![]() The chemical species HA, A - and H 3O + are said to be in equilibrium when their concentrations do not change with the passing of time. Where HA is an acid that dissociates into A -, (known as the conjugate base of the acid) and a hydrogen ion which combines with a water molecule to make a hydronium ion. In aqueous solution, the equilibrium of acid dissociation can be written symbolically as: ![]() It is the equilibrium constant for a chemical reaction known as dissociation of acid–base reactions. The decomposition temperature is not known.Īn acid dissociation constant, K a, is a quantitative measure of the strength of an acid in solution. ![]() S = sublimes, d = decomposes, * measured at 25☌, 2* measured at 50☌, 3* measured at 15☌, 4* measured at 115☌, 5* Measured at solid stateĭ? = Boiling temperature at 1 atm is estimated from low pressure measurements. See also boiling and melting point of hydrocarbons, alcohols and acids, pKa of amines, diamines and cyclic organic nitrogen compounds and pKa of inorganic acids and bases, as well as acid base indicators, Acid-base properties of aqueous solutions of salts with ions from both acids and bases and Buffer solutionsįor full table with Common Names, Boiling temperatures and Densities - rotate the screen! Group In the table below, pK a1 and pK a2 for water solutions at 25☌ are given together with boiling and melting point, density and molecular weight, as well as number of carbon, hydrogen and oxygen atoms in each molecule.īelow the table, figures showing the fractions of the different acid forms in aqueous solutions at varying pH are given for some common diprotic organic acids (values calculated from the tabulated pK as). Definitions of the acid dissociation constant and pKa are given below the figures, together with the definition of some classes of organic acids. ![]()
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