Ch.15 - Acid and Base EquilibriumWorksheetSee 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: 1. For Mn3+, write an equation that shows how the cation acts as an acid.2. For C5H5NH+, write an equation that shows how the cation acts as an acid.

Problem

1. For Mn3+, write an equation that shows how the cation acts as an acid.

2. For C5H5NH+, write an equation that shows how the cation acts as an acid.

Solution

To determine if a cation would produce a neutral or acidic solution in water, we will follow this set of rules.


For cations

• transition metal

▪ charge of +2 or higher → acidic

▪ less than +2 → neutral solution

• main group metal

▪ charge of +3 or higher → acidic

▪ less than +3 → neutral solution 

• amines - compounds with only nitrogen or hydrogen (i,e. NH3) or with carbon, nitrogen and hydrogen

▪ positive amines → acidic

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