Question

Explain why trichloroacetic acid, \(\mathrm{CCl}_{3} \mathrm{COOH},\) is a stronger acid than acetic acid, \(\mathrm{CH}_{3} \mathrm{COOH}\).

Short answer

Trichloroacetic acid (CCl3COOH) is a stronger acid than acetic acid (CH3COOH) due to the effect of the three chlorine atoms. The electronegativity of the chlorine atoms pulls electron density away from the -COOH group, making it easier for the proton (H+) to be released, thus increasing the acidity.

Step-by-step solution

Understand the Concept of Acidity

The acidity of a molecule is determined by how easily it can lose a proton (H+). In this comparison, both acetic acid and trichloroacetic acid can lose a proton from the -COOH group, becoming -COO-.

Practicing Inductive Effect on Acetic Acid

In acetic acid, the CH3 group is attached to the -COOH acid group. Carbon (C) and Hydrogen (H) exhibit similar electronegativities, meaning there is no significant \'pull\' or shift of electron density from the -COOH group. Hence, the ability of acetic acid to lose a H+ from the -COOH group is not significantly affected by the CH3 group.

Practicing Inductive Effect on Trichloroacetic Acid

In contrast, trichloroacetic acid (CCl3COOH) has three Chlorine (Cl) atoms attached to the -COOH group. Chlorine is highly electronegative and therefore, each of them will pull electron density towards itself. This makes the H+ of the -COOH group more positively charged and therefore, easier to be released as a proton.

Comparing the Acidity

The more easily a molecule can lose a H+ proton, the stronger an acid it is. Therefore, trichloroacetic acid is a stronger acid than acetic acid because the CCl3 group in trichloroacetic acid pulls electron density away from the -COOH group, thereby reducing the proton’s electron density and making it easier for the proton to be released.

Key concepts

Inductive Effect

The inductive effect is a fundamental concept in organic chemistry that significantly influences the acidity of a molecule. It refers to the shifting of electron density through sigma bonds in a molecule, caused by the presence of atoms with differing electronegativities. This effect can either increase or decrease the acidity of a molecule based on the nature of the substituents attached to it.

In the context of acids such as trichloroacetic acid and acetic acid, the inductive effect plays a pivotal role. Substituents that pull electron density away from the acidic site, known as electron-withdrawing groups, can stabilize the negative charge on the acid's conjugate base. As a result, they enhance the molecule's ability to release a proton (H+). On the other hand, electron-donating groups destabilize the conjugate base and make the release of the proton more difficult.

Understanding the inductive effect helps explain why different acids exhibit varying levels of strength. In general:

• Highly electronegative atoms increase acidity due to strong electron-withdrawing character.
• Groups further away from the acidic center have a reduced effect on acidity.

Recognizing and predicting these effects can aid in understanding wider chemical reactivity and interactions.

Trichloroacetic Acid

Trichloroacetic acid (TCA) is a highly effective and stronger acid compared to acetic acid, due to the presence of three chlorine atoms (Cl) in its structure. These three chlorine atoms introduce a significant inductive effect. By pulling electron density away from the carboxyl group (-COOH), they enhance TCA's ability to lose a proton.

Chlorine is a very electronegative element, meaning it has a strong tendency to attract electrons. With three chlorine atoms in TCA, there is a substantial pull on the electron cloud of the molecule.

• This pull increases the positive character of the hydrogen atom bonded to the oxygen in the -COOH group.
• It makes it easier for the hydrogen to be released as a proton, resulting in stronger acidic behavior.

Trichloroacetic acid serves as a powerful example of how the inductive effect can be exploited to increase the strength of acids in chemical applications.

Acetic Acid

Acetic acid, known by its formula \( ext{CH}_3 ext{COOH}\), is a weaker acid in comparison to trichloroacetic acid. The reason lies in the nature of its substituent, the methyl group (CH3). The methyl group is not significantly electronegative compared to chlorine. As such, it does not provide a substantial electron-withdrawing effect.

In acetic acid:

• The carbon and hydrogen in the CH3 group exhibit similar electronegativities, making the acid less effective in losing a proton.
• This lack of strong electron withdrawal does not help in stabilizing the negative charge of the conjugate base.

As a result, the overall acidity of acetic acid is less than that of trichloroacetic acid.
However, acetic acid is still a widely used weak acid in both industrial and household applications. Its mild acidity allows it to be used safely in various products, from food preservatives to cleaning agents.