The predicted boiling point of liquid A, which has both London dispersion forces and dipole-dipole interactions, is expected to be higher than the boiling point of liquid B, which has only London dispersion forces.The reason for this prediction is that the strength of intermolecular forces plays a significant role in determining the boiling point of a substance. A higher boiling point indicates stronger intermolecular forces holding the molecules together, requiring more energy to break those forces and transition from a liquid to a gas phase.London dispersion forces are weak, temporary attractive forces that arise due to the random movement of electrons in molecules. These forces are present in all molecules, regardless of their polarity. The strength of London dispersion forces increases with the size and shape of the molecules.Dipole-dipole interactions, on the other hand, are stronger intermolecular forces that occur between polar molecules. These forces arise due to the attraction between the positive and negative ends of polar molecules.Since liquid A has both London dispersion forces and dipole-dipole interactions, the overall intermolecular forces in liquid A are stronger than those in liquid B, which has only London dispersion forces. As a result, it will require more energy to break the intermolecular forces in liquid A, leading to a higher boiling point compared to liquid B.