Hydrogen bonding is exhibited between a polar molecule containing hydrogens with another molecule with an electronegative polar functional group that has available lone-pair electrons. A good example of this would be water. Water is a polar molecule since it is asymmetrical and has a negative and positive end. The hydrogen bonding occurs between the oxygen of one molecule with the hydrogen of another. This accounts for surface tension on water.
Now, to answer your question, Water has stronger hydrogen bonding, but not stronger hydrogen bonds than HF, but it does have stronger hydrogen bonds than ammonia.
There are two things that affect the intermolecular forces in these molecules: the strength of the H-bond itself, and the number of them that can be formed between neighboring molecules.
The larger the difference in electronegativity of the H atom and the other atom (N, O, and F), the stronger the H-bond. Therefore the order is N < O < F.
However, HF can only form one H-bond to one neighbor, while water can form two thus promoting more intermolecular interactions. Ammonia, while it has 3 N-H bonds, has far weaker H-bonds due to the lower electron density on the N-atom compared to the O-atom in water.
Lastly, I would like to add that CH4 (methane) is not polar so it is not able to form hydrogen bonds with other molecules.
Thanks for the question!