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 22.8QAP
Calculate the theoretical potential of each of the following cells.Is the cell reaction spontaneous as written or spontaneous in the opposite direction?
(a) Bi|BiO+ (0.0300 M),H+ (0.100 M)||I- (0.100 M), AgI(sat’d)|Ag
(b) Zn|Zn2+(5.75 × 10-4M)||Fe(CN)64-(530 × 10-2 M),Fe(CN)63-(6.75 × 10-2M)|Pt
(c) Pt,H2O (0.200 atm)|HCI(8.25 × 10-4M), AgCI(sat’d)| Ag
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Write the individual electrode reactions and the total cell reaction for each of
the following cells. In each cell the negative electrode is at the left.
(a) Pb | PbSO,(s), SO,-- || Cu++ | Cu
(b) Cd | Cd*+ || H+ | H:(g)
(c) Zn | Zn++ || Fe+*+, Fe++ | Pt
12.
For the following reaction that occurs at 25°C.
3Zn(s) + 2Cr3*(aq) 3Zn2*(aq) + 2Cr(s)
(a)
Write the cell notation.
(b)
Calculate the standard electrode potential, E°cell.
Calculate the cell potential if the concentrations of Cr3+ and Zn2+ ions are 0.10
M and 0.0090 M respectively.
(c)
(d)
Calculate the equilibrium constant for the reaction:
3Zn(s) + 2Cr3"(aq) 3Zn2*(aq) + 2Cr(s)
[+0.02 V, +0.06 V, 1.1×10²]
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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Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Calculate the standard cell potential of the following cell at 25C. Sn(s)Sn2+(aq)I2(aq)I(aq)arrow_forwardWhat is the cell potential (Ecell) of a spontaneous cell that is run at 25C and contains [Cr3+] = 0.10 M and [Ag+] = 1.0 104 M?arrow_forwardGalvanic cells harness spontaneous oxidationreduction reactions to produce work by producing a current. They do so by controlling the flow of electrons from the species oxidized to the species reduced. How is a galvanic cell designed? What is in the cathode compartment? The anode compartment? What purpose do electrodes serve? Which way do electrons always flow in the wire connecting the two electrodes in a galvanic cell? Why is it necessary to use a salt bridge or a porous disk in a galvanic cell? Which way do cations flow in the salt bridge? Which way do the anions flow? What is a cell potential and what is a volt?arrow_forward
- What is the cell potential of the following cell at 25C? Ni(s)Ni2+(1.0M)Sn2(1.5104M)Sn(s)arrow_forwardThe cell potential of the following cell at 25C is 0.480 V. ZnZn2+(1M)H+(testsolution)H2(1atm)Pt What is the pH of the test solution?arrow_forwardCalculate the standard cell potential of the cell corresponding to the oxidation of oxalic acid, H2C2O4, by permanganate ion. MnO4. 5H2C2O4(aq)+2MnO4(aq)+6H+(aq)10CO2(g)+2Mn2+(aq)+8H2O(l) See Appendix C for free energies of formation: Gf for H2C2O4(aq) is 698 kJ.arrow_forward
- Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.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_forwardCalculate the cell potential of a cell operating with the following reaction at 25C, in which [Cr2O32] = 0.020 M, [I] = 0.015 M, [Cr3+] = 0.40 M, and [H+] = 0.60 M. Cr2O72(aq)+6I(aq)+14H+(aq)2Cr3+(aq)+3I2(s)+7H2O(l)arrow_forward
- A typical total phosphate concentration in a cell, [HPO42] + [H2PO4], is 2.0 102 M. What are the concentrations of HPO42 and HPO4 at pH 7.40?arrow_forwardCalculate the cell potential of a cell operating with the following reaction at 25C, in which [MnO4] = 0.010 M, [Br] = 0.010 M. [Mn2] = 0.15 M, and [H] = 1.0 M. 2MNO4(aq)+10Br(aq)+16H+(aq)2MN2(aq)+5Br2(l)+8H2O(l)arrow_forwardConsider the following galvanic cell: A 15 0-mole sample of NH is added to the Ag compartment (assume 1.00 L of total solution after the addition). The silver ion reacts with ammonia to form complex ions as shown: Ag+(aq)+NH3(aq)AgNH3+(aq)K1=2.1103AgNH3+(aq)+NH3(aq)Ag(NH3)2+(aq)K2=8.2103 Calculate the cell potential after the addition of 15.0 moles of NH3.arrow_forward
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