posted by Anonymous .
It says prepare a theoretical titration of 25 mL of 0.1037 M formic acid (HCOOH; pKa= 3.75) solution (diluted to 100mL volume with deionized water) by 0.0964 M solution of KOH.
It asks to determine the volume of KOH solution needed to reach equivalence point. But I don't even know where to begin.
Formic acid is a monoprotic acid and KOH is a monohydroxy base; therefore, the reaction is 1:1 as follows:
HCOOH + KOH ==> HCOOK + H2O
So moles HCOOH initially = M x L = ??
moles KOH need to exactly neutralize that HCOOH is the same.
Then M KOH = moles KOH/L KOH
You know M KOH and you know moles KOH, solve for L KOH.
When the reaction is 1:1, you can use the simple formula of
mL HCOOH x M HCOOH = mL KOH x M KOH.
You know three of the four; therefore, you can calculate the fourth. You should get the same answer either way.
DrBob222, why don't you just post the damn answer?