Is it right to say that a dilute acid is stronger than the same acid which has higher molarity? By Ostwald's dilution law I can say that dissociation degree for the dilute sample is more. So it is a better electrolyte. But I also find that pH for concentrated sample is appreciably more. Ka=(conc.)*alpha*alpha(for weak electrolytes) So [H+]=sqrt(Ka*conc.) Actually I can not stomach what I have heard-that a dilute acid is stronger than its concentrated counterpart. I have always thought the more concentrated the stronger it is.