1. The problem statement, all variables and given/known data 1.5000 g of diprotic weak acid H2A was dissolved in 100.00 mL volumetric flask. 25.00 mL aliqouts of this solution was titrated with a monoprotic strong base NaOH (0.08000 M). The titre volume of NaOH was 40.00 mL. Calculate the molecular weight of H2A. 2. Relevant equations N/A 3. The attempt at a solution 1 mole of H2A contains 2 moles of H+ 1 mole of NaOH contains 1 mole of OH- 2CaVa = CbVb 2 (Ca)(0.02500 L) = (0.0800 M)(0.04000L) Ca = 0.0640 M #moles of H2A = CaVa = (0.0640 M)(0.10000 L) = 0.00640 mol molecular mass of H2A = mass/# moles = 1.5000 g / 0.00640 mol = 234.375 g/mol My answer is 234.375 but something seems odd about it. Can anyone tell me if I missed something or did something wrong? Thanks!