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On the other hand, if a chemical is a weak acid its conjugate base will not necessarily be strong. Consider that ethanoate, the conjugate base of ethanoic acid, has a base splitting constant (Kb) of about 5.6 × 10 −10, making it a weak base. In order for a species to have a strong conjugate base it has to be a very weak acid, like water.
Sodium amide is a standard base for dehydrohalogenations. [9] It induces the loss of two equivalents of hydrogen bromide from a vicinal dibromoalkane to give a carbon–carbon triple bond, as in a preparation of phenylacetylene. [10] Usually two equivalents of sodium amide yields the desired alkyne.
The requirement for a good leaving group is relaxed in conjugate base elimination reactions. These reactions include loss of a leaving group in the β position of an enolate as well as the regeneration of a carbonyl group from the tetrahedral intermediate in nucleophilic acyl substitution.
A Lewis base is often a Brønsted–Lowry base as it can donate a pair of electrons to H +; [11] the proton is a Lewis acid as it can accept a pair of electrons. The conjugate base of a Brønsted–Lowry acid is also a Lewis base as loss of H + from the acid leaves those electrons which were used for the A—H bond as a lone pair on the ...
An acid–base reaction is, thus, the removal of a hydrogen ion from the acid and its addition to the base. [21] The removal of a hydrogen ion from an acid produces its conjugate base, which is the acid with a hydrogen ion removed. The reception of a proton by a base produces its conjugate acid, which is the base with a hydrogen ion added.
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.
Structures of three kinds of amides: an organic amide (carboxamide), a sulfonamide, and a phosphoramide. In chemistry, the term amide (/ ˈ æ m aɪ d / or / ˈ æ m ɪ d / or / ˈ eɪ m aɪ d /) [1] [2] [3] is a compound with the functional group R n E(=O) x NR 2, where x is not zero, E is some element, and each R represents an organic group or hydrogen. [4]
As a result, its pK aH is 13.6 [2] (pK b of 0.4) meaning that guanidine is a very strong base in water; in neutral water, it exists almost exclusively as guanidinium. Due to this, most guanidine derivatives are salts containing the conjugate acid.