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  2. Base (chemistry) - Wikipedia

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

    Strong bases hydrolyze in water almost completely, resulting in the leveling effect." [7] In this process, the water molecule combines with a strong base, due to the water's amphoteric ability; and, a hydroxide ion is released. [7] Very strong bases can even deprotonate very weakly acidic C–H groups in the absence of water.

  3. Lewis acids and bases - Wikipedia

    en.wikipedia.org/wiki/Lewis_acids_and_bases

    A Lewis base is also a Brønsted–Lowry base, but a Lewis acid does not need to be a Brønsted–Lowry acid. The classification into hard and soft acids and bases ( HSAB theory ) followed in 1963. The strength of Lewis acid-base interactions, as measured by the standard enthalpy of formation of an adduct can be predicted by the Drago–Wayland ...

  4. Organic base - Wikipedia

    en.wikipedia.org/wiki/Organic_base

    An organic base is an organic compound which acts as a base. Organic bases are usually, but not always, proton acceptors. They usually contain nitrogen atoms, which can easily be protonated. For example, amines or nitrogen-containing heterocyclic compounds have a lone pair of electrons on the nitrogen atom and can thus act as proton acceptors. [1]

  5. Alkali - Wikipedia

    en.wikipedia.org/wiki/Alkali

    Alkalis are all Arrhenius bases, ones which form hydroxide ions (OH −) when dissolved in water. Common properties of alkaline aqueous solutions include: Moderately concentrated solutions (over 10 −3 M) have a pH of 10 or greater. This means that they will turn phenolphthalein from colorless to pink.

  6. Weak base - Wikipedia

    en.wikipedia.org/wiki/Weak_base

    The position of equilibrium varies from base to base when a weak base reacts with water. The further to the left it is, the weaker the base. [5] When there is a hydrogen ion gradient between two sides of the biological membrane, the concentration of some weak bases are focused on only one side of the membrane. [6]

  7. Brønsted–Lowry acid–base theory - Wikipedia

    en.wikipedia.org/wiki/Brønsted–Lowry_acid...

    H 2 O is a base because it accepts a proton from CH 3 COOH and becomes its conjugate acid, the hydronium ion, (H 3 O +). [9] The reverse of an acid–base reaction is also an acid–base reaction, between the conjugate acid of the base in the first reaction and the conjugate base of the acid.

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  9. 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.