equilibrium concentrations of Fe3+ and Fe2+ in solution. II. Before the equivalence point, the indicator electrode potential is calculated using the Fe3+ half-reaction because only [Fe3] and [Fe2*] are known. III. At the equivalence point, the indicator potential is the average of E" for Fet and Cet. IV. After the equivalence point, the indicator electrode potential is calculated using the Ce** half-reaction because only [Ce"] and [Ce2*] are known. 1, II, II, and IV I, II, and IV II, III, and IV 1, I1. and IV
7. Suggest an electrochemical cell to determine a. the pH of a given solution. b. Ksp of AgBr. c. the concentration of NaCl solution potentiometrically.
Which of the following is an example of an indicator electrode for bromide measurements in seawater? Group of answer choices Ion selective electrode Standard hydrogen electrode Saturated calomel electrode Silver-silver chloride electrode
Chapter 21 Values A table of standard electrode potentials is necessary for many of the following question(s). Calculate the standard cell potential for the cell, Cd|Cd 2*(1 M||Cu 2*(1 M|Cu. O a. -0.74 V O b. +0.06 V O C. -0.06 V O d. +0.74 V e. 0.00 V
A solution prepared by mixing 60.0 mL of 0.360 M AGNO, and 60.0 mL of 0.360 M TINO, was titrated with 0.720 M NaBr in a cell containing a silver indicator electrode and a reference electrode with a constant potential of 0.175 V. The reference electrode is attached to the positive terminal of the potentiometer, and the silver electrode is attached to the negative terminal. The solubility constant of TIBr is Kp = 3.6 × 10-6 and the solubility constant of AgBr is = 5.0 x 10-13. Ksp Which precipitate forms first? O TIBI O AgBr Which of the expressions shows how the cell potential, E, depends on [Ag*]? E = 0.175 V – [0.799 V – 0.05916log ([Ag+])] 1 E = |0.799 V – 0.05916log - 0.175 V [Ag*) E = [0.799 V – 0.05916log ([Ag*]D] – 0.175 V E = 0.175 V - |0.799 V – 0.05916log [Ag* * (ল) Calculate the first and second equivalence points of the titration. first equivalence point: mL second equivalence point: mL What is the cell potential after each of the given volumes of 0.720 M NaBr have been…
A 30.0 mL solution of 0.0180 M Rh3+ in 1 M HClO4 was titrated with 0.0900 M Ce4+ to give Rh6+ and Ce3+. Calculate the potential (vs. Ag | AgCl) at the equivalence point. At what volume of titrant will the potential be equal to the standard potential of the Ce half-reaction (ignoring the Ag | AgCl electrode)?
Balance the equation 7 please and answer 8 thank youuu