Here's why:

* Acid strength is about the tendency to donate a proton (H+) Stronger acids donate protons more readily.

* Reaction rate is about the speed of a reaction. It depends on several factors, including:

* Collision frequency: How often reactant molecules collide.

* Activation energy: The minimum energy required for a reaction to occur.

* Orientation: How molecules collide, which needs to be favorable for the reaction.

Stronger acids can react faster in some cases because:

* They form more reactive intermediates: The protonated form of a weaker base is a better electrophile (attracts electrons) and can lead to faster reactions.

* They can catalyze reactions: Stronger acids can protonate substrates and increase their reactivity.

However, it's not always true:

* Other factors can influence reaction rates: The nature of the base, solvent, temperature, etc., all play a role.

* Weaker acids can sometimes react faster: If a weaker acid is more sterically accessible or forms a more stable intermediate, it can react faster than a stronger acid.

In summary:

Acid strength and reaction rate are distinct concepts. While stronger acids can sometimes react faster, it's not a universal rule. Many other factors influence reaction rates.