(a)
Interpretation:
When the 0.65 M KOH is replaced by 0.65 M NH3,whether the value of
Concept introduction:
The relation between hydrogen ion concentration and hydroxide ion concentration is represented as follows:
In an
If oxidation takes place on an electrode, that electrode is called anode. The species in that electrode remove electrons and itself gets oxidized.
If reduction takes place on an electrode, that electrode is called cathode. The species in that electrode absorbs electrons and itself gets reduced.
The electrode potential of cell can be calculated as follows:
Nernst equation for a cell can be represented as follows:
Here,
z = number of moles of electrons transferred in the cell and Q is ratio of concentration of products to reactant in a cell.
(b)
Interpretation:
The value of
Concept introduction:
Ammonia is weak base. Therefore, partially ionized in water as follows:
For the above reaction, the base equilibrium constant can be calculated as follows:
Here,
In an electrochemical cell, there are two electrodes that can be observed.
If oxidation takes place on an electrode, that electrode is called anode. The species in that electrode remove electrons and itself gets oxidized.
If reduction takes place on an electrode, that electrode is called cathode. The species in that electrode absorbs electrons and itself gets reduced.
The electrode potential of cell can be calculated as follows:
Nernst equation for a cell can be represented as follows:
Here,
z = number of moles of electrons transferred in the cell and Q is ratio of concentration of products to reactant in a cell.
Want to see the full answer?
Check out a sample textbook solutionChapter 19 Solutions
Selected Solutions Manual For General Chemistry: Principles And Modern Applications
- How long would it take to reduce 1 mole of each of the following ions using the current indicated? Assume the voltage is sufficient to perform the reduction. (a) AR3+, 1.234 A. (b) Ca2+, 22.2 A. (c) Cr5+, 37.45 A. (d) Au3+, 3.57 Aarrow_forwardElectrolysis of a solution of CuSO4(aq) to give copper metal is carried out using a current of 0.66 A. How long should electrolysis continue to produce 0.50 g of copper?arrow_forwardFor the following half-reaction, = 2.07 V: A1F63(aq)+3eAl(s)+6F(aq) Using data from Table 17-1, calculate the equilibrium constant at 25C for the reaction A13+(aq)+6F(aq)A1F63(aq)K=?arrow_forward
- How long would it take to electroplate a metal surface with 0.500 g nickel metal from a solution of Ni2+ with a current of 4.00 A?arrow_forwardHydrogen gas is produced when water is electrolyzed. 2H2O(g)2H2(g)+O2(g) A balloonist wants to fill a balloon with hydrogen gas. How long must a current of 12.0 A be used in the electrolysis of water to fill the balloon to a volume of 10.00 L and a pressure of 0.924 atm at 22°C?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_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
- Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning