Enter a chemical equation for the ionization in water of CH3CH2COOH. Is the acid strong or weak? Select the Lewis structure for the ion formed by the acid when it ionizes.
Chemical equation:
Note: Include physical states.
CH3CH2COOH(l) + H2O(l) ==> H3O^+(aq) + CH3CH2COO^-(aq)
The chemical equation for the ionization in water of CH3CH2COOH (acetic acid) is:
CH3CH2COOH + H2O ⇌ CH3CH2COO- + H3O+
This equation shows that acetic acid reacts with water to produce the acetate ion (CH3CH2COO-) and hydronium ion (H3O+).
Acetic acid is a weak acid because it does not completely ionize in water. Only a small percentage of the acid molecules dissociate into ions.
Regarding the Lewis structure for the acetate ion (CH3CH2COO-), it can be represented as follows:
H H
| |
H - C - C - O(-)
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CH3
To determine the chemical equation for the ionization of CH3CH2COOH in water, we need to understand that CH3CH2COOH is a weak acid.
A weak acid partially dissociates or ionizes in water, whereas a strong acid completely dissociates. The ionization of CH3CH2COOH generates its conjugate base CH3CH2COO- and a hydronium ion H3O+.
The chemical equation for the ionization of CH3CH2COOH in water can be written as:
CH3CH2COOH + H2O → CH3CH2COO- + H3O+
To select the Lewis structure for the ion formed by the acid when it ionizes, we need to understand the Lewis structure concept.
The Lewis structure represents the arrangement of atoms and their bonds in a molecule or ion. It helps us understand the valence electrons, bonding, and overall structure.
Since CH3CH2COOH ionizes to form the CH3CH2COO- ion, we need to remove a hydrogen ion (H+) from CH3CH2COOH and add a negative charge to the carbon atom (C) in order to create the CH3CH2COO- ion.
The Lewis structure of the ion formed (CH3CH2COO-) would look like:
H3C - C - COO-
This structure represents two Carbon atoms bonded to each other with one Carbon atom bonded to three Hydrogen atoms (H3C-) and one Oxygen atom (O) bonded to the Carbon atom (COO-). The negative charge (-) indicates the presence of an extra electron, giving the ion a negative charge.
It's important to note that the Lewis structure is a simplified representation, and the actual structure of the ion may have resonance structures or other factors to consider depending on the context and level of detail required.