How could the dipole force enhance the strength of the london force in a polaric molecule?

Dipole-Dipole interactions are interactions between two atoms that have a large difference in electronegativity (the difference is smaller than ionic interactions). This means that one of the two atoms interacting is bit more electronegative than the other atom, which will cause this atom to have a permanent delta- (aka a permanent negative dipole), which will most likely attract the atom with a Delta+ (less electronegative atom). Example the interaction between the H of a HCl and the Cl of another HCl adjacent to it--> H-Cl----H-Cl. This on a microscopic level, happens because you have a positive atom that changes direction in order to interact with the negative atom of the second compound. So the H of 1st HCl will try to "fit in". HF is another example of Dipole-Dipole interaction within the same molecule. These interactions do not occur in apolar compounds because of unideal geometric configurations, e.g. planarity---> the total dipolar charge would be 0.

London forces are temporary interactions between two adjacent atoms that result when the electrons in these two atoms occupy positions that make the atoms form temporary dipoles. This is because the two atoms have little electronegativity difference, which makes them also to be weaker. In this case the electronic distribution is uneven/asymmetrical. For example you have 3 electrons on the right side of a cloud and none on the right sight of the cloud that surrounds the nucleus. This causes rapid polarization (you have a negative delta on the right side of the nucleus where the 3 electrons are and you have +ive delta on the opposite side, aka left side). This situation may influence neighbouring molecule/s/atom/s, causing them to "counter-polarize" (you have an induced dipole), aka forming a dipole where deltas are opposite to the original atom. E.g. F-F---F-F This happens when the difference in electronegativity is really poor.

This practically means, that London Forces are weaker than Dipole forces because they are less stable/non-permanent and therefore short lasting/temporary. Dipole forces are more permanent because they are stronger interactions within two atoms, you have them when an atom has a different electronegativity by the atom it is interacting with.

DIPOLE-DIPOLE is generally JUST for polar molecules (not apolar), whereas London could be for both Polar and Apolar.