We recently did an experiment in chem lab with titrations and we are supposed to find out the molarities of some unknown solutions. I thought that I was doing my calculations right, but the checking program that I am using keeps telling me that I am wrong. We made a standard solution that was 0.09769 M and was 250 mL. We used 25mL aliquots of this solution to titrate against an unknown concentration of NaOH. The mean volume of the base that was used was 23.10 mL. I thought, since our acid was KHP with one titratable proton, that I could just use the equation M1V1=M2V2 like so: (0.09769M)(25.00mL)=M2(23.10mL)...can you please explain where my thinking where wrong?