Acids, Bases, and Salts

These flashcards cover key concepts regarding acids, bases, and their properties, as discussed in the lecture notes.

What is the Arrhenius definition of acids and bases?

Acids are substances that produce hydronium ions (H3O+) in water, while bases produce hydroxide ions (OH–) in water.

What is the Brønsted–Lowry definition of acids and bases?

Acids are proton (H+) donors, and bases are proton (H+) acceptors.

What is the Lewis definition of acids and bases?

Acids are electron pair acceptors, and bases are electron pair donors.

What occurs in an Arrhenius acid-base reaction?

The H+ ions from the acid combine with the OH- ions from the base to form water.

What is a conjugate acid-base pair?

A conjugate acid results from a base after it accepts a proton, and a conjugate base results from an acid after it donates a proton.

How does polarity affect the strength of binary acids?

Binary acid strength increases as you move to the right across a period and down a group in the periodic table.

What is the significance of Ka in acid strength?

Ka is the acid dissociation constant, and the larger the Ka, the stronger the acid.

What are strong acids and their characteristics?

Strong acids completely ionize in water and are strong electrolytes; examples include HCl, HBr, HI, H2SO4.

What does pH measure?

pH measures the acidity or basicity of a solution, defined as pH = −log[H3O+].

What is the relationship between [H3O+] and [OH–] in water at 25 °C?

At 25 °C, [H3O+] = [OH–] = 1.0 × 10−7 M, maintaining the ion product constant Kw of 1.0 × 10−14.