A 100.0 mL sample of 0.100 M formic acid, CHOOH, is titrated with 0.200 M KOH. Calculate the pH after 40.0 mL of 0.200 M KOH has been added.
The Ph of the new acid/base is now "poo"
To calculate the pH after 40.0 mL of 0.200 M KOH has been added, we need to determine the concentration of CHOOH and KOH remaining in the solution.
First, let's calculate the number of moles of formic acid (CHOOH) in the initial solution:
Molarity (M) = moles/liter
0.100 M CHOOH = moles/0.100 L
moles of CHOOH = 0.100 M × 0.100 L
Next, we determine the number of moles of KOH added:
Molarity (M) = moles/liter
0.200 M KOH = moles/0.040 L
moles of KOH = 0.200 M × 0.040 L
Now, we need to determine which component is limiting in the reaction. Since the stoichiometry between CHOOH and KOH in this reaction is 1:1, the limiting reagent is the one with fewer moles.
From the above calculations, we can determine that the moles of CHOOH are initially higher than the moles of KOH.
Now, let's calculate the moles of CHOOH and KOH remaining after 40.0 mL of 0.200 M KOH has been added:
moles of CHOOH remaining = moles of CHOOH initially - moles of KOH added
moles of CHOOH remaining = (moles of CHOOH initially) - (moles of KOH)
Finally, we can determine the concentration of CHOOH remaining by dividing the moles of CHOOH remaining by the total volume of the solution:
Molarity (M) = moles/liter
Concentration of CHOOH remaining = (moles of CHOOH remaining) / (total volume of solution in liters)
Using the concentration of CHOOH remaining, we can calculate the pOH and then convert it to pH using the equation pH = 14 - pOH.
I hope this helps!