Acids and bases

Acid

An electron pair acceptor.

Base

An electron pair donor.

Protonated form

The form of a molecule where a proton is available to donate.

Deprotonated form

The form of a molecule where the proton is off the molecule.

Sodium bicarbonate

A common base, also known as baking soda, used as an antacid and source of CO₂.

Sodium carbonate

A common base used in soap production, general cleaning, and water softening.

Potassium hydroxide

A common base used in soap production, batteries, and electroplating.

Sodium hydroxide (Lye)

A common base used in petroleum processing and soap/plastic manufacturing.

Ammonia

A common base used in detergents, fertilizers, and explosive manufacturing.

Magnesium hydroxide

A common base known as milk of magnesia, used as a laxative for constipation.

Aluminum hydroxide

A common base used as an antacid to relieve heartburn and indigestion.

Acid-base solutions

Aqueous solutions that conduct electricity due to electrolytes/ions formed in solution.

Hydronium ions

Ions formed when hydrogen ions react with water.

Hydroxide ions

Ions produced by bases in aqueous solutions.

Salt

A product formed when acids and bases react together.

Acids

Substances that taste sour, have a pH < 7, and turn blue litmus paper red.

Bases

Substances that taste bitter, have a pH > 7, and turn red litmus paper blue.

Neutralization reaction

A reaction in which equal moles of acid and base form salt and water.

pH scale

A method of expressing the concentration of acids and bases, where pH < 7 is acidic, pH = 7 is neutral, and pH > 7 is basic.

Conjugate acid-base pair

Two substances that differ by the presence or absence of a proton (H⁺).

Amphoteric compound

A substance that can react as both an acid and a base, depending on the reaction.

Strong Acid

An acid that completely dissociates in solution.

Weak Acid

An acid that does not fully dissociate in solution.

Strong Base

A base that completely dissociates in solution.

Weak Base

A base that does not fully dissociate in solution.

Titration

A laboratory technique to determine the concentration of a substance by reacting it with a known concentration of another substance.

Titrant

The solution of known concentration used in titration.

Analyte

The solution of unknown concentration being tested in titration.

Diprotic

A substance that can donate two protons.

Triprotic

A substance that can donate three protons.

Hydrochloric acid

Strong acid represented as HCl.

Hydrobromic acid

Strong acid represented as HBr.

Hydroiodic acid

Strong acid represented as HI.

Nitric acid

Strong acid represented as HNO₃.

Sulfuric acid

Strong acid represented as H₂SO₄; only the first proton is strong.

Chloric acid

Strong acid represented as HClO₃.

Perchloric acid

Strong acid represented as HClO₄.

Lithium hydroxide

Strong base represented as LiOH.

Sodium hydroxide

Strong base represented as NaOH.

Potassium hydroxide

Strong base represented as KOH.

Rubidium hydroxide

Strong base represented as RbOH.

Cesium hydroxide

Strong base represented as CsOH.

Strontium hydroxide

Strong base represented as Sr(OH)₂.

Calcium hydroxide

Strong base represented as Ca(OH)₂.

Barium hydroxide

Strong base represented as Ba(OH)₂.

Alkali metals

Group of metals that can react with acids to produce hydrogen.

Carbonates

Compounds that react with acids to produce carbon dioxide.

Electrolytes

Substances that dissociate into ions and conduct electricity in solution.