Principles of Instrumental Analysis
7th Edition
ISBN: 9781305577213
Author: Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher: Cengage Learning
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Chapter 22, Problem 22.13QAP
From the standard potentials
calculate the solubility product constant for TlCl.
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Consider the cell:
Pt(s) | H2(g, 0.100 bar) | H+(aq, pH = 2.54) || Cl−(aq, 0.200 M) | Hg2Cl2(s) | Hg() | Pt(s)
Use the following information to calculate the cell potential.
Hg22+(aq) + 2e− ® 2Hg() E ° = 0.796 V
2H+(aq) + 2e− ® H2(g) E ° = 0.000 V
Hg2Cl2(s) ® Hg22+(aq) + 2Cl−(aq) Ksp = 1.2 × 10−18
The standard reaction Gibbs energy for the electrochemical reaction Cr2O7^2- + 2 Fe + 14 H+ → 2 Cr3+ + 2 Fe3+ 7 H2O is -793 kJ mol-1. Calculate the standard cell potential.
Consider the cell:
Pt(s) | H2(g, 0.100 bar) | H+(aq, pH = 2.54) || Cl−(aq, 0.200 M) | Hg2Cl2(s) | Hg() | Pt(s)
Use the following information to calculate the cell potential.
Hg2Cl2(s) + 2e− ® 2Hg() + 2Cl−(aq) E ° = 0.268 V
2H+(aq) + 2e− ® H2(g) E ° = 0.000 V
Chapter 22 Solutions
Principles of Instrumental Analysis
Ch. 22 - Calculate the electrode potentials of the...Ch. 22 - Prob. 22.2QAPCh. 22 - For each of the following half-cells, compare...Ch. 22 - For each of the following half-cells, compare...Ch. 22 - Prob. 22.5QAPCh. 22 - Calculate the electrode potentials for the...Ch. 22 - Calculate the theoretical potential of each of the...Ch. 22 - Calculate the theoretical potential of each of the...Ch. 22 - Prob. 22.9QAPCh. 22 - Prob. 22.10QAP
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- Calculate the standard cell potential of the following cell at 25C. Sn(s)Sn2+(aq)I2(aq)I(aq)arrow_forwardFrom the standard potentials Ag2SeO4(s)+2e2Ag(s)+SeO42-E0=0.355V Ag++2eAg(s)E0=0.799V calculate the solubility product constant for Ag2SeO4.arrow_forwardConsider the cell: Pt(s) | H₂(g, 0.100 bar) | H+ (aq, pH = 2.54) || Cl(aq, 0.200 M) | Hg₂Cl₂(s) | Hg(1) | Pt(s) Use the following information to calculate the cell potential. Hg₂²+ (aq) + 2e- → 2Hg(1) 2H+ (aq) + 2e- → H₂(g) Hg₂Cl₂(s) → Hg₂²+(aq) + 2Cl¯(aq) E° = 0.796 V E° = 0.000 V Ksp = 1.2 X 10-18arrow_forward
- The standard reduction potential of the Pb2+/Pb electrode is -0.13 V and the standard cell potential of the cell, Ni(s)|Ni2+(aq)|Pb2+(aq)|Pb(s), is +0.10 V. What is the standard reduction potential of the Ni2+/Ni electrode?arrow_forwardThe standard potential of the cell Ag(s)|AgI(s)|AgI(aq)|Ag(s) is +0.9509 V at 25 °C. Calculate the equilibrium constant for the dissolution of AgI(s).arrow_forwardThe standard potential of the cell Bi(s)|Bi2S3(s)|Bi2S3(aq)|Bi(s) is +0.96 V at 25 °C. Calculate the equilibrium constant for the dissolution of Bi2S3(s).arrow_forward
- 3 Co(s) + 2 NO 3- (aq) + 8 H+ (aq) = 3 Co 2+ (aq) + 2 NO (g) + 4 H2O (l) Determine the cell potential for the reaction at a pH of 4.0 ( you will need to use the Nernst equation) Assume that all concentrations, other than that of H+, are standard.arrow_forwardThe standard reaction Gibbs energy for the reaction: K2CrO4 (aq) + 2 Ag (s) + 2 FeCl3 (s) → Ag2CrO4 (s) + 2 FeCl2 (aq) + 2 KCl (aq) is – 62.5 kJ mol-1. Calculate the standard potential of the corresponding galvanic cell. [+0.324] The answer is in the bracket, I would like to know how it was obtained. Thank you!arrow_forwardConsider the cell diagram for an electrochemical cell: Pt | Ti2+(aq), Ti3+(aq) || Br2(g), Br-(aq) | Pt If the overall standard potential of the cell is 1.40 V, which of the following statements is false? The cell is a galvanic cell, and the anode involves losing 1 electron from Ti2+to Ti3+. The cell is an electrolytic cell, and the cathode involves losing 1 electron from Ti2+to Ti3+ The cell is a galvanic cell, and the cathode involves gaining 2 electrons from Br2to Br-. The cell is an electrolytic cell, and the anode involves gaining 2 electrons from Br2to Br-. a. 1 and 3b. 2 onlyc. 1 onlyd. 2 and 4arrow_forward
- Calculate the standard cell potential (E∘cell�cell∘) for the reaction X(s)+Y+(aq)⇌X+(aq)+Y(s)X(�)+Y+(��)⇌X+(��)+Y(�) if K=2.25×10−3�=2.25×10−3. Express your answer to three significant figuresarrow_forwardThe emf of the cell Pt | H2 (1 bar) | HCl (aq) | AgCl (s) | Ag was found to be 0.517 V at 25oC. Calculate the pH of the HCl solution.arrow_forwardPt(k)| Fe³+(aq), Fe²+(aq) // I-(aq) | 12(k) | Calculate the standard cell potential for the Pt(k) Cell and interpret whether the reaction taking place in the cell will proceed spontaneously under standard conditions. E° (Pt|Fe³+, Fe²+) = 0.77 V . E°( 12 | I-) = 0.53 Varrow_forward
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