Dilution Question

[Mr. Study]

Hey guys,

I just need some help on the theory behind dilutions of weak and strong acids.

I know strong acids have a high Ka value and weak acids have a low Ka value but could someone explain using, if possible, equilibrium terms, why is it that a strong acid, if diluted, will have a greater change in pH than when compared to a weak acid?

Thanks.

[DisaFear]

Good question Mr. Study.

I'm not too sure, but I'll give it a go. Feel free to correct me, people, if I seem wrong.

We know that pH=-log[H₃0⁺]
We know that strong acids can be said to virtually ionize 100% in water - high concentration of H⁺ ions.

We know that weak acids do not completely ionize - their H⁺ concentration will be lower (right?) than that of a strong acid. There will be some of the products in the solution still.

So, since there's more free H⁺ ions in dissociated strong acid solutions, their pH's can be influenced more by changes?

Seem correct?