- #1

Mary1910

- 31

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**1. Homework Statement .**

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.