autoprotolízis

Autoprotolysis is a chemical process where a substance, typically a solvent, undergoes a proton transfer reaction with itself. This means one molecule of the substance donates a proton to another molecule of the same substance. This is a specific type of autoionization, where ions are formed from neutral molecules. The most common example is the autoprotolysis of water, which results in the formation of hydronium ions (H3O+) and hydroxide ions (OH-). This reaction is represented by the equation 2H2O <=> H3O+ + OH-. The extent to which a solvent undergoes autoprotolysis is quantified by its autoprotolysis constant, K_s. This constant is temperature-dependent and indicates the equilibrium concentration of the ions formed. Solvents that readily undergo autoprotolysis are known as protic solvents, due to their ability to donate protons. Examples of protic solvents include alcohols and carboxylic acids, which also exhibit autoprotolysis, albeit to a lesser extent than water. The reverse of autoprotolysis, where a proton is transferred from one molecule to another, is also possible, leading to the reformation of the original neutral molecules. Understanding autoprotolysis is crucial in fields like acid-base chemistry and electrochemistry, as it influences the pH of solutions and the conductivity of solvents.