Please check if my table 4 is correct Part IIIFor the saturated solution of CUCU, in the anode halt-cell, and 1.UM Lu" in the cathode halt-cell,the measured cell potential is 0.148VTable 3. Cel Potentials of Concentration Copper CellAnode:Сopper (Cu]Сорper [Cu]CathodeCathodeAnode electrolyteMeasured-Log(Anode]electrolyteconcentration, Mconcentration, MPotential, V1.01.00.0000.101.010.0280.0101.020.0530.00101.030.0800.000101.040.1090.0000101.00.1550.00000101.060.185Measured Potential vs Loga20001500100a050a0000050LogGraph 3. Ecell vs - Log[concentration of Anode solution, M]Table 4. Final ResultsE.. saturated solution of CuC20..VEquation of the trendline in terms of E.. and0.148Hints:Ccell = C Cell-Use the trendline to determine logarithm molarity of Cu' in the anode departmentTake antilog and find molarity of Cu': Molar solubility CuC;0, since solution is saturatedWrite expression for Ksp and use [Cu*)-[CuC;0,1to calculate KspSlope Value0.0309- log (M)4.97Molarity Cu?.M1.071"10*-5Molar solubility CuCz0.. M1.071"10*-5K., CuC20.1.147"10*-104.43E-10Accepted KspExperimental Error, X74.11Measured Potential

E is given to be equal to 0.148

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

Principles of Instrumental Analysis

7th Edition

ISBN:9781305577213

Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Chapter24: Coulometry

Section: Chapter Questions

Problem 24.4QAP: Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose...

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Question

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

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