Arrhenius Theory

• Arrhenius theory defines an acid as a substance that yields hydrogen ions (H+) when it dissociates in water
• Arrhenius theory describes the behavior of an acid in an aqueous environment
• Examples of Arrhenius acids include hydrochloric acid, sulfuric acid, nitric acid, acetic acid, and phosphoric acid
• Whether an acid is strong (e.g. HCl, H2SO4, HNO3) or weak (e.g. CH3COOH, H3PO4), it can still be classified as an Arrhenius acid as long as it can give H+ or produce H3O+ in water
• Arrhenius theory defines a base as a substance that yields hydroxide ions (OH-) when it dissociates in water
• Examples of Arrhenius bases include sodium hydroxide, potassium hydroxide, and calcium hydroxide
• When an Arrhenius acid is mixed with an Arrhenius base, a double displacement reaction occurs, yielding water and a salt as products
• The strength of acids is dependent on the extent of their ionization in water. Strong acids completely ionize/dissociate, while weak acids do not
• In summary, the Arrhenius theory defines an acid as a substance that can give H+ when placed in water, and a base as a substance that can give OH-. A double displacement reaction occurs when an Arrhenius acid is mixed with an Arrhenius base, yielding water and a salt as products