Table 4. Final Results E.. saturated solution of CuC;0.. V Equation of the trendline in terms of E.. and Slope Value 0.148 ro 0591VAalloalM 0.0309 - log (M) 4.97 Molarity Cu.M 1.071"10*-5 Molar solubility CuC20.. M 1.071"10*-5 K., CuCz0, Accepted Ksp Experimental Error, X 1.147 10-10 4.43E-10 74.11
Table 4. Final Results E.. saturated solution of CuC;0.. V Equation of the trendline in terms of E.. and Slope Value 0.148 ro 0591VAalloalM 0.0309 - log (M) 4.97 Molarity Cu.M 1.071"10*-5 Molar solubility CuC20.. M 1.071"10*-5 K., CuCz0, Accepted Ksp Experimental Error, X 1.147 10-10 4.43E-10 74.11
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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Please check if my table 4 is correct
![Part III
For the saturated solution of CUCU, in the anode halt-cell, and 1.UM Lu" in the cathode halt-cell,
the measured cell potential is 0.148V
Table 3. Cel Potentials of Concentration Copper Cell
Anode:
Сopper (Cu]
Сорper [Cu]
Cathode
Cathode
Anode electrolyte
Measured
-Log(Anode]
electrolyte
concentration, M
concentration, M
Potential, V
1.0
1.0
0.000
0.10
1.0
1
0.028
0.010
1.0
2
0.053
0.0010
1.0
3
0.080
0.00010
1.0
4
0.109
0.000010
1.0
0.155
0.0000010
1.0
6
0.185
Measured Potential vs Log
a200
0150
0100
a050
a000
0050
Log
Graph 3. Ecell vs - Log[concentration of Anode solution, M]
Table 4. Final Results
E.. saturated solution of CuC20..V
Equation of the trendline in terms of E.. and
0.148
Hints:
Ccell = C Cell-
Use the trendline to determine logarithm molarity of Cu' in the anode department
Take antilog and find molarity of Cu': Molar solubility CuC;0, since solution is saturated
Write expression for Ksp and use [Cu*)-[CuC;0,1to calculate Ksp
Slope Value
0.0309
- log (M)
4.97
Molarity Cu?.M
1.071"10*-5
Molar solubility CuCz0.. M
1.071"10*-5
K., CuC20.
1.147"10*-10
4.43E-10
Accepted Ksp
Experimental Error, X
74.11
Measured Potential](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F435327ce-ad1d-47b0-9d05-42b05e19b7ae%2F8783cb51-15f6-4ff1-a19e-5e421190f106%2Fbtc01df_processed.png&w=3840&q=75)
Transcribed Image Text:Part III
For the saturated solution of CUCU, in the anode halt-cell, and 1.UM Lu" in the cathode halt-cell,
the measured cell potential is 0.148V
Table 3. Cel Potentials of Concentration Copper Cell
Anode:
Сopper (Cu]
Сорper [Cu]
Cathode
Cathode
Anode electrolyte
Measured
-Log(Anode]
electrolyte
concentration, M
concentration, M
Potential, V
1.0
1.0
0.000
0.10
1.0
1
0.028
0.010
1.0
2
0.053
0.0010
1.0
3
0.080
0.00010
1.0
4
0.109
0.000010
1.0
0.155
0.0000010
1.0
6
0.185
Measured Potential vs Log
a200
0150
0100
a050
a000
0050
Log
Graph 3. Ecell vs - Log[concentration of Anode solution, M]
Table 4. Final Results
E.. saturated solution of CuC20..V
Equation of the trendline in terms of E.. and
0.148
Hints:
Ccell = C Cell-
Use the trendline to determine logarithm molarity of Cu' in the anode department
Take antilog and find molarity of Cu': Molar solubility CuC;0, since solution is saturated
Write expression for Ksp and use [Cu*)-[CuC;0,1to calculate Ksp
Slope Value
0.0309
- log (M)
4.97
Molarity Cu?.M
1.071"10*-5
Molar solubility CuCz0.. M
1.071"10*-5
K., CuC20.
1.147"10*-10
4.43E-10
Accepted Ksp
Experimental Error, X
74.11
Measured Potential
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