1. A 0.5452 g sample which contained the monoprotic weak acid, propanoic acid, CH3CH2COOH, was dissolved in ~ 75.0 mL of water and titrated to the equivalence point with 35.81 mL of a 0.0893 M (molarity) NaOH solution.
a. How many moles of propanoic acid were titrated?
b. Was this a pure sample of propanoic acid?
c. If the sample were not, calculate its percent purity.
2. A 0.5062 g sample of a mixture of oxalic acid, H2C2O4, and NaCl was titrated to the equivalence point. The titration required 19.43 mL of 0.1271 M (molarity) NaOH. Oxalic is a diprotic acid.
a. Write a balanced equation for the reaction.
b. Why isn't NaCl shown in the balanced equation above?
c. How many moles of H2C2O4 were titrated?
d. What was the original mass of H2C2O4 in the sample?
e. What percent of the sample was H2C2O4?