"In chemistry, there are three definitions in common use of the word 'base': Arrhenius bases, Brønsted bases, and Lewis bases."
These are bases that do not contain a nitrogen atom. Examples include hydroxide ion (OH-), oxide ion (O2-), and carbonate ion (CO32-).
Definition of inorganic bases: Inorganic bases are compounds that can accept protons or donate electrons to neutralize acids by reacting with them chemically.
Classification of inorganic bases: Inorganic bases can be classified into strong and weak bases, depending on their ability to accept protons or donate electrons.
Properties of inorganic bases: Inorganic bases can exhibit properties such as basicity, reactivity, solubility, and heat of neutralization.
Examples of inorganic bases: Examples of commonly used inorganic bases include alkali metal hydroxides (NaOH, KOH), ammonia (NH3), and metal oxides (MgO, CaO).
Acid-base reactions: Inorganic bases can interact with acids to form salts and water, in a process called acid-base reactions.
Acid-base titrations: Inorganic bases can be quantitatively analyzed by titrating them with a standard acid solution to determine their concentration.
Lewis acid-base theory: The Lewis acid-base theory is a more general concept that defines an acid as an electron pair acceptor and a base as an electron pair donor.
Bronsted-Lowry acid-base theory: The Bronsted-Lowry acid-base theory defines an acid as a proton donor and a base as a proton acceptor.
pH and pOH: Inorganic bases can affect the pH of a solution by neutralizing acids or by producing hydroxide ions (OH-) in water. The pOH is a measure of the hydroxide ion concentration in a solution.
Buffer solutions: Inorganic bases can be used in buffer solutions to maintain a stable pH, by preventing changes in the hydrogen ion concentration in a solution.
Acidic and basic properties of salts: Salts can have acidic or basic properties depending on their anions and cations. The hydrolysis of salts can produce acidic or basic solutions.
Applications of inorganic bases: Inorganic bases have numerous applications in industries such as agriculture, water treatment, and pharmaceuticals, among others.
Health hazards of inorganic bases: Some inorganic bases can be corrosive or toxic to humans and the environment, and their handling requires proper safety precautions.
Redox reactions: Inorganic bases can be involved in redox reactions, in which electrons are transferred between species leading to oxidation and reduction reactions.
Sodium hydroxide (NaOH): A strong base also known as caustic soda used in various industrial processes.
Potassium hydroxide (KOH): A strong base used in the production of soaps, detergents, and fertilizers.
Calcium hydroxide (Ca(OH)2): A strong base also known as slaked lime used in construction, agriculture, and wastewater treatment.
Ammonia (NH3): A weak base commonly used in household cleaning products, fertilizers, and refrigeration.
Sodium bicarbonate (NaHCO3): A weak base commonly used in baking, as an antacid, and in fire extinguishers.
Magnesium hydroxide (Mg(OH)2): A weak base used in antacids and laxatives.
Aluminum hydroxide (Al(OH)3): A weak base used in antacids and as a flame retardant in plastics.
Zinc oxide (ZnO): A weak base used in sunscreen, cosmetics, and as a food additive.
Carbonate ions (CO32-): A weak base found in baking soda, limestone, and coral reefs.
Hydrogen carbonate (HCO3-): A weak base found in baking powder and in the blood as a buffer to maintain pH levels.
"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."