2 Question 4 of 23 >For each reaction, calculate the value of the equilibrium constant (Keq) and the electrode potential of the system at theequivalence point (Eeg) of a hypothetical titration.Co³+ + Ti²+ Co²+ + Ti³+E Co²+/Co²+ = 1.900 VET¹/T²+ = -0.370 VKeq=Eeq =V Question 4 of 23 >Select the indicator that can be used to signal the end point of the hypothetical titration. Shown in parenthesis is thereduction potential and the number of electrons transferred in the oxidation or reduction of the indicator.O phenosafranine (E = +0.28 V, n = 1)diphenylamine (Ein = +0.76 V, n = 2)O 2,3'-diphenylamine dicarboxylic acid (En = +1.12 V, n = 2)O indigo tetrasulfonate (Ein = +0.36 V, n = 2)O diphenylamine sulfonic acid (E = +0.85 V, n = 2)Omethylene blue (Ein = +0.53 V, n = 2)O erioglaucin A (EIn = +0.98 V, n = 2)Keq2 Cut + SeO2 + 4H+ 2 Cu²+ + H₂SO3 + H₂OE Cu²+/Cut = 0.150 VE Seo /H₂SeO,=Eeq == 1.200 V(assume the H+ concentration is 0.055 M)V

Answered: Image /qna-images/answer/eb99049d-0225-41de-861a-1abcb0f0c136.jpg

For each reaction, calculate the value of the equilibrium constant (Keq) and the electrode potential of the system at the equivalence point (Eeq) of a hypothetical titration. Co³+ + Ti²+ Co²+ + Ti³+ E Co³+/Co²+ = 1.900 V ET¹+²+ = -0.370 V Keq = Eeq = V

For each reaction, calculate the value of the equilibrium constant (Keq) and the electrode potential of the system at the equivalence point (Eeq) of a hypothetical titration. Co³+ + Ti²+ Co²+ + Ti³+ E Co³+/Co²+ = 1.900 V ET¹+²+ = -0.370 V Keq = Eeq = V

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter19: Applications Of Standard Electrode Potentials

Section: Chapter Questions

Problem 19.4QAP

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