Ch.15 - Acid and Base EquilibriumWorksheetSee 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 large molecule X is classified as a Lewis acid, and another molecule, Y, is a Bronsted-Lowry acid. Which of the following best describes a comparable behavior in aqueous solution?a. Both molecules will tend to acquire a net positive chargeb. Both molecules will release hydroxide ionsc. Only molecule Y will react with the waterd. Both molecules will release hydrogen gase. Both molecules will tend to acquire a net negative charge

Problem

A large molecule X is classified as a Lewis acid, and another molecule, Y, is a Bronsted-Lowry acid. Which of the following best describes a comparable behavior in aqueous solution?

a. Both molecules will tend to acquire a net positive charge

b. Both molecules will release hydroxide ions

c. Only molecule Y will react with the water

d. Both molecules will release hydrogen gas

e. Both molecules will tend to acquire a net negative charge

Solution

We are asked which of the following statements will be true for a Lewis and Bronstead-Lowry acid. 


Based on the Lewis definition:

Lewis acid is an electron pair acceptor.

Some characteristics of a Lewis acid:

When hydrogen is connected to an electronegative element such as P, O, N, S or halogens

▪ hydrogen gains a partially positive charge → makes hydrogen act as a Lewis acid

Positively charged metal ions

▪ can accept negative electron pairs → can act as Lewis Acids


Let’s define a Bronsted-Lowry Acid. Recall also that Bronsted-Lowry acids and bases occurs in pairs called conjugate acid/base pairs.

Bronsted-Lowry acid → proton (H+) donor

Conjugate base → one less hydrogen form of the Bronsted-Lowry acid


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