Label the following reaction components as weaker acid, conjugate base and the species that predominate at equilibrium (two may be present for this one)
ethylamine + acetone (equilibrium arrows) ethylammonium + acetone enolate
Please help!
To determine which components in the reaction are the weaker acid, conjugate base, and the species that predominate at equilibrium, you need to evaluate the acidity and basicity of each compound involved.
1. Ethylamine (CH3CH2NH2) is a weak base because it has a lone pair of electrons on the nitrogen atom that can accept a proton (H+). It can act as a nucleophile in reactions due to the presence of the lone pair.
2. Acetone (CH3COCH3) does not have any acidic or basic properties. It is a neutral molecule that does not readily donate or accept protons.
Now let's consider how these compounds react and identify the weaker acid, conjugate base, and the species that predominate at equilibrium.
In the given reaction:
ethylamine + acetone ⇌ ethylammonium + acetone enolate
Ethylamine (CH3CH2NH2) donates a proton to acetone (CH3COCH3) via a nucleophilic attack by its nitrogen lone pair on the carbonyl carbon of acetone. This leads to the formation of ethylammonium (CH3CH2NH3+) and acetone enolate as the products.
- Weaker acid: In this case, the weaker acid is ethylamine. It donates a proton to acetone to form the conjugate acid, which is ethylammonium.
- Conjugate base: The conjugate base is the species that remains after the acid donates a proton. In this reaction, the conjugate base is acetone, which has accepted the proton from ethylamine to form the acetone enolate.
- Species that predominate at equilibrium: At equilibrium, there is a mixture of both ethylammonium and acetone enolate species present.
Remember, the position of the equilibrium depends on various factors like the acidity of the weak acid and the basicity of the conjugate base, temperature, and other conditions specific to the reaction.