Graph 3. Ecell vs - Log[concentration of Anode solution, M] Table 4. Final Results Ecell saturated solution of CuC,04, 0.148 Equation of the trendline in terms of Ecell and log (M) Slope Value - log (M) Molarity Cu", M Molar solubility CuC,04, M Ksp CuC,O, Accepted Ksp Experimental Error, % 4.43E-10
Graph 3. Ecell vs - Log[concentration of Anode solution, M] Table 4. Final Results Ecell saturated solution of CuC,04, 0.148 Equation of the trendline in terms of Ecell and log (M) Slope Value - log (M) Molarity Cu", M Molar solubility CuC,04, M Ksp CuC,O, Accepted Ksp Experimental Error, % 4.43E-10
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter19: Principles Of Chemical Reactivity: Electron Transfer Reactions
Section19.5: Electrochemical Cells Under Nonstandard Conditions
Problem 19.7CYU: The half-cells Ag+(aq. 1.0 M)|Ag(s) and H+(aq, ? M)|H2(1.0 bar) are linked by a salt bridge to...
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Please show calculations for how to get calculated potential using nernst equation and -log
-Log needed to create graph to solve table 4
![Graph 3. Ecell vs - Log[concentration of Anode solution, M]
Table 4. Final Results
Ecell saturated solution of CuC204, V
0.148
Equation of the trendline in terms of Ecell and log (M)
Slope Value
- log (M)
Molarity Cu*, M
Molar solubility CuC,04, M
Ksp CuC,0,
Accepted Ksp
Experimental Error, %
4.43E-10](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F435327ce-ad1d-47b0-9d05-42b05e19b7ae%2Fd6867910-1c88-44d5-9742-b5d2b69f9da5%2Fx56z9b8_processed.png&w=3840&q=75)
Transcribed Image Text:Graph 3. Ecell vs - Log[concentration of Anode solution, M]
Table 4. Final Results
Ecell saturated solution of CuC204, V
0.148
Equation of the trendline in terms of Ecell and log (M)
Slope Value
- log (M)
Molarity Cu*, M
Molar solubility CuC,04, M
Ksp CuC,0,
Accepted Ksp
Experimental Error, %
4.43E-10
![For the saturated solution of CuC,0, in the anode half-cell, and 1.0M Cu“ in the cathode half-cell,
the measured cell potential is 0.148V
Table 3. Cell Potentials of Concentration Copper Cell
Anode:
Copper (Cu)
Cathode
Copper (Cu)
Cathode
Anode electrolyte
Measured
electrolyte
-Log[Anode]
concentration, M
Potential, V
concentration, M
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
0.185](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F435327ce-ad1d-47b0-9d05-42b05e19b7ae%2Fd6867910-1c88-44d5-9742-b5d2b69f9da5%2Fxusmsi_processed.png&w=3840&q=75)
Transcribed Image Text:For the saturated solution of CuC,0, in the anode half-cell, and 1.0M Cu“ in the cathode half-cell,
the measured cell potential is 0.148V
Table 3. Cell Potentials of Concentration Copper Cell
Anode:
Copper (Cu)
Cathode
Copper (Cu)
Cathode
Anode electrolyte
Measured
electrolyte
-Log[Anode]
concentration, M
Potential, V
concentration, M
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
0.185
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