Acid-base reactions and calculations – basic principles
How it works
Acid-base reactions according to Brønsted are chemical reactions in which protons are transferred. An acid donates protons, a base accepts them. In aqueous solutions, during neutralization oxonium ions and hydroxide ions react to form water; the corresponding salt is also formed. The pH value describes how acidic or basic an aqueous solution is. The strength of an acid or base depends on how far proton donation or proton uptake proceeds in water. In calculations, substance concentration, volume, amount of substance, and in simple cases the pH value are used.
In acid-base reactions, an acid gives off a proton (H⁺), and a base takes it up. The reaction equation must be balanced. For strong monoprotic acids in dilute aqueous solution, pH = –log[H₃O⁺] applies approximately. For neutralizations, the amounts of substance must react in the stoichiometric ratio of the reaction equation; for example n(HCl) = n(NaOH), but n(NaOH) = 2·n(H₂SO₄).
An example
Which statement best describes a neutralization reaction in aqueous solution?
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50 Exercises
To the learning unit →Own explanation and own practice exercises by AmyMath. Subject reference framework: Chemistry. The topic assignment may vary by federal state.