"In chemistry, there are three definitions in common use of the word 'base': Arrhenius bases, Brønsted bases, and Lewis bases."
This topic covers the physical and chemical properties of bases.
Acids and bases: This topic covers the basic definitions of acids and bases, their properties, and their behavior in aqueous solutions.
pH scale: This topic discusses the pH scale and its relationship to acid and base strength.
Acid-base reactions: This topic covers the basics of acid-base reactions, including the concepts of conjugate acids and bases.
Bronsted-Lowry theory: This topic discusses the Bronsted-Lowry theory of acids and bases and their conjugates.
Lewis theory: This topic covers the Lewis theory of acids and bases and their conjugates.
Strong and weak acids and bases: This topic discusses the differences between strong and weak acids and bases, and how to distinguish between them.
Acid-base equilibrium: This topic covers the equilibrium between acids and their conjugate bases, and bases and their conjugate acids.
Neutralization reactions: This topic discusses neutralization reactions and their importance in everyday life.
Acid-base indicators: This topic covers the use of acid-base indicators to measure the acidity or basicity of a solution.
Buffer solutions: This topic discusses the concept of buffer solutions and how they work to maintain pH levels.
Titration: This topic covers the process of titration and its application in determining unknown concentrations of acid and base solutions.
Properties of water: This topic covers the unique properties of water that make it an important solvent for acids and bases.
Arrhenius theory: This topic discusses the Arrhenius theory of acids and bases and their conjugates.
Acid and base constants: This topic covers the acid and base dissociation constants and their significance in acid-base chemistry.
Amphoteric substances: This topic discusses amphoteric substances and their ability to act as both acids and bases.
Acid rain: This topic covers the causes and effects of acid rain and the role of acid-base reactions in its formation.
Applications in industry: This topic covers the use of acid-base reactions in various industrial processes, such as production of fertilizers and pharmaceuticals.
Biological systems: This topic discusses the importance of acid-base reactions in biological systems, including maintaining the pH of blood and digestion of food.
Arrhenius Base: A substance that dissociates in water to produce hydroxide ions (OH-).
Bronsted-Lowry Base: A substance that accepts a proton (H+) from an acid to form a conjugate acid.
Lewis Base: A substance that donates an electron pair to form a covalent bond with a Lewis acid.
Strong Base: A base that completely dissociates in water to produce hydroxide ions (OH-) and has a high pH.
Weak Base: A base that only partially dissociates in water to produce hydroxide ions (OH-) and has a low pH.
Acidic Base: A base that can act as a weak acid due to the presence of acidic functional groups.
Non-Nucleophilic Base: A base that does not donate its electron pair easily and prefers to carry out elimination reactions.
Nucleophilic Base: A base that readily donates its electron pair and prefers to carry out substitution reactions.
Organic Base: A base that contains a carbon atom and is commonly used in organic synthesis.
Inorganic Base: A base that does not contain a carbon atom, such as hydroxide ion or ammonia.
Redox Base: A base that participates in oxidation-reduction reactions and can act as an oxidizing or reducing agent.
Catalytic Base: A base that participates in a chemical reaction as a catalyst without being consumed in the reaction.
Amphiprotic Base: A base that can act as both an acid and a base depending on the reaction conditions.
Superbase: A base that is highly reactive and can deprotonate even weakly acidic compounds.
"In 1884, Svante Arrhenius proposed that a base is a substance which dissociates in aqueous solution to form hydroxide ions OH−."
"They are slippery to the touch, can taste bitter and change the color of pH indicators (e.g., turn red litmus paper blue)."
"Bases yield solutions in which the hydrogen ion activity is lower than it is in pure water, i.e., the water has a pH higher than 7.0 at standard conditions."
"A soluble base is called an alkali if it contains and releases OH− ions quantitatively."
"Metal oxides, hydroxides, and especially alkoxides are basic, and conjugate bases of weak acids are weak bases."
"Bases reduce the concentration of hydronium (H3O+) ions in water, whereas acids increase this concentration."
"A reaction between aqueous solutions of an acid and a base is called neutralization."
"It produces a solution of water and a salt in which the salt separates into its component ions."
"Any additional such salt precipitates out of the solution."
"A base is a substance that can accept hydrogen cations (H+)—otherwise known as protons."
"Hence, Arrhenius bases are a subset of Brønsted bases."
"Some non-aqueous solvents contain Brønsted bases which react with solvated protons."
"In the Lewis theory, a base is an electron pair donor which can share a pair of electrons with an electron acceptor which is described as a Lewis acid."
"One notable example is boron trifluoride (BF3)."
"Some other definitions of both bases and acids have been proposed in the past."
"All definitions agree that bases are substances that react with acids, as originally proposed by G.-F. Rouelle in the mid-18th century."
"These ions can react with hydrogen ions (H+ according to Arrhenius) from the dissociation of acids to form water in an acid-base reaction."
"Some non-aqueous solvents contain Brønsted bases which react with solvated protons, resulting in an increase in the concentration of hydroxide ion."
"Base is an electron pair donor which can share a pair of electrons with an electron acceptor which is described as a Lewis acid."