Answered: (a) Draw a well labelled diagram of a…

(a) Draw a well labelled diagram of a reference electrode (b) From the Figure below describe labels i to viii Current/A viii 2 iv vi iii vii Potential/V

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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Potentiometric Titrations

Potentiometric titration is one of the important titration methods and is mainly carried out to characterize acid solutions. It follows a method similar to that of the normal titration technique, but the main difference is that there is no indicator used in the potentiometric titrations. Instead of using an indicator, electrodes are employed for monitoring the whole titration process. A scientist named Robert Behrend did the potentiometric titration for the first time, and it was done using the mercurous solution and potassium chloride.

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what is the answer of part a and b please ?
[References) What are the reaction quotient (Q) and the calculated value of the cell potential (Ecell) at 298 K for an electrochemical cell with the following reaction, when the Hg2+ concentration is 7.35x104 M and the Mg²* concentration is 1.25 M? Hg"(aq) + Mg(s) Hg(l) + Mg²+(aq) E°cell = 3.225 V Q= Ecel =|
(Q86) What is the value (in V) of the standard cell potential (E°CELL) for the following reaction that occurs in an electrochemical cell at 25°C? Fe3+ (aq) + Cu* (aq) ---> Fe²+ (aq) + Cu2+ (aq) The reduction potentials for the two half-reactions involved are: Fe3+ + e- --> Fe2+ (E°RED) = 0.77 V Cu2+ + e- --> Cu* (E°RED) = 0.16 V %3D
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The ECellat 25oC forthe electrolytic cellCu0(s)| Cu2+(aq, 1M)|| Mn2+(aq, 0.1 M)| Mn0(s)was found to be -1.521 V. Calculate E°Redfor the half-cell Mn2+(aq, 1 M)| Mn0(s). Use the E°Red= +0.339 V for the Cu half-cell as in B above.
+2 t- 4) Consider the following redox reactions and their standard cell potentials: (acidic conditions) (basic conditions) S,0, (aq) + Cl2(g) = HCI0(aq) + So,"(aq) (acidic conditions) cell =-1.31 V E°cell = +0.10 V E° cell = +0.37 V E°. C2(g) + Bio*(aq) = Bi(s)+ HCIO(aq) So(aq) + 03(g) = S20 (aq) + 02(g) a) Using the ½ rxn method, balance the three redox reactions under the conditions indicated. b) Write each balanced redox reaction in the spontaneous direction and indicate its corresponding standard cell potential. c) Between these 3 redox reactions there are FOUR oxidizing agents and FOUR reducing agents. (Hint: You may need to consider the balanced equations.) i) Place the FOUR oxidizing agents in order of decreasing oxidizing strength. (From the strongest OA to the weakest OA.) ii) Place the FOUR reducing agents in order of decreasing reducing strength. ( (From the strongest RA to the weakest RA.)
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