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.
DrBob222, why don't you just post the damn 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.
To determine the volume of KOH solution needed to reach the equivalence point in this theoretical titration, we can use the concept of stoichiometry and the equation for the reaction between formic acid (HCOOH) and KOH.
Let's start by writing the balanced chemical equation for the reaction between formic acid and KOH:
HCOOH + KOH → HCOOK + H2O
From the balanced equation, we can see that the molar ratio between formic acid (HCOOH) and KOH is 1:1. This means that one mole of formic acid reacts with one mole of KOH.
Next, we need to determine the number of moles of formic acid present in the 25 mL of the 0.1037 M formic acid solution. To do this, we will use the formula:
moles = concentration (M) × volume (L)
Given that the volume is 25 mL, we need to convert it to liters:
25 mL = 25/1000 = 0.025 L
Now, we can calculate the number of moles of formic acid:
moles of formic acid = 0.1037 M × 0.025 L = 0.0025925 moles
Since the reaction between formic acid and KOH has a 1:1 molar ratio, we know that 0.0025925 moles of KOH will be required to reach the equivalence point.
Finally, we can determine the volume of the 0.0964 M KOH solution needed to provide 0.0025925 moles of KOH. We can use the formula:
volume (L) = moles / concentration (M)
volume of KOH solution = 0.0025925 moles / 0.0964 M = 0.0269 L
However, we need to convert this volume from liters to milliliters:
volume of KOH solution = 0.0269 L × 1000 = 26.9 mL
Therefore, approximately 26.9 mL of the 0.0964 M KOH solution is needed to reach the equivalence point in this titration.