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In chemistry, an acid–base reaction is a chemical reaction that occurs between an acid and a base.It can be used to determine pH via titration.Several theoretical frameworks provide alternative conceptions of the reaction mechanisms and their application in solving related problems; these are called the acid–base theories, for example, Brønsted–Lowry acid–base theory.
Bases and acids are seen as chemical opposites because the effect of an acid is to increase the hydronium (H 3 O +) concentration in water, whereas bases reduce this concentration. A reaction between aqueous solutions of an acid and a base is called neutralization , producing a solution of water and a salt in which the salt separates into its ...
volume (acid) × concentration (H + ions from dissociation) = volume (base) × concentration (OH − ions) In general, for an acid AH n at concentration c 1 reacting with a base B(OH) m at concentration c 2 the volumes are related by: n v 1 c 1 = m v 2 c 2. An example of a base being neutralized by an acid is as follows. Ba(OH) 2 + 2 H + → Ba ...
Acids and bases are aqueous solutions, as part of their Arrhenius definitions. [1] An example of an Arrhenius acid is hydrogen chloride (HCl) because of its dissociation of the hydrogen ion when dissolved in water. Sodium hydroxide (NaOH) is an Arrhenius base because it dissociates the hydroxide ion when it is dissolved in water. [3]
Litmus is a water-soluble mixture of different dyes extracted from lichens.It is often absorbed onto filter paper to produce one of the oldest forms of pH indicator, used to test materials for acidity.
Perchloric acid: a powerful oxidizing agent; readily forms explosive mixtures; mainly used in the production of rocket fuel: Phosphoric acid: a mineral acid with many industrial uses; commonly used in the laboratory preparation of hydrogen halides Phosphorus pentachloride: one of the most important phosphorus chlorides; a chlorinating reagent.
[5] [6] [7] In the Brønsted–Lowry theory acids and bases are defined by the way they react with each other, generalising them. This is best illustrated by an equilibrium equation. acid + base ⇌ conjugate base + conjugate acid. With an acid, HA, the equation can be written symbolically as:
The course is usually run with a concurrent lab section that gives students an opportunity to experience a laboratory environment and carry out experiments with the material learned in the course. These labs can consist of acid-base titrations , kinetics , equilibrium reactions , and electrochemical reactions .