Why does it take more base to neutralize a weak acid than a strong acid

So on the pH versus volume graph, it showed that HCOOH required more volume of the same 0.2 mol/L NaOH as compared to HCl.

It seems like it would make sense if it required more NaOH to neutralize the HCl instead of the HCOOH.

Does this have anything to do with collision theory and limiting reagents? I'm really confused.

If you have equal volumes of HCl and HCOOH with equal concentrations, then it will require the same amount of 0.2M NaOH to neutralize both of them. At the equivalence point, the pH of the strong acid - strong base titration will be a pH of 7, but at the equivalence point of the weak acid - strong base titration the equivalence point will be above a pH of 7. The equivalence point will be basic, owing to the hydrolysis of the formate ion (HCOO-). BUT! The volume of added NaOH will be the same to reach either equivalence point provided that the same volume of acids with the same concentrations are used.

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I'm afraid that Emnee's comment, "... the greater strength of the acid will reduce the amount of kinetic energy needed for the products to react and therefore being neutralised (sic)." is nonsense. The kinetic energy of the molecules is a function of temperature only. The "strength" of the acid refers to the degree of dissociation of the acid (not a concentration) and when reacting with a strong base, it won't matter whether its a strong acid or a weak acid, the neutralization reaction will go to completion. The only thing that affects the amount of NaOH used will be the number of available ionizable protons on the acids. This means that if you have the same volume and concentration of either a strong acid or a weak acid you will have the same number of available hydrogen ions to react with OH- ions.

the greater strength of the acid will reduce the amount of kinetic energy needed for the products to react and therefore being neutralised.