1.Use standard reduction potentials to rationalize quantitatively why:(6 points)(a) Al liberates H2 from dilute HCl, but Ag does not;(b) Cl2 liberates Br2 from aqueous KBr solution, but does not liberate C12 from aqueous KClsolution;c) a method of growing Ag crystals is to immerse a zinc foil in an aqueous solution of AgNO3.

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Answered: 1. Use standard reduction potentials to…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter22: Bulk Electrolysis: Electrogravimetry And Coulometry

Section: Chapter Questions

Problem 22.20QAP

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3. Determine the oxidationnumber for the indicated elementin each of the followingsubstances: (a) S in SO2 , (b) Cin COCl2 , (c) Mn in MnO4- ,(d)N in N2H4 , (e) N in HNO2 ,(f) Cr in Cr2O72-
Tausonite, a mineral composed of Sr, O, and Ti, has the cubicunit cell shown in the drawing. (a) What is the empiricalformula of this mineral? (b) How many oxygens are coordinatedto titanium? (c) To see the full coordination environmentof the other ions, we have to consider neighboringunit cells. How many oxygens are coordinated to strontium?
(b) The stepwise stability constants for two metal ion/ligand combinations are tabulated below. log K₁ log K₂ log K₂ Fet/en 4.3 3.3 2.0 Fe²/bipy 5.9 5.2 10.0
(b) Using diagrams and chemical structures, explain why zinc is a suitable metal in carbonic anhydrase and carboxypeptidase. (c) Mollusks are blue-blonds Give a detailed aro [5]
Give detailed Solution with explanation needed..don't give Handwritten answer..don't use Ai for answering this...??&??
1. A 0.9882 gram sample of iron ore is dissolved, the iron reduced to Fe2+, and the solution was titrated with 36.40 mL of 0.02065 M KMnO4 in acid solution. (a) Write the titration reaction. (b) Calculate the %FeO (M.M. = 71.85) in the sample. 2. A sample of primary standard grade K2Cr2O7 (MM = 294.20) weighing 0.2153 g is dissolved, the solution acidified and excess KI added. The liberated I2 requires 44.86 mL of the Na2S2O3 for titration. (a) Write the titration reaction. (b) Calculate the molarity of the titrant solution. Box the final answer.
The E° values for two low-spin iron complexes in acidic solution are as follows: [Fe(o-phen),]**(aq) + e- [Fe(0-phen),]2*(aq) E° = 1.12 V [Fe(CN),* (aq) + e [Fe(CN)6]* (aq) E° = 0.36 V (a) Is it thermodynamically favorable to reduce both Fe(III) complexes to their Fe(II) analogs? Explain. (b) Which com- plex, [Fe(0-phen)3]* or [Fe(CN)6]*, is more difficult to reduce? (c) Suggest an explanation for your answer to (b).
1. For each of the following oxidation-reduction reactions, write the fully balanced half reactions. Also write the fully balanced net reaction that occurs for each reaction. (a) Iodide (I) is dissolved in an acidic aqueous solution of iodate (IO; ) to form I3'. (b) Dinitrogen tetraoxide (N204) gas is bubbled into a basic aqueous solution.
3. Metal ion complexation is known to affect the half-wave potential for the reduction of a metal ion. M+ + Hg+ne → M(Hg) MxAMAX (n-x)+ [1] [2] The relationship between the molar concentrations of the ligand CL and the shift in the half-wave potential is: = (E) E (-0.0592/n)logK - (0.0592x/n)logcL [3] Where (E) and E½ are half-wave potentials for the complexed and uncomplexed cation, respectively, K, is the formation constant for the complex, and x is the molar combining ratio of the complexing agent to cation. The following polarographic data were obtained for the reduction of Pb2+ to its amalgam from solutions that were 2.00 x 10-3 M in Pb2+, 0.100 M in KNO3, and different concentrations of the anion A. From the half-wave potentials, find (i) the formula of the complex, and (ii) its formation constant Kſ. Concentration A, M 0.0000 E vs. SCE, V -0.405 0.0200 -0.473 0.0600 -0.507 0.1007 -0.516 0.3000 -0.547 0.5000 -0.558
Explain the separation of Fe2O3 from bauxite with equations
5. a) Use the rules in Example 4.4 (p. 99) and calculate sizes of octahedral and tetrahedral cavities in titanium and in zirconium. Use values for atomic radii given in Fig. 9.1 (p.291). (3 points) b) Consider the formation of carbides (MC) of these metals. Which metal is able to accommodate carbon atoms better, and which cavities (octahedral or tetrahedral) would be better suited to accommodate C atoms into metal's lattice? (4 points)
An aqueous solution of SO2 reduces (a) aqueous KMnO4 toMnSO4(aq), (b) acidic aqueous K2Cr2O7 to aqueous Cr3 + ,(c) aqueous Hg2(NO3)2 to mercury metal. Write balancedequations for these reactions.

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