The ester methyl butanoate has the odor and flavor of strawberries. (14.3, 14.4)


c Write the balanced chemical equation for the acid hydrolysis of methyl butanoate.

Verified step by step guidance

1. Identify the reactants and products involved in the acid hydrolysis of methyl butanoate. The reactants are methyl butanoate and water, and the products are butanoic acid and methanol.
2. Write the unbalanced chemical equation for the reaction: ${\text{C}}_5{\text{H}}_{10}{\text{O}}_2+{\text{H}}_2\text{O}\to {\text{C}}_4{\text{H}}_8{\text{O}}_2+{\text{CH}}_3\text{OH}$.
3. Balance the carbon atoms. There are 5 carbon atoms on the left side (in methyl butanoate) and 5 on the right side (4 in butanoic acid and 1 in methanol).
4. Balance the hydrogen atoms. There are 12 hydrogen atoms on the left side (10 in methyl butanoate and 2 in water) and 12 on the right side (8 in butanoic acid and 4 in methanol).
5. Balance the oxygen atoms. There are 3 oxygen atoms on the left side (2 in methyl butanoate and 1 in water) and 3 on the right side (2 in butanoic acid and 1 in methanol).

Key Concepts

Ester Hydrolysis

Ester hydrolysis is a chemical reaction where an ester reacts with water to form an alcohol and a carboxylic acid. This process can occur under acidic or basic conditions, but in this case, we focus on acid hydrolysis, which involves the presence of an acid catalyst. The reaction is important in organic chemistry as it helps in understanding the behavior of esters in various environments.

Balanced Chemical Equation

A balanced chemical equation represents a chemical reaction with equal numbers of each type of atom on both sides of the equation. Balancing is crucial because it reflects the law of conservation of mass, ensuring that matter is neither created nor destroyed during the reaction. In the case of methyl butanoate hydrolysis, the equation must accurately depict the reactants and products involved.

Acid Catalysis

Acid catalysis involves the use of an acid to increase the rate of a chemical reaction without being consumed in the process. In the context of ester hydrolysis, the acid donates protons to the ester, facilitating the breakdown of the ester bond. This concept is essential for understanding how the reaction proceeds more efficiently under acidic conditions compared to neutral or basic environments.