Acids, Bases, Buffers, and Redox Reactions

These flashcards cover key concepts related to acids, bases, buffers, and redox reactions from the lecture notes.

Acetic Acid

A weak acid with a pH around 3, often represented as CH3COOH.

pH

The measure of the acidity or basicity of a solution, calculated as -log[H3O+].

pOH

The measure of the hydroxide ion concentration in a solution; related to pH by the equation pH + pOH = 14.

Buffer

A solution that resists changes in pH when small amounts of acid or base are added.

Hydronium Ion (H3O+)

The ion formed when water gains a hydrogen ion; represents acidity.

Hydroxide Ion (OH-)

The ion formed when water loses a hydrogen ion; represents basicity.

Redox Reaction

A chemical reaction involving reduction and oxidation, where electrons are transferred between reactants.

Oxidation

The process by which a substance loses electrons, leading to an increase in oxidation state.

Reduction

The process by which a substance gains electrons, leading to a decrease in oxidation state.

Reducing Agent

The substance that donates electrons and is oxidized in a redox reaction.

Oxidizing Agent

The substance that accepts electrons and is reduced in a redox reaction.

Calcium Carbonate (CaCO3)

A compound that is commonly found in rocks and is a key player in buffering systems in water.

Acid Rain

Rainwater with a pH less than 5.7, often caused by atmospheric pollution.

Electrode

A conductor through which an electric current enters or leaves an electrolyte or solution.

Cathode

The electrode where reduction occurs in an electrochemical cell.

Anode

The electrode where oxidation occurs in an electrochemical cell.

Rechargeable Battery

A battery that can be recharged by reversing the chemical reactions that occur during discharging.