Principles of Instrumental Analysis
7th Edition
ISBN: 9781305577213
Author: Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Question
Chapter 22, Problem 22.10QAP
Interpretation Introduction
Interpretation:
The
Concept introduction:
The electrode potential for the reaction of a cell can be defined as the electromotive force or the potential difference induced between the metal electrode and the solution. The Nernst equation is used for the calculation of electrode potential.
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
The solubility-product constant for Ag2SO3 is 1.5x10-14. Calculate E0 for the process
Calculate the solubility of AgBr in a 1.00 M aqueous solution of ammonia, given:
AgBr(s) ⇌ Ag+(aq) + Br-(aq) Ksp = 7.7 x 10-13
Ag+(aq) + 2 NH3(aq) ⇌ Ag(NH3)2+(aq) Kf = 1.7 x 107
[Hint: combine these reactions into a single reaction].
Calculate the equilibrium constant, K, for the following reaction at 25˚C.
2 Fe3+(aq) + Cu(s) → 2 Fe2+(aq) + Cu2+(aq) E° = 0.41 V
Give your answer in scientific notation (e.g. 211 is 2.11e2)
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
Knowledge Booster
Similar questions
- Aluminum ions react with the hydroxide ion to form the precipitate Al(OH)3(s), but can also react to form the soluble complex ion Al(OH)4. In terms of solubility, Al(OH)3(s) will be more soluble in very acidic solutions as well as more soluble in very basic solutions. a. Write equations for the reactions that occur to increase the solubility of Al(OH)3(s) in very acidic solutions and in very basic solutions. b. Lets study the pH dependence of the solubility of Al(OH)3(s) in more detail. Show that the solubility of Al(OH)3, as a function of [H+], obeys the equation S=[H+]3Ksp/Kw3+KKw/[H+] where S = solubility = [Al3+] + [Al(OH)4] and K is the equilibrium constant for Al(OH)3(s)+OH(aq)Al(OH)4(aq) c. The value of K is 40.0 and Ksp for Al(OH)3 is 2 1032. Plot the solubility of Al(OH)3 in the pH range 412.arrow_forwardCalculate the biological standard Gibbs energies of reactions of the following reactions and half-reactions:(a) 2 NADH(aq) + O2(g) + 2 H+(aq) → 2 NAD+(aq) + 2 H2O(I) E⊕=+1.14 V(b) Malate(aq) + NAD+(aq) → oxaloacetate(aq) + NADH(aq) + H+(aq) E⊕=-0.154 V(c) O2(g) + 4H+(aq) + 4 e- → 2 H2O(I) E⊕ = +0.81 Varrow_forwardRose was studying the electric field effect on bacterial growth when he unknowingly carried out an anodic reaction on the platinum electrode that led to the discovery of the anticancer drug cisplatin, cis-[PtCl2(NH3)2]. > Determine the formation constant (Kf) of cisplatin at 25 °C.arrow_forward
- Determine the values of equilibrium constant (Kc) and ΔG° for the following reaction :Ni(s) + 2Ag+ (aq) → Ni2+ (aq) + 2Ag(s),E° = 1.05 V(1F = 96500 C mol-1)arrow_forward1. Calcium carbonate undergoes thermal decomposition CaCO3(s) ⇌ CaO(s) + CO2(g) at high temperatures. The equilibrium constant for the reaction is 0.0120 at 900 K. Calculate the partial pressure of carbon dioxide, CO2, when calcium carbonate, CaCO3, is heated at 900 K. 2. Calculate the standard cell potential for the reaction Zn(s)|Zn^2+(aq)||MnO^4-(aq), Mn^2+(aq), H+(aq)|Pt(s) 3. 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.arrow_forwardDetermine the values of equilibrium constant (Kc) and AG° for the following reaction:Ni(s) + 2Ag+(aq) —–> Ni+2(aq) + 2Ag(s),E° = 1.05 V (IF = 96500 C mol-1)arrow_forward
- .The solubility-product constant for Ag2SO3 is 1.5x10-14. Calculate E0 for the process Ag2SO3(s) +2e → 2Ag + SO3-2arrow_forwardThe equilibrium constant for the reaction CO(g) + H2O(g) ⇌ CO2(g) + H2(g) is K = 1.03 × 105 at 298.15 K. Calculate the standard reaction Gibbs energy at this temperature.arrow_forwardWhat do the solubility rules tell you about changing the temp and the pH of Alkaline Earth metals (Ba2+, Sr2+, Ca2+, Mg2+arrow_forward
- Calculate the solubility of silver acetate,AgCH3COO , in an aqueous solution buffered at pH = 4.00 . Take the value of Ksp for silver acetate to be 1.9 x 10^-3 M2.arrow_forwardCalculate the value of the normal potential of the reaction AgCl(s) + e- → Ag(s) + Cl- at a temperature of 25°C, knowing the value of the solubility product of silver chloride pKsp=9.74 and the normal potential of the reaction Ag+ + e- ↔ Ag E°=+0.799V.arrow_forward7) Write Electrochemical equations for the oxidation and reduction processes which occur during: i. The corrosion of aluminium by air-free sulfuric acid ii. Corrosion of iron in aerated sulfuric acid containing ferric sulphate iii. Corrosion of copper in aerated sulfuric acid containing ferric sulphate iv. Corrosion of nickel in seawater v. Corrosion of iron in air-free ferric chloride solution vi. The uniform corrosion of a 50% iron-chromium alloy in aerated hydrochloric acidarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Principles of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning