Question

Classify each of the following compounds as an acid, base, or both. Be sure to answer all parts.

(a) CH3CH2OH
(b) CH3CH2CH2CH3
(c) CH3CO2CH3

Answer 1

Step-by-step explanation:

According to Bronsted-Lowry an acid is defined as the specie which is able to donate hydrogen ions when dissolved in water.

For example,
`HCl \rightarrow H^(+) + Cl^(-)`

On the other hand, bases are the species which are able to donate hydroxide ions when dissolved in water.

For example,
`NaOH \rightarrow Na^(+) + OH^(-)`

In
`CH_(3)CH_(2)OH` compound, when it will lose hydrogen ion then it will result in the formation of a
`CH_(3)CH_(2)O^(-)` (alkoxide ion). As the carbon atoms are donating their positive charge towards the
`O^(-)` ion so, it will become unstable in nature.

As a result, it will neither give a hydrogen ion or a hydroxide ion.

In
`CH_(3)CH_(2)CH_(2)CH_(3)`, there is no difference in the electronegativity of both carbon and hydrogen atoms. Therefore, this compound is not polar in nature hence, it will neither give a hydrogen or hydroxide ion.

In
`CH_(3)CO_(2)CH_(3)` there is presence of no -OH group. Hence, it will neither give a hydroxide or hydrogen ion.

Thus, we can conclude that none of the given compounds will act as an acid or a base.