1. The problem statement, all variables and given/known data. This question is based on an experiment to determine the mass of ASA. Information from the experiment : • ASA is a weak acid with a Ka value of 3.2 x 10^-4. • An ASA tablet has an approximate mass of 500 g. • The experiment used a titration with a standardized 0.100 mol/L NaOH. The balanced equation is HC9H7O4(aq) + NaOH(aq) -> NaC9H7O4(aq) + H2O(l) a) What volume of base will you substitute into the formula when you calculate the number of moles of base used? 2. Relevant equations. n=m/M v=n/c 3. The attempt at the solution First determine molar mass of HC9H7O4 =180.17 g/mol n=m/M =(0.500g ) / (180.17g/mol) =2.78 x 10^-3 mol v=n/c =(2.78 x 10^-3) / (0.1mol/L) =0.0278 mL =27.8 L Could someone let me know if I determined the volume of the base correctly? Thanks.