Reactions in Aqueous Solutions I: Acids, Bases & Salts

These flashcards cover key concepts, definitions, and theories related to acids, bases, and aqueous solutions from Chapter 10 of the Chemistry textbook.

Aqueous acidic solutions have a sour taste, change blue litmus to red, generate hydrogen with metals, form salts and water with metal oxides and hydroxides, react with salts of weaker acids, and conduct electricity.

What are the properties of aqueous acidic solutions?

Acids are substances that produce H+ in aqueous solutions, and bases are substances that produce OH- in aqueous solutions.

What is the Arrhenius Theory?

Protons generated in acid-base reactions are surrounded by water and are commonly represented as H3O+, which is called the hydronium ion.

What is the significance of the hydronium ion (H3O+)?

An acid is a proton donor (H+), and a base is a proton acceptor.

What does the Brønsted-Lowry Theory state?

Water is amphoteric and can react with itself; this reaction is called autoionization.

What is autoionization of water?

Amphoteric species can behave as both acids and bases.

What characterizes amphoteric species?

For binary acids, acid strength increases with decreasing H-X bond strength.

How does acid strength correlate with bond strength in binary acids?

The strongest acid in water is H3O+, and acids stronger than this react with water to produce H3O+.

What is the leveling effect in water?

Acidic salts are formed by the reaction of polyprotic acids with less than the stoichiometric amount of base.

What are acidic salts?

A Lewis acid is an electron pair acceptor, while a Lewis base is an electron pair donor.

What defines a Lewis acid and a Lewis base?