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  2. Neutralization (chemistry) - Wikipedia

    en.wikipedia.org/wiki/Neutralization_(chemistry)

    Animation of a strong acid–strong base neutralization titration (using phenolphthalein). The equivalence point is marked in red. The equivalence point is marked in red. In chemistry, neutralization or neutralisation (see spelling differences ) is a chemical reaction in which acid and a base react with an equivalent quantity of each other.

  3. Acid strength - Wikipedia

    en.wikipedia.org/wiki/Acid_strength

    Lewis acids reacting with Lewis bases in gas phase and non-aqueous solvents have been classified in the ECW model, and it has been shown that there is no one order of acid strengths. [12] The relative acceptor strength of Lewis acids toward a series of bases, versus other Lewis acids, can be illustrated by C-B plots.

  4. Conjugate (acid-base theory) - Wikipedia

    en.wikipedia.org/wiki/Conjugate_(acid-base_theory)

    If a chemical is a strong acid, its conjugate base will be weak. [3] An example of this case would be the splitting of hydrochloric acid HCl in water. Since HCl is a strong acid (it splits up to a large extent), its conjugate base (Cl −) will be weak. Therefore, in this system, most H + will be hydronium ions H 3 O +

  5. Acid–base reaction - Wikipedia

    en.wikipedia.org/wiki/Acid–base_reaction

    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.

  6. Acid dissociation constant - Wikipedia

    en.wikipedia.org/wiki/Acid_dissociation_constant

    The quantitative behaviour of acids and bases in solution can be understood only if their pK a values are known. In particular, the pH of a solution can be predicted when the analytical concentration and p K a values of all acids and bases are known; conversely, it is possible to calculate the equilibrium concentration of the acids and bases in ...

  7. Enthalpy of neutralization - Wikipedia

    en.wikipedia.org/wiki/Enthalpy_of_neutralization

    When a strong acid, HA, reacts with a strong base, BOH, the reaction that occurs is + + as the acid and the base are fully dissociated and neither the cation B + nor the anion A − are involved in the neutralization reaction. [1] The enthalpy change for this reaction is -57.62 kJ/mol at 25 °C.

  8. HSAB theory - Wikipedia

    en.wikipedia.org/wiki/HSAB_theory

    HSAB is an acronym for "hard and soft (Lewis) acids and bases".HSAB is widely used in chemistry for explaining the stability of compounds, reaction mechanisms and pathways. It assigns the terms 'hard' or 'soft', and 'acid' or 'base' to chemical species.

  9. Hammett acidity function - Wikipedia

    en.wikipedia.org/wiki/Hammett_acidity_function

    The Hammett acidity function (H 0) is a measure of acidity that is used for very concentrated solutions of strong acids, including superacids.It was proposed by the physical organic chemist Louis Plack Hammett [1] [2] and is the best-known acidity function used to extend the measure of Brønsted–Lowry acidity beyond the dilute aqueous solutions for which the pH scale is useful.