Principles of Instrumental Analysis, 6th Edition
6th Edition
ISBN: 9788131525579
Author: Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher: Cenage 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, 6th Edition
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_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_forwardWhat is the cell potential of the following cell at 25C? Ni(s)Ni2+(1.0M)Sn2(1.5104M)Sn(s)arrow_forward
- The 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_forwardHalide 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_forward
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