1. Identify the compound

   Ethyl acetate is an ester with structure: $\mathrm{CH_3COOCH_2CH_3}$

2. Check for possible intermolecular forces

   The main intermolecular forces to consider are:

   • London dispersion forces
   • Dipole-dipole interactions
   • Hydrogen bonding

3. Does ethyl acetate show London dispersion forces?

   Yes. All molecules exhibit London dispersion forces due to temporary induced dipoles.

4. Does ethyl acetate show dipole-dipole interactions?

   Yes. Ethyl acetate is a polar molecule because it contains a polar ester group: $\mathrm{R-COOR'}$ The carbonyl group $\mathrm{C=O}$ creates a permanent dipole, so molecules attract via dipole-dipole forces.

5. Does ethyl acetate show hydrogen bonding between its own molecules?

   No. For hydrogen bonding in a pure liquid, the molecule must contain a hydrogen directly bonded to highly electronegative atoms like $\mathrm{O}$, $\mathrm{N}$, or $\mathrm{F}$.

   In ethyl acetate, there is oxygen present, so it can accept hydrogen bonds, but it has no $\mathrm{O-H}$ or $\mathrm{N-H}$ bond to donate hydrogen bonds.

   Therefore, pure ethyl acetate does not exhibit intermolecular hydrogen bonding among its own molecules.

6. Conclusion

   The predominant intermolecular forces in liquid ethyl acetate are: $\text{London dispersion forces and dipole-dipole interactions}$

7. Option analysis

   • A: Dipole-dipole and hydrogen bonding $\rightarrow$ Incorrect (no self hydrogen bonding)
   • B: Hydrogen bonding and London dispersion $\rightarrow$ Incorrect
   • C: London dispersion, dipole-dipole and hydrogen bonding $\rightarrow$ Incorrect
   • D: London dispersion and dipole-dipole $\rightarrow$ Correct

Therefore, the correct answer is D.