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

• Ethyl acetate ($$\text{CH}_3\text{COOC}_2\text{H}_5$$): An organic ester. Esters undergo chemical reactions like hydrolysis under strongly acidic or strongly basic conditions, but are quite stable in neutral environments.
• Sodium chloride solution ($$\text{NaCl}_{(aq)}$$): A salt of a strong acid ($$\text{HCl}$$) and a strong base ($$\text{NaOH}$$). Dissolving it in water yields a completely neutral solution ($$\text{pH} = 7$$) containing stable, unreactive $$\text{Na}^+$$ and $$\text{Cl}^-$$ ions.

When ethyl acetate is mixed with aqueous sodium chloride, no chemical transformation takes place. This is due to several key factors:

• The solution is neutral, so there are no catalytic $$\text{H}^+$$ or $$\text{OH}^-$$ ions available to drive ester hydrolysis or saponification.
• The chloride ion ($$\text{Cl}^-$$) is an extremely weak nucleophile in an aqueous environment because it is heavily stabilized by hydration shells. It cannot attack the carbonyl carbon of the ester to displace the ethoxide leaving group.

Because there is no thermodynamic driving force or kinetic pathway for a reaction, the components simply coexist as a physical mixture without changing their chemical identities.

Since no chemical reaction occurs, the final composition of the solution remains exactly the same as the initial reactants mixed together:

$$\text{CH}_3\text{COOC}_2\text{H}_5 + \text{NaCl}$$

Answer: Option A — $$\text{CH}_3\text{COOC}_2\text{H}_5 + \text{NaCl}$$