Chapter 14: Acids and Bases – Study Notes

Acids and Bases

Introduction to Acids and Bases

Acids and bases are two fundamental categories of compounds in chemistry, each with distinct properties and important roles in chemical reactions and everyday life. This chapter explores their properties, definitions, reactions, and quantitative aspects.

Properties of Acids

General Properties

• Sour taste: Many acids, such as citric acid in lemons, have a characteristic sour taste.

• Reaction with metals: Acids can dissolve many metals, producing hydrogen gas.

• Effect on indicators: Acids turn blue litmus paper red.

Common Acids and Their Uses

• Hydrochloric acid (HCl): Found in stomach acid, used in cleaning metals and food processing.

• Sulfuric acid (H2SO4): Used in fertilizers, batteries, and manufacturing.

• Nitric acid (HNO3): Used in explosives and dyes.

• Acetic acid (HC2H3O2): Responsible for the sour taste of vinegar.

Carboxylic Acids

Carboxylic acids contain the carboxyl group (–COOH) and are common in biological systems.

Properties of Bases

General Properties

• Bitter taste: Bases often taste bitter (e.g., caffeine in coffee).

• Slippery feel: Bases feel slippery because they react with oils on skin to form soap-like substances.

• Effect on indicators: Bases turn red litmus paper blue.

Common Bases and Their Uses

• Sodium hydroxide (NaOH): Used in soap and drain cleaners.

• Potassium hydroxide (KOH): Used in manufacturing and cleaning.

• Sodium bicarbonate (NaHCO3): Baking soda, used as an antacid.

Definitions of Acids and Bases

Arrhenius Definition

• Acid: Produces H+ ions in aqueous solution.

• Base: Produces OH− ions in aqueous solution.

Brønsted–Lowry Definition

• Acid: Proton (H+) donor.

• Base: Proton (H+) acceptor.

This definition applies to a wider range of reactions, including those not in water.

Conjugate Acid-Base Pairs

In Brønsted–Lowry reactions, acids and bases form conjugate pairs, differing by one proton.

Reactions of Acids and Bases

Neutralization Reactions

When an acid reacts with a base, water and a salt are formed. The general equation is:

$\mathrm{Acid + Base \rightarrow Water + Salt}$

Net ionic equation for many neutralizations:

$\mathrm{H^+ (aq) + OH^- (aq) \rightarrow H_2O (l)}$

Acid Reactions with Metals and Metal Oxides

• Acid + Metal: Produces hydrogen gas and a salt.

• Acid + Metal Oxide: Produces water and a salt.

Acid–Base Titration

Principle of Titration

Titration is a laboratory technique to determine the concentration of an unknown acid or base by reacting it with a solution of known concentration.

Strong and Weak Acids and Bases

Strong Acids

Strong acids completely ionize in solution. Examples include HCl, HNO3, HBr, HClO4, HI, and H2SO4 (first proton only).

Weak Acids

Weak acids only partially ionize in solution. Examples include HF, acetic acid, and carbonic acid.

Strong Bases

Strong bases completely dissociate in solution. Examples include NaOH, KOH, Ba(OH)2, Sr(OH)2, Ca(OH)2, LiOH.

Weak Bases

Weak bases only partially react with water to produce OH−. Ammonia (NH3) is a common weak base.

Self-Ionization of Water and the Ion Product Constant

Self-Ionization of Water

Water can act as both an acid and a base, producing small, equal concentrations of H3O+ and OH− in pure water.

$\mathrm{2H_2O(l) \rightleftharpoons H_3O^+(aq) + OH^-(aq)}$

Ion Product Constant for Water (Kw)

At 25°C:

$\mathrm{K_w = [H_3O^+][OH^-] = 1.0 \times 10^{-14}}$

The pH Scale

Definition and Interpretation

The pH scale expresses the acidity or basicity of a solution based on the concentration of H3O+ ions.

• pH < 7: Acidic

• pH = 7: Neutral

• pH > 7: Basic

Calculating pH

The pH is calculated as:

$\mathrm{pH = -\log [H_3O^+]}$

To find [H3O+] from pH:

$\mathrm{[H_3O^+] = 10^{-pH}}$

Buffers

Definition and Function

A buffer is a solution containing significant amounts of both a weak acid and its conjugate base. Buffers resist changes in pH when small amounts of acid or base are added.

Chemistry and Health Connections

Alkaloids

Alkaloids are organic bases found in plants, often with medicinal or toxic properties (e.g., morphine, caffeine, coniine).

Antifreeze Poisoning

Ethylene glycol (antifreeze) is metabolized to glycolic acid, which can overwhelm the blood's buffer system, leading to dangerous drops in blood pH.

Summary Table: Strong and Weak Acids and Bases

Type	Examples	Ionization/Dissociation
Strong Acid	HCl, HNO3, H2SO4 (1st proton), HBr, HI, HClO4	Complete
Weak Acid	HF, CH3COOH, H2CO3	Partial
Strong Base	NaOH, KOH, Ba(OH)2, Sr(OH)2	Complete
Weak Base	NH3, C5H5N	Partial

Key Equations and Concepts

• Neutralization: $\mathrm{H^+ + OH^- \rightarrow H_2O}$

• Ion product of water: $\mathrm{K_w = [H_3O^+][OH^-] = 1.0 \times 10^{-14}}$

• pH calculation: $\mathrm{pH = -\log [H_3O^+]}$

• [H3O+] from pH: $\mathrm{[H_3O^+] = 10^{-pH}}$