Which of the statements below are true for the titration of Fe2* with standard Cet? I. The indicator electrode potential before the addition of Cet solution is calculated using the Fe+ half-reaction after calculating the equilibrium
Which of the statements below are true for the titration of Fe2* with standard Cet? I. The indicator electrode potential before the addition of Cet solution is calculated using the Fe+ half-reaction after calculating the equilibrium
Chapter10: Potentiometry And Redox Titrations
Section: Chapter Questions
Problem 3P
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Question
![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](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F386f8283-9ac2-474e-b6c8-1cd7a8987d20%2Fda64bac4-b3b5-4600-90ae-745cf73c1175%2Fy1i4sck_processed.jpeg&w=3840&q=75)
Transcribed Image Text: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
Transcribed Image Text:Which statements are true for redox indicators?
1. The color change occurs when the indicator goes
from its oxidized form to its reduced form.
II. The color for the oxidized state of the indicator
occurs when the ratio of the reduced state to the
oxidized state is 1:10.
II. The range over which the indicator functions is E
IV. The color for the reduced state of the indicator
occurs when the ratio of the reduced state to the
oxidized state is is 1:10.
Il and IV
1, I, and IV
1, Il, and tll
I, II, II, and IV
1, Ill, and IV
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