Select the charge balance equation for an aqueous solution of MnCl, that ionizes to Mn²+, Cl-, MnCl+, and MnOH+.[H+] + 2 [Mn2+] + [MnCI+] + [MnOH+] = [CI] + [OH-][Mn2+] + [MnCl+] + [MnOH+] = [CI] + [OH-]O 2 [Mn2+] + [MnCI+] + [MnOH+] = [CI] + [OH-]O 2 [Mn2+] + [MnCl+] + [MnOH+] = [Cl¯]O [Mn2+] + [MnCl+] + [MnOH+] = 2 [CI] + [OH-]O [H+] + [Mn²+] + [MnCl+] + [MnOH+] = 2 [CI] + [OH-]O [H+] + [Mn²+] + [MnCI+] + [MnOH+] = [CI] + [OH¯]O [Mn2+] + [MnCl+] + [MnOH+¹] = 2 [CI]O [Mn²+] + [MnCl*] + [MnOH+] = [CI¯]Select the mass balance equation for the same solution.2 [Mn²+] + [MnCl+] + [MnOH+] = [MnCl+] + [CI]O [Mn²+] + [MnCI+] + [MnOH+] = [MnCl*] + 2 [Cl¯]O2 [Mn²+] = [CI]O [Mn²+] + [MnCl+] + [MnOH+] = 2 ([MnCl+] + [CI¯])O 2 ([Mn²+] + [MnCl+] + [MnOH+]) = [MnCI+] + [CI]

Given equation for aquous solution of MnCl2 that ionises to Mn2+,Cl-,MnCl+ and MnOH+.

Select the charge balance equation for an aqueous solution of MnCl₂ that ionizes to Mn2+, Cl-, MnCI+, and MnOH+. [H+] + 2 [Mn²+] + [MnCl+] + [MnOH+] = [CI] + [OH-] [Mn²+] + [MnCI+] + [MnOH+] = [CI] + [OH-] 2 [Mn²+] + [MnC1+] + [MnOH+] = [CI] + [OH-] O2 [Mn2+] + [MnCl+] + [MnOH+] = [CI] O [Mn2+] + [MnC1+] + [MnOH+] = 2 [CI] + [OH¯] O [H+] + [Mn²+] + [MnCI+] + [MnOH+] = 2 [CI] + [OH-] [H+] + [Mn²+] + [MnCl+] + [MnOH+] = [CI¯] + [OH¯] [Mn2+] + [MnC1+] + [MnOH+] = 2 [CI] O [Mn²+] + [MnCl+] + [MnOH+] = [CI¯] Select the mass balance equation for the same solution. O 2 [Mn²+] + [MnCI+] + [MnOH+] = [MnCl+] + [CI] [Mn²+] + [MnCI+] + [MnOH+] = [MnCI+] + 2 [CI] 2 [Mn²+] = [CI] [Mn²+] + [MnC1+] + [MnOH+] = 2 ([MnCI+] + [CI]) O 2 ([Mn²+] + [MnCI+] + [MnOH+]) = [MnCI+] + [CI]

Select the charge balance equation for an aqueous solution of MnCl₂ that ionizes to Mn2+, Cl-, MnCI+, and MnOH+. [H+] + 2 [Mn²+] + [MnCl+] + [MnOH+] = [CI] + [OH-] [Mn²+] + [MnCI+] + [MnOH+] = [CI] + [OH-] 2 [Mn²+] + [MnC1+] + [MnOH+] = [CI] + [OH-] O2 [Mn2+] + [MnCl+] + [MnOH+] = [CI] O [Mn2+] + [MnC1+] + [MnOH+] = 2 [CI] + [OH¯] O [H+] + [Mn²+] + [MnCI+] + [MnOH+] = 2 [CI] + [OH-] [H+] + [Mn²+] + [MnCl+] + [MnOH+] = [CI¯] + [OH¯] [Mn2+] + [MnC1+] + [MnOH+] = 2 [CI] O [Mn²+] + [MnCl+] + [MnOH+] = [CI¯] Select the mass balance equation for the same solution. O 2 [Mn²+] + [MnCI+] + [MnOH+] = [MnCl+] + [CI] [Mn²+] + [MnCI+] + [MnOH+] = [MnCI+] + 2 [CI] 2 [Mn²+] = [CI] [Mn²+] + [MnC1+] + [MnOH+] = 2 ([MnCI+] + [CI]) O 2 ([Mn²+] + [MnCI+] + [MnOH+]) = [MnCI+] + [CI]

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter17: Electrochemistry And Its Applications

Section: Chapter Questions

Problem 17QRT

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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)?
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.
An electrochemical cell is made by placing an iron electrode in 1.00 L of 0.15 M FeSO4 solution and a copper electrode in 1.00 L of 0.040 M CuSO4 solution. a What is the initial voltage of this cell when it is properly constructed? b Calculate the final concentration of Cu2+ in this cell if it is allowed to produce an average current of l.25 amp for 375 s.
Use Table 17.1 to predict what reaction, if any, will occur if sulfur is added to acidic aqueous solutions of the following species at standard conditions. (a) MgBr2 (b) Sn(NO3)2(c) Cr(ClO3)2
An electrochemical cell is made by placing a zinc electrode in 1.00 L of 0.200 M ZnSO4 solution and a copper electrode in 1.00 L of 0.0100 M CuCl2 solution. a What is the initial voltage of this cell when it is properly constructed? b Calculate the final concentration of Cu2+ in this cell if it is allowed to produce an average current of 1.0 amp for 225 s.
In some old European churches, the stained-glass windowshave so darkened from corrosion and age that hardly anylight comes through. Microprobe analysis showed that tinycracks anddefects on the glass surface were enriched ininsoluble Mn(III) and Mn(IV) compounds. From AppendixE, suggest a reducing agent and conditions that might successfullyconvert thesecompounds to soluble Mn(II) withoutsimultaneously reducing Fe(III) (which gives the glassits colors) to Fe(II). Take MnO2 as representative of theinsoluble Mn(III) and Mn(IV) compounds.
Answer the following questions by referring to standard electrode potentials at 25C. a Will oxygen, O2, oxidize iron(II) ion in solution under standard conditions? b Will copper metal reduce 1.0 M Ni2(aq) to metallic nickel?
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.
Order the following oxidizing agents by increasing strength under standard-state conditions: Ag+(aq); Cd2+(aq); MnO4(aq) (in acidic solution).
Copper(I) ion disproportionates to copper metal and copper(ll) ion. (See Study Question 99.) 2 Cu+(aq) Cu(s) + Cu2 + (aq) (a) What two half-reactions make up the disproportionation reaction? (b) Use values of the standard reduction potentials for the two half-reactions in part (a) to determine whether this disproportionation reaction is product-favored at equilibrium. (c) What is the equilibrium constant for this reaction? If you have a solution that initially contains 0.10 mol of Cu+ in 1.0 L of water, what are the concentrations of Cu+ and Cu2+ at equilibrium?
Use Table 17.1 to select (a) a reducing agent in acidic solution that converts ClO3- to Cl2 but not Cr2O72- to Cr3+. (b) an oxidizing agent that converts Mg to Mg2+ but not Mn to Mn2+. (c) a reducing agent in basic solution that converts NO2- to NO3- but not OH- to O2.
Calculate the cell potential of a cell operating with the following reaction at 25C, in which [Cr2O32] = 0.020 M, [I] = 0.015 M, [Cr3+] = 0.40 M, and [H+] = 0.60 M. Cr2O72(aq)+6I(aq)+14H+(aq)2Cr3+(aq)+3I2(s)+7H2O(l)

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