Ch.18 - ElectrochemistryWorksheetSee all chapters
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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 voltaic cell that uses a salt bridge to complete the electrical circuit.How is electrical balance maintained in the left beaker as Zn2+ ions are formed at the anode?

Problem

Two beakers are filled with liquid, and are connected by a salt bridge (allows ion migration).  The beaker on the left contains a Zn (solid) electrode (anode, negative) while the beaker on the right contains a Cu (solid) electrode (cathode, positive). The reaction in the left beaker is Zn (solid) goes to Zn2+ (aqueous) plus 2 e-.  The reaction in the right beaker is Cu2+ (aqueous) plus 2 e- goes to Cu (solid).  A voltmeter is connected to both electrodes; electron flow through the voltmeter is from the Zn anode toward the Cu cathode, and registers 1.10 volts.  Through the salt bridge, anions (e.g. NO3-) migrate toward the anode and cations (e.g. Na+) migrate toward the cathode.
A voltaic cell that uses a salt bridge to complete the electrical circuit.

How is electrical balance maintained in the left beaker as Zn2+ ions are formed at the anode?