Why are water and dimethane not miscible?

Question

Both water and dichloromethane have dipole-dipole intermolecular forces, so shouldn't they be miscible?

If they aren't miscible, shouldn't they separate
according to their densities, which are in proportion to their intermolecular forces?

Answer 1

Your word "dimethane" is wrong and confusing.
Water forms extensive hydrogen bonding between molecules, while dichloromethane does not. Thus complete miscibility of water and dichloromethane requires to destroy massive hydrogen bonding and therefore not favored. The boiling point of dichloromethane is 39 °C. At room temperature both are liquids. Therefore, they should separate
according to their densities. But why do you say "which are in proportion to their intermolecular forces"?