"In chemistry, there are three definitions in common use of the word "base": Arrhenius bases, Brønsted bases, and Lewis bases."
These are bases that readily accept protons (hydrogen ions) in aqueous solutions, and dissociate completely. Examples include sodium hydroxide (NaOH), potassium hydroxide (KOH), and calcium hydroxide (Ca(OH)2).
Definition of strong bases: This topic covers the definition of strong bases and how they differ from weak bases. It also explains their characteristic properties.
Examples of strong bases: This topic explains the various examples of strong bases which includes group 1 hydroxides (LiOH, NaOH, KOH, etc.), group 2 hydroxides (Ca(OH)2, Sr(OH)2, Ba(OH)2), etc.
Sources and properties of strong bases: This topic explains the various sources and characteristic properties of strong bases, including their solubility in water, high pH, and high reactivity.
Acid-base reactions involving strong bases: This topic explains the acid-base reactions that occur when a strong base is mixed with an acid, leading to the formation of salt and water.
Titration of strong bases: This topic covers the process of titration of strong bases with a standard solution of an acid. It includes the procedure, the equipment used, and the calculations involved.
Uses of strong bases: This topic explains the various applications of strong bases in different areas, including chemical synthesis, analytical chemistry, and manufacturing.
Strong bases in biology: This topic covers the role of strong bases in biological systems, including their function as enzyme activators and their involvement in pH regulation.
Strong bases in industry: This topic covers the various applications of strong bases in industries such as water treatment, oil refining, and metal processing.
Safety precautions when working with strong bases: This topic covers the safety measures that should be taken when working with strong bases, such as the use of gloves and protective clothing, safety goggles, and a fume hood.
Environmental impact of strong bases: This topic covers the potential environmental impact of strong bases, including their effects on water quality, air pollution, and soil health.
Alkali metal hydroxides: These are strong bases that contain alkali metals (such as Na, K, Li) and hydroxide ions. Examples include sodium hydroxide (NaOH), potassium hydroxide (KOH), and lithium hydroxide (LiOH). They are highly soluble in water and have a high pH.
Alkaline earth metal hydroxides: These are strong bases that contain alkaline earth metals (such as Mg, Ca, Sr) and hydroxide ions. Examples include magnesium hydroxide (Mg(OH)2), calcium hydroxide (Ca(OH)2), and strontium hydroxide (Sr(OH)2). They are less soluble in water than alkali metal hydroxides.
Organic bases: These are strong bases that contain carbon and nitrogen. Examples include pyridine (C5H5N), trimethylamine (N(CH3)3), and aniline (C6H5NH2). They have weakly basic properties and are typically used in organic chemistry.
Strong Lewis bases: These are electron pair donors that can react with acids to form adducts. Examples include ammonia (NH3), phosphine (PH3), and water (H2O). They are commonly used in chemical synthesis and catalysis.
Hydrides of electropositive metals: These are strong bases that contain an electropositive metal and a hydride ion. Examples include sodium hydride (NaH), potassium hydride (KH), and lithium hydride (LiH). They are typically used in organic chemistry as reducing agents or as bases for deprotonation.
"In 1884, Svante Arrhenius proposed that a base is a substance which dissociates in aqueous solution to form hydroxide ions OH−."
"These ions can react with hydrogen ions (H+ according to Arrhenius) from the dissociation of acids to form water in an acid–base reaction."
"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."
"A base is a substance that can accept hydrogen cations (H+)—otherwise known as protons."
"Arrhenius bases are a subset of Brønsted bases. However, there are also other Brønsted bases which accept protons, such as aqueous solutions of ammonia (NH3) or its organic derivatives (amines)."
"Some non-aqueous solvents contain Brønsted bases which react with solvated protons."
"G. N. Lewis realized that water, ammonia, and other bases can form a bond with a proton due to the unshared pair of electrons that the bases possess."
"The Lewis theory is more general than the Brønsted model because the Lewis acid is not necessarily a proton, but can be another molecule (or ion) with a vacant low-lying orbital which can accept a pair of electrons."
"One notable example is boron trifluoride (BF3)."
"Some other definitions of both bases and acids have been proposed in the past, but are not commonly used today."