Acids, Bases, and Salts: Chemistry in Our Daily Lives

Defining Acids and BasesPage 5

Acids and bases are defined by the Arrhenius theory: acids dissociate in aqueous solutions to release Hydrogen ions (H+), while bases release Hydroxide ions (OH-). These ions dictate the chemical reactivity and properties of everyday substances.

Characteristics of Acids and BasesPage 6

Acids have a pH below 7, a sour taste, and turn blue litmus paper red. Examples include Acetic Acid (vinegar), Ascorbic Acid (Vitamin C), and stomach Hydrochloric Acid. Bases have a pH above 7, a bitter, slippery feel, and turn red litmus paper blue. Examples include Sodium Bicarbonate (baking soda), Magnesium Hydroxide (antacids), and Ammonium Hydroxide (cleaning agents).

The pH Scale and IndicatorsPage 8

The pH scale ranges from 0 to 14, where 7 is neutral. It is logarithmic, meaning each whole number shift represents a tenfold change in Hydrogen ion concentration. pH indicators use dye blends to change color, allowing for the determination of a substance's acidity or alkalinity.

Neutralization and Salt FormationPage 9

Neutralization is the reaction between an acid and a base, resulting in the formation of water and a salt (an ionic compound consisting of a cation from the base and an anion from the acid).

Safety and Environmental ImpactPage 10

Concentrated acids and bases are corrosive, requiring proper safety gear. Environmentally, the formation of acid rain—caused by sulfur and nitrogen oxides—poses risks to aquatic ecosystems, vegetation, and infrastructure, highlighting the need for responsible chemical management.