On mixing ethyl acetate with aqueous sodium chloride, the composition of the resultant solution is
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Q: Why doesn't NaCl react with water to form HCl and NaOH?

NaCl is a salt of a strong acid and a strong base. Its constituent ions ($\text{Na}^+$ and $\text{Cl}^-$) are very weak conjugate acids/bases, meaning they have virtually no affinity to react with water molecules. Thus, no hydrolysis occurs.

Q: Can water alone hydrolyze the ester without any catalyst?

Technically, yes, but the reaction is incredibly slow at room temperature—so slow that for all practical laboratory purposes, we consider it as 'no reaction' unless an acidic or basic catalyst is added.

Q: What if we used sodium acetate instead of sodium chloride?

Sodium acetate is a salt of a weak acid and a strong base. Its aqueous solution is basic due to the hydrolysis of the acetate ion. This basic medium would slowly catalyze the hydrolysis of ethyl acetate.

Q: Is ethyl acetate completely soluble in the aqueous NaCl solution?

Ethyl acetate is only slightly soluble in water. In a real laboratory scenario, if you mix significant amounts, you would likely see two separate liquid layers, further preventing any meaningful interaction.

Q: Why is this question asked if the answer is 'no reaction'?

Examiners love these questions because they test whether you blindly apply formulas or actually understand the prerequisites for a chemical reaction. It checks your grasp on salt hydrolysis and ester properties simultaneously.

Question

On mixing ethyl acetate with aqueous sodium chloride, the composition of the resultant solution is

Options:

(A) $	ext{CH}_3	ext{COOC}_2	ext{H}_5 + 	ext{NaCl}$

(B) $	ext{CH}_3	ext{COONa} + 	ext{C}_2	ext{H}_5	ext{OH}$

(C) $	ext{CH}_3	ext{COCl} + 	ext{C}_2	ext{H}_5	ext{OH} + 	ext{NaOH}$

(D) $	ext{CH}_3	ext{Cl} + 	ext{C}_2	ext{H}_5	ext{COONa}$

Sigma Percentile · Accepted Answer

Sometimes, the most profound chemistry questions are the ones where absolutely nothing happens. This problem is a classic example of testing your fundamental understanding of reaction conditions and the nature of salts in an aqueous medium.

### Analyzing the Setup
We are given two components to mix: **ethyl acetate** ($	ext{CH}_3	ext{COOC}_2	ext{H}_5$) and an **aqueous solution of sodium chloride** ($	ext{NaCl}$).

Ethyl acetate is a common ester. In organic chemistry, esters are known to undergo a reaction called hydrolysis, where water breaks the ester bond to form a carboxylic acid and an alcohol. However, this reaction is notoriously slow in pure water. To make it happen at a measurable rate, we need a catalyst.

### The Nature of Aqueous Sodium Chloride
Let's shift our focus to the other component: aqueous $	ext{NaCl}$. Sodium chloride is the salt of a strong acid ($	ext{HCl}$) and a strong base ($	ext{NaOH}$).

When dissolved in water, it dissociates completely into $	ext{Na}^+$ and $	ext{Cl}^-$ ions. Because both parent compounds are strong, neither the sodium ion nor the chloride ion has any tendency to react with water. This means they do not undergo salt hydrolysis. Consequently, the concentration of $	ext{H}^+$ and $	ext{OH}^-$ ions in the solution remains equal to that of pure water, making the solution **perfectly neutral** with a $	ext{pH}$ of $7$.

### The Requirements for Ester Hydrolysis
For the hydrolysis of an ester to proceed, the medium must be either **acidic** (providing excess $	ext{H}^+$ ions) or **basic** (providing excess $	ext{OH}^-$ ions). These ions act as catalysts, lowering the activation energy required to break the ester linkage.

Since our aqueous $	ext{NaCl}$ solution is strictly neutral, it fails to provide the necessary acidic or basic environment.

### The Final Verdict
Without the required catalyst, the ethyl acetate molecules and the sodium and chloride ions simply float around each other without interacting chemically. There is no bond breaking and no bond forming.

Therefore, the resultant solution is merely a physical mixture of the original reactants. The correct composition of the resultant solution is simply **$	ext{CH}_3	ext{COOC}_2	ext{H}_5 + 	ext{NaCl}$**.

Animated Solution for Chemistry - Ionic Equilibrium: On mixing ethyl acetate with aqueous sodium chloride, the composition of the resultant solution is

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Visualized Solution

\text{Analyzing the Reactants}

\text{Nature of Aqueous NaCl}

\text{Conditions for Ester Hydrolysis}

\text{Final Conclusion}

The Sigma Insight: Hydrolsis of Salts

Analyzing the Setup

The Nature of Aqueous Sodium Chloride Let's shift our focus to the other component: aqueous $NaCl$

The Requirements for Ester Hydrolysis For the hydrolysis of an ester to proceed, the medium must be either acidic (providing excess $H^{+}$ ions) or basic (providing excess $OH^{-}$ ions)

The Final Verdict Without the required catalyst, the ethyl acetate molecules and the sodium and chloride ions simply float around each other without interacting chemically

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