Prepare a theoretical titration curve for titration of 25.0 mL of 0.1037M formic
ID: 627683 • Letter: P
Question
Prepare a theoretical titration curve for titration of 25.0 mL of 0.1037M formic acid (HCOOH; pKa=3.75) solution (diluted to 100 mL volume with deionized water) by 0.0964M solution of KOH determine the volume of KOH solution needed to reach the equivalence point. calculate pH of the starting solution (remember, it was diluted to 100 mL) calculate pH at the equivalence point (the total volume is now more than 100 mL!) calculate pH at points between the start of titration and equivalence point; choose points so that they will be more dense where change in pH is faster. calculate pH at points from equivalence point up until 150% of volume at equivalence point.Explanation / Answer
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.