[hamil]

Lets say I have an acid that when mixed with water does not disassociate completely. For this situation, the pH would not be what would be calculated from the mol-volume relationship. If I did a titration on the acid mixture, should I expect a correct or erroneous determination of the molarity of the acid mixture. Put another way, would the disassociation of the acid change as the acid approaches neutralization?

[Borek]

Think in terms of LeChatelier's principle. By adding base you remove one of the dissociation products. What effect would you expect?

[hamil]

I would think that as some of the H was neutralized that more would be produced and that the titration would give the molarity of the acid mixture as if it disassociated completely, yes??

[Borek]

Yes.