1. Temperature: As temperature increases, the molecules gain more kinetic energy and vibrate more intensely. This increased vibration disrupts the electrostatic interactions holding the hydrogen bond together.

2. Solvent: Polar solvents can compete with the hydrogen bonding interactions. For example, water molecules can form hydrogen bonds with the molecules that were previously hydrogen bonded to each other, thus weakening the original bond.

3. pH: Extreme pH values can disrupt the charge distribution of the molecules involved in hydrogen bonding. For instance, a low pH (acidic) can protonate the acceptor molecule, weakening the hydrogen bond. Similarly, a high pH (basic) can deprotonate the donor molecule, achieving the same effect.

4. Distance: The strength of a hydrogen bond is inversely proportional to the distance between the donor and acceptor atoms. As the distance increases, the electrostatic interactions weaken.

5. Bond Angle: The optimal angle for a hydrogen bond is linear (180°). Deviations from this angle can reduce the strength of the bond.

6. Substituents: The presence of bulky substituents near the hydrogen bonding site can create steric hindrance, making it difficult for the molecules to approach each other and form a strong bond.

7. Electrostatic Interactions: The presence of other strong electrostatic interactions (like ionic bonds) can compete with hydrogen bonds and weaken them.

8. Entropy: The formation of a hydrogen bond restricts the freedom of movement of the involved molecules, decreasing entropy. This decrease in entropy makes the formation of hydrogen bonds less favorable, especially at higher temperatures.

It is important to remember that these factors are interconnected and often act in combination to affect the strength of hydrogen bonds.