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: Bars of iron are put into each of the three beakers as shown here.In which beaker - A, B, or C - would you expect the iron to show the most corrosion?

Solution: Bars of iron are put into each of the three beakers as shown here.In which beaker - A, B, or C - would you expect the iron to show the most corrosion?

Problem

Bars of iron are put into each of the three beakers as shown here.
A diagram shows three beakers with an electrode: Beaker A has pure water (pH equals 7.0); Beaker B has a dilute HCl (aqueous) solution (pH equals 4.0); and Beaker C has a dilute NaOH (aqueous) solution (pH equals 10.0).

In which beaker - A, B, or C - would you expect the iron to show the most corrosion?

Solution

We are asked to determine in what solution is the corrosion of iron most likely to take place the fastest.


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