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: A chemist designs an ion-specific probe for measuring [Ag +] in an NaCl solution saturated with AgCl. One half-cell has an Ag wire electrode immersed in the unknown AgCl-saturated NaCl solution. It is

Problem

A chemist designs an ion-specific probe for measuring [Ag +] in an NaCl solution saturated with AgCl. One half-cell has an Ag wire electrode immersed in the unknown AgCl-saturated NaCl solution. It is connected through a salt bridge to the other half-cell, which has a calomel reference electrode [a platinum wire immersed in a paste of mercury and calomel (Hg2Cl2)] in a saturated KCl solution. The measured Ecell is 0.060 V.

(a) Given the following standard half-reactions, calculate [Ag +].

Calomel: Hg2Cl2(s) + 2e ⟶ 2Hg(l) + 2Cl(aq)             E° = 0.24 V
Silver: Ag+(aq) + e ⟶ Ag(s)                                         E° = 0.80 V

(Hint: Assume that [Cl] is so high that it is essentially constant.)