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Acid-base reaction, a type of chemical process in which one or more hydrogen ions are exchanged between species that may be neutral (molecules, such as water or acetic acid), or electrically charged (ions, such as ammonium, carbonate, or hydroxide).
What happens during an acid–base reaction? How do acids and bases neutralize one another (or cancel each other out)?
Acid–base reaction - Equilibria, Neutralization, pH: Certain general principles apply to any solvent with both acidic and basic properties—for example, water, alcohols, ammonia, amines, and acetic acid. Denoting the solvent molecule by SH, proton transfer can give rise to the ions SH2+ and S−, sometimes called lyonium and lyate ions ...
Acid–base reaction - Bronsted-Lowry, Definition, Chemistry: In order to resolve the various difficulties in the hydrogen–hydroxide ion definitions of acids and bases, a new, more generalized definition was proposed in 1923 almost simultaneously by J.M. Brønsted and T.M. Lowry.
An acid–base reaction is a type of chemical reaction that involves the exchange of one or more hydrogen ions, H +, between species that may be neutral (molecules, such as water, H 2 O) or electrically charged (ions, such as ammonium, NH 4+; hydroxide, OH −; or carbonate, CO 32−).
Acids (including Lewis acids) and bases act as powerful catalysts for a great variety of chemical reactions, in the laboratory, in industry, and in processes occurring in nature. Historically, catalytic action was regarded as one of the essential characteristics of acids, and the parallel occurrence of catalytic action and electrical ...
Acid-base reactions (neutralization) Since acids donate hydrogen ions and bases accept hydrogen ions, it is no surprise that combining an acid with a base produces a chemical reaction. The free hydrogen ions (H + ) released from the acid combine with the free hydroxide ions from the base (OH − ) to form water (H 2 O) and a salt:
Acidic solvents. The most important strongly acidic solvent is sulfuric acid, which is able to protonate a wide variety of compounds containing oxygen or nitrogen. Thus, water, alcohols, ethers, ketones, nitro compounds, and sulfones all act as bases in sulfuric acid.
Acid–base reaction - Dissociation Constants, Aqueous Solution: The classical method for determining the dissociation constant of an acid or a base is to measure the electrical conductivity of solutions of varying concentrations.
Acid–base reaction - Dissociation, Molecular Acids, Water: In this instance, water acts as a base. The equation for the dissociation of acetic acid, for example, is CH3CO2H + H2O ⇄ CH3CO2− + H3O+.