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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Question
Chapter 23, Problem 23.19QAP
Interpretation Introduction
Interpretation:
The formation constant for the following reaction should be predicted.
Concept introduction:
Formation constant measures the strength of interaction between the reactant and the complex. It is equal to the ratio of complex or product to the reactants.
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Chapter 23 Solutions
Principles of Instrumental Analysis
Ch. 23 - Prob. 23.1QAPCh. 23 - Prob. 23.2QAPCh. 23 - Prob. 23.3QAPCh. 23 - Prob. 23.4QAPCh. 23 - Prob. 23.5QAPCh. 23 - Prob. 23.6QAPCh. 23 - Prob. 23.7QAPCh. 23 - Prob. 23.8QAPCh. 23 - Prob. 23.9QAPCh. 23 - List the advantages and disadvantages of a...
Ch. 23 - Prob. 23.11QAPCh. 23 - What arc the advantages of microfabricated ISEs?...Ch. 23 - Prob. 23.13QAPCh. 23 - Prob. 23.14QAPCh. 23 - Prob. 23.15QAPCh. 23 - The following cell was used for the determination...Ch. 23 - The following cell was used to determine the pSO4...Ch. 23 - The formation constant for the mercury(II) acetate...Ch. 23 - Prob. 23.19QAPCh. 23 - The cell Ag|AgCl(sat’d)||H+(a = x)|glass electrode...Ch. 23 - The following cell was found to have a potential...Ch. 23 - The following cell was found to have a potential...Ch. 23 - The following cell was found to have a potential...Ch. 23 - Prob. 23.24QAPCh. 23 - Prob. 23.25QAPCh. 23 - Prob. 23.26QAPCh. 23 - Prob. 23.27QAP
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- The following cell was found to have a potential of 0.124 V: Ag|AgCl(sat’d)||Cu2+ (3.25 10-3 M|mernbrane electrode for Cu2+ When the solution of known copper activity was replaced with an unknown solution, the potential was found to be 0.055 V. What was the pCu of this unknown solution? Neglect the junction potential.arrow_forwardThe following cell was found to have a potential of —0.492 V: Ag|AgCl(sat’d)||HA(0.200 M),NaA(0.300 M)|H2(1.00 atm),Pt Calculate the dissociation constant of HA, neglecting the junction potential.arrow_forwardThe standard reduction potential for the reaction [Co( H 2 O)6]3+(aq)+e[CO( H 2 O)6]2+(aq) is about 1.8 V. The reduction potential for the reaction [Co( NH 3 )6]3+(aq)+e[Co( NH 3 )6]2+(aq) is +0.1 V. Calculate the cell potentials to show whether the complex ions,. [Co( H 2 O)6]2+ and or [Co( NH 3 )6]2+, can be oxidized to the corresponding Cobalt (III) complex by oxygen.arrow_forward
- Calculate the standard potential for the half-reaction Al (C2O4)2- + 3e- Al(s ) + 2C2O42- if the formation constant for the complex is 1.3 1013.arrow_forwardThe cell Ag|AgCl(sat’d)||H+(a = x)|glass electrode has a potential of —0.2094 V when the solution in the right-hand compartment is a buffer of pH 4.006. The following potentials are obtained when the buffer is replaced with unknowns: (a) —0.2806 V and (b) —0.2132 V. Calculate the pH and the hydrogen ion activity of each unknown. (c) Assuming anuncertainty of 0.001 Vin the junction potential, what is the range of hydrogen ion activities withinwhich the true value might be expected to lie?arrow_forwardThe formation constant for the mercury(II) acetate complex is Hg2++ 2OAc- Hg(OAc)2(aq) Kf = 2.7 108 Calculate the standard potential for the half-reaction Hg(OAc)2(aq) + 2e- Hg(l) + 2OAc-arrow_forward
- Repeat the directions for Question 106 using a cell constructed of a strip of nickel immersed in a 1.0-M Ni2+ solution and a strip of silver dipping into a 1.0-M Ag+ solution. Write the balanced chemical equation for the reaction that is product-favored. Calculate the cell potential. Draw a sketch of the cell and indicate the anode, cathode, and direction of electron flow.arrow_forwardAn aqueous solution of an unknown salt of vanadium is electrolyzed by a current of 2.50 amps for 1.90 hours. The electroplating is carried out with an efficiency of 95.0%, resulting in a deposit of 2.850 g of vanadium. a How many faradays are required to deposit the vanadium? b What is the charge on the vanadium ions (based on your calculations)?arrow_forwardA galvanic cell is based on the following half-reactions: In this cell, the copper compartment contains a copper electrode and [Cu2+] = 1.00 M, and the vanadium compartment contains a vanadium electrode and V2+ at an unknown concentration. The compartment containing the vanadium (1.00 L of solution) was titrated with 0.0800 M H2EDTA2, resulting in the reaction H2EDTA2(aq)+V2+(aq)VEDTA2(aq)+2H+(aq)K=? The potential of the cell was monitored to determine the stoichiometric point for the process, which occurred at a volume of 500.0 mL H2EDTA2 solution added. At the stoichiometric point, was observed to be 1 .98 V. The solution was buffered at a pH of 10.00. a. Calculate before the titration was carried out. b. Calculate the value of the equilibrium constant, K, for the titration reaction. c. Calculate at the halfway point in the titration.arrow_forward
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