This question is based on an experiment to determine the mass of ASA.

Question

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 mg.
• The experiment used a titration with a standardized 0.100 mol/L NaOH.
What volume of base will you substitute into the formula when you calculate the number of moles of base used? I know from looking at the balanced equation that NaOH reacts 1:1 molar with the ASA. HC9H7O4(aq) + NaOH(aq)  NaC9H7O4(aq) + H2O(l)
I am just unsure of how to calculate what volume of base to substitute. Any help is appreciated.

Answer 1

Are you titrating the ASA with NaOH? If so use the volume NaOH in the titration.
Then mols = M NaOH x L NaOH