Properties and Reactions of Bases - Concentrated or strong bases are caustic on organic matter and react violently with acidic substances. - Aqueous solutions or molten bases dissociate into ions and conduct electricity. - Bases turn red litmus paper blue, phenolphthalein pink, keep bromothymol blue in its natural blue color, and turn methyl orange-yellow. - The pH of a basic solution at standard conditions is greater than seven. - Bases are bitter.

Neutralization and Alkalinity of Bases - Bases react with water to produce a conjugate acid and a conjugate base. - The equilibrium constant (Kb) for this reaction can be found using the equation: Kb = [BH+][OH-]/[B]. - Bases that react with water have relatively small equilibrium constant values. - Bases with lower equilibrium constant values are weaker. - Some bases, like ammonia, react with water to increase the concentration of hydroxide ions. - Bases react with acids to neutralize each other at a fast rate. - When dissolved in water, strong bases like sodium hydroxide ionize into hydroxide and sodium ions. - When solutions of a base and an acid are mixed, the H+ and OH- ions combine to form water molecules. - Equal quantities of a base and an acid neutralize, leaving only a salt in solution. - Weak bases, like baking soda, should be used to neutralize acid spills. - Bases can neutralize acids even if they don't contain OH groups, like sodium carbonate and ammonia. - Both sodium carbonate and ammonia accept H+ when dissolved in water. - pH can be calculated for aqueous solutions of bases. - Carbon, nitrogen, and oxygen can act as bases by accepting an electron pair bond. - Compounds with resonance stabilization, like sodium acetate, are weaker bases.

Strong Bases - Strong bases can remove a proton from even a very weak acid in an acid-base reaction. - Examples of strong bases include hydroxides of alkali metals and alkaline earth metals. - Some strong bases, like alkaline earth hydroxides, have low solubility. - Low solubility allows for the use of metal hydroxides in antacids to prevent harm to tissues. - Strong bases can stop an increase in the concentration of the hydroxide ion. - Superbases are stronger bases than the hydroxide ion. - Examples of superbases include ethoxide ion, meta-diethynylbenzene dianion, para-diethynylbenzene dianion, and lithium monoxide anion.

Weak Bases and Lewis Bases - A weak base does not fully ionize in an aqueous solution. - Protonation of a weak base is incomplete. - Ammonia is an example of a weak base. - The equilibrium constant for the reaction between ammonia and water is small. - Weak bases have a limited extent of reaction or degree of ionization. - A Lewis base is a molecule with high-energy lone pairs of electrons. - Lewis bases can form adducts with low-energy vacant orbitals in acceptor molecules. - Electron-pair acceptors include neutral molecules and high oxidation state metal ions. - Adducts involving metal ions are described as coordination complexes. - Lewis acid-base reactions involve the sharing of an electron pair and the creation of a high dipole moment.

Uses and Applications of Bases - Basic substances can be used as insoluble heterogeneous catalysts. - Examples include metal oxides like magnesium oxide, calcium oxide, and barium oxide. - Potassium fluoride on alumina and some zeolites also serve as basic catalysts. - Transition metals make good catalysts, many of which are basic substances. - Basic catalysts are used in various chemical reactions such as hydrogenation and the Michael reaction. - Bases are used in the production of various chemicals and materials. - They are utilised in the manufacturing of detergents and cleaning agents. - Bases play a role in wastewater treatment to neutralize acidity. - Many biological processes, such as enzyme activity, are pH-dependent. - Bases are used in agriculture to adjust soil pH for optimal plant growth. - Sodium hydroxide is used in soap, paper, and rayon manufacturing. - Calcium hydroxide is used in the manufacture of bleaching powder and for cleaning sulfur dioxide in power plants. - Magnesium hydroxide is used as an antacid for stomach acidity. - Sodium carbonate is used as washing soda and for water softening. - Sodium bicarbonate is used in cooking, baking powders, and as an antacid.