159. A ga Cu(s) E° = 0.34 V Cu*(aq) + 2e¯ v²*(aq) + 2e¯ –→ V(s) - E° = -1.20 V - In this cell, the copper compartment contains a copper elec- trode and [Cu²+] = 1.00 M, and the vanadium compartment contains a vanadium electrode and V²* at an unknown con- centration. The compartment containing the vanadium (1.00 L of solution) was titrated with 0.0800 M H;EDTA²-, resulting in the reaction H,EDTA²¯(aq) + V²*(aq)=VEDTA²¯(aq) + 2H*(ao) K = ? The potential of the cell was monitored to determine the stoi chiometric point for the process, which occurred at a volume of 500.0 mL H;EDTA²- solution added. At the stoichiometric point, Ecell Was observed to be 1.98 V. The solution was buff- ered at a pH of 10.00. r bs a. Calculate Ecell before the titration was carried out. b. Calculate the value of the equilibrium constant, K, for the titration reaction. c. Calculate Ecell at the halfway point in the titration.
159. A ga Cu(s) E° = 0.34 V Cu*(aq) + 2e¯ v²*(aq) + 2e¯ –→ V(s) - E° = -1.20 V - In this cell, the copper compartment contains a copper elec- trode and [Cu²+] = 1.00 M, and the vanadium compartment contains a vanadium electrode and V²* at an unknown con- centration. The compartment containing the vanadium (1.00 L of solution) was titrated with 0.0800 M H;EDTA²-, resulting in the reaction H,EDTA²¯(aq) + V²*(aq)=VEDTA²¯(aq) + 2H*(ao) K = ? The potential of the cell was monitored to determine the stoi chiometric point for the process, which occurred at a volume of 500.0 mL H;EDTA²- solution added. At the stoichiometric point, Ecell Was observed to be 1.98 V. The solution was buff- ered at a pH of 10.00. r bs a. Calculate Ecell before the titration was carried out. b. Calculate the value of the equilibrium constant, K, for the titration reaction. c. Calculate Ecell at the halfway point in the titration.
Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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159
![159. A ga
Cu(s)
E° = 0.34 V
Cu*(aq) + 2e¯
v²*(aq) + 2e¯ –→ V(s)
-
E° = -1.20 V
-
In this cell, the copper compartment contains a copper elec-
trode and [Cu²+] = 1.00 M, and the vanadium compartment
contains a vanadium electrode and V²* at an unknown con-
centration. The compartment containing the vanadium (1.00 L
of solution) was titrated with 0.0800 M H;EDTA²-, resulting
in the reaction
H,EDTA²¯(aq) + V²*(aq)=VEDTA²¯(aq) +
2H*(ao)
K = ?
The potential of the cell was monitored to determine the stoi
chiometric point for the process, which occurred at a volume
of 500.0 mL H;EDTA²- solution added. At the stoichiometric
point, Ecell Was observed to be 1.98 V. The solution was buff-
ered at a pH of 10.00.
r bs
a. Calculate Ecell before the titration was carried out.
b. Calculate the value of the equilibrium constant, K, for the
titration reaction.
c. Calculate Ecell at the halfway point in the titration.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdc4c42cb-72ac-4de9-81a0-acc94505501a%2F4d178435-e5a3-4993-b50f-b53e07fea7d9%2Fidasq2s.png&w=3840&q=75)
Transcribed Image Text:159. A ga
Cu(s)
E° = 0.34 V
Cu*(aq) + 2e¯
v²*(aq) + 2e¯ –→ V(s)
-
E° = -1.20 V
-
In this cell, the copper compartment contains a copper elec-
trode and [Cu²+] = 1.00 M, and the vanadium compartment
contains a vanadium electrode and V²* at an unknown con-
centration. The compartment containing the vanadium (1.00 L
of solution) was titrated with 0.0800 M H;EDTA²-, resulting
in the reaction
H,EDTA²¯(aq) + V²*(aq)=VEDTA²¯(aq) +
2H*(ao)
K = ?
The potential of the cell was monitored to determine the stoi
chiometric point for the process, which occurred at a volume
of 500.0 mL H;EDTA²- solution added. At the stoichiometric
point, Ecell Was observed to be 1.98 V. The solution was buff-
ered at a pH of 10.00.
r bs
a. Calculate Ecell before the titration was carried out.
b. Calculate the value of the equilibrium constant, K, for the
titration reaction.
c. Calculate Ecell at the halfway point in the titration.
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