Design a cell that would allow you to determine theKsp of PbSO4(s) from electrochemical data.Determine the Ksp of PbSO4(s) at 25°C:PbSO4(s) = Pb2+(aq) + SO4²-(aq)

Given : Balanced chemical equation ionization of PbSO4. To find : Ksp of PbSO4 at 25°C. Solution :…

Answered: Design a cell that would allow you to…

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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Write the cell notation for an electrochemical cell consisting of an anode where Mg (s) is oxidized to Mg2+ (aq) and a cathode where Ag+ (aq) is reduced to Ag (s) . Assume all aqueous solutions have a concentration of 1 mol/L.
Consider the following galvanic cell: Li (s) | 0.095M LiCl (aq) || 0.032M Sn(NO3)2 (aq) | Sn (s) Using Appendix H in the textbook, determine the Ecell of this galvanic cell. 2.54 V - 2.88 V O -2.92 V 2.88 V 2.92 V
Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C.2 Al(s) + 3 Mg2+(aq) → 2 Al3+(aq) + 3 Mg(s)Mg2+(aq) + 2 e⁻ → Mg(s) E° = -2.37 VAl3+(aq) + 3 e⁻ → Al(s) E° = -1.66 V A) 1.0 × 1024 B) 1.1 × 10-73 C) 1.1 × 1072 D) 8.9 × 10-73 E) 4.6 × 1031
Consider the following voltaic cell at 25°C: Al(s) | Al3*(0.20 M, aq) || Al3+(0.75 M, aq) | Al(s) If the standard reduction potential for the Al3+(aq) /Al(s) redox couple is -1.66 V, what is the overall cell reaction and the cell potential of the voltaic cell shown above? The overall cell reaction is Al3+(0.20 M, ag) Al3*(0.75 M, ag) and Ecell = -0.0113 V. The overall cell reaction is Al3*(0.75 M, aq) AI3+(0.20 M, ag) and Ecell = +0.0113 V. None of these The overall cell reaction is Al3+(0.20 M, aq) Al3*(0.75 M, ag) and Ecell = +0.0113 V. There is no overall cell reaction and Ecell 0.00 V. %3D The overall cell reaction is Al3+(0.75 M, aq) Als*(0.20 M, aq) and Ecell = -0.0113 V.
For the cell: Zn(s) + 2H† (aq) →→ Zn2+(aq) + H2 (g) If [Zn2+] = 1 M, PH2 = 1 atm, and E = 0.123 V what is pH?
Consider the following galvanic cell: E° (V) U3+ + 3 e− → U(s) −1.642 In3+ + 2e− → In+ −0.444 What is the potential of the galvanic cell when In3+ is 0.023 M, In+ is 0.37 M, and U3+ is 0.076 M?
Consider a galvanic electrochemical cell constructed using Cr/Cr³⁺ and Zn/Zn²⁺ at 25 °C. The following half-reactions are provided for each metal: Cr³⁺(aq) + 3 e⁻ → Cr(s) E°red = -0.744 V Zn²⁺(aq) + 2 e⁻ → Zn(s) E°red = -0.763 V Given that the standard cell potential is 0.019 V and the overall equation is 2 Cr³⁺ (aq) + 3 Zn (s) → 2 Cr (s) + 3 Zn²⁺ (aq), what is the cell potential for this cell at 25 °C when [Zn²⁺] = 0.0323 M and [Cr³⁺] = 0.1736 M?
When [Pb2+] = 1.49 M, the observed cell potential at 298 K for an electrochemical cell with the reaction shown below is 0.749 V. What is the Zn2+ concentration in this cell? Pb2+(aq) + Zn(s) → Pb(s) + Zn²+(aq) [Zn2+] = mol/L
Consider the following voltaic cellat 25°C: Al(s) | Al3*(0.20 M, aq) || Al3+(0.75 M, aq) | Al(s) If the standard reduction potential for the Al3+(aq) /Al(s) redox couple is -1.66 V, what is the overall cell reaction and the cell potential of the voltaic cell shown above? (Reference the cell as written above.) The overall cell reaction is Al3+(0.75 M, aq) AIS*(0.20 M, ag) and E°cell = +0.0113 V. There is no overall cell reaction and E°cell = 0.00 V. The overall cell reaction is Al3+(0.20 M, aq) Als*(0.75 M, aq) and E°cell = +0.0113 V. The overall cell reaction is Al3+(0.20 M, aq) →A13+(0.75 M, ag) and E°cell| = -0.0113 V. The overall cell reaction is Al3*(0.75 M, aq) →AI3*(0.20 M, aq) and E°cell = -0.0113 V. None of these
What is the cell potential (EO) for a galvanic cell formed from the following two half-reactions? PbO2(s) + 3 H*(a) + HSO4-(aq) + 2 e-+ PBSO4(s) + 2 E° = 1.690 V %3D H20(1) PbSO4(s) + H*(aq) + 2 e- → Pb(s) + HSO4-(aq) E° = -0.356 V (A) +1.334 V (B) -2.046 V c) +2.046 V D) +2.758 V
Write the cell notation for an electrochemical cell consisting of an anode where Cu (s) is oxidized to Cu²+ (aq) and a cathode where Fe³+ (aq) is reduced to Fe²+ (aq) at a platinum electrode. Assume all aqueous solutions have a concentration of 1 mol/L.
Consider the following cell: Ni(s)|Ni2+(aq, 0.100 M)||Cl–(aq, 0.200 M)|Cl2(g, 1.50 atm)|Pt If the standard voltage for this cell is 1.59 V at 25oC, calculate the voltage of this cell.

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Design a cell that would allow you to determine the Ksp of PBSO4(s) from electrochemical data. Determine the Ksp of PbSO4(s) at 25°C: PBSO4(s) = Pb2+(aq) + SO4²-(aq)