(a)
Interpretation:
The table for reduction potential of various species is given. The reagent that is capable of the given reduction is to be picked.
Concept introduction:
The species with higher reduction potential undergoes reduction thus, oxidizing the other species while the species with lower reduction potential undergoes oxidation and thus, reduces the other species.
To determine: The species that are capable of the given reductions.
(b)
Interpretation:
The table for reduction potential of various species is given. The reagent that is capable of the given reduction is to be picked.
Concept introduction:
The species with higher reduction potential undergoes reduction thus, oxidizing the other species while the species with lower reduction potential undergoes oxidation and thus, reduces the other species.
To determine: The species that are capable of the given reductions.
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Chapter 17 Solutions
Chemistry: An Atoms First Approach
- 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.arrow_forwardAn electrochemical cell consists of a nickel metal electrode immersed in a solution with [Ni2+] = 1.0 M separated by a porous disk from an aluminum metal electrode immersed in a solution with [Al3+] = 1.0 M. Sodium hydroxide is added to the aluminum compartment, causing Al(OH)3(s) to precipitate. After precipitation of Al(OH)3 has ceased, the concentration of OH is 1.0 104 M and the measured cell potential is 1.82 V. Calculate the Ksp value for Al(OH)3. Al(OH)3(s)Al3+(aq)+3OH(aq)Ksp=?arrow_forwardIf the SHE was assigned a value of 3.00 V rather than 0.00 V, what would happen to all of the values listed in the table of standard reduction potentials?arrow_forward
- Consider the following reduction potentials: Co3++ 3e Co = 1.26 V Co2++ 2e Co = 0.28 V a. When cobalt metal dissolves in 1.0 M nitric acid, will Co3+ or Co2+ be the primary product (assuming standard conditions)? b. Is it possible to change the concentration of HNO3 to get a different result in part a? Concentrated HNO3 is about 16 M.arrow_forwardCalculate the cell potential of a cell operating with the following reaction at 25C, in which [MnO4] = 0.010 M, [Br] = 0.010 M. [Mn2] = 0.15 M, and [H] = 1.0 M. 2MNO4(aq)+10Br(aq)+16H+(aq)2MN2(aq)+5Br2(l)+8H2O(l)arrow_forwardCalculate 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)arrow_forward
- Galvanic cells harness spontaneous oxidationreduction reactions to produce work by producing a current. They do so by controlling the flow of electrons from the species oxidized to the species reduced. How is a galvanic cell designed? What is in the cathode compartment? The anode compartment? What purpose do electrodes serve? Which way do electrons always flow in the wire connecting the two electrodes in a galvanic cell? Why is it necessary to use a salt bridge or a porous disk in a galvanic cell? Which way do cations flow in the salt bridge? Which way do the anions flow? What is a cell potential and what is a volt?arrow_forwardIdentify the reaction at the anode, reaction at the cathode, the overall reaction, and the approximate potential required for the electrolysis of the following molten salts. Assume standard states and that the standard reduction potentials in Appendix L are the same as those at each of the melting points. Assume the efficiency is 100%. (a) CaCl2. (b) LiH. (c) AlCl3. (d) CrBr3arrow_forwardA galvanic cell is based on the following half-reactions: In this cell, the silver compartment contains a silver electrode and excess AgCl(s) (Ksp = 1.6 1010), and the copper compartment contains a copper electrode and [Cu2+] = 2.0 M. a. Calculate the potential for this cell at 25C. b. Assuming 1.0 L of 2.0 M Cu2+ in the copper compartment, calculate the moles of NH3 that would have to be added to give a cell potential of 0.52 Vat 25C (assume no volume change on addition of NH3). Cu2+(aq)+4NH3(aq)Cu(NH3)42+(aq)K=1.01013arrow_forward
- What is the maximum work you can obtain from 30.0 g of nickel in the following cell when the cell potential is 0.97 V? Ni(s)Ni2+(aq)Ag+(aq)Ag(s)arrow_forwardConsider 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.arrow_forwardCopper(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?arrow_forward
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