Ch.18 - ElectrochemistryWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: The cell in the figure  could be used to provide a measure of the pH in the cathode compartment.Calculate the pH of the cathode compartment solution if the cell emf at 298 K is measured to be +0.684 V

Problem

The cell in the figure The figure shows a voltaic cell where Zn is the anode and a standard hydrogen electrode is the cathode compartment. A voltmeter depicts the value equal to 0.76. Solid Zn loses two electrons to form an aqueous Zn two plus ion. Two aqueous H plus ions gain two electrons to form gaseous H2. could be used to provide a measure of the pH in the cathode compartment.

Calculate the pH of the cathode compartment solution if the cell emf at 298 K is measured to be +0.684 V when [Zn2+] = 0.30 M and PH2  = 0.90 atm .