Concept explainers
The concentration of a hydrogen peroxide solution can be conveniently determined by titration against a standardised potassium permanganate solution in an acidic medium according to the following unbalanced equation:
(a) Balance this equation. (b) If 36.44 mL of a
Interpretation:
The balance equation for the given reaction and the molarity of
Concept introduction:
Oxidation is the addition of the electronegative element and the removal of the electropositive element in a chemical reaction. Reduction is the addition of the electropositive element and the removal of the electronegative element in a chemical reaction.
The chemical reaction in which oxidation and reduction take place simultaneously or the gain and loss of electrons take place in the chemical reaction is called a redox reaction.
A galvanic cell is made up of two half-cells that are cathodic and anodic. This cell converts chemical energy into electrical energy.
When the cell constant is positive and free energy is negative, then the reaction will occur spontaneously.
Answer to Problem 67AP
Solution:
a)
The overall balanced equation is as follows:
b)
Explanation of Solution
a) Balance the equation
Consider that the galvanic cellis made up of
The cell diagram is as follows:
The number of electrons that takes part in the two half-cell reactions should be the same.
Adding the two half-cell reactions gives the overall cell reaction, which is as follows:
Hence, the overall balanced equation is as follows:
b) Molality of the
The volume of
The number of moles of
Substitute the value of the concentration and the volume in the above expression as follows:
The overall balanced equation is as follows:
From the balance equation, 2 moles of
The number of moles of
The molarity of
Substitute the value of the number of moles and the volume in the above expression as follows:
Therefore, the molarity of
Want to see more full solutions like this?
Chapter 19 Solutions
Loose-leaf Version For Chemistry
- An electrode is prepared from liquid mercury in contact with a saturated solution of mercury(I) chloride, Hg2Cl, containing 1.00 M Cl . The cell potential of the voltaic cell constructed by connecting this electrode as the cathode to the standard hydrogen half-cell as the anode is 0.268 V. What is the solubility product of mercury(I) chloride?arrow_forwardAn electrolysis experiment is performed to determine the value of the Faraday constant (number of coulombs per mole of electrons). In this experiment, 28.8 g of gold is plated out from a AuCN solution by running an electrolytic cell for two hours with a current of 2.00 A. What is the experimental value obtained for the Faraday Constant?arrow_forwardA 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_forward
- Order the following oxidizing agents by increasing strength under standard-state conditions: Mg2+(aq), Hg2+(aq), Pb2+(aq).arrow_forwardWhat is the standard cell potential you would obtain from a cell at 25C using an electrode in which Hg22+(aq) is in contact with mercury metal and an electrode in which an aluminum strip dips into a solution of Al3+(aq)?arrow_forwardAn aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning