Use the standard reduction potentials for the reactions:
to calculate the value of
How does your answer compare with the value listed in Table 12.4?
Table 12.4
Values for a few compounds illustrate the wide range over which solubility product constants can vary. | |
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Chapter 13 Solutions
Chemistry for Engineering Students
- An 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_forwardAn 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)?arrow_forwardGiven the following two standard reduction potentials, solve for the standard reduction potential of the half-reaction M3++eM2+ (Hint: You must use the extensive property G to determine the standard reduction potential.)arrow_forward
- 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_forwardAnswer 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?arrow_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
- Iron(II) ion undergoes a disproportionation reaction to give Fe(s) and the iron(III) ion. That is, iron(II) ion is both oxidized and reduced within the same reaction. 3 Fe2+(aq) Fe(s) + 2 Fe3+(aq) (a) What two half-reactions make up the disproportionation reaction? (b) Use the 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?arrow_forwardConsider 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_forward
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