About the Book
Please note that the content of this book primarily consists of articles available from Wikipedia or other free sources online. Pages: 58. Chapters: Carboxylic acid, Carbonic acid, Boric acid, Acid-base reaction, Hydronium, Strong acid, Acid dissociation constant, Hydrogen sulfide, Weak acid, Acids in wine, Hydrofluoric acid, Lewis acids and bases, Piranha solution, Hydrogen iodide, Gastric acid, Helium hydride ion, Chiral Lewis acid, Silicic acid, Hexafluorosilicic acid, Perrhenic acid, Fluoroboric acid, Oleum, Resin acid, Isocyanic acid, Hydrazoic acid, Orthocarbonic acid, Arsenous acid, Hypofluorous acid, Sulfur oxoacid, Acidity function, Hexafluorophosphoric acid, Nitrosylsulfuric acid, Thiocyanic acid, Xenic acid, Alpha acid, Homoconjugation, Molybdic acid, Fulminic acid, Tungstic acid, Lithium borate, Tellurous acid, Diprotic acid, Binary acid, Ortho acid, Monobasic acid, Metaoxyacids, Tribasic acid, Dibasic acid, Cyclopropene acid, ACGT, Lyonium ion, Acidifier. Excerpt: An acid dissociation constant, Ka, (also known as acidity constant, or acid-ionization constant) is a quantitative measure of the strength of an acid in solution. It is the equilibrium constant for a chemical reaction known as dissociation in the context of acid-base reactions. The equilibrium can be written symbolically as: HA A + H, where HA is a generic acid that dissociates by splitting into A, known as the conjugate base of the acid, and the hydrogen ion or proton, H, which, in the case of aqueous solutions, exists as a solvated hydronium ion. In the example shown in the figure, HA represents acetic acid, and A the acetate ion. The chemical species HA, A and H are said to be in equilibrium when their concentrations do not change with the passing of time. The dissociation constant is usually written as a quotient of the equilibrium concentrations (in mol/L), denoted by, and: Due to the many orders of magnitude spanned by Ka values, a logarithmic measure of the acid dissociation consta...
