Mr. T. Rains was given a 50.0 mL sample of 0.150 M solution ofHCOOH. Using a buret, he transferred 25.0 mL of the weak acidinto a 250 mL Erlenmeyer flask. He then titrated the acidwith a standardized solution of 0.0987 M NaOH.
a. How many moles of the weak acid were added to theErlenmeyer flask?
b. How many moles of NaOH are required to neutralize(reach the equivalence point) the sample of weak acid?
c. How many milliliters of the NaOH are required toneutralize the sample of weak acid?
d. How many moles of NaOH have been added at one half ofthe volume in part 'c' (volume at the half equivalencepoint)?
e. How many moles of the weak acid have reacted at thehalf equivalence point?
f. Calculate the pH of the solution at the half equivalence point.
g. Explain how the pH at the half equivalence point isrelaated to Ka for the weak acid.