[References]Calculate the pH of the cathode compartment for the following reaction given Ecell = 3.01 V when Cr = 0.17 M, Al+ = 0.32 M, and%3DCr3O,-= 0.54 M.2A1(s) + Cr2 07 (aq) + 14H (aq) → 2Al* (aq) + 2Cr* (aq) + 7H2O(1)You may need to use the following data:Cr2 O,2- +14H + 6e 2Cr*+ + 7H20 E = 1.33 VAlšt + 3e - AlE° = –1.66 V(Enteryour answer to two significant figures.)pH =Submit AnswerTry Another Version10 item attempts remainingot12:49 PM12/6/2021CHIearch

In a given question , we have to find out the pH of a solution in a cathode compartment.

Calculate the pH ôf thể cathode compartment for the following reaction given Ecell = 3.01 V when Cr* = 0.17 M, Al* = 0.32 M, and A1³+ %3D = 0.54 M. 2Al(s) + Cr2 O,2-(aq) + 14H (ag) 2A1+ (ag) + 2Cr+ (aq) + 7H2O(1) You may need to use the following data: Cr2 O, +14H+ +6e 2Cr+ + 7H2O E = 1.33 V Al+ + 3e Al E = -1.66 V (Enter your answer to two significant figures.) pH = Submit Answer Try Another Version 10 item attempts remaining

Calculate the pH ôf thể cathode compartment for the following reaction given Ecell = 3.01 V when Cr* = 0.17 M, Al* = 0.32 M, and A1³+ %3D = 0.54 M. 2Al(s) + Cr2 O,2-(aq) + 14H (ag) 2A1+ (ag) + 2Cr+ (aq) + 7H2O(1) You may need to use the following data: Cr2 O, +14H+ +6e 2Cr+ + 7H2O E = 1.33 V Al+ + 3e Al E = -1.66 V (Enter your answer to two significant figures.) pH = Submit Answer Try Another Version 10 item attempts remaining

Principles of Instrumental Analysis

7th Edition

ISBN:9781305577213

Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Chapter24: Coulometry

Section: Chapter Questions

Problem 24.5QAP: What cathode potential (versus SCE) would be required to lower the total Hg(II) concentration of the...

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An alloy made up of tin and copper is prepared by simultaneously electroplating the two metals from a solution containing Sn(NO3)2 and Cu(NO3)2.If 20.0% of the total current is used to plate tin, while 80.0% is used to plate copper, what is the percent composition of the alloy?
The 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.
What cathode potential (versus SCE) would be required to lower the total Hg(II) concentration of the following solutions to 1.00 10-6 M (assume reaction product in each case is elemental Hg): (a) an aqueous solution of Hg2+? (b) a solution with an equilibrium SCN- concentration of 0.100 M? Hg2+ + 2SCN- Hg(SCN)2(aq) = Kf = 1.8 107 c) a solution with an equilibrium Br- concentration of 0.100 M? HgBr42++ 2e- Hg(l) + 4Br- E0= 0.223 V
A 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.
The saturated calomel electrode. abbreviated SCE. is often used as a reference electrode in making electrochemica1 measurements. The SCE is composed of mercury in contact with a saturated solution of calomel (Hg2Cl2). The electrolyte solution is saturated KCI. is +0.242 V relative to the standard hydrogen electrode. Calculate the potential for each of the following galvanic cells containing a saturated calomel electrode and the given half-cell components at standard conditions. In each case. indicate whether the SCE is the cathode or the anode. Standard reduction potentials are found in Table 17.1. a. Cu2++2eCu b. Fe3++e-Fe2+ c. AgCl+e-Ag+Cl- d. Al3++3eAl e. Ni2++2eNi
An 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)?
Consider 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.